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Introductory Chemistry: Concepts and Critical Thinking, 7e (Corwin)

Chapter 1  Introduction to Chemistry

 

Key Terms

 

1) What is the term for the pseudoscience that attempted to discover a universal cure for disease and a magic elixir for immortality?

  1. A) alchemy
  2. B) biochemistry
  3. C) inorganic chemistry
  4. D) organic chemistry
  5. E) none of the above

Answer:  A

Section:  Key Terms

 

2) What is the term for the study of chemical substances derived from plants and animals?

  1. A) biochemistry
  2. B) green chemistry
  3. C) inorganic chemistry
  4. D) organic chemistry
  5. E) none of the above

Answer:  A

Section:  Key Terms

 

3) What is the term for the study of the composition and properties of matter?

  1. A) alchemy
  2. B) biochemistry
  3. C) chemistry
  4. D) science
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

4) What is the term for the procedure of collecting data and recording observations under controlled conditions?

  1. A) alchemy
  2. B) chemistry
  3. C) experiment
  4. D) science
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

 

5) What is the term for the design of products and processes that reduce or eliminate hazardous chemical substances?

  1. A) biochemistry
  2. B) green chemistry
  3. C) inorganic chemistry
  4. D) organic chemistry
  5. E) none of the above

Answer:  B

Section:  Key Terms

 

6) What is the term for a tentative proposal of a scientific principle that attempts to explain the meaning of a set of data collected in an experiment?

  1. A) estimation
  2. B) hypothesis
  3. C) natural law
  4. D) theory
  5. E) none of the above

Answer:  B

Section:  Key Terms

 

7) What is the term for the study of chemical substances that do not contain the element carbon?

  1. A) biochemistry
  2. B) green chemistry
  3. C) inorganic chemistry
  4. D) organic chemistry
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

8) What is the term for an extensively tested proposal of a scientific principle that states a measurable relationship at different conditions?

  1. A) experiment
  2. B) hypothesis
  3. C) natural law
  4. D) theory
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

9) What is the term for the study of chemical substances that contain the element carbon?

  1. A) biochemistry
  2. B) green chemistry
  3. C) inorganic chemistry
  4. D) organic chemistry
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

 

10) What is the term for the methodical exploration of nature and the logical explanation of the observations?

  1. A) alchemy
  2. B) chemistry
  3. C) experiment
  4. D) science
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

11) What is the term for an investigation that entails performing an experiment, proposing a hypothesis, testing the hypothesis, and stating a theory or law?

  1. A) alchemy
  2. B) chemistry
  3. C) science
  4. D) scientific method
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

12) What is the term for an extensively tested proposal of a scientific principle that explains the behavior of nature?

  1. A) experiment
  2. B) hypothesis
  3. C) natural law
  4. D) theory
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

Questions for Chapter 1

 

1) What two forces were responsible for bringing the natural world into existence according to the beliefs of the ancient Chinese?

  1. A) male and female
  2. B) positive and negative
  3. C) shiva and vishnu
  4. D) yin and yang
  5. E) none of the above

Answer:  D

Section:  1.1 Evolution of Chemistry

 

2) What four elements composed everything in nature according to the beliefs of the ancient Greeks?

  1. A) air, earth, fire, and water
  2. B) air, earth, salt, and water
  3. C) air, ashes, fire, and water
  4. D) smoke, earth, fire, and water
  5. E) none of the above

Answer:  B

Section:  1.1 Evolution of Chemistry

 

3) Which of the following was a basic element in nature according to Aristotle?

  1. A) ashes
  2. B) ether
  3. C) salt
  4. D) smoke
  5. E) none of the above

Answer:  B

Section:  1.1 Evolution of Chemistry

 

4) Who is generally considered the founder of the scientific method?

  1. A) Aristotle
  2. B) Robert Boyle
  3. C) John Dalton
  4. D) Antoine Lavoisier
  5. E) none of the above

Answer:  B

Section:  1.1 Evolution of Chemistry

 

5) What book helped establish the scientific method by arguing that theories are no better than the experiments on which they are based?

  1. A) Elementary Treatise on Chemistry
  2. B) Methods of Chemical Research
  3. C) Scientific Investigations of Gases
  4. D) The Sceptical Chymist
  5. E) none of the above

Answer:  D

Section:  1.1 Evolution of Chemistry

 

6) Which of the following is a basic step in the scientific method?

  1. A) perform an experiment and collect data
  2. B) analyze experimental data and propose a hypothesis
  3. C) test a hypothesis and state a theory or law
  4. D) all of the above
  5. E) none of the above

Answer:  D

Section:  1.1 Evolution of Chemistry

 

7) What is the difference between a hypothesis and a scientific theory?

  1. A) A hypothesis is a tentative proposal and a theory is a tested proposal.
  2. B) A theory is a tentative proposal and a hypothesis is a tested proposal.
  3. C) A hypothesis requires an experiment and a theory does not.
  4. D) A theory requires an experiment and a hypothesis does not.
  5. E) none of the above

Answer:  A

Section:  1.1 Evolution of Chemistry

 

 

8) What is the difference between a scientific theory and a natural law?

  1. A) A theory is a tentative proposal and a law is a tested proposal.
  2. B) A law is a tentative proposal and a theory is a tested proposal.
  3. C) A theory explains behavior and a law states a measurable relationship.
  4. D) A law explains behavior and a theory states a measurable relationship.
  5. E) none of the above

Answer:  C

Section:  1.1 Evolution of Chemistry

 

9) What question can we ask in order to distinguish between a theory and a law?

  1. A) Does the statement concern atoms?
  2. B) Does the statement concern gases?
  3. C) Is the statement comprehensible?
  4. D) Is the statement measurable?
  5. E) none of the above

Answer:  D

Section:  1.1 Evolution of Chemistry

 

10) Which of the following statements is a scientific theory?

  1. A) Atoms contain protons, neutrons, and electrons.
  2. B) Equal volumes of gases contain the same number of molecules.
  3. C) The energy of two gas molecules is the same before and after a collision.
  4. D) all of the above
  5. E) none of the above

Answer:  D

Section:  1.1 Evolution of Chemistry

 

11) Which of the following statements is a natural law?

  1. A) The mass of substances, before and after a chemical change, is the same.
  2. B) If the volume of a gas doubles, the pressure decreases by a factor of two.
  3. C) The energy derived from a change in mass is found by E = mc2.
  4. D) all of the above
  5. E) none of the above

Answer:  D

Section:  1.1 Evolution of Chemistry

 

12) Who is generally considered the founder of modern chemistry?

  1. A) Aristotle
  2. B) Robert Boyle
  3. C) John Dalton
  4. D) Antoine Lavoisier
  5. E) none of the above

Answer:  D

Section:  1.2 Modern Chemistry

 

 

13) Which of the following is a branch of chemistry?

  1. A) biochemistry
  2. B) inorganic chemistry
  3. C) organic chemistry
  4. D) all of the above
  5. E) none of the above

Answer:  D

Section:  1.2 Modern Chemistry

 

14) Which of the following is a branch of chemistry?

  1. A) analytical chemistry
  2. B) environmental chemistry
  3. C) physical chemistry
  4. D) all of the above
  5. E) none of the above

Answer:  D

Section:  1.2 Modern Chemistry

 

15) In which of the following industries does chemistry play an important role?

  1. A) agriculture
  2. B) medicine
  3. C) petrochemical
  4. D) pharmaceutical
  5. E) all of the above

Answer:  E

Section:  1.2 Modern Chemistry

 

16) In which of the following industries does chemistry play an important role?

  1. A) construction
  2. B) electronics
  3. C) paper
  4. D) transportation
  5. E) all of the above

Answer:  E

Section:  1.2 Modern Chemistry

 

17) Petrochemicals are derived from which of the following of resources?

  1. A) atmosphere
  2. B) petroleum
  3. C) seawater
  4. D) trees
  5. E) none of the above

Answer:  B

Section:  1.2 Modern Chemistry

 

 

18) Which of the following is derived from a petrochemical?

  1. A) a fuel
  2. B) a paint
  3. C) a pesticide
  4. D) all of the above
  5. E) none of the above

Answer:  D

Section:  1.2 Modern Chemistry

 

19) Which of the following is derived from a petrochemical?

  1. A) detergents
  2. B) dyes
  3. C) plastics
  4. D) textiles
  5. E) all of the above

Answer:  E

Section:  1.2 Modern Chemistry

 

20) Which of the following professions requires a knowledge of chemistry?

  1. A) dentist
  2. B) nurse
  3. C) pharmacist
  4. D) sports trainer
  5. E) all of the above

Answer:  E

Section:  1.2 Modern Chemistry

 

21) In a survey by the American Chemical Society, how did entering college students rate chemistry in their daily lives?

  1. A) highly relevant
  2. B) moderately relevant
  3. C) somewhat relevant
  4. D) rarely relevant
  5. E) irrelevant

Answer:  A

Section:  1.3 Learning Chemistry

 

22) In a survey by the American Chemical Society, what percentage of entering college students thought that chemistry is a difficult subject?

  1. A) 1%
  2. B) 5%
  3. C) 10%
  4. D) 83%
  5. E) 100%

Answer:  D

Section:  1.3 Learning Chemistry

 

 

23) Is it possible to observe one visual image and have two different perceptions?

  1. A) yes
  2. B) It is only possible if the image is large.
  3. C) It is only possible if the image is in color.
  4. D) It is only possible if the image is in black and white.
  5. E) no

Answer:  A

Section:  1.3 Learning Chemistry

 

24) Why would a student at first find a problem impossible to solve when later the solution is obvious?

  1. A) The student did not have biology.
  2. B) The student did not have chemistry.
  3. C) The student did not have physics.
  4. D) The student had an unconscious assumption.
  5. E) none of the above

Answer:  D

Section:  1.3 Learning Chemistry

 

25) What is the unconscious assumption that prevents connecting the following nine dots with four straight, continuous lines?

 

 

 

  1. A) A line cannot be longer than 1 inch.
  2. B) A line cannot be drawn at a 45° angle.
  3. C) A line cannot be drawn at a 90° angle.
  4. D) A line cannot be drawn past a dot.
  5. E) none of the above

Answer:  D

Section:  1.3 Learning Chemistry

 

26) Which of the following is a positive association with the study of chemistry?

  1. A) Chemistry is relevant to our daily lives.
  2. B) Chemistry offers career opportunities.
  3. C) Chemistry has biomedical applications.
  4. D) Chemistry benefits society.
  5. E) all of the above

Answer:  E

Section:  1.3 Learning Chemistry

 

 

27) Which of the following is a positive association with the practice of chemistry?

  1. A) Chemistry experiments may be fun.
  2. B) Chemistry experiments may cause injury.
  3. C) Chemistry experiments may be foul smelling.
  4. D) Chemistry experiments may produce toxic waste.
  5. E) none of the above

Answer:  A

Section:  1.3 Learning Chemistry

 

28) What subject is referred to as the central science?

  1. A) biology
  2. B) chemistry
  3. C) geology
  4. D) physics
  5. E) none of the above

Answer:  B

Section:  General Exercises

 

29) What subject is said to be at the crossroads of biology, physics, and geology?

  1. A) biochemistry
  2. B) chemistry
  3. C) environmental chemistry
  4. D) geochemistry
  5. E) none of the above

Answer:  B

Section:  General Exercises

 

30) What is the minimum number of straight, continuous lines that are necessary to connect the following nine dots?

 

 

 

  1. A) 1
  2. B) 2
  3. C) 3
  4. D) 4
  5. E) 5

Answer:  A

Section:  General Exercises

 

 

Chemistry Connection “Worth Your Salt?”

 

1) “Worth your salt” refers to people who earn which of the following?

  1. A) high wages
  2. B) low wages
  3. C) respect
  4. D) salt rations
  5. E) none of the above

Answer:  C

 

2) “Salt money” paid to laborers in Roman times gives rise to what modern term?

  1. A) salary
  2. B) salt of the earth
  3. C) salt rations
  4. D) solarium
  5. E) none of the above

Answer:  A

 

3) What are the sources of ordinary table salt?

  1. A) mining rock salt
  2. B) dissolving salt beds
  3. C) evaporating salt water
  4. D) all of the above
  5. E) none of the above

Answer:  D

 

4) Table salt contains which of the following for proper thyroid function?

  1. A) potassium bromide
  2. B) potassium chloride
  3. C) potassium iodide
  4. D) potassium oxide
  5. E) all of the above

Answer:  C

 

Chemistry Conncection “A Student Success Story”

 

1) Which element was rare and valuable until 1886 when an inexpensive way of producing the metal from its mineral ore was discovered?

  1. A) aluminum
  2. B) copper
  3. C) nickel
  4. D) silicon
  5. E) none of the above

Answer:  A

 

 

2) Who was the American chemistry student that discovered an inexpensive method for producing aluminum metal from its ore?

  1. A) Frederick Alum
  2. B) Thomas Edison
  3. C) Charles Goodyear
  4. D) Charles Hall
  5. E) none of the above

Answer:  D

 

3) Who was the French chemist that discovered an inexpensive method for producing aluminum metal from its ore?

  1. A) Frederick Alum
  2. B) Jacques Charles
  3. C) Paul Héroult
  4. D) Antoine Lavoisier
  5. E) none of the above

Answer:  C

 

 

Introductory Chemistry: Concepts and Critical Thinking, 7e (Corwin)

Chapter 2  The Metric System

 

Key Terms

 

1) What is the term for the amount of energy required to raise one gram of water one degree on the Celsius scale?

  1. A) Calorie
  2. B) calorie
  3. C) joule
  4. D) kilocalorie
  5. E) none of the above

Answer:  B

Section:  Key Terms

 

2) What is the term for the base unit of temperature in the metric system?

  1. A) Celsius degree (°C)
  2. B) Fahrenheit degree (°F)
  3. C) Kelvin unit (K)
  4. D) all of the above
  5. E) none of the above

Answer:  A

Section:  Key Terms

 

3) What is the term for a unit that expresses the volume occupied by a cube 1 centimeter on a side?

  1. A) cm2
  2. B) cm3
  3. C) mm2
  4. D) mm3
  5. E) none of the above

Answer:  B

Section:  Key Terms

 

4) What is the term for the amount of mass in a unit volume?

  1. A) density
  2. B) specific mass
  3. C) specific gravity
  4. D) specific volume
  5. E) none of the above

Answer:  A

Section:  Key Terms

 

 

5) What is the term for a nondecimal system of measurement without any base unit for length, mass, or volume?

  1. A) English system
  2. B) metric system
  3. C) International System (SI)
  4. D) all of the above
  5. E) none of the above

Answer:  A

Section:  Key Terms

 

6) What is the term for a statement of two exactly equal values?

  1. A) exact equivalent
  2. B) exact value
  3. C) identical equivalent
  4. D) identical value
  5. E) none of the above

Answer:  A

Section:  Key Terms

 

7) What is the term for the base unit of temperature in the English system?

  1. A) Celsius degree (°C)
  2. B) Fahrenheit degree (°F)
  3. C) Kelvin unit (K)
  4. D) all of the above
  5. E) none of the above

Answer:  B

Section:  Key Terms

 

8) What is the term for the base unit of mass in the metric system?

  1. A) gram
  2. B) liter
  3. C) meter
  4. D) second
  5. E) none of the above

Answer:  A

Section:  Key Terms

 

9) What is the term that refers to the flow of energy from an object at a higher temperature to an object at a lower temperature?

  1. A) calorie
  2. B) heat
  3. C) specific heat
  4. D) joule
  5. E) none of the above

Answer:  B

Section:  Key Terms

 

 

10) What is the term that refers to a measurement system with seven base units?

  1. A) English system
  2. B) metric system
  3. C) International System (SI)
  4. D) all of the above
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

11) What is the term for a unit of energy in the SI system?

  1. A) Calorie
  2. B) calorie
  3. C) joule
  4. D) kilocalorie
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

12) What is the term for the base unit of temperature in the SI system?

  1. A) Celsius degree (°C)
  2. B) Fahrenheit degree (°F)
  3. C) Kelvin unit (K)
  4. D) all of the above
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

13) What is the term for the base unit of volume in the metric system?

