TEST BANK
,Part I: Fundamentals of Chemistry
1. Introduction: Matter, Energy, and Measurement
Properties and classification of matter, physical and
chemical changes, units, measurements, significant
figures, and energy.
2. Atoms, Molecules, and Ions
Atomic theory, subatomic particles, isotopes, the
periodic table, chemical formulas, molecules, ions, and
naming inorganic compounds.
3. Chemical Reactions and Reaction Stoichiometry
Balancing equations, the mole concept, molar mass,
chemical calculations, limiting reactants, and percentage
yield.
4. Reactions in Aqueous Solution
Aqueous solutions, precipitation reactions, acid–base
reactions, oxidation–reduction reactions, and solution
stoichiometry.
5. Thermochemistry
Heat, work, energy changes, enthalpy, calorimetry, and
thermochemical calculations.
Part II: Atomic Structure and Chemical Bonding
6. Electronic Structure of Atoms
1
,Quantum theory, electromagnetic radiation, atomic
spectra, orbitals, quantum numbers, and electron
configurations.
7. Periodic Properties of the Elements
Periodic trends, atomic and ionic radii, ionization
energy, electron affinity, and properties of metals and
nonmetals.
8. Basic Concepts of Chemical Bonding
Lewis structures, the octet rule, ionic and covalent
bonds, bond energies, and electronegativity.
9. Molecular Geometry and Bonding Theories
Molecular shapes, VSEPR theory, bond polarity,
hybridization, valence bond theory, and molecular orbital
theory.
Part III: States of Matter and Solutions
10. Gases
Gas laws, the ideal gas equation, gas mixtures, partial
pressures, and kinetic molecular theory.
11. Liquids and Intermolecular Forces
Intermolecular attractions, phase changes, vapor
pressure, viscosity, surface tension, and hydrogen
bonding.
12. Solids and Modern Materials
Crystalline solids, crystal structures, unit cells,
metallic solids, semiconductors, and modern materials.
2
,13. Properties of Solutions
Solution formation, concentration, solubility,
temperature effects, colligative properties, and osmotic
pressure.
Part IV: Chemical Kinetics, Equilibrium, and
Thermodynamics
14. Chemical Kinetics
Reaction rates, rate laws, reaction orders, activation
energy, catalysts, and reaction mechanisms.
15. Chemical Equilibrium
Dynamic equilibrium, equilibrium constants, reaction
quotients, and Le Châtelier's principle.
16. Acid–Base Equilibria
Acid–base theories, strong and weak acids and bases, pH,
pOH, ionization constants, and equilibrium calculations.
17. Aqueous Equilibria: Buffers, Titrations, and
Solubility
Buffer systems, acid–base titrations, indicators,
solubility equilibria, and complex-ion formation.
18. Chemistry of the Environment
Atmospheric chemistry, air and water pollution,
environmental contaminants, and chemical processes
affecting the environment.
19. Chemical Thermodynamics
3
,Entropy, spontaneity, Gibbs free energy, and the
relationship between thermodynamics and equilibrium.
Part V: Electrochemistry, Nuclear Chemistry, and the
Elements
20. Electrochemistry
Redox reactions, galvanic and electrolytic cells,
electrode potentials, batteries, and electrolysis.
21. Nuclear Chemistry
Radioactivity, nuclear reactions, radioactive decay,
half-life, nuclear energy, and applications of
radioisotopes.
22. Chemistry of the Nonmetals
Properties, preparation, reactions, and compounds of
hydrogen and the nonmetallic elements.
23. Transition Metals and Coordination Chemistry
Transition-metal properties, coordination compounds,
ligands, complex ions, and coordination chemistry.
Part VI: Organic and Biological Chemistry
24. The Chemistry of Life: Organic and Biological
Chemistry
Organic compounds, functional groups, molecular
structures, carbohydrates, proteins, lipids, nucleic
acids, and the chemistry underlying biological processes.
4
,Chapter 1: Introduction: Matter, Energy, and Measurement
Core Focus: Properties and classification of matter,
physical and chemical changes, units, measurements,
significant figures, and energy.
Question 1: In the context of Introduction, which
fundamental definition or classification is accurate?
A) It is directly proportional to temperature and
inversely proportional to mass under standard
conditions.
B) It remains constant regardless of external
perturbations due to conservation laws.
C) It exhibits characteristic periodic or
stoichiometric dependence determined by fundamental
atomic and molecular interactions.
D) It decreases exponentially as a function of
activation energy and reaction quotient.
E) It is exclusively observed in heterogeneous
mixtures under extreme pressure.
Answer: C
Explanation: Fundamental principles established in
Chapter 1 dictate that system properties and chemical
behaviors are governed by underlying structural,
thermodynamic, or kinetic factors corresponding to option
C.
Question 2: Calculate or determine the outcome when
analyzing systems involving physical and chemical
changes.
A) It is directly proportional to temperature and
inversely proportional to mass under standard conditions.
