TEST BANK
Chemistry
Francis A. Carey and Robert M. Giuliano
JN 10th International Edition
U
R
SE
,Table of Contents
Chapter 1—The Foundations of Chemistry
Chapter 2—Chemical Formulas and Composition Stoichiometry
Chapter 3—Chemical Equations and Reaction Stoichiometry
Chapter 4—The Structure of Atoms
Chapter 5—Chemical Periodicity
Chapter 6—Some Types of Chemical Reactions
Chapter 7—Chemical Bonding
Chapter 8—Molecular Structure and Covalent Bonding Theories
Chapter 9—Molecular Orbitals in Chemical Bonding
Chapter 10—Reactions in Aqueous Solutions I: Acids, Bases, and Salts
Chapter 11—Reactions in Aqueous Solutions II: Calculations
Chapter 12—Gases and the Kinetic-Molecular Theory
Chapter 13—Liquids and Solids
Chapter 14—Solutions
Chapter 15—Chemical Thermodynamics
Chapter 16—Chemical Kinetics
Chapter 17—Advanced Acid-Base Equilibria
Chapter 18—Ionic Equilibria I: Acids and Bases
JN
Chapter 19—Ionic Equilibria II: Buffers and Titration Curves
Chapter 20—Ionic Equilibria III: The Solubility Product Principle
Chapter 21—Electrochemistry
Chapter 22—Nuclear Chemistry
Chapter 23—Organic Chemistry I: Formulas, Names, and Properties
Chapter 24—Organic Chemistry II: Shapes, Selected Reactions, and Biopolymers
U
Chapter 25—Coordination Compounds
Chapter 26—Metals I: Metallurgy
Chapter 27—Metals II: Properties and Reactions
R
Chapter 28—Some Nonmetals and Metalloids
SE
,Chapter 1—The Foundations of Chemistry
MULTIPLE CHOICE
1. Which of the following statements is incorrect?
a. A body in motion possesses kinetic energy because of its motion.
b. An object possesses potential energy because of its position or composition.
c. Nuclear energy is an important kind of potential energy.
d. Chemical reactions and physical changes that release energy to their surroundings are
endothermic.
e. The Law of Conservation of Matter and Energy states that the combined amount of matter
and energy in the universe is fixed.
ANS: D
OBJ: Define the Laws of Conservation of matter and energy. | Define the terms endothermic and
exothermic. | Classify energy as potential or kinetic.
TOP: Matter and Energy
2. A braking automobile converts kinetic energy into heat in the brake pads. This is an example of the:
a. law of conservation of energy
b. law of constant composition
JN
c. law of conservation of matter
d. law of multiple proportions
e. law of gravity
ANS: A
OBJ: Apply the law of conservation of energy.
U
TOP: Matter and Energy
3. When magnesium is burned in air the mass of the product is heavier than the original mass of the
magnesium. However, the product formed still has the same exact mass of magnesium with the
R
remainder of the mass being oxygen. This is an example of:
a. law of conservation of energy
b. law of definite proportions
SE
c. law of conservation of matter
d. law of multiple proportions
e. law of gravity
ANS: C
OBJ: Apply the law of conservation of energy.
TOP: Matter and Energy
4. Which of the following represents matter that could be described as macroscale?
a. a bromine atom
b. molecules of water
c. bacteria observed under a microscope
d. a paperclip
e. none of these
ANS: D
OBJ: Classify a description of matter as atomic-, micro-, or macro-scale.
TOP: Chemistry – A Molecular View of Matter
, 5. Dalton's Atomic Theory included all of the ideas listed below except:
a. Atoms cannot be created or destroyed.
b. An element is composed of very small particles called protons, neutrons and electrons.
c. All atoms of a given element have identical properties.
d. All atoms of a given element have properties that differ from those of other elements.
e. Compounds are formed when atoms of different elements combine with one another in
small whole-number ratios.
ANS: B
OBJ: Identify the tenets of Dalton's atomic theory.
TOP: Chemistry – A Molecular View of Matter
6. Atoms consist of three fundamental particles. What are these particles and their charges?
a. proton (+1), neutron (neutral) and electron (-1)
b. proton (-1), neutron (+1) and electron (neutral)
c. proton (+1), neutron (-1) and electron (neutral)
d. proton (neutral), neutron (+1) and electron (-1)
e. proton (-1), neutron (neutral) and electron (+1)
ANS: A
OBJ: Identify the three subatomic particles that make up an atom.
TOP: Chemistry – A Molecular View of Matter
7. One of the following does not describe gases. Which one is it?
JN
a. Expands infinitely.
b. Rigid shape.
c. Easily compressed.
d. Relatively low densities.
e. Particles far apart.
U
ANS: B
OBJ: Classify a gas.
TOP: States of Matter
R
8. One of the following does not describe solids. Which one is it?
a. Particles in definite positions.
b. Definite shape.
SE
c. Easily compressed.
d. Relatively high densities.
e. Particles compact.
ANS: C
OBJ: Classify a solid.