  1. A) gram
  2. B) liter
  3. C) meter
  4. D) second
  5. E) none of the above

Answer:  B

Section:  Key Terms

 

14) What is the term for the base unit of length in the metric system?

  1. A) gram
  2. B) liter
  3. C) meter
  4. D) second
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

 

15) What is the term for a decimal system of measurement with base units for length, mass, and volume?

  1. A) English system
  2. B) metric system
  3. C) troy system
  4. D) all of the above
  5. E) none of the above

Answer:  B

Section:  Key Terms

 

16) What is the term that expresses the amount of a single quantity compared to an entire sample; an expression of parts per hundred parts?

  1. A) percent
  2. B) proportion
  3. C) quotient
  4. D) reciprocal
  5. E) none of the above

Answer:  A

Section:  Key Terms

 

17) What is the term for the relationship between a fraction and its inverse?

  1. A) percent
  2. B) proportion
  3. C) ratio
  4. D) reciprocal
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

18) What is the term for the base unit of time in the metric system?

  1. A) gram
  2. B) liter
  3. C) meter
  4. D) second
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

19) What is the term for the ratio of the density of a substance compared to the density of water at 4 °C?

  1. A) density
  2. B) specific mass
  3. C) specific gravity
  4. D) specific volume
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

 

20) What is the term for the amount of energy required to raise one gram of any substance one degree on the Celsius scale?

  1. A) calorie
  2. B) heat
  3. C) specific heat
  4. D) joule
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

21) What is the term for the average energy of molecules in motion?

  1. A) heat
  2. B) joule
  3. C) specific heat
  4. D) temperature
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

22) What is the term for a systematic method of problem solving which proceeds from a given value to a desired value by the conversion of units?

  1. A) algebraic analysis
  2. B) metric analysis
  3. C) problem analysis
  4. D) unit analysis
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

23) What is the term for a statement of two equivalent quantities?

  1. A) unit analysis
  2. B) unit equation
  3. C) unit equivalent
  4. D) unit factor
  5. E) none of the above

Answer:  B

Section:  Key Terms

 

24) What is the term for the ratio of two equivalent quantities?

  1. A) unit analysis
  2. B) unit equation
  3. C) unit equivalent
  4. D) unit factor
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

 

25) What is the term for the technique of determining the volume of a solid or a gas by measuring the volume of water it displaces?

  1. A) volume by calculation
  2. B) volume by difference
  3. C) volume by displacement
  4. D) volume by immersion
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

Questions for Chapter 2

 

1) Which of the following is a base unit and symbol in the metric system?

  1. A) meter (m)
  2. B) gram (g)
  3. C) liter (L)
  4. D) all of the above
  5. E) none of the above

Answer:  D

Section:  2.1 Basic Units and Symbols

 

2) Which of the following is a base unit and symbol in the metric system?

  1. A) centimeter (cm)
  2. B) kilogram (kg)
  3. C) milliliter (mL)
  4. D) all of the above
  5. E) none of the above

Answer:  E

Section:  2.1 Basic Units and Symbols

 

3) Which of the following is a base unit and symbol in the metric system?

  1. A) decimeter (dm)
  2. B) gram (gm)
  3. C) liter (L)
  4. D) all of the above
  5. E) none of the above

Answer:  C

Section:  2.1 Basic Units and Symbols

 

4) What is the symbol for the metric unit micrometer?

  1. A) cm
  2. B) mm
  3. C) Mm
  4. D) µm
  5. E) none of the above

Answer:  D

Section:  2.1 Basic Units and Symbols

 

 

5) What is the symbol for the metric unit nanogram?

  1. A) mg
  2. B) Ng
  3. C) ng
  4. D) µg
  5. E) none of the above

Answer:  C

Section:  2.1 Basic Units and Symbols

 

6) What is the symbol for the metric unit microliter?

  1. A) cL
  2. B) mL
  3. C) ML
  4. D) µL
  5. E) none of the above

Answer:  D

Section:  2.1 Basic Units and Symbols

 

7) What is the name corresponding to the metric symbol km?

  1. A) kilomega
  2. B) kilometer
  3. C) kilomicro
  4. D) kilomilli
  5. E) none of the above

Answer:  B

Section:  2.1 Basic Units and Symbols

 

8) What is the name corresponding to the metric symbol dg?

  1. A) decagram
  2. B) decigram
  3. C) dekagram
  4. D) dekigram
  5. E) none of the above

Answer:  B

Section:  2.1 Basic Units and Symbols

 

9) What is the name corresponding to the metric symbol mL?

  1. A) megaliter
  2. B) metroliter
  3. C) microliter
  4. D) milliliter
  5. E) none of the above

Answer:  D

Section:  2.1 Basic Units and Symbols

 

 

10) What physical quantity is expressed by the metric unit centimeter?

  1. A) length
  2. B) mass
  3. C) volume
  4. D) density
  5. E) none of the above

Answer:  A

Section:  2.1 Basic Units and Symbols

 

11) What physical quantity is expressed by the metric unit kilogram?

  1. A) length
  2. B) mass
  3. C) volume
  4. D) density
  5. E) none of the above

Answer:  B

Section:  2.1 Basic Units and Symbols

 

12) What physical quantity is expressed by the metric unit milliliter?

  1. A) length
  2. B) mass
  3. C) volume
  4. D) density
  5. E) none of the above

Answer:  C

Section:  2.1 Basic Units and Symbols

 

13) According to the metric system, 1 Tm = ________ m.

  1. A) 1 x 1012
  2. B) 1 x 109
  3. C) 1 x 106
  4. D) 1 x 103
  5. E) none of the above

Answer:  A

Section:  2.2 Metric Conversion Factors

 

14) According to the metric system, 1 Gg = ________ g.

  1. A) 1 x 1012
  2. B) 1 x 109
  3. C) 1 x 106
  4. D) 1 x 103
  5. E) none of the above

Answer:  B

Section:  2.2 Metric Conversion Factors

 

 

15) According to the metric system, 1 ML = ________ L.

  1. A) 1 x 1012
  2. B) 1 x 109
  3. C) 1 x 106
  4. D) 1 x 103
  5. E) none of the above

Answer:  C

Section:  2.2 Metric Conversion Factors

 

16) According to the metric system, 1 m = ________ dm.

  1. A) 1 x 101
  2. B) 1 x 102
  3. C) 1 x 103
  4. D) 1 x 106
  5. E) none of the above

Answer:  A

Section:  2.2 Metric Conversion Factors

 

17) According to the metric system, 1 g = ________ cg.

  1. A) 1 x 101
  2. B) 1 x 102
  3. C) 1 x 103
  4. D) 1 x 106
  5. E) none of the above

Answer:  B

Section:  2.2 Metric Conversion Factors

 

18) According to the metric system, 1 L = ________ mL.

  1. A) 1 x 101
  2. B) 1 x 102
  3. C) 1 x 103
  4. D) 1 x 106
  5. E) none of the above

Answer:  C

Section:  2.2 Metric Conversion Factors

 

19) According to the metric system, 1 s = ________ µs.

  1. A) 1 x 103
  2. B) 1 x 106
  3. C) 1 x 109
  4. D) 1 x 1012
  5. E) none of the above

Answer:  B

Section:  2.2 Metric Conversion Factors

 

 

20) According to the metric system, 1 s = ________ ns.

  1. A) 1 x 103
  2. B) 1 x 106
  3. C) 1 x 109
  4. D) 1 x 1012
  5. E) none of the above

Answer:  C

Section:  2.2 Metric Conversion Factors

 

21) According to the metric system, 1 s = ________ ps.

  1. A) 1 x 103
  2. B) 1 x 106
  3. C) 1 x 109
  4. D) 1 x 1012
  5. E) none of the above

Answer:  D

Section:  2.2 Metric Conversion Factors

 

22) What is the first step in the unit analysis method of problem solving?

  1. A) Write down the unit asked for in the answer.
  2. B) Write down the given value related to the answer.
  3. C) Apply a unit factor to convert a unit in the given value.
  4. D) Round off the answer in the calculator display.
  5. E) none of the above

Answer:  A

Section:  2.3 Metric-Metric Conversions

 

23) What is the second step in the unit analysis method of problem solving?

  1. A) Write down the unit asked for in the answer.
  2. B) Write down the given value related to the answer.
  3. C) Apply a unit factor to convert a unit in the given value.
  4. D) Round off the answer in the calculator display.
  5. E) none of the above

Answer:  B

Section:  2.3 Metric-Metric Conversions

 

24) What is the third step in the unit analysis method of problem solving?

  1. A) Write down the unit asked for in the answer.
  2. B) Write down the given value related to the answer.
  3. C) Apply a unit factor to convert a unit in the given value.
  4. D) Round off the answer in the calculator display.
  5. E) none of the above

Answer:  C

Section:  2.3 Metric-Metric Conversions

 

 

25) What is the three-step sequence in applying the unit analysis method of

problem solving?

  1. A) 1-unknown unit, 2-unit factor, 3-relevant given value
  2. B) 1-unknown unit, 2-relevant given value, 3-unit factor
  3. C) 1-relevant given value, 2-unknown unit, 3-unit factor
  4. D) 1-unit factor, 2-unknown unit, 3-relevant given value
  5. E) 1-unit factor, 2-relevant given value, 3-unknown unit

Answer:  B

Section:  2.3 Metric-Metric Conversions

 

26) What is the three-step sequence in applying the unit analysis method of

problem solving?

  1. A) 1-unit factor, 2-unknown unit, 3-relevant given value
  2. B) 1-unit factor, 2-relevant given value, 3-unknown unit
  3. C) 1-unknown unit, 2-relevant given value, 3-unit factor
  4. D) 1-unknown unit, 2-unit factor, 3-relevant given value
  5. E) 1-relevant given value, 2-unknown unit, 3-unit factor

Answer:  C

Section:  2.3 Metric-Metric Conversions

 

27) What is the three-step sequence in applying the unit analysis method of

problem solving?

  1. A) 1-relevant given value, 2-unknown unit, 3-unit factor
  2. B) 1-unit factor, 2-unknown unit, 3-relevant given value
  3. C) 1-unknown unit, 2-unit factor, 3-relevant given value
  4. D) 1-unknown unit, 2-relevant given value, 3-unit factor
  5. E) 1-unit factor, 2-relevant given value, 3-unknown unit

Answer:  D

Section:  2.3 Metric-Metric Conversions

 

28) If a 20.0 mL test tube measures 15.0 cm, what is the length in meters?

  1. A) 0.150 m
  2. B) 1.50 m
  3. C) 15.0 m
  4. D) 1500 m
  5. E) none of the above

Answer:  A

Section:  2.3 Metric-Metric Conversions

 

29) If a 250 mL beaker weighs 95.4 g, what is the mass in kilograms?

  1. A) 0.0954 kg
  2. B) 0.954 kg
  3. C) 95.4 kg
  4. D) 95,400 kg
  5. E) none of the above

Answer:  A

Section:  2.3 Metric-Metric Conversions

 

 

30) If a 125 mL Erlenmeyer flask weighs 88.5 g, what is the volume in liters?

  1. A) 0.125 L
  2. B) 1.25 L
  3. C) 125 L
  4. D) 125,000 L
  5. E) none of the above

Answer:  A

Section:  2.3 Metric-Metric Conversions

 

31) If an automobile airbag inflates in 25 µs, what is the time in seconds?

  1. A) 0.000 025 s
  2. B) 0.000 25 s
  3. C) 25,000 s
  4. D) 25,000,000 s
  5. E) none of the above

Answer:  A

Section:  2.3 Metric-Metric Conversions

 

32) If a downhill ski measures 185 cm, what is the length in decimeters?

  1. A) 1.85 dm
  2. B) 18.5 dm
  3. C) 1850 dm
  4. D) 18,500 dm
  5. E) none of the above

Answer:  B

Section:  2.3 Metric-Metric Conversions

 

33) If a glass marble weighs 3150 mg, what is the mass in centigrams?

  1. A) 3.15 cg
  2. B) 31.5 cg
  3. C) 315 cg
  4. D) 31,050 cg
  5. E) none of the above

Answer:  C

Section:  2.3 Metric-Metric Conversions

 

34) If a can of soda contains 355 mL, what is the volume in deciliters?

  1. A) 0.355 dL
  2. B) 3.55 dL
  3. C) 35.5 dL
  4. D) 3550 dL
  5. E) none of the above

Answer:  B

Section:  2.3 Metric-Metric Conversions

 

 

35) If a computer chip switches off-on-off in 0.015 µs, what is the switching time in nanoseconds?

  1. A) 0.000 000 015 ns
  2. B) 0.000 015 ns
  3. C) 15 ns
  4. D) 15,000 ns
  5. E) none of the above

Answer:  C

Section:  2.3 Metric-Metric Conversions

 

36) If Earth is 1.50 x 108 km from the Sun, what is the distance in Tm?

  1. A) 1.50 x 10-1Tm
  2. B) 1.50 x 102Tm
  3. C) 1.50 x 105Tm
  4. D) 1.50 x 1023Tm
  5. E) none of the above

Answer:  A

Section:  2.3 Metric-Metric Conversions

 

37) If Earth is 1.50 x 108 km from the Sun, what is the distance in Gm?

  1. A) 1.50 x 10-1Gm
  2. B) 1.50 x 102Gm
  3. C) 1.50 x 105Gm
  4. D) 1.50 x 1020Gm
  5. E) none of the above

Answer:  B

Section:  2.3 Metric-Metric Conversions

 

38) If Earth is 1.50 x 108 km from the Sun, what is the distance in Mm?

  1. A) 1.50 x 10-1Mm
  2. B) 1.50 x 102Mm
  3. C) 1.50 x 105Mm
  4. D) 1.50 x 1017Mm
  5. E) none of the above

Answer:  C

Section:  2.3 Metric-Metric Conversions

 

39) If the radius of a potassium atom is 2.27 x 10-7 mm, what is the radius in µm?

  1. A) 2.27 x 10-16µm
  2. B) 2.27 x 10-10µm
  3. C) 2.27 x 10-4µm
  4. D) 2.27 x 105µm
  5. E) none of the above

Answer:  C

Section:  2.3 Metric-Metric Conversions

 

 

40) If the radius of a silicon atom is 1.18 x 10-8 cm, what is the radius in nm?

  1. A) 1.18 x 10-15nm
  2. B) 1.18 x 10-10nm
  3. C) 1.18 x 10-1nm
  4. D) 1.18 x 103nm
  5. E) none of the above

Answer:  C

Section:  2.3 Metric-Metric Conversions

 

41) If the radius of a nickel atom is 1.25 x 10-9 dm, what is the radius in pm?

  1. A) 1.25 x 10-20pm
  2. B) 1.25 x 10-18pm
  3. C) 1.25 x 10-10pm
  4. D) 1.25 x 102pm
  5. E) none of the above

Answer:  D

Section:  2.3 Metric-Metric Conversions

 

42) Which of the following English-metric equivalents is correct?

  1. A) 1 in. = 2.54 cm
  2. B) 1 lb = 454 g
  3. C) 1 qt = 946 mL
  4. D) all of the above
  5. E) none of the above

Answer:  D

Section:  2.4 Metric-English Conversions

 

43) Which of the following English-metric equivalents is correct?

  1. A) 1 in. = 454 cm
  2. B) 1 lb = 2.54 g
  3. C) 1 qt = 946 mL
  4. D) all of the above
  5. E) none of the above

Answer:  C

Section:  2.4 Metric-English Conversions

 

44) Which of the following English-metric equivalents is correct?

  1. A) 1 in. = 2.54 cm
  2. B) 1 lb = 454 g
  3. C) 1 qt = 946 mL
  4. D) 1 sec = 1.00 s
  5. E) all of the above

Answer:  E

Section:  2.4 Metric-English Conversions

 

 

45) Which of the following unit factors is derived from 1 meter = 39.4 inches?