5
,Part I: Fundamentals of Chemistry
1. Introduction: Matter, Energy, and Measurement
Properties and classification of matter, physical and
chemical changes, units, measurements, significant
figures, and energy.
2. Atoms, Molecules, and Ions
Atomic theory, subatomic particles, isotopes, the
periodic table, chemical formulas, molecules, ions, and
naming inorganic compounds.
3. Chemical Reactions and Reaction Stoichiometry
Balancing equations, the mole concept, molar mass,
chemical calculations, limiting reactants, and percentage
yield.
4. Reactions in Aqueous Solution
Aqueous solutions, precipitation reactions, acid–base
reactions, oxidation–reduction reactions, and solution
stoichiometry.
5. Thermochemistry
Heat, work, energy changes, enthalpy, calorimetry, and
thermochemical calculations.
Part II: Atomic Structure and Chemical Bonding
6. Electronic Structure of Atoms
1
,Quantum theory, electromagnetic radiation, atomic
spectra, orbitals, quantum numbers, and electron
configurations.
7. Periodic Properties of the Elements
Periodic trends, atomic and ionic radii, ionization
energy, electron affinity, and properties of metals and
nonmetals.
8. Basic Concepts of Chemical Bonding
Lewis structures, the octet rule, ionic and covalent
bonds, bond energies, and electronegativity.
9. Molecular Geometry and Bonding Theories
Molecular shapes, VSEPR theory, bond polarity,
hybridization, valence bond theory, and molecular orbital
theory.
Part III: States of Matter and Solutions
10. Gases
Gas laws, the ideal gas equation, gas mixtures, partial
pressures, and kinetic molecular theory.
11. Liquids and Intermolecular Forces
Intermolecular attractions, phase changes, vapor
pressure, viscosity, surface tension, and hydrogen
bonding.
12. Solids and Modern Materials
Crystalline solids, crystal structures, unit cells,
metallic solids, semiconductors, and modern materials.
2
,13. Properties of Solutions
Solution formation, concentration, solubility,
temperature effects, colligative properties, and osmotic
pressure.
Part IV: Chemical Kinetics, Equilibrium, and
Thermodynamics
14. Chemical Kinetics
Reaction rates, rate laws, reaction orders, activation
energy, catalysts, and reaction mechanisms.
15. Chemical Equilibrium
Dynamic equilibrium, equilibrium constants, reaction
quotients, and Le Châtelier's principle.
16. Acid–Base Equilibria
Acid–base theories, strong and weak acids and bases, pH,
pOH, ionization constants, and equilibrium calculations.
17. Aqueous Equilibria: Buffers, Titrations, and
Solubility
Buffer systems, acid–base titrations, indicators,
solubility equilibria, and complex-ion formation.
18. Chemistry of the Environment
Atmospheric chemistry, air and water pollution,
environmental contaminants, and chemical processes
affecting the environment.
19. Chemical Thermodynamics
3
,Entropy, spontaneity, Gibbs free energy, and the
relationship between thermodynamics and equilibrium.
Part V: Electrochemistry, Nuclear Chemistry, and the
Elements
20. Electrochemistry
Redox reactions, galvanic and electrolytic cells,
electrode potentials, batteries, and electrolysis.
21. Nuclear Chemistry
Radioactivity, nuclear reactions, radioactive decay,
half-life, nuclear energy, and applications of
radioisotopes.
22. Chemistry of the Nonmetals
Properties, preparation, reactions, and compounds of
hydrogen and the nonmetallic elements.
23. Transition Metals and Coordination Chemistry
Transition-metal properties, coordination compounds,
ligands, complex ions, and coordination chemistry.
Part VI: Organic and Biological Chemistry
24. The Chemistry of Life: Organic and Biological
Chemistry
Organic compounds, functional groups, molecular
structures, carbohydrates, proteins, lipids, nucleic
acids, and the chemistry underlying biological processes.
4
,Chapter 1: Introduction: Matter, Energy, and Measurement
Core Focus: Properties and classification of matter,
physical and chemical changes, units, measurements,
significant figures, and energy.
Question 1: In the context of Introduction, which
fundamental definition or classification is accurate?
A) It is directly proportional to temperature and
inversely proportional to mass under standard
conditions.
B) It remains constant regardless of external
perturbations due to conservation laws.
C) It exhibits characteristic periodic or
stoichiometric dependence determined by fundamental
atomic and molecular interactions.
D) It decreases exponentially as a function of
activation energy and reaction quotient.
E) It is exclusively observed in heterogeneous
mixtures under extreme pressure.
Answer: C
Explanation: Fundamental principles established in
Chapter 1 dictate that system properties and chemical
behaviors are governed by underlying structural,
thermodynamic, or kinetic factors corresponding to option
C.
Question 2: Calculate or determine the outcome when
analyzing systems involving physical and chemical
changes.
A) It is directly proportional to temperature and
inversely proportional to mass under standard conditions.
5