TOP: States of Matter
9. Which response lists characteristics of liquids?
I. Volume does not vary much upon heating.
II. Shape is constant.
III. Easily compressed.
IV. Fills the container completely.
V. Flows.
Chemistry
Francis A. Carey and Robert M. Giuliano
JN 10th International Edition
U
R
SE
,Table of Contents
Chapter 1—The Foundations of Chemistry
Chapter 2—Chemical Formulas and Composition Stoichiometry
Chapter 3—Chemical Equations and Reaction Stoichiometry
Chapter 4—The Structure of Atoms
Chapter 5—Chemical Periodicity
Chapter 6—Some Types of Chemical Reactions
Chapter 7—Chemical Bonding
Chapter 8—Molecular Structure and Covalent Bonding Theories
Chapter 9—Molecular Orbitals in Chemical Bonding
Chapter 10—Reactions in Aqueous Solutions I: Acids, Bases, and Salts
Chapter 11—Reactions in Aqueous Solutions II: Calculations
Chapter 12—Gases and the Kinetic-Molecular Theory
Chapter 13—Liquids and Solids
Chapter 14—Solutions
Chapter 15—Chemical Thermodynamics
Chapter 16—Chemical Kinetics
Chapter 17—Advanced Acid-Base Equilibria
Chapter 18—Ionic Equilibria I: Acids and Bases
JN
Chapter 19—Ionic Equilibria II: Buffers and Titration Curves
Chapter 20—Ionic Equilibria III: The Solubility Product Principle
Chapter 21—Electrochemistry
Chapter 22—Nuclear Chemistry
Chapter 23—Organic Chemistry I: Formulas, Names, and Properties
Chapter 24—Organic Chemistry II: Shapes, Selected Reactions, and Biopolymers
U
Chapter 25—Coordination Compounds
Chapter 26—Metals I: Metallurgy
Chapter 27—Metals II: Properties and Reactions
R
Chapter 28—Some Nonmetals and Metalloids
SE
,Chapter 1—The Foundations of Chemistry
MULTIPLE CHOICE
1. Which of the following statements is incorrect?
a. A body in motion possesses kinetic energy because of its motion.
b. An object possesses potential energy because of its position or composition.
c. Nuclear energy is an important kind of potential energy.
d. Chemical reactions and physical changes that release energy to their surroundings are
endothermic.
e. The Law of Conservation of Matter and Energy states that the combined amount of matter
and energy in the universe is fixed.
ANS: D
OBJ: Define the Laws of Conservation of matter and energy. | Define the terms endothermic and
exothermic. | Classify energy as potential or kinetic.
TOP: Matter and Energy
2. A braking automobile converts kinetic energy into heat in the brake pads. This is an example of the:
a. law of conservation of energy
b. law of constant composition
JN
c. law of conservation of matter
d. law of multiple proportions
e. law of gravity
ANS: A
OBJ: Apply the law of conservation of energy.
U
TOP: Matter and Energy
3. When magnesium is burned in air the mass of the product is heavier than the original mass of the
magnesium. However, the product formed still has the same exact mass of magnesium with the
R
remainder of the mass being oxygen. This is an example of:
a. law of conservation of energy
b. law of definite proportions
SE
c. law of conservation of matter
d. law of multiple proportions
e. law of gravity
ANS: C
OBJ: Apply the law of conservation of energy.
TOP: Matter and Energy
4. Which of the following represents matter that could be described as macroscale?
a. a bromine atom
b. molecules of water
c. bacteria observed under a microscope
d. a paperclip
e. none of these
ANS: D
OBJ: Classify a description of matter as atomic-, micro-, or macro-scale.
TOP: Chemistry – A Molecular View of Matter
, 5. Dalton's Atomic Theory included all of the ideas listed below except:
a. Atoms cannot be created or destroyed.
b. An element is composed of very small particles called protons, neutrons and electrons.
c. All atoms of a given element have identical properties.
d. All atoms of a given element have properties that differ from those of other elements.
e. Compounds are formed when atoms of different elements combine with one another in
small whole-number ratios.
ANS: B
OBJ: Identify the tenets of Dalton's atomic theory.
TOP: Chemistry – A Molecular View of Matter
6. Atoms consist of three fundamental particles. What are these particles and their charges?
a. proton (+1), neutron (neutral) and electron (-1)
b. proton (-1), neutron (+1) and electron (neutral)
c. proton (+1), neutron (-1) and electron (neutral)
d. proton (neutral), neutron (+1) and electron (-1)
e. proton (-1), neutron (neutral) and electron (+1)
ANS: A
OBJ: Identify the three subatomic particles that make up an atom.
TOP: Chemistry – A Molecular View of Matter
7. One of the following does not describe gases. Which one is it?
JN
a. Expands infinitely.
b. Rigid shape.
c. Easily compressed.
d. Relatively low densities.
e. Particles far apart.
U
ANS: B
OBJ: Classify a gas.
TOP: States of Matter
R
8. One of the following does not describe solids. Which one is it?
a. Particles in definite positions.
b. Definite shape.
SE
c. Easily compressed.
d. Relatively high densities.
e. Particles compact.
ANS: C
OBJ: Classify a solid.
TOP: States of Matter
9. Which response lists characteristics of liquids?
I. Volume does not vary much upon heating.
II. Shape is constant.
III. Easily compressed.
IV. Fills the container completely.
V. Flows.