  1. A) 1 m/1 in.
  2. B) 1 m/39.4 in.
  3. C) 39.4 in./39.4 m
  4. D) 1 in./39.4 m
  5. E) none of the above

Answer:  B

Section:  2.4 Metric-English Conversions

 

46) Which of the following unit factors is derived from 1 kilogram = 2.20 pounds?

  1. A) 1 kg/1 lb
  2. B) 1 kg/2.20 lb
  3. C) 1 lb/1 kg
  4. D) 1 lb/2.20 kg
  5. E) none of the above

Answer:  B

Section:  2.4 Metric-English Conversions

 

47) Which of the following unit factors is derived from 1 liter = 1.06 quarts?

  1. A) 1 L/1 qt
  2. B) 1 L/1.06 qt
  3. C) 1 qt/1 L
  4. D) 1 qt/1.06 L
  5. E) none of the above

Answer:  B

Section:  2.4 Metric-English Conversions

 

48) If a copper wire is 195 cm long, what is the length in inches?

  1. A) 43.0 in.
  2. B) 76.8 in.
  3. C) 195 in.
  4. D) 495 in.
  5. E) 885 in.

Answer:  B

Section:  2.4 Metric-English Conversions

 

49) If a silver chain has a mass of 25.0 g, what is the mass in pounds?

  1. A) 0.0551 lb
  2. B) 0.0264 lb
  3. C) 18.1 lb
  4. D) 37.8 lb
  5. E) 11,400 lb

Answer:  A

Section:  2.4 Metric-English Conversions

 

 

50) If a water bottle contains 375 mL, what is the volume in quarts?

  1. A) 0.396 qt
  2. B) 0.826 qt
  3. C) 1.21 qt
  4. D) 2.52 qt
  5. E) 355,000 qt

Answer:  A

Section:  2.4 Metric-English Conversions

 

51) If the Moon is 246,000 miles from Earth, what is the distance in kilometers?

(Given: 1 mi = 1.61 km )

  1. A) 0.000 006 54 km
  2. B) 15,300 km
  3. C) 153,000 km
  4. D) 396,000 km
  5. E) 3,960,000 km

Answer:  D

Section:  2.4 Metric-English Conversions

 

52) If 842 pounds of Moon samples have been collected from lunar landings, what is the mass expressed in kilograms? (Given: 1 kg = 2.20 lb)

  1. A) 309 kg
  2. B) 383 kg
  3. C) 3830 kg
  4. D) 1850 kg
  5. E) 11,100 kg

Answer:  B

Section:  2.4 Metric-English Conversions

 

53) If an automobile gas tank holds 17.4 gallons, what is the volume in liters?

(Given: 1 gal = 3.785 L)

  1. A) 0.218 L
  2. B) 3.785 L
  3. C) 4.60 L
  4. D) 17.4 L
  5. E) 65.9 L

Answer:  E

Section:  2.4 Metric-English Conversions

 

54) If a 10K race is 10.0 km, what is the distance in yards?

(Given: 1 yd = 0.914 m)

  1. A) 0.00914 yd
  2. B) 0.0109 yd
  3. C) 9140 yd
  4. D) 10,000 yd
  5. E) 10,900 yd

Answer:  E

Section:  2.4 Metric-English Conversions

 

55) If the mass of Mars is 6.42 x 1023 kg, what is the mass in pounds?

(Given: 1 lb = 454 g)

  1. A) 1.41 x 1018lb
  2. B) 2.91 x 1023lb
  3. C) 6.42 x 1023lb
  4. D) 1.41 x 1024lb
  5. E) 2.91 x 1024lb

Answer:  D

Section:  2.4 Metric-English Conversions

 

56) If a patient is injected with 0.500 L of IV saline, what is the volume in quarts?

(Given: 1 qt = 946 mL)

  1. A) 5.29 x 10-7qt
  2. B) 0.500 qt
  3. C) 0.529 qt
  4. D) 4.73 qt
  5. E) 4.73 x 105qt

Answer:  C

Section:  2.4 Metric-English Conversions

 

57) If a 125 micron tissue slice is 125 µm thick, what is the thickness in inches?

  1. A) 4.92 x 10-7
  2. B) 4.92 x 10-3
  3. C) 3.18 x 10-2
  4. D) 3.18 x 106
  5. E) 4.92 x 109

Answer:  B

Section:  2.4 Metric-English Conversions

 

58) If 500 mL of liquid mercury weighs 6.53 kg, what is the mass in pounds?

  1. A) 1.44 lb
  2. B) 2.96 lb
  3. C) 7.19 lb
  4. D) 14.4 lb
  5. E) 2960 lb

Answer:  D

Section:  2.4 Metric-English Conversions

 

59) If 10.0 kg of water occupies 10.0 liters, what is the volume in quarts?

  1. A) 9.46 x 106qt
  2. B) 10.6 qt
  3. C) 10.0 qt
  4. D) 9.46 qt
  5. E) 1.06 x 10-5qt

Answer:  B

Section:  2.4 Metric-English Conversions

 

 

60) A sample of white gold is: 18.0 g gold, 3.0g silver, 2.0 g cobalt, and 1.0 g platinum. What is the percent platinum in the sample?

  1. A) 4.2%
  2. B) 8.3%
  3. C) 13%
  4. D) 25%
  5. E) 75%

Answer:  A

Section:  2.5 The Percent Concept

 

61) A sample of rose gold is: 12.0 g gold, 5.0g silver, and 7.0 g copper. What is the percent copper in the sample?

  1. A) 12%
  2. B) 29%
  3. C) 50%
  4. D) 58%
  5. E) 75%

Answer:  B

Section:  2.5 The Percent Concept

 

62) A sample of lime gold is: 14.0 g gold, 7.0g silver, and 3.0 g copper. What is the percent copper in the sample?

  1. A) 3.0%
  2. B) 13%
  3. C) 29%
  4. D) 58%
  5. E) 67%

Answer:  B

Section:  2.5 The Percent Concept

 

63) A sample of 10K gold contains the following: 10.0 g gold, 4.0 g silver, 5.0g copper, and 5.0 g nickel. What is the percent gold in the sample?

  1. A) 10%
  2. B) 14%
  3. C) 42%
  4. D) 58%
  5. E) 71%

Answer:  C

Section:  2.5 The Percent Concept

 

64) A sample of 18K gold contains the following: 18.0 g gold, 3.0 g silver, and 3.0 g copper. What is the percent gold in the sample?

  1. A) 6.0%
  2. B) 18%
  3. C) 25%
  4. D) 33%
  5. E) 75%

Answer:  E

Section:  2.5 The Percent Concept

 

65) A sample of 22K gold contains the following: 22 g gold, 1.0 g silver, and 1.0 g copper. What is the percent gold in the sample?

  1. A) 1.0%
  2. B) 4.5%
  3. C) 9.1%
  4. D) 92%
  5. E) 96%

Answer:  D

Section:  2.5 The Percent Concept

 

66) Sterling silver contains 925 parts silver and 75 parts copper by mass. What is the percent silver in sterling silver in the sample?

  1. A) 7.50%
  2. B) 8.11%
  3. C) 12.3%
  4. D) 92.5%
  5. E) 100%

Answer:  D

Section:  2.5 The Percent Concept

 

67) Sterling silver contains 925 parts silver and 75 parts copper by mass. What is the percent copper in sterling silver in the sample?

  1. A) 7.5%
  2. B) 8.1%
  3. C) 12%
  4. D) 93%
  5. E) 100%

Answer:  A

Section:  2.5 The Percent Concept

 

68) If a penny has a mass of 3.015 g and is 95.0% copper, what is the mass of copper in the coin?

  1. A) 0.151 g
  2. B) 0.286 g
  3. C) 0.603 g
  4. D) 1.51 g
  5. E) 2.86 g

Answer:  E

Section:  2.5 The Percent Concept

 

69) If a penny has a mass of 3.015 g and is 5.00% zinc, what is the mass of zinc in the coin?

  1. A) 0.151 g
  2. B) 0.286 g
  3. C) 0.603 g
  4. D) 1.51 g
  5. E) 2.86 g

Answer:  A

Section:  2.5 The Percent Concept

 

 

70) If a penny has a mass of 2.507 g and is 2.5% copper, what is the mass of copper in the coin?

  1. A) 0.063 g
  2. B) 0.24 g
  3. C) 0.63 g
  4. D) 2.4 g
  5. E) 6.3 g

Answer:  A

Section:  2.5 The Percent Concept

 

71) If a penny has a mass of 2.507 g and is 97.5% zinc, what is the mass of zinc in the coin?

  1. A) 0.0627 g
  2. B) 0.244 g
  3. C) 0.627 g
  4. D) 2.38 g
  5. E) 2.44 g

Answer:  E

Section:  2.5 The Percent Concept

 

72) If a 5¢ coin has a mass of 5.07 g and is 75.0% copper, what is the mass of copper in the coin?

  1. A) 0.203 g
  2. B) 0.676 g
  3. C) 1.27 g
  4. D) 1.69 g
  5. E) 3.80 g

Answer:  E

Section:  2.5 The Percent Concept

 

73) If a 5¢ coin has a mass of 5.07 g and is 25.0% nickel, what is the mass of nickel in the coin?

  1. A) 0.203 g
  2. B) 0.676 g
  3. C) 1.27 g
  4. D) 1.69 g
  5. E) 3.80 g

Answer:  C

Section:  2.5 The Percent Concept

 

74) Stainless steel is an alloy of iron, chromium, nickel, and manganese metals. If a 5.00g sample is 18.0% chromium, what is the mass of chromium in the sample?

  1. A) 0.0450 g
  2. B) 0.0900 g
  3. C) 0.450 g
  4. D) 0.900 g
  5. E) 1.80 g

Answer:  D

Section:  2.5 The Percent Concept

 

 

75) Stainless steel is an alloy of iron, chromium, nickel, and manganese metals. If a 5.00g sample is 10.5% nickel, what is the mass of nickel in the sample?

  1. A) 0.0263 g
  2. B) 0.0525 g
  3. C) 0.263 g
  4. D) 0.525 g
  5. E) 1.05 g

Answer:  D

Section:  2.5 The Percent Concept

 

76) Stainless steel is an alloy of iron, chromium, nickel, and manganese metals. If a 5.00g sample is 2.00% manganese, what is the mass of manganese in the sample?

  1. A) 0.00500 g
  2. B) 0.0100 g
  3. C) 0.0500 g
  4. D) 0.100 g
  5. E) 0.200 g

Answer:  D

Section:  2.5 The Percent Concept

 

77) Sterling silver is composed of 92.5% silver and 7.5% copper. If a sterling silver ring contains 6.55 g of silver, what is the mass of the ring?

  1. A) 0.0708 g
  2. B) 0.491 g
  3. C) 6.06 g
  4. D) 7.08 g
  5. E) 87.3 g

Answer:  D

Section:  2.5 The Percent Concept

 

78) A ruby contains 52.7% aluminum, 47.1% oxygen, and traces of chromium. If the ruby contains 0.125 g of aluminum, what is the mass of the gemstone?

  1. A) 0.0659 g
  2. B) 0.125 g
  3. C) 0.237 g
  4. D) 0.265 g
  5. E) 0.625 g

Answer:  C

Section:  2.5 The Percent Concept

 

79) A sapphire contains 52.7% aluminum, 47.1% oxygen, and traces of titanium. If the sapphire contains 0.155 g of oxygen, what is the mass of the gemstone?

  1. A) 0.0730 g
  2. B) 0.155 g
  3. C) 0.294 g
  4. D) 0.329 g
  5. E) 0.775 g

Answer:  D

Section:  2.5 The Percent Concept

 

80) If a brass block measures 3.80 cm by 2.55 cm by 1.25 cm, what is the volume of the rectangular solid?

  1. A) 0.0826 cm3
  2. B) 1.19 cm3
  3. C) 1.86 cm3
  4. D) 7.75 cm3
  5. E) 12.1 cm3

Answer:  E

Section:  2.6 Volume by Calculation

 

81) If a copper block measures 5.15 cm by 1.25 cm by 1.25 cm, what is the volume of the rectangular solid?

  1. A) 0.124 cm3
  2. B) 3.30 cm3
  3. C) 4.12 cm3
  4. D) 6.44 cm3
  5. E) 8.05 cm3

Answer:  E

Section:  2.6 Volume by Calculation

 

82) If a stainless steel block measures 5.05 cm by 1.50 cm by 1.25 cm, what is the volume of the rectangular solid?

  1. A) 0.106 cm3
  2. B) 2.69 cm3
  3. C) 4.21 cm3
  4. D) 6.06 cm3
  5. E) 9.47 cm3

Answer:  E

Section:  2.6 Volume by Calculation

 

83) A sheet of aluminum foil has a volume of 0.555 cm3. If the foil measures 10.0cm by 10.0 cm, what is the thickness of the foil?

  1. A) 0.000 555 cm
  2. B) 0.005 55 cm
  3. C) 0.0555 cm
  4. D) 55.5 cm
  5. E) 180 cm

Answer:  B

Section:  2.6 Volume by Calculation

 

 

84) A piece of tin foil has a volume of 0.645 mm3. If the foil measures 10.0 mm by 12.5mm, what is the thickness of the foil?

  1. A) 0.000 516 mm
  2. B) 0.005 16 mm
  3. C) 0.0516 mm
  4. D) 80.6 mm
  5. E) 194 mm

Answer:  B

Section:  2.6 Volume by Calculation

 

85) A sheet of gold foil has a volume of 0.750 cm3. If the foil measures 50.0cm by 10.0cm, what is the thickness of the foil?

  1. A) 0.000 150 cm
  2. B) 0.001 50 cm
  3. C) 0.0150 cm
  4. D) 375 cm
  5. E) 667 cm

Answer:  B

Section:  2.6 Volume by Calculation

 

86) If a steel solid has a volume of 46.5 cm3, what is the volume in cubic inches?

  1. A) 2.84 in.3
  2. B) 7.21 in.3
  3. C) 18.3 in.3
  4. D) 118 in.3
  5. E) 762 in.3

Answer:  A

Section:  2.6 Volume by Calculation

 

87) If a bronze solid has a volume of 25.5 cm3, what is the volume in cubic inches?

  1. A) 1.56 in.3
  2. B) 3.95 in.3
  3. C) 10.0 in.3
  4. D) 64.8 in.3
  5. E) 418 in.3

Answer:  A

Section:  2.6 Volume by Calculation

 

88) If a copper solid has a volume of 8.75 cm3, what is the volume in cubic inches?

  1. A) 0.534 in.3
  2. B) 1.36 in.3
  3. C) 3.44 in.3
  4. D) 22.2 in.3
  5. E) 143 in.3

Answer:  A

Section:  2.6 Volume by Calculation

 

89) A sample of steel is added to a 100-mL graduated cylinder with 45.0 mL of water. Ifthe resulting water level is 55.5 mL, what is the volume of the steel?

  1. A) 10.5 mL
  2. B) 44.5 mL
  3. C) 55.0 mL
  4. D) 89.5 mL
  5. E) 100.5 mL

Answer:  A

Section:  2.7 Volume by Displacement

 

90) A sample of brass is added to a 100-mL graduated cylinder with 55.5 mL of water. If the resulting water level is 68.0 mL, what is the volume of the brass?

  1. A) 12.5 mL
  2. B) 32.0 mL
  3. C) 44.5 mL
  4. D) 87.5 mL
  5. E) 123.5 mL

Answer:  A

Section:  2.7 Volume by Displacement

 

91) A sample of baking soda is heated and releases carbon dioxide gas into a 1000-mL flask. If the flask initially contains 752 mL of water and 305mL remain after the gas has displaced a portion of the water, what is the volume of the gas?

  1. A) 248 mL
  2. B) 305 mL
  3. C) 447 mL
  4. D) 695 mL
  5. E) 752 mL

Answer:  C

Section:  2.7 Volume by Displacement

 

92) If the density of air is 1.29 g/L, which of the following is a unit factor?

  1. A) 1 g/1 L
  2. B) 1 g/1.29 L
  3. C) 1.29 g/1 L
  4. D) 1.29 g/1.29 L
  5. E) 1.29 L/1 g

Answer:  C

Section:  2.8 The Density Concept

 

93) If the density of alcohol is 0.813 g/mL, which of the following is a unit factor?

  1. A) 1 g/1 mL
  2. B) 1 g/0.813 mL
  3. C) 0.813 g/1 mL
  4. D) 0.813 g/0.813 mL
  5. E) 0.813 mL/1 g

Answer:  C

Section:  2.8 The Density Concept

 

94) If the density of silver is 10.5 g/cm3, which of the following is a unit factor?

  1. A) 1 g/1 mL
  2. B) 1 g/10.5 mL
  3. C) 10.5 g/1 mL
  4. D) 10.5 g/10.5 mL
  5. E) 10.5 mL/1 g

Answer:  C

Section:  2.8 The Density Concept

 

95) A 10.0 cm3 volume of alcohol has a mass of 0.00705 kg. What is the density of the alcohol in grams per cubic centimeter?

  1. A) 0.0705 g/cm3
  2. B) 0.705 g/cm3
  3. C) 7.05 g/cm3
  4. D) 10.0 g/cm3
  5. E) 70.5 g/cm3

Answer:  B

Section:  2.8 The Density Concept

 

96) A 10.0 mL volume of mercury has a mass of 0.136 kg. What is the density of mercury in grams per milliliter?

  1. A) 1.36 g/mL
  2. B) 7.35 g/mL
  3. C) 13.6 g/mL
  4. D) 73.5 g/mL
  5. E) 136 g/mL

Answer:  C

Section:  2.8 The Density Concept

 

97) A block of aluminum has a mass of 39.589 g and measures 5.10 cm by 2.50 cm by 1.15 cm. What is the density of the rectangular aluminum block?

  1. A) 0.370 g/cm3
  2. B) 2.70 g/cm3
  3. C) 3.11 g/cm3
  4. D) 14.7 g/cm3
  5. E) 22.3 g/cm3

Answer:  B

Section:  2.8 The Density Concept

 

 

98) A block of copper has a mass of 143.584 g and measures 5.05 cm by 2.55 cm by 1.25 cm. What is the density of the rectangular copper block?

  1. A) 0.112 g/cm3
  2. B) 8.92 g/cm3
  3. C) 11.1 g/cm3
  4. D) 28.4 g/cm3
  5. E) 29.0 g/cm3

Answer:  B

Section:  2.8 The Density Concept

 

99) Osmium is one of the most dense elements (22.5 g/cm3). What is the mass of 10.0cm3 of the metal?

  1. A) 0.444 g
  2. B) 2.25 g
  3. C) 22.5 g
  4. D) 225 g
  5. E) 444 g

Answer:  D

Section:  2.8 The Density Concept

 

100) The density of ethyl ether is 0.714 g/mL. What is the mass of 10.0 mL of ether?

  1. A) 0.0714 g
  2. B) 1.40 g
  3. C) 7.14 g
  4. D) 14.0 g
  5. E) 71.4 g

Answer:  C

Section:  2.8 The Density Concept

 

101) Ethyl alcohol has a density less than water (d = 0.789 g/mL). What is the volume of 35.5 g of ethyl alcohol?

  1. A) 2.80 mL
  2. B) 4.50 mL
  3. C) 28.0 mL
  4. D) 45.0 mL
  5. E) 280 mL

Answer:  D

Section:  2.8 The Density Concept

 

102) Platinum is one of the most dense elements (d = 21.5 g/cm3). What is the volume of a 10.0 g sample of the metal?

  1. A) 0.465 cm3
  2. B) 2.15 cm3
  3. C) 21.5 cm3
  4. D) 215 cm3
  5. E) 465 cm3

Answer:  A

Section:  2.8 The Density Concept

 

103) Magnesium is one of the least dense elements (d = 1.74 g/cm3). What is the volume of a 10.0 g sample of the metal?

  1. A) 5.75 cm3
  2. B) 10.0 cm3
  3. C) 17.4 cm3
  4. D) 57.5 cm3
  5. E) 174 cm3

Answer:  A

Section:  2.8 The Density Concept

 

104) A glass cylinder contains four liquid layers: mercury (d = 13.6 g/mL), chloroform (d = 1.49 g/mL), water (d = 1.00 g/mL), and ether (d = 0.708 g/mL). If an ice cube (d=0.92 g/mL) is dropped into the cylinder, where does it come to rest?

  1. A) on top of the ether layer
  2. B) on top of the water layer
  3. C) on top of the chloroform layer
  4. D) on top of the mercury layer
  5. E) on the bottom of the cylinder

Answer:  B

Section:  2.8 The Density Concept

 

105) A glass cylinder contains four liquid layers: mercury (d = 13.6 g/mL), chloroform (d = 1.49 g/mL), water (d = 1.00 g/mL), and ether (d = 0.708 g/mL). If a marble (d=2.7 g/mL). is dropped into the cylinder, where does it come to rest?

  1. A) on top of the ether layer
  2. B) on top of the water layer
  3. C) on top of the chloroform layer
  4. D) on top of the mercury layer
  5. E) on the bottom of the cylinder

Answer:  D

Section:  2.8 The Density Concept

 

106) A glass cylinder contains four liquid layers: mercury (d = 13.6 g/mL), chloroform (d = 1.49 g/mL), water (d = 1.00 g/mL), ether (d = 0.708 g/mL). If a gold nugget (d=19.3 g/mL) is dropped into the cylinder, where does it come to rest?

  1. A) on top of the ether layer
  2. B) on top of the water layer
  3. C) on top of the chloroform layer
  4. D) on top of the mercury layer
  5. E) on the bottom of the cylinder

Answer:  E

Section:  2.8 The Density Concept

 

 

107) A glass cylinder contains four liquid layers: mercury (d = 13.6 g/mL), chloroform (d = 1.49 g/mL), water (d = 1.00 g/mL), ether (d = 0.708 g/mL). If a rubber stopper (d = 1.2 g/mL) is dropped into the cylinder, where does it come to rest?

  1. A) on top of the ether layer
  2. B) on top of the water layer
  3. C) on top of the chloroform layer
  4. D) on top of the mercury layer
  5. E) on the bottom of the cylinder

Answer:  C

Section:  2.8 The Density Concept

 

108) A glass cylinder contains four liquid layers: mercury (d = 13.6 g/mL), chloroform (d = 1.49 g/mL), water (d = 1.00 g/mL), ether (d = 0.708 g/mL). If a cork stopper (d = 0.50 g/mL) is dropped into the cylinder, where does it come to rest?

  1. A) on top of the ether layer
  2. B) on top of the water layer
  3. C) on top of the chloroform layer
  4. D) on top of the mercury layer
  5. E) on the bottom of the cylinder

Answer:  A

Section:  2.8 The Density Concept

 

109) What are the freezing point and boiling point of water on the Fahrenheit scale?

  1. A) -32 °F and 212 °F
  2. B) 0 °F and 100 °F
  3. C) 0 °F and 212 °F
  4. D) 32 °F and 100 °F
  5. E) 32 °F and 212 °F

Answer:  E

Section:  2.9 Temperature

 

110) What are the freezing point and boiling point of water on the Celsius scale?

  1. A) 0 °C and 100 °C
  2. B) 0 °C and 212 °C
  3. C) 32 °C and 100 °C
  4. D) 32 °C and 212 °C
  5. E) 273 °C and 373 °C

Answer:  A

Section:  2.9 Temperature

 

111) What are the freezing point and boiling point of water on the Kelvin scale?

  1. A) 0 K and 100 K
  2. B) 0 K and 273 K
  3. C) 100 K and 273 K
  4. D) 100 K and 373 K
  5. E) 273 K and 373 K

Answer:  E

Section:  2.9 Temperature

 

 

112) Table salt melts at 801 °C. What is the melting point on the Fahrenheit scale?

  1. A) 427 °F
  2. B) 1384 °F
  3. C) 1410 °F
  4. D) 1470 °F
  5. E) 1490 °F

Answer:  D

Section:  2.9 Temperature

 

113) An antifreeze solution freezes at -100 °C. What is the freezing point on the Fahrenheit scale?

  1. A) -212 °F
  2. B) -148 °F
  3. C) -88 °F
  4. D) -82 °F
  5. E) -73 °F

Answer:  B

Section:  2.9 Temperature

 

114) Aluminum melts at 1220 °F. What is the melting point on the Celsius scale?

  1. A) 646 °C
  2. B) 660 °C
  3. C) 696 °C
  4. D) 2138 °C
  5. E) 2164 °C

Answer:  B

Section:  2.9 Temperature

 

115) Rubbing alcohol freezes at -129 °F. What is the freezing point on the Celsius scale?

  1. A) -290 °C
  2. B) -200 °C
  3. C) -103 °C
  4. D) -89.4 °C
  5. E) -54 °C

Answer:  D

Section:  2.9 Temperature

 

116) Liquid hydrogen boils at -252 °C. What is the boiling point on the Kelvin scale?

  1. A) -525 K
  2. B) -252 K
  3. C) -21 K
  4. D) 21 K
  5. E) 525 K

Answer:  D

Section:  2.9 Temperature

 

 

117) Liquid argon boils at -186 °C. What is the boiling point on the Kelvin scale?

  1. A) -459 K
  2. B) -186 K
  3. C) -87 K
  4. D) 87 K
  5. E) 459 K

Answer:  D

Section:  2.9 Temperature

 

118) A rare metal alloy is a superconductor at -225 °C. What is the temperature on the Kelvin scale?

  1. A) -498 K
  2. B) -225 K
  3. C) -48 K
  4. D) 48 K
  5. E) 498 K

Answer:  D

Section:  2.9 Temperature

 

119) Liquid helium boils at 4 K. What is the boiling point on the Celsius scale?

  1. A) -277 °C
  2. B) -269 °C
  3. C) 4 °C
  4. D) 269 °C
  5. E) 277 °C

Answer:  B

Section:  2.9 Temperature

 

120) Liquid krypton boils at 121 K. What is the boiling point on the Celsius scale?

  1. A) -394 °C
  2. B) -152 °C
  3. C) 121 °C
  4. D) 152 °C
  5. E) 394 °C

Answer:  B

Section:  2.9 Temperature

 

121) A rare metal alloy is a superconductor at 55 K. What is the temperature on the Celsius scale?

  1. A) -328 °C
  2. B) -218 °C
  3. C) -55 °C
  4. D) 218 °C
  5. E) 328 °C

Answer:  B

Section:  2.9 Temperature

 

 

122) Which of the following can express the total amount of heat energy in a sealed, insulated chamber?

  1. A) 20.0 °C
  2. B) 68.0 °F
  3. C) 293.0 K
  4. D) 20.0 kcal
  5. E) all of the above

Answer:  D

Section:  2.10 The Heat Concept

 

123) Which of the following can express the average amount of heat energy in a sealed, insulated chamber?

  1. A) 20.0 °C
  2. B) 68.0 cal
  3. C) 293.0 kcal
  4. D) 20.0 J
  5. E) all of the above

Answer:  A

Section:  2.10 The Heat Concept

 

124) When 100.0 g of gasoline undergoes combustion, 9560 kJ of energy are released. Express the heat released in kilocalories. (Given: 4.184 J = 1 cal)

  1. A) 2.28 x 103kcal
  2. B) 2.28 x 106kcal
  3. C) 2.28 x 109kcal
  4. D) 4.00 x 104kcal
  5. E) 4.00 x 107kcal

Answer:  A

Section:  2.10 The Heat Concept

 

125) Which of the following are base units and symbols in the English system?

  1. A) inch (in.), ounce (oz), pint (pt)
  2. B) foot (ft), pound (lb), quart (qt)
  3. C) yard (yd), pound (lb), gallon (gal)
  4. D) mile (mi), ton (ton), gallon (gal)
  5. E) The English system does not have base units.

Answer:  E

Section:  General Exercises

 

126) Which of the following are base units and symbols in the International system?

  1. A) centimeter (cm), gram (g), second (s)
  2. B) meter (m), gram (g), second (s)
  3. C) meter (m), kilogram (kg), second (s)
  4. D) kilometer (km), kilogram (kg), second (s)
  5. E) The International system does not have base units.

Answer:  C

Section:  General Exercises

 

 

127) In performing a multistep multiplication or division calculation, when should you round off the answer in the calculator display?

  1. A) after each step in the calculation
  2. B) after the first unit factor
  3. C) after the second unit factor
  4. D) after the final calculation
  5. E) none of the above

Answer:  D

Section:  General Exercises

 

128) Which of the following is equivalent to the volume of a 1-cm cube?

  1. A) 1 L
  2. B) 1 cL
  3. C) 1 dL
  4. D) 1 kL
  5. E) 1 mL

Answer:  E

Section:  General Exercises

 

129) Which of the following is equivalent to the volume of a 10-cm cube?

  1. A) 1 L
  2. B) 1 cL
  3. C) 1 dL
  4. D) 1 kL
  5. E) 1 mL

Answer:  A

Section:  General Exercises

 

130) Which of the following is equivalent to the volume of a 1.00-L flask?

  1. A) 1.00 cm3
  2. B) 10.0 cm3
  3. C) 100 cm3
  4. D) 946 cm3
  5. E) 1000 cm3

Answer:  E

Section:  General Exercises

 

131) The density of water at 3.98 °C is 1.00 g/mL. What is the density in g/cm3?

  1. A) 1.00 g/cm3
  2. B) 2.54 g/cm3
  3. C) 3.98 g/cm3
  4. D) 16.4 g/cm3
  5. E) 62.4 g/cm3

Answer:  A

Section:  General Exercises

 

 

132) How many significant digits are justified by the unit factor 1 m/100 cm?

  1. A) 1
  2. B) 2
  3. C) 3
  4. D) infinite
  5. E) impossible to determine

Answer:  D

Section:  General Exercises

 

133) How many significant digits are justified by the unit factor 1 lb/454 g?

  1. A) 1
  2. B) 2
  3. C) 3
  4. D) infinite
  5. E) impossible to determine

Answer:  C

Section:  General Exercises

 

134) If a diamond weighs 1.33 carats, what is the mass in grams? (Given: 1 ct = 200 mg)

  1. A) 0.133 g
  2. B) 0.150 g
  3. C) 0.200 g
  4. D) 0.266 g
  5. E) 6.65 g

Answer:  D

Section:  General Exercises

 

135) How many minutes are required for sunlight to travel from the Sun to Earth? (Assume the Sun is 93,000,000 miles from Earth and sunlight travels at 1.86 x 105 miles per second.)

  1. A) 0.0020 minute
  2. B) 2.0 minutes
  3. C) 8.3 minutes
  4. D) 500 minutes
  5. E) 830 minutes

Answer:  C

Section:  General Exercises

 

136) How many minutes are required for sunlight to travel from the Sun to Mars? (Assume the Sun is 2.28 x 108 kilometers from Mars and sunlight travels at 2.99 x 105 kilometers per second.)

  1. A) 0.00131 minutes
  2. B) 0.0787 minutes
  3. C) 12.7 minutes
  4. D) 763 minutes
  5. E) 45,800 minutes

Answer:  C

Section:  General Exercises

 

 

137) A hybrid vehicle has a mileage rating of 22 km/L. What is the gas mileage in miles per gallon? (Given: 1 mi = 1.61 km, and 1 gal = 3.78 L)

  1. A) 3.6 mi/gal
  2. B) 9.4 mi/gal
  3. C) 35 mi/gal
  4. D) 52 mi/gal
  5. E) 130 mi/gal

Answer:  D

Section:  General Exercises

 

138) An Indy 500 car can travel 111 m/s. What is the speed of the car in miles per hour? (Given: 1 mi = 1.61 km, and 1 h = 3600 s)

  1. A) 111 mi/h
  2. B) 178 mi/h
  3. C) 248 mi/h
  4. D) 400 mi/h
  5. E) 643 mi/h

Answer:  C

Section:  General Exercises

 

139) Why does a sterling silver spoon weigh more than a stainless steel spoon of the same size?

  1. A) sterling silver is less valuable than stainless steel
  2. B) sterling silver is more valuable than stainless steel
  3. C) sterling silver is less dense than stainless steel
  4. D) sterling silver is more dense than stainless steel
  5. E) none of the above

Answer:  D

Section:  General Exercises

 

140) The density of carbon tetrachloride is 1.60 g/cm3. What is the density of the liquid expressed in SI units (kg/m3)?

  1. A) 0.160 kg/m3
  2. B) 1.60 kg/m3
  3. C) 16.0 kg/m3
  4. D) 1.60 x 103kg/m3
  5. E) 1.60 x 106kg/m3

Answer:  D

Section:  General Exercises

 

141) Calculate the volume of Earth assuming it is spherical and has a radius (r) of 6370 km. The volume of a sphere equals 4πr3/3, and π = 3.14.

  1. A) 2.58 x 1011km3
  2. B) 3.45 x 1011km3
  3. C) 6.37 x 1011km3
  4. D) 1.03 x 1012km3
  5. E) 1.08 x 1012km3

Answer:  E

Section:  General Exercises

 

142) Calculate a length of copper wire having a diameter of 0.200 cm and a mass of 15.620 g. The density of copper is 8.92 g/cm3. The volume of wire equals πd2 L/4, and  π = 3.14, d = diameter, and L = length)

  1. A) 1.80 x 10-4 cm
  2. B) 4.00 x 10-4 cm
  3. C) 5.50 x 10-2cm
  4. D) 1.75 cm
  5. E) 55.8 cm

Answer:  E

Section:  General Exercises

 

143) What is the difference between a cup of coffee and a drop of coffee at 95 °C?

  1. A) Temperature is greater in the cup of coffee.
  2. B) Heat is greater in the cup of coffee.
  3. C) Temperature is greater in the drop of coffee.
  4. D) Heat is greater in the drop of coffee.
  5. E) Temperature and heat are the same for a cup and drop of coffee.

Answer:  B

Section:  General Exercises

 

Critical Thinking – The  International System of Units (SI)

 

1) Which of the following is an official quantity in SI?

  1. A) length
  2. B) mass
  3. C) time
  4. D) all of the above
  5. E) none of the above

Answer:  D

 

2) Which of the following is an official quantity in SI?

  1. A) density
  2. B) energy
  3. C) volume
  4. D) all of the above
  5. E) none of the above

Answer:  E

 

3) Which of the following is an official quantity in SI?

  1. A) amount of substance
  2. B) electric current
  3. C) light intensity
  4. D) all of the above
  5. E) none of the above

Answer:  D

 

 

4) Which of the following is a base unit in SI?

  1. A) centimeter
  2. B) kilogram
  3. C) liter
  4. D) all of the above
  5. E) none of the above

Answer:  B

 

5) Which of the following is a base unit in SI?

  1. A) degree Fahrenheit
  2. B) degree Celsius
  3. C) Kelvin
  4. D) all of the above
  5. E) none of the above

Answer:  C

 

6) Which of the following is a base unit in SI?

  1. A) ampere
  2. B) candela
  3. C) mole
  4. D) all of the above
  5. E) none of the above

Answer:  D

 

Chemistry Connection – The Olympics

 

1) Which running competition in the Olympic Summer Games is approximately equal to 440 yards?

  1. A) 100 meters
  2. B) 200 meters
  3. C) 400 meters
  4. D) 1000 meters
  5. E) 2000 meters

Answer:  C

 

2) Which swimming competition in the Olympic Summer Games is approximately equal to 100 yards?

  1. A) 100 meters
  2. B) 200 meters
  3. C) 500 meters
  4. D) 50 kilometers
  5. E) 100 kilometers

Answer:  A

 

3) Which skiing competition in the Olympic Winter Games is approximately equal to 10 kilometers?

  1. A) 5000 yards
  2. B) 10,000 yards
  3. C) 10 miles
  4. D) 15 miles
  5. E) 20 miles

Answer:  B

 

4) Which of the following is a running event in the Olympic Summer Games?

  1. A) 100 inches
  2. B) 100 feet
  3. C) 100 yards
  4. D) 100 meters
  5. E) 100 miles

Answer:  D

 

5) Which of the following is a swimming event in the Olympic Summer Games?

  1. A) 50 yards
  2. B) 100 yards
  3. C) 200 yards
  4. D) 400 yards
  5. E) 400 meters

Answer:  E

 

6) Which of the following is a skiing event in the Olympic Winter Games?

  1. A) 50 kilometers
  2. B) 50 miles
  3. C) 5000 feet
  4. D) 500 yards
  5. E) 1000 yards

Answer:  A

 

Critical Thinking – World Trade Center

 

1) Which of the following is the largest “footprint”?

  1. A) 150 square feet
  2. B) 150 feet square
  3. C) 150 square inches
  4. D) 150 inches square
  5. E) Answers A and B are the same.

Answer:  B

 

2) Which of the following is the smallest “footprint”?

  1. A) 150 square feet
  2. B) 150 feet square
  3. C) 150 square yards
  4. D) 150 yards square
  5. E) Answers A and B are the same.

Answer:  A

 

 

3) What is the proposed height of the World Trade Center Freedom Tower?

  1. A) 1776 feet
  2. B) 1776 yards
  3. C) 1776 meters
  4. D) 1776 decimeters
  5. E) none of the above

Answer:  A

 

 

 

Introductory Chemistry: Concepts and Critical Thinking, 7e (Corwin)

Chapter 11  Liquids and Solids

 

Key Terms

 

1) What is the term that describes a compound which has lost water of hydration?

  1. A) anhydrous
  2. B) deliquescent
  3. C) efflorescent
  4. D) hygroscopic
  5. E) none of the above

Answer:  A

Section:  Key Terms

 

2) What is the term for the temperature at which the vapor pressure of a liquid is equal to the atmospheric pressure?

  1. A) absolute zero
  2. B) boiling point
  3. C) critical point
  4. D) vapor point
  5. E) none of the above

Answer:  B

Section:  Key Terms

 

3) What is the term for the angle formed by two atoms bonded to the central atom in a molecule?

  1. A) atomic angle
  2. B) bond angle
  3. C) central angle
  4. D) molecular angle
  5. E) none of the above

Answer:  B

Section:  Key Terms

 

4) What is the term for a substance in the solid state that contains particles which repeat in a regular geometric pattern?

  1. A) crystalline solid
  2. B) geometric solid
  3. C) noncrystalline solid
  4. D) regular solid
  5. E) none of the above

Answer:  A

Section:  Key Terms

 

 

5) What is the term for water purified by an ion exchange method?

  1. A) deionized water
  2. B) distilled water
  3. C) hard water
  4. D) soft water
  5. E) none of the above

Answer:  A

Section:  Key Terms

 

6) What is the term for an attraction between two molecules with permanent dipoles?

  1. A) dipole force
  2. B) dispersion force
  3. C) hydrogen bond
  4. D) intermolecular bond
  5. E) none of the above

Answer:  A

Section:  Key Terms

 

7) What is the term for an attraction between two molecules with temporary dipoles?

  1. A) dipole force
  2. B) dispersion force
  3. C) hydrogen bond
  4. D) intermolecular bond
  5. E) none of the above

Answer:  B

Section:  Key Terms

 

8) What is the term for water purified by boiling and collecting the condensed vapor?

  1. A) deionized water
  2. B) distilled water
  3. C) hard water
  4. D) soft water
  5. E) none of the above

Answer:  B

Section:  Key Terms

 

9) What is the term for the chemical reaction produced from passing electrical current through an aqueous solution?

  1. A) decomposition
  2. B) deionization
  3. C) distillation
  4. D) electrolysis
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

 

10) What is the term for water containing a variety of different cations and anions?

  1. A) deionized water
  2. B) distilled water
  3. C) hard water
  4. D) soft water
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

11) What is the term for the heat required to convert a solid to a liquid at its melting point?

  1. A) heat of crystallization
  2. B) heat of fusion
  3. C) heat of vaporization
  4. D) specific heat
  5. E) none of the above

Answer:  B

Section:  Key Terms

 

12) What is the term for the heat required to convert a liquid to a gas at its boiling point?

  1. A) heat of crystallization
  2. B) heat of fusion
  3. C) heat of vaporization
  4. D) specific heat
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

13) What is the term for a compound which contains a specific number of water molecules in a crystalline compound?

  1. A) anhydrous
  2. B) deliquescent
  3. C) efflorescent
  4. D) hydrate
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

14) What is the term for an intermolecular attraction based on permanent dipoles involving a H atom bonded to an O or N atom?

  1. A) dipole force
  2. B) dispersion force
  3. C) hydrogen bond
  4. D) intermolecular bond
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

 

15) What is the term for a crystalline solid composed of ions which repeat in a regular pattern?

  1. A) ionic solid
  2. B) metallic solid
  3. C) molecular solid
  4. D) regular solid
  5. E) none of the above

Answer:  A

Section:  Key Terms

 

16) What is the term for a compound which reacts with water to produce a basic

solution?

  1. A) anhydrous
  2. B) hydrate
  3. C) metal oxide
  4. D) nonmetal oxide
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

17) What is the term for a crystalline solid composed of metal atoms which repeat in a regular pattern?

  1. A) ionic solid
  2. B) metallic solid
  3. C) molecular solid
  4. D) regular solid
  5. E) none of the above

Answer:  B

Section:  Key Terms

 

18) What is the term for a crystalline solid composed of molecules which repeat in a regular pattern?

  1. A) ionic solid
  2. B) metallic solid
  3. C) molecular solid
  4. D) regular solid
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

19) What is the term for the overall direction of partial negative charge in a molecule having two or more dipoles?

  1. A) charge dipole
  2. B) directional dipole
  3. C) electron dipole
  4. D) net dipole
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

 

20) What is the term for a compound which reacts with water to produce an acidic solution?

  1. A) anhydrous
  2. B) hydrate
  3. C) metal oxide
  4. D) nonmetal oxide
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

21) What is the term for water containing sodium ions and a variety of anions?

  1. A) deionized water
  2. B) distilled water
  3. C) hard water
  4. D) soft water
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

22) What is the term for the amount of energy required to raise one gram of any substance one degree on the Celsius scale?

  1. A) calorie
  2. B) heat
  3. C) specific heat
  4. D) joule
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

23) What is the term for the resistance of a liquid to spread and its tendency to form spherical droplets?

  1. A) dipole attraction
  2. B) dispersion forces
  3. C) surface tension
  4. D) viscosity
  5. E) none of the above

Answer:  C

Section:  Key Terms

 

24) What is the term for the pressure exerted by vapor molecules above a liquid in a closed container when the rates of vaporization and condensation are equal?

  1. A) atmospheric pressure
  2. B) gas pressure
  3. C) partial pressure
  4. D) vapor pressure
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

 

25) What is the term for the resistance of a liquid to flow?

  1. A) dipole attraction
  2. B) dispersion forces
  3. C) surface tension
  4. D) viscosity
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

26) What is the term for the number of water molecules in a hydrate?

  1. A) anhydrous water
  2. B) deliquescent water
  3. C) efflorescent water
  4. D) water of hydration
  5. E) none of the above

Answer:  D

Section:  Key Terms

 

Questions for Chapter 11

 

1) Which of the following is an observed property of liquids?

  1. A) Liquids flow readily.
  2. B) Liquids do not compress or expand significantly.
  3. C) Liquids have a variable shape and fixed volume.
  4. D) Liquids are more dense than gases.
  5. E) all of the above

Answer:  E

Section:  11.1 Properties of Liquids

 

2) Which of the following is an observed property of liquids?

  1. A) Liquids have a fixed shape and variable volume.
  2. B) Liquids that are soluble mix homogeneously.
  3. C) Liquids compress and expand significantly.
  4. D) Liquids are less dense than gases.
  5. E) none of the above

Answer:  B

Section:  11.1 Properties of Liquids

 

3) Which of the following is an observed property of liquids?

  1. A) Liquids are less dense than gases.
  2. B) Liquids compress or expand significantly.
  3. C) Liquids have a fixed shape and variable volume.
  4. D) Liquids that are insoluble mix homogeneously.
  5. E) none of the above

Answer:  E

Section:  11.1 Properties of Liquids

 

 

4) Predict the physical state of ammonia at -50 °C (Mp = -77 °C, Bp = -33 °C) and normal atmospheric pressure.

  1. A) solid
  2. B) liquid
  3. C) gas
  4. D) solid and liquid
  5. E) liquid and gas

Answer:  B

Section:  11.1 Properties of Liquids

 

5) Predict the physical state of ammonia at -95 °C (Mp = -77 °C, Bp = -33 °C) and normal atmospheric pressure.

  1. A) solid
  2. B) liquid
  3. C) gas
  4. D) solid and liquid
  5. E) liquid and gas

Answer:  A

Section:  11.1 Properties of Liquids

 

6) Predict the physical state of ammonia at -15 °C (Mp = -77 °C, Bp = -33 °C) and normal atmospheric pressure.

  1. A) solid
  2. B) liquid
  3. C) gas
  4. D) solid and liquid
  5. E) liquid and gas

Answer:  C

Section:  11.1 Properties of Liquids

 

7) Predict the physical state of argon at -187 °C (Mp = -189 °C, Bp = -186 °C) and normal atmospheric pressure.

  1. A) solid
  2. B) liquid
  3. C) gas
  4. D) solid and liquid
  5. E) liquid and gas

Answer:  B

Section:  11.1 Properties of Liquids

 

8) Predict the physical state of argon at -197 °C (Mp = -189 °C, Bp = -186 °C) and normal atmospheric pressure.

  1. A) solid
  2. B) liquid
  3. C) gas
  4. D) solid and liquid
  5. E) liquid and gas

Answer:  A

Section:  11.1 Properties of Liquids

 

9) Predict the physical state of argon at -100 °C (Mp = -189 °C, Bp = -186 °C) and normal atmospheric pressure.

  1. A) solid
  2. B) liquid
  3. C) gas
  4. D) solid and liquid
  5. E) liquid and gas

Answer:  C

Section:  11.1 Properties of Liquids

 

10) What is the strongest intermolecular force in a liquid containing molecules with nonpolar bonds?

  1. A) covalent bonds
  2. B) dipole forces
  3. C) dispersion forces
  4. D) hydrogen bonds
  5. E) none of the above

Answer:  C

Section:  11.2 The Intermolecular Bond Concept

 

11) What is the strongest intermolecular force in a liquid containing molecules with H-O bonds?

  1. A) covalent bonds
  2. B) dipole forces
  3. C) dispersion forces
  4. D) hydrogen bonds
  5. E) none of the above

Answer:  D

Section:  11.2 The Intermolecular Bond Concept

 

12) What is the strongest intermolecular force in a liquid containing molecules with H-N bonds?

  1. A) covalent bonds
  2. B) dipole forces
  3. C) dispersion forces
  4. D) hydrogen bonds
  5. E) none of the above

Answer:  D

Section:  11.2 The Intermolecular Bond Concept

 

13) Which of the following is true of the intermolecular attractions in liquids?

  1. A) Nonpolar molecules are attracted by temporary dipole forces.
  2. B) Polar molecules are attracted by temporary dipole forces.
  3. C) Polar molecules are attracted by permanent dipole forces.
  4. D) all of the above
  5. E) none of the above

Answer:  D

Section:  11.2 The Intermolecular Bond Concept

 

 

14) Which of the following is true of the intermolecular attractions in liquids?

  1. A) Nonpolar molecules are attracted by dispersion forces.
  2. B) Nonpolar molecules are attracted by dipole forces.
  3. C) Nonpolar molecules are attracted by hydrogen bonds.
  4. D) all of the above
  5. E) none of the above

Answer:  A

Section:  11.2 The Intermolecular Bond Concept

 

15) Which of the following is true of the intermolecular attractions in liquids?

  1. A) All polar molecules are attracted by dispersion forces.
  2. B) All polar molecules are attracted by dipole forces.
  3. C) Some polar molecules are attracted by hydrogen bonds.
  4. D) all of the above
  5. E) none of the above

Answer:  D

Section:  11.2 The Intermolecular Bond Concept

 

16) If the molecules in a liquid have a strong attraction for each other, which of the following properties has a relatively high value?

  1. A) boiling point
  2. B) viscosity
  3. C) surface tension
  4. D) all of the above
  5. E) none of the above

Answer:  D

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

17) If the molecules in a liquid have a strong attraction for each other, which of the following properties has a relatively low value?

  1. A) boiling point
  2. B) surface tension
  3. C) vapor pressure
  4. D) viscosity
  5. E) all of the above

Answer:  C

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

18) If the molecules in a liquid have a weak attraction for each other, which of the following properties has a relatively high value?

  1. A) boiling point
  2. B) surface tension
  3. C) vapor pressure
  4. D) viscosity
  5. E) all of the above

Answer:  C

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

 

19) Consider the following liquids with similar molar masses. Predict which has the strongest intermolecular attraction based only on vapor pressure data.

  1. A) acetic acid (vapor pressure @ 20 °C = 14 mm Hg)
  2. B) butane (vapor pressure @ 20 °C = 1550 mm Hg)
  3. C) ethyl chloride (vapor pressure @ 20 °C = 1050 mm Hg)
  4. D) ethyl methyl ether (vapor pressure @ 20 °C = 1260 mm Hg)
  5. E) isopropyl alcohol (vapor pressure @ 20 °C = 35 mm Hg)

Answer:  A

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

20) Consider the following liquids with similar molar masses. Predict which has the weakest intermolecular attraction based only on vapor pressure data.

  1. A) acetic acid (vapor pressure @ 20 °C = 14 mm Hg)
  2. B) butane (vapor pressure @ 20 °C = 1550 mm Hg)
  3. C) ethyl chloride (vapor pressure @ 20 °C = 1050 mm Hg)
  4. D) ethyl methyl ether (vapor pressure @ 20 °C = 1260 mm Hg)
  5. E) isopropyl alcohol (vapor pressure @ 20 °C = 35 mm Hg)

Answer:  B

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

21) Consider the following liquids with similar molar masses. Predict which has the weakest intermolecular attraction based only on vapor pressure data.

  1. A) butyl alcohol (vapor pressure @ 20 °C = 6 mm Hg)
  2. B) ethyl ether (vapor pressure @ 20 °C = 450 mm Hg)
  3. C) pentane (vapor pressure @ 20 °C = 430 mm Hg)
  4. D) propionic acid (vapor pressure @ 20 °C = 5 mm Hg)
  5. E) propyl chloride (vapor pressure @ 20 °C = 300 mm Hg)

Answer:  B

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

22) Consider the following liquids with similar molar masses. Predict which has the strongest intermolecular attraction based only on boiling point data.

  1. A) acetic acid (Bp @ 760 mm Hg = 118 °C)
  2. B) butane (Bp @ 760 mm Hg = -0.5 °C)
  3. C) ethyl chloride (Bp @ 760 mm Hg = 12 °C)
  4. D) ethyl methyl ether (Bp @ 760 mm Hg = 11 °C)
  5. E) propyl alcohol (Bp @ 760 mm Hg = 97 °C)

Answer:  A

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

23) Consider the following liquids with similar molar masses. Predict which has the weakest intermolecular attraction based only on boiling point data.

  1. A) acetic acid (Bp @ 760 mm Hg = 118 °C)
  2. B) butane (Bp @ 760 mm Hg = -0.5 °C)
  3. C) ethyl chloride (Bp @ 760 mm Hg = 12 °C)
  4. D) ethyl methyl ether (Bp @ 760 mm Hg = 11 °C)
  5. E) propyl alcohol (Bp @ 760 mm Hg = 97 °C)

Answer:  B

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

24) Consider the following liquids with similar molar masses. Predict which has the strongest intermolecular attraction based only on boiling point data.

  1. A) butyl alcohol (Bp @ 760 mm Hg = 117 °C)
  2. B) ethyl ether (Bp @ 760 mm Hg = 35 °C)
  3. C) pentane (Bp @ 760 mm Hg = 36 °C)
  4. D) propionic acid (Bp @ 760 mm Hg = 141 °C)
  5. E) propyl chloride (Bp @ 760 mm Hg = 47 °C)

Answer:  D

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

25) Consider the following liquids with similar molar masses. Predict which liquid has the highest boiling point based only on vapor pressure data.

  1. A) pentane (vapor pressure @ 20 °C = 430 mm Hg)
  2. B) methyl acetate (vapor pressure @ 20 °C = 205 mm Hg)
  3. C) butyl alcohol (vapor pressure @ 20 °C = 6 mm Hg)
  4. D) propyl chloride (vapor pressure @ 20 °C = 300 mm Hg)
  5. E) ethyl ether (vapor pressure @ 20 °C = 450 mm Hg)

Answer:  C

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

26) Consider the following liquids with similar molar masses. Predict which liquid has the lowest boiling point based only on vapor pressure data.

  1. A) pentane (vapor pressure @ 20 °C = 430 mm Hg)
  2. B) methyl acetate (vapor pressure @ 20 °C = 205 mm Hg)
  3. C) butyl alcohol (vapor pressure @ 20 °C = 6 mm Hg)
  4. D) propyl chloride (vapor pressure @ 20 °C = 300 mm Hg)
  5. E) ethyl ether (vapor pressure @ 20 °C = 450 mm Hg)

Answer:  E

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

27) Consider the following liquids with similar molar masses. Predict which liquid has the highest boiling point based only on vapor pressure data.

  1. A) acetic acid (vapor pressure @ 20 °C = 14 mm Hg)
  2. B) butane (vapor pressure @ 20 °C = 1550 mm Hg)
  3. C) ethyl chloride (vapor pressure @ 20 °C = 1050 mm Hg)
  4. D) ethyl methyl ether (vapor pressure @ 20 °C = 1260 mm Hg)
  5. E) isopropyl alcohol (vapor pressure @ 20 °C = 35 mm Hg)

Answer:  A

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

28) Consider the following liquids with similar molar masses. Predict which liquid has the lowest boiling point based only on vapor pressure data.

  1. A) acetic acid (vapor pressure @ 20 °C = 14 mm Hg)
  2. B) butane (vapor pressure @ 20 °C = 1550 mm Hg)
  3. C) ethyl chloride (vapor pressure @ 20 °C = 1050 mm Hg)
  4. D) ethyl methyl ether (vapor pressure @ 20 °C = 1260 mm Hg)
  5. E) isopropyl alcohol (vapor pressure @ 20 °C = 35 mm Hg)

Answer:  B

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

29) Consider the following liquids with similar molar masses. Predict which liquid has the strongest intermolecular attraction based on viscosity data.

  1. A) butyl alcohol (viscosity @ 20 °C = 2.95 centipoise)
  2. B) ethyl ether (viscosity @ 20 °C = 0.23 centipoise)
  3. C) ethyl formate (viscosity @ 20 °C = 0.40 centipoise)
  4. D) propionic acid (viscosity @ 20 °C = 1.10 centipoise)
  5. E) propyl chloride (viscosity @ 20 °C = 0.35 centipoise)

Answer:  A

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

30) Consider the following liquids with similar molar masses. Predict which liquid has the weakest intermolecular attraction based on viscosity data.

  1. A) butyl alcohol (viscosity @ 20 °C = 2.95 centipoise)
  2. B) ethyl ether (viscosity @ 20 °C = 0.23 centipoise)
  3. C) ethyl formate (viscosity @ 20 °C = 0.40 centipoise)
  4. D) propionic acid (viscosity @ 20 °C = 1.10 centipoise)
  5. E) propyl chloride (viscosity @ 20 °C = 0.35 centipoise)

Answer:  B

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

31) Consider the following liquids with similar molar masses. Predict which liquid has the strongest intermolecular attraction based on surface tension data.

  1. A) butyl alcohol (surface tension @ 20 °C = 25 dynes/cm)
  2. B) ethyl ether (surface tension @ 20 °C = 17 dynes/cm)
  3. C) ethyl formate (surface tension @ 20 °C = 24 dynes/cm)
  4. D) propionic acid (surface tension @ 20 °C = 27 dynes/cm)
  5. E) propyl chloride (surface tension @ 20 °C = 18 dynes/cm)

Answer:  D

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

32) Consider the following liquids with similar molar masses. Predict which liquid has the weakest intermolecular attraction based on surface tension data.

  1. A) butyl alcohol (surface tension @ 20 °C = 25 dynes/cm)
  2. B) ethyl ether (surface tension @ 20 °C = 17 dynes/cm)
  3. C) ethyl formate (surface tension @ 20 °C = 24 dynes/cm)
  4. D) propionic acid (surface tension @ 20 °C = 27 dynes/cm)
  5. E) propyl chloride (surface tension @ 20 °C = 18 dynes/cm)

Answer:  B

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

33) The vapor pressure of mercury is 1 mm Hg at 126 °C; 10 mm Hg at 184 °C; 400mm Hg at 323 °C; 100 mm Hg at 262 °C; 760 mm Hg at 357 °C. What is the normal boiling point of mercury?

  1. A) 126 °C
  2. B) 184 °C
  3. C) 262 °C
  4. D) 323 °C
  5. E) 357 °C

Answer:  E

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

34) The vapor pressure of methanol is 1 mm Hg at -44 °C; 10 mm Hg at -16 °C; 100mm Hg at 21 °C; 760 mm Hg at 65 °C; 1520 mm Hg at 84 °C. What is the normal boiling point of methanol?

  1. A) -44 °C
  2. B) -16 °C
  3. C) 21 °C
  4. D) 65 °C
  5. E) 84 °C

Answer:  D

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

35) The vapor pressure of ethanol is 360 mm Hg at 60 °C; 600 mm Hg at 72 °C; 760mm Hg at 78 °C; 810 mm Hg at 80 °C; 1190 mm Hg at 90 °C. What is the normal boiling point of ethanol?

  1. A) 60 °C
  2. B) 72 °C
  3. C) 78 °C
  4. D) 80 °C
  5. E) 90 °C

Answer:  C

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

36) The vapor pressure of acetone is 1 torr at -59 °C; 100 torr at 8 °C; 400 torr at 40 °C; 760 torr at 56 °C; 1520 torr at 79 °C. What is the normal boiling point of acetone?

  1. A) -59 °C
  2. B) 8 °C
  3. C) 40 °C
  4. D) 56 °C
  5. E) 79 °C

Answer:  D

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

37) The vapor pressure of ethyl ether is 7.87 in. Hg at 2 °C; 11.8 in. Hg at 12 °C; 27.5 in. Hg at 32 °C; 29.9 in. Hg at 35 °C; 39.3 in. Hg at 42 °C. What is the normal boiling point of ethyl ether?

  1. A) 2 °C
  2. B) 12 °C
  3. C) 32 °C
  4. D) 35 °C
  5. E) 42 °C

Answer:  D

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

38) The vapor pressure of chloroform is 0.001 atm at -58 °C; 0.132 atm at 10 °C; 0.526 atm at 43 °C; 1.00 atm at 61 °C; 2.00 atm at 84 °C. What is the normal boiling point of chloroform?

  1. A) -58 °C
  2. B) 10 °C
  3. C) 43 °C
  4. D) 61 °C
  5. E) 84 °C

Answer:  D

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

39) The vapor pressure of a chlorofluorocarbon (CFC) is 0.193 psi at -98 °C; 1.91 psi at -70 °C; 14.7 psi at -30 °C; 29.4 psi at -12 °C; 73.5 psi at 16 °C. What is the normal boiling point of the CFC?

  1. A) -98 °C
  2. B) -69 °C
  3. C) -30 °C
  4. D) -12 °C
  5. E) 16 °C

Answer:  C

Section:  11.3 Vapor Pressure, Boiling Point, Viscosity, and Surface Tension

 

40) Which of the following is an observed property of solids?

  1. A) Solids have a fixed shape and fixed volume.
  2. B) Solids can be crystalline or noncrystalline.
  3. C) Solids do not compress or expand significantly.
  4. D) Solids are usually more dense than liquids.
  5. E) all of the above

Answer:  E

Section:  11.4 Properties of Solids

 

41) Which of the following is an observed property of solids?

  1. A) Solids have a variable shape and fixed volume.
  2. B) Solids can have noncrystalline structures.
  3. C) Solids compress and expand significantly.
  4. D) Solids are usually less dense than liquids.
  5. E) none of the above

Answer:  B

Section:  11.4 Properties of Solids

 

42) Which of the following is an observed property of solids?

  1. A) Solids have a rigid shape and variable volume.
  2. B) Solids always have crystalline structures.
  3. C) Solids compress and expand significantly.
  4. D) Solids are usually less dense than liquids.
  5. E) none of the above

Answer:  E

Section:  11.4 Properties of Solids

 

43) Predict the physical state of krypton at -155 °C (Mp = -157 °C, Bp = -152 °C) and normal atmospheric pressure.

  1. A) solid
  2. B) liquid
  3. C) gas
  4. D) solid and liquid
  5. E) liquid and gas

Answer:  B

Section:  11.4 Properties of Solids

 

 

44) Predict the physical state of krypton at -175 °C (Mp = -157 °C, Bp = -152 °C) and normal atmospheric pressure.

  1. A) solid
  2. B) liquid
  3. C) gas
  4. D) solid and liquid
  5. E) liquid and gas

Answer:  A

Section:  11.4 Properties of Solids

 

45) Predict the physical state of krypton at -150 °C (Mp = -157 °C, Bp = -152 °C) and normal atmospheric pressure.

  1. A) solid
  2. B) liquid
  3. C) gas
  4. D) solid and liquid
  5. E) liquid and gas

Answer:  C

Section:  11.4 Properties of Solids

 

46) Which of the following are types of crystalline solids?

  1. A) ionic
  2. B) metallic
  3. C) molecular
  4. D) all of the above
  5. E) none of the above

Answer:  D

Section:  11.5 Crystalline Solids

 

47) Which of the following types of crystalline solids have ions arranged in regular geometric patterns?

  1. A) ionic
  2. B) metallic
  3. C) molecular
  4. D) all of the above
  5. E) none of the above

Answer:  A

Section:  11.5 Crystalline Solids

 

48) Which of the following types of crystalline solids have molecules arranged in regular geometric patterns?

  1. A) ionic
  2. B) metallic
  3. C) molecular
  4. D) all of the above
  5. E) none of the above

Answer:  C

Section:  11.5 Crystalline Solids

 

 

49) Which of the following types of crystalline solids have metal atoms arranged in regular geometric patterns?

  1. A) ionic
  2. B) metallic
  3. C) molecular
  4. D) all of the above
  5. E) none of the above

Answer:  B

Section:  11.5 Crystalline Solids

 

50) Which of the following is an example of an ionic crystalline solid?

  1. A) calcite, CaCO3
  2. B) fluorite, CaF2
  3. C) iron pyrite, FeS2
  4. D) silver chloride, AgCl
  5. E) all of the above

Answer:  E

Section:  11.5 Crystalline Solids

 

51) Which of the following is an example of an ionic crystalline solid?

  1. A) halite, NaCl
  2. B) phosphorus, P4
  3. C) sucrose, C12H22O11
  4. D) urea, CO(NH2)2
  5. E) none of the above

Answer:  A

Section:  11.5 Crystalline Solids

 

52) Which of the following is an example of a molecular crystalline solid?

  1. A) DDT, C14H9Cl5
  2. B) ice, H2O
  3. C) sulfur, S8
  4. D) vitamin D, C27H44O
  5. E) all of the above

Answer:  E

Section:  11.5 Crystalline Solids

 

53) Which of the following is an example of a molecular crystalline solid?

  1. A) dry ice, CO2
  2. B) fluorite, CaF2
  3. C) marble, CaCO3
  4. D) iron pyrite, FeS2
  5. E) none of the above

Answer:  A

Section:  11.5 Crystalline Solids

 

 

54) Which of the following is an example of a metallic crystalline solid?

  1. A) potassium, K
  2. B) titanium, Ti
  3. C) vanadium, V
  4. D) all of the above
  5. E) none of the above

Answer:  D

Section:  11.5 Crystalline Solids

 

55) Which of the following is an example of a metallic crystalline solid?

  1. A) charcoal, C
  2. B) diamond, C
  3. C) graphite, C
  4. D) all of the above
  5. E) none of the above

Answer:  E

Section:  11.5 Crystalline Solids

 

56) Calculate the number of calories required to raise 10.0 g of water from 25.0 °C to 75.0 °C. The specific heat of water is 1.00 cal/(g x °C).

  1. A) 10.0 cal
  2. B) 50.0 cal
  3. C) 2.50 x 102cal
  4. D) 5.00 x 102cal
  5. E) 7.50 x 102cal

Answer:  D

Section:  11.6 Changes of Physical State

 

57) Calculate the number of calories released when 25.0 g of water cools from 95.0 °C to 20.0 °C. The specific heat of water is 1.00 cal/(g x °C).

  1. A) 25.0 cal
  2. B) 75.0 cal
  3. C) 5.00 x 102cal
  4. D) 1.88 x 103cal
  5. E) 2.38 x 103cal

Answer:  D

Section:  11.6 Changes of Physical State

 

58) Calculate the heat absorbed when 10.0 g of ice at 0 °C melts to water at the same temperature. The specific heat of water is 1.00 cal/(g x °C); the heat of fusion is 80.0cal/g; and the heat of vaporization is 540.0 cal/g.

  1. A) 8.0 cal
  2. B) 10.0 cal
  3. C) 54.0 cal
  4. D) 8.00 x 102cal
  5. E) 5.40 x 103cal

Answer:  D

Section:  11.6 Changes of Physical State

 

59) Calculate the heat released when 25.0 g of water at 0 °C crystallizes to ice at the same temperature. The specific heat of water is 1.00 cal/(g x °C); the heat of fusion is 80.0 cal/g; and the heat of vaporization is 540.0 cal/g.

  1. A) 3.20 cal
  2. B) 21.6 cal
  3. C) 25.0 cal
  4. D) 2.00 x 103cal
  5. E) 1.35 x 104cal

Answer:  D

Section:  11.6 Changes of Physical State

 

60) Calculate the heat required to convert 10.0 g of water at 100 °C to steam at 100 °C. The specific heat of water is 1.00 cal/(g x °C); the heat of fusion is 80.0 cal/g; and the heat of vaporization is 540.0 cal/g.

  1. A) 8.0 cal
  2. B) 10.0 cal
  3. C) 54.0 cal
  4. D) 8.00 x 102cal
  5. E) 5.40 x 103cal

Answer:  E

Section:  11.6 Changes of Physical State

 

61) Calculate the heat released when 25.0 g of steam at 100 °C condenses to a liquid at 100 °C. The specific heat of water is 1.00 cal/(g x °C); the heat of fusion is 80.0 cal/g; and the heat of vaporization is 540.0 cal/g.

  1. A) 3.20 cal
  2. B) 21.6 cal
  3. C) 25.0 cal
  4. D) 2.00 x 103cal
  5. E) 1.35 x 104cal

Answer:  E

Section:  11.6 Changes of Physical State

 

62) Calculate the heat required to convert 10.0 g of water at 25.0 °C to steam at 100.0 °C. The specific heat of water is 1.00 cal/(g x °C); the heat of fusion is 80.0 cal/g; and the heat of vaporization is 540.0 cal/g.

  1. A) 7.50 x 102cal
  2. B) 8.00 x 102cal
  3. C) 1.05 x 103cal
  4. D) 1.55 x 103cal
  5. E) 6.15 x 103cal

Answer:  E

Section:  11.6 Changes of Physical State

 

 

63) Calculate the heat released when 10.0 g of water at 25.0 °C cools to ice at 0.0 °C. The specific heat of water is 1.00 cal/(g x °C); the heat of fusion is 80.0 cal/g; and the heat of vaporization is 540.0 cal/g.

  1. A) 2.50 x 102cal
  2. B) 1.05 x 103cal
  3. C) 5.15 x 103cal
  4. D) 5.40 x 103cal
  5. E) 5.65 x 103cal

Answer:  B

Section:  11.6 Changes of Physical State

 

64) Calculate the heat required to convert 10.0 g of ice at 0.0 °C to steam at 100.0 °C. The specific heat of water is 1.00 cal/(g x °C); the heat of fusion is 80.0 cal/g; and the heat of vaporization is 540.0 cal/g.

  1. A) 1.80 x 103cal
  2. B) 5.40 x 103cal
  3. C) 6.20 x 103cal
  4. D) 6.40 x 103cal
  5. E) 7.20 x 103cal

Answer:  E

Section:  11.6 Changes of Physical State

 

65) Calculate the heat released when 25.0 g of steam at 100.0 °C cools to ice at 0.0 °C. The specific heat of water is 1.00 cal/(g x °C); the heat of fusion is 80.0 cal/g; and the heat of vaporization is 540.0 cal/g.

  1. A) 4.50 x 103cal
  2. B) 1.35 x 104cal
  3. C) 1.55 x 104cal
  4. D) 1.60 x 104cal
  5. E) 1.80 x 104cal

Answer:  E

Section:  11.6 Changes of Physical State

 

66) How many pairs of bonding electrons are in a water molecule?

  1. A) 0
  2. B) 1
  3. C) 2
  4. D) 3
  5. E) 4

Answer:  C

Section:  11.7 Structure of Water

 

67) How many pairs of nonbonding electrons are in a water molecule?

  1. A) 0
  2. B) 1
  3. C) 2
  4. D) 3
  5. E) 4

Answer:  C

Section:  11.7 Structure of Water

 

68) What is the experimentally observed bond angle in a water molecule?

  1. A) 90°
  2. B) 104.5°
  3. C) 109.5°
  4. D) 120°
  5. E) 180°

Answer:  B

Section:  11.7 Structure of Water

 

69) What is the type of bond between H-O in a water molecule?

  1. A) coordinate covalent bond
  2. B) hydrogen bond
  3. C) nonpolar covalent bond
  4. D) polar covalent bond
  5. E) none of the above

Answer:  D

Section:  11.7 Structure of Water

 

70) Which of the following illustrates the bond polarity between H-O in water?

  1. A) (δ+) H–O (δ+)
  2. B) (δ+) H–O (δ-)
  3. C) (δ-) H–O (δ+)
  4. D) (δ-) H–O (δ-)
  5. E) (δ) H–O (δ)

Answer:  B

Section:  11.7 Structure of Water

 

71) How many dipoles are in a water molecule?

  1. A) 0
  2. B) 1
  3. C) 2
  4. D) 3
  5. E) 4

Answer:  C

Section:  11.7 Structure of Water

 

72) How many net dipoles are in a water molecule?

  1. A) 0
  2. B) 1
  3. C) 2
  4. D) 3
  5. E) none of the above

Answer:  B

Section:  11.7 Structure of Water

 

 

73) Which of the following is an intermolecular bond between water molecules?

  1. A) coordinate covalent bond
  2. B) hydrogen bond
  3. C) nonpolar covalent bond
  4. D) polar covalent bond
  5. E) all of the above

Answer:  B

Section:  11.7 Structure of Water

 

74) Which of the following properties of water is much higher than predicted?

  1. A) melting point
  2. B) boiling point
  3. C) heat of fusion
  4. D) heat of vaporization
  5. E) all of the above

Answer:  E

Section:  11.8 Physical Properties of Water

 

75) Which of the following explains why ice floats on water?

  1. A) Ice has a greater density than water.
  2. B) Ice has a greater heat of fusion than water.
  3. C) Ice has a greater molar mass than water.
  4. D) Ice has a greater specific heat than water.
  5. E) Ice has a greater volume than an equal mass of water.

Answer:  E

Section:  11.8 Physical Properties of Water

 

76) Which of the following explains why a needle can float on water?

  1. A) The density of the water is greater than the needle.
  2. B) The molar mass of the water is greater than the needle.
  3. C) The surface tension of the water supports the needle.
  4. D) The vapor pressure of the water supports the needle.
  5. E) The viscosity of the water supports the needle.

Answer:  C

Section:  11.8 Physical Properties of Water

 

77) Which of the following accounts for the unusually high melting point of ice?

  1. A) the crystalline structure of ice
  2. B) the density of ice
  3. C) the hydrogen bonds in ice
  4. D) the molar mass of ice
  5. E) the specific heat of ice

Answer:  C

Section:  11.8 Physical Properties of Water

 

 

78) Which of the following accounts for the unusually high boiling point of water?

  1. A) the density of water
  2. B) the hydrogen bonds in water
  3. C) the molar mass of water
  4. D) the specific heat of water
  5. E) the surface tension in water

Answer:  B

Section:  11.8 Physical Properties of Water

 

79) Which of the following accounts for the unusually high heat of fusion for ice?

  1. A) the crystalline structure of ice
  2. B) the density of ice
  3. C) the hydrogen bonds in ice
  4. D) the molar mass of ice
  5. E) the specific heat of ice

Answer:  C

Section:  11.8 Physical Properties of Water

 

80) Which of the following accounts for the high heat of vaporization for water?

  1. A) the density of water
  2. B) the hydrogen bonds in water
  3. C) the molar mass of water
  4. D) the specific heat of water
  5. E) the surface tension in water

Answer:  B

Section:  11.8 Physical Properties of Water

 

81) What are the products from the electrolysis of water?

  1. A) hydrogen and oxygen
  2. B) hydrogen and ozone
  3. C) hydrogen and hydrogen peroxide
  4. D) hydrogen peroxide and oxygen
  5. E) none of the above

Answer:  A

Section:  11.9 Chemical Properties of Water

 

82) What are the products from the reaction of water and an active metal?

  1. A) a metal oxide and hydrogen gas
  2. B) a metal oxide and oxygen gas
  3. C) a metal hydroxide and hydrogen gas
  4. D) a metal hydroxide and oxygen gas
  5. E) none of the above

Answer:  C

Section:  11.9 Chemical Properties of Water

 

 

83) What is(are) the product(s) from the reaction of water and a metal oxide?

  1. A) a metal hydroxide
  2. B) a metal hydroxide and hydrogen peroxide
  3. C) a metal hydroxide and hydrogen gas
  4. D) a metal hydroxide and oxygen gas
  5. E) none of the above

Answer:  A

Section:  11.9 Chemical Properties of Water

 

84) What is the product from the reaction of water and a nonmetal oxide?

  1. A) an acid
  2. B) a base
  3. C) a nonmetal hydroxide and hydrogen gas
  4. D) a nonmetal hydroxide and oxygen gas
  5. E) none of the above

Answer:  A

Section:  11.9 Chemical Properties of Water

 

85) Complete the following chemical equation and indicate the products.

H2O(l)

  1. A) H + O
  2. B) H2+ O2
  3. C) H2+ O3
  4. D) H2O2+ O2
  5. E) H2O2+ O3

Answer:  B

Section:  11.9 Chemical Properties of Water

 

86) Complete the following chemical equation and indicate the products.

K(s) + H2O(l) →

  1. A) K2O + H2
  2. B) K2O + H2O2
  3. C) KOH + H2
  4. D) KOH + O2
  5. E) KOH + H2O2

Answer:  C

Section:  11.9 Chemical Properties of Water

 

87) Complete the following chemical equation and indicate the products.

Sr(s) + H2O(l) →

  1. A) SrO + H2
  2. B) SrO + H2O2
  3. C) Sr(OH)2+ H2
  4. D) Sr(OH)2+ O2
  5. E) Sr(OH)2+ H2O2

Answer:  C

Section:  11.9 Chemical Properties of Water

 

88) Complete the following chemical equation and indicate the product(s).

Li2O(s) + H2O(l) →

  1. A) LiOH
  2. B) LiOH + H2
  3. C) LiOH + O2
  4. D) LiOH + O3
  5. E) LiOH + H2O2

Answer:  A

Section:  11.9 Chemical Properties of Water

 

89) Complete the following chemical equation and indicate the product(s).

MgO(s) + H2O(l) →

  1. A) Mg(OH)2
  2. B) Mg(OH)2+ H2
  3. C) Mg(OH)2+ O2
  4. D) Mg(OH)2+ O3
  5. E) Mg(OH)2+ H2O2

Answer:  A

Section:  11.9 Chemical Properties of Water

 

90) Complete the following chemical equation and indicate the product(s).

ZnO(s) + H2O(l) →

  1. A) Zn(OH)2
  2. B) Zn(OH)2+ H2
  3. C) Zn(OH)2+ O2
  4. D) Zn(OH)2+ O3
  5. E) Zn(OH)2+ H2O2

Answer:  A

Section:  11.9 Chemical Properties of Water

 

91) Complete the following chemical equation and indicate the product(s).

CO2(g) + H2O(l) →

  1. A) CH3OH
  2. B) HC2H3O2
  3. C) H2CO3
  4. D) CO + H2O2
  5. E) CO + H2+ O2

Answer:  C

Section:  11.9 Chemical Properties of Water

 

 

92) Complete the following chemical equation and indicate the product(s).

SO2(g) + H2O(l) →

  1. A) H2SO3
  2. B) H2SO4
  3. C) H2S + H2O2
  4. D) SO3+ H2O2
  5. E) SO3+ H2

Answer:  A

Section:  11.9 Chemical Properties of Water

 

93) Complete the following chemical equation and indicate the product(s).

SO3(g) + H2O(l) →

  1. A) H2SO3
  2. B) H2SO4
  3. C) H2S + H2O2
  4. D) SO2+ H2O2
  5. E) SO3+ H2

Answer:  B

Section:  11.9 Chemical Properties of Water

 

94) What is the product from the reaction of hydrogen and oxygen gases?

  1. A) an acid
  2. B) a base
  3. C) a hydrate
  4. D) hydrogen peroxide
  5. E) water

Answer:  E

Section:  11.9 Chemical Properties of Water

 

95) What are the products from the complete combustion of a hydrocarbon?

  1. A) carbon and water
  2. B) carbon monoxide and hydrogen
  3. C) carbon monoxide and water
  4. D) carbon dioxide and hydrogen
  5. E) carbon dioxide and water

Answer:  E

Section:  11.9 Chemical Properties of Water

 

96) What are the products from a neutralization reaction?

  1. A) metal oxide and water
  2. B) nonmetal oxide and hydrogen
  3. C) salt and water
  4. D) salt and hydrogen
  5. E) none of the above

Answer:  C

Section:  11.9 Chemical Properties of Water

 

 

97) What are the products from the decomposition of a hydrate?

  1. A) anhydrous compound and hydrogen
  2. B) anhydrous compound and oxygen
  3. C) anhydrous compound and water
  4. D) metal hydroxide and hydrogen
  5. E) metal hydroxide and water

Answer:  C

Section:  11.9 Chemical Properties of Water

 

98) Complete the following chemical reaction and indicate the product(s).

H2(g) + O2(g)

  1. A) H + O
  2. B) H2+ O2
  3. C) H2+ O3
  4. D) H2O
  5. E) H2O2

Answer:  D

Section:  11.9 Chemical Properties of Water

 

99) Complete the following chemical reaction and indicate the products.

CH4(g) + O2(g)

  1. A) C + H2O
  2. B) CO + H2
  3. C) CO + H2O
  4. D) CO2+ H2
  5. E) CO2+ H2O

Answer:  E

Section:  11.9 Chemical Properties of Water

 

100) Complete the following chemical reaction and indicate the products.

C2H4(g) + O2(g)

  1. A) C + H2O
  2. B) CO + H2
  3. C) CO + H2O
  4. D) CO2+ H2
  5. E) CO2+ H2O

Answer:  E

Section:  11.9 Chemical Properties of Water

 

 

101) Complete the following chemical reaction and indicate the products.

C2H5OH(g) + O2(g)

  1. A) C + H2O
  2. B) CO + H2
  3. C) CO + H2O
  4. D) CO2+ H2
  5. E) CO2+ H2O

Answer:  E

Section:  11.9 Chemical Properties of Water

 

102) Complete the following chemical reaction and indicate the products.

HNO3(aq) + Ca(OH)2(aq) →

  1. A) Ca(NO2)2and H2
  2. B) Ca(NO2)2and H2O
  3. C) Ca(NO3)2and H2
  4. D) Ca(NO3)2and O2
  5. E) Ca(NO3)2and H2O

Answer:  E

Section:  11.9 Chemical Properties of Water

 

103) Complete the following chemical reaction and indicate the products.

HC2H3O2(aq) + KOH(aq) →

  1. A) KHCO3and H2
  2. B) KHCO3and H2O
  3. C) KC2H3O2and H2
  4. D) KC2H3O2and O2
  5. E) KC2H3O2and H2O

Answer:  E

Section:  11.9 Chemical Properties of Water

 

104) Complete the following chemical reaction and indicate the products.

HCl(aq) + NH4OH(aq) →

  1. A) NH4Cl and O2
  2. B) NH4Cl and H2O
  3. C) NH4Cl and H2O2
  4. D) NH3, Cl2, and H2O
  5. E) NH3, HCl, and H2O

Answer:  B

Section:  11.9 Chemical Properties of Water

 

 

105) Complete the following chemical reaction and indicate the products.

CoSO4 • H2O(s)

  1. A) CoSO3and H2
  2. B) CoSO4and H2
  3. C) CoSO3and H2O
  4. D) CoSO4and H2O
  5. E) CoSO4,H2, and O2

Answer:  D

Section:  11.9 Chemical Properties of Water

 

106) Complete the following chemical reaction and indicate the products.

Na3PO4 • 10H2O(s)

  1. A) Na3PO3and H2
  2. B) Na3PO4and O2
  3. C) Na3PO3and H2O
  4. D) Na3PO4and H2O
  5. E) Na3PO4,H2, and O2

Answer:  D

Section:  11.9 Chemical Properties of Water

 

107) Complete the following chemical reaction and indicate the products.

Ni(NO3)2 • 6H2O(s)

  1. A) Ni(NO3)2and H2
  2. B) Ni(NO2)2and H2
  3. C) Ni(NO3)2and H2O
  4. D) Ni(NO2)2and H2O
  5. E) Ni(NO3)2,H2, and O2

Answer:  C

Section:  11.9 Chemical Properties of Water

 

108) What is the systematic name for MnSO4 • H2O?

  1. A) manganese sulfate hydrate
  2. B) manganese sulfate monohydrate
  3. C) manganese(II) sulfite monohydrate
  4. D) manganese(II) sulfate monohydrate
  5. E) manganese(II) sulfate dihydrate

Answer:  D

Section:  11.10 Hydrates

 

 

109) What is the systematic name for CuSO4 • 5H2O?

  1. A) copper sulfate hydrate
  2. B) copper sulfate pentahydrate
  3. C) copper(II) sulfate hydrate
  4. D) copper(II) sulfate dihydrate
  5. E) copper(II) sulfate pentahydrate

Answer:  E

Section:  11.10 Hydrates

 

110) What is the systematic name for CoCl3 • 6H2O?

  1. A) cobalt chloride hydrate
  2. B) cobalt chloride hexahydrate
  3. C) cobalt(III) chloride hydrate
  4. D) cobalt(III) chloride trihydrate
  5. E) cobalt(III) chloride hexahydrate

Answer:  E

Section:  11.10 Hydrates

 

111) What is the chemical formula for sodium chromate tetrahydrate?

  1. A) Na2CrO4 2H2O
  2. B) Na2CrO4 3H2O
  3. C) Na2CrO4 4H2O
  4. D) Na2Cr2O7 3H2O
  5. E) Na2Cr2O7 4H2O

Answer:  C

Section:  11.10 Hydrates

 

112) What is the chemical formula for strontium nitrate hexahydrate?

  1. A) Sr(NO2)2 H2O
  2. B) Sr(NO2)2 6H2O
  3. C) Sr(NO3)2 H2O
  4. D) Sr(NO3)2 6H2O
  5. E) Sr(NO3)2 7H2O

Answer:  D

Section:  11.10 Hydrates

 

113) What is the chemical formula for sodium carbonate decahydrate?

  1. A) NaC2H3O2 10H2O
  2. B) Na2CO3 4H2O
  3. C) Na2CO3 10H2O
  4. D) NaHCO3 H2O
  5. E) NaHCO3 10H2O

Answer:  C

Section:  11.10 Hydrates

 

 

114) What is the percentage of water in NiCl2 • 2H2O?

  1. A) 10.8%
  2. B) 12.2%
  3. C) 13.8%
  4. D) 21.8%
  5. E) 27.7%

Answer:  D

Section:  11.10 Hydrates

 

115) What is the percentage of water in CoCl2 • 6H2O?

  1. A) 7.57%
  2. B) 12.2%
  3. C) 13.9%
  4. D) 45.4%
  5. E) 83.1%

Answer:  D

Section:  11.10 Hydrates

 

116) What is the percentage of water in gypsum, CaSO4 • 2H2O?

  1. A) 10.4%
  2. B) 13.2%
  3. C) 20.9%
  4. D) 23.3%
  5. E) 26.4%

Answer:  C

Section:  11.10 Hydrates

 

117) What is the percentage of water in borax, Na2B4O7 • 10H2O?

  1. A) 4.72%
  2. B) 8.95%
  3. C) 47.2%
  4. D) 82.1%
  5. E) 89.5%

Answer:  C

Section:  11.10 Hydrates

 

118) What is the percentage of water in Ni(NO3)2 • 2H2O?

  1. A) 8.23%
  2. B) 8.97%
  3. C) 9.85%
  4. D) 16.5%
  5. E) 19.7%

Answer:  D

Section:  11.10 Hydrates

 

 

119) An unknown hydrate of zinc sulfate, ZnSO4 • XH2O, is heated to give 43.8% water. What is the water of crystallization (X) for the hydrate?

  1. A) 1
  2. B) 4
  3. C) 6
  4. D) 7
  5. E) 10

Answer:  D

Section:  11.10 Hydrates

 

120) An unknown hydrate of iron(II) sulfate, FeSO4 • XH2O, is heated to give 45.3% water. What is the water of crystallization (X) for the hydrate?

  1. A) 1
  2. B) 4
  3. C) 6
  4. D) 7
  5. E) 10

Answer:  D

Section:  11.10 Hydrates

 

121) An unknown hydrate of sodium dichromate, Na2Cr2O7 • XH2O, is heated to give 12.1% water. What is the water of crystallization (X) for the hydrate?

  1. A) 1
  2. B) 2
  3. C) 3
  4. D) 4
  5. E) 12

Answer:  B

Section:  11.10 Hydrates

 

122) An unknown hydrate of cobalt(II) cyanide, Co(CN)2 • XH2O, is heated to give 32.7% water. What is the water of crystallization (X) for the hydrate?

  1. A) 2
  2. B) 3
  3. C) 4
  4. D) 6
  5. E) 10

Answer:  B

Section:  11.10 Hydrates

 

123) An unknown hydrate of calcium nitrate, Ca(NO3)2 • XH2O, is heated to give 30.5% water. What is the water of crystallization (X) for the hydrate?

  1. A) 2
  2. B) 3
  3. C) 4
  4. D) 6
  5. E) 10

Answer:  C

Section:  11.10 Hydrates

 

124) An unknown hydrate of chromium(III) acetate, Cr(C2H3O2)3 • XH2O, is heated to give 7.29% water. What is the water of crystallization (X) for the hydrate?

  1. A) 1
  2. B) 4
  3. C) 6
  4. D) 8
  5. E) 12

Answer:  A

Section:  11.10 Hydrates

 

125) Which physical state is described by the following analogy?

A beaker of marbles is covered with honey. When shaken, the marbles

move about slowly and randomly as they overcome their stickiness.

  1. A) solid
  2. B) liquid
  3. C) gas
  4. D) all of the above
  5. E) none of the above

Answer:  B

Section:  General Exercises

 

126) Which physical state is described by the following analogy?

A beehive is surrounded by flying honey bees. When approached

with a lit torch, the honey bees move about much faster.

  1. A) solid
  2. B) liquid
  3. C) gas
  4. D) all of the above
  5. E) none of the above

Answer:  C

Section:  General Exercises

 

127) Predict the physical state of water at 100 °C (Bp = 100 °C) and 1.1 atm pressure.

  1. A) solid
  2. B) liquid
  3. C) gas
  4. D) all of the above
  5. E) none of the above

Answer:  B

Section:  General Exercises

 

 

128) Predict the physical state of nitrogen at 77 K (Bp = 77 K) and 1.1 atm pressure.

  1. A) solid
  2. B) liquid
  3. C) gas
  4. D) all of the above
  5. E) none of the above

Answer:  B

Section:  General Exercises

 

129) Predict the physical state of helium at 4 K (Bp = 4 K) and 1.1 atm pressure.

  1. A) solid
  2. B) liquid
  3. C) gas
  4. D) all of the above
  5. E) none of the above

Answer:  B

Section:  General Exercises

 

130) Which of the following describes a molecular liquid conceptually?

  1. A) Molecules move about randomly.
  2. B) Molecules are attracted to each other.
  3. C) Molecules at the surface may vaporize.
  4. D) Molecules are in contact with each other.
  5. E) all of the above

Answer:  E

Section:  General Exercises

 

131) Which of the following describes a molecular solid conceptually?

  1. A) Molecules are in fixed positions.
  2. B) Molecules are attracted to each other.
  3. C) Molecules form regular or random patterns.
  4. D) Molecules are in contact with each other.
  5. E) all of the above

Answer:  E

Section:  General Exercises

 

132) Which of the following is true of a hydrogen bond in liquids?

  1. A) It exists between hydrogen and an electronegative atom.
  2. B) It is the result of dipole attraction.
  3. C) Its bond energy is less than a covalent bond.
  4. D) Its bond length is longer than a covalent bond.
  5. E) all of the above

Answer:  E

Section:  General Exercises

 

 

133) A 73.6 g sample of aluminum is heated to 95.0 °C and dropped into 100.0 g of water at 20.0 °C. If the resulting temperature of the water is 30.0 °C, what is the specific heat of the metal?

  1. A) 0.143 cal/(g x °C)
  2. B) 0.209 cal/(g x °C)
  3. C) 0.418 cal/(g x °C)
  4. D) 0.486 cal/(g x °C)
  5. E) 0.679 cal/(g x °C)

Answer:  B

Section:  General Exercises

 

134) Based only on intermolecular attraction, predict which of the following liquids has the highest vapor pressure.

  1. A) CH3-CO-OH
  2. B) CH3-CH2-O-CH3
  3. C) CH3-CH2-S-CH3
  4. D) CH3-CH2-CH2-Cl
  5. E) CH3-CH2-CH2-CH2-CH3

Answer:  E

Section:  General Exercises

 

135) Based only on intermolecular attraction, predict which of the following liquids has the highest boiling point.

  1. A) CH3-CO-OH
  2. B) CH3-CH2-O-CH3
  3. C) CH3-CH2-S-CH3
  4. D) CH3-CH2-CH2-Cl
  5. E) CH3-CH2-CH2-CH2-CH3

Answer:  A

Section:  General Exercises

 

136) Based only on intermolecular attraction, predict which of the following liquids has the highest viscosity.

  1. A) CH3-CO-OH
  2. B) CH3-CH2-O-CH3
  3. C) CH3-CH2-S-CH3
  4. D) CH3-CH2-CH2-Cl
  5. E) CH3-CH2-CH2-CH2-CH3

Answer:  A

Section:  General Exercises

 

 

137) Based only on intermolecular attraction, predict which of the following liquids has the highest surface tension.

  1. A) CH3-CO-OH
  2. B) CH3-CH2-O-CH3
  3. C) CH3-CH2-S-CH3
  4. D) CH3-CH2-CH2-Cl
  5. E) CH3-CH2-CH2-CH2-CH3

Answer:  A

Section:  General Exercises

 

138) Which of the following types of crystalline solids is hard and brittle, has a high melting point, and conducts electricity only when melted?

  1. A) ionic
  2. B) metallic
  3. C) molecular
  4. D) all of the above
  5. E) none of the above

Answer:  A

Section:  General Exercises

 

139) Which of the following types of crystalline solids has a low melting point, is generally insoluble in water, and is a nonconductor of electricity?

  1. A) ionic
  2. B) metallic
  3. C) molecular
  4. D) all of the above
  5. E) none of the above

Answer:  C

Section:  General Exercises

 

140) Which of the following types of crystalline solids is malleable, ductile, and a conductor of electricity?

  1. A) ionic
  2. B) metallic
  3. C) molecular
  4. D) all of the above
  5. E) none of the above

Answer:  B

Section:  General Exercises

 

 

141) Calculate the heat necessary to convert 10.0 g of solid benzene at its melting point to vapor at its boiling point. The specific heat of liquid benzene is 0.580 cal/(g x °C), the heat of fusion for benzene is 31.0 cal/g, and the heat of vaporization is 94.0 cal/g. The melting point of benzene is 5.5 °C and the boiling point is 80.1 °C.

  1. A) 430 cal
  2. B) 740 cal
  3. C) 1250 cal
  4. D) 1293 cal
  5. E) 1683 cal

Answer:  E

Section:  General Exercises

 

142) A hydrate of sodium acetate is heated to give 39.7% water. What is the chemical formula for the hydrate?

  1. A) Na2CO3 H2O
  2. B) Na2CO3 3H2O
  3. C) NaC2H3O2 H2O
  4. D) NaC2H3O2 3H2O
  5. E) Na2C2O4 2H2O

Answer:  D

Section:  General Exercises

 

143) Plaster of Paris is a hydrate of calcium sulfate. If the hydrate is 6.20% water, what is the chemical formula for Plaster of Paris?

  1. A) CaSO4 1/2H2O
  2. B) CaSO4 1H2O
  3. C) CaSO4 2H2O
  4. D) CaSO4 3H2O
  5. E) CaSO4 15H2O

Answer:  A

Section:  General Exercises

 

Chemistry Connection – Water Purification

 

1) Which of the following cations is found in hard water?

  1. A) Ca2+
  2. B) Fe3+
  3. C) Mg2+
  4. D) Na+
  5. E) all of the above

Answer:  E

 

 

2) Which of the following anions is found in hard water?

  1. A) Cl-
  2. B) CO32-
  3. C) PO43-
  4. D) SO42-
  5. E) all of the above

Answer:  E

 

3) Which of the following cations is found in soft water?

  1. A) Ca2+
  2. B) Fe3+
  3. C) Mg2+
  4. D) Na+
  5. E) all of the above

Answer:  D

 

4) Which of the following anions is found in soft water?

  1. A) Cl-
  2. B) CO32-
  3. C) PO43-
  4. D) SO42-
  5. E) all of the above

Answer:  E

 

5) Which of the following cations is found in deionized water?

  1. A) Na+
  2. B) Mg2+
  3. C) Ca2+
  4. D) Fe3+
  5. E) none of the above

Answer:  E

 

6) Which of the following anions is found in deionized water?

  1. A) Cl-
  2. B) CO32-
  3. C) SO42-
  4. D) PO43-
  5. E) none of the above

Answer:  E

 

 

Critical Thinking – Bottled Water

 

1) What is the approximate percentage of all Americans who drink bottled water?

  1. A) 1%
  2. B) 5%
  3. C) 50%
  4. D) 75%
  5. E) 100%

Answer:  C

 

2) What is the difference between bottled water and tap water?

  1. A) Bottled water is distilled water.
  2. B) Bottled water is deionized water.
  3. C) Bottled water has minerals added.
  4. D) Bottled water originates from natural springs.
  5. E) Bottled water varies with its source.

Answer:  E

 

3) What is found in tap water that is not found in bottled water?

  1. A) Tap water contains air.
  2. B) Tap water contains carbonation.
  3. C) Tap water contains chlorine.
  4. D) Tap water contains fluoride.
  5. E) Tap water contains minerals.

Answer:  C

 

4) Which of the following is responsible for bubbles in sparkling mineral water?

  1. A) carbon dioxide
  2. B) air
  3. C) chlorine
  4. D) oxygen
  5. E) none of the above

Answer:  A

 

5) Which of the following is true of bottled water?

  1. A) Bottled water is superior in terms of purity.
  2. B) Bottled water is superior in terms health benefits.
  3. C) Bottled water is more strictly regulated by the EPA.
  4. D) Bottled water has lower levels of bacteria.
  5. E) none of the above

Answer:  E