Question 1

Which of the following would be regarded as compounds?

Accepted Answer

A)  H₂O, O₂, and CH₄ 
B)  H₂O and O₂ 
C)  O₂ and CH₄ 
D)  CH₄ and O₂, but not H₂O 
E)  H₂O and CH₄, but not O₂ 
A)  H₂O, O₂, and CH₄ 
B)  H₂O and O₂ 
C)  O₂ and CH₄ 
D)  CH₄ and O₂, but not H₂O 
E)  H₂O and CH₄, but not O₂

Question 2

-Based on electron configuration, which of these elements in the figure above would exhibit a chemical behavior most like that of oxygen?

Accepted Answer

A)  carbon 
B)  hydrogen 
C)  nitrogen 
D)  sulfur 
E)  phosphorus 
A)  carbon 
B)  hydrogen 
C)  nitrogen 
D)  sulfur 
E)  phosphorus

Question 3

Which of the following explains most specifically the attraction of water molecules to one another?

Accepted Answer

A)  nonpolar covalent bond 
B)  polar covalent bond 
C)  ionic bond 
D)  hydrogen bond 
E)  hydrophobic interaction 
A)  nonpolar covalent bond 
B)  polar covalent bond 
C)  ionic bond 
D)  hydrogen bond 
E)  hydrophobic interaction

Question 4

-Which drawing in the figure above depicts the electron configuration of an atom that can form covalent bonds with two hydrogen atoms?

Accepted Answer

A)  A 
B)  B 
C)  C 
D)  D 
E)  E 
A)  A 
B)  B 
C)  C 
D)  D 
E)  E

Question 5

-How many electrons does an atom of sulfur have in its valence shell (see the figure above)?

Accepted Answer

A)  4 
B)  6 
C)  8 
D)  16 
E)  32 
A)  4 
B)  6 
C)  8 
D)  16 
E)  32

Question 6

Which one of the atoms shown would be most likely to form a cation with a charge of +1?

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 7

-What causes the shape of the molecule shown above?

Accepted Answer

A)  the configuration of the 2 p orbitals in the carbon atom 
B)  the configuration of the 1 s orbital in the carbon atom 
C)  the configuration of the sp hybrid orbitals of the electrons shared between the carbon and hydrogen atoms 
D)  the packing of the carbon and hydrogen atoms in a crystal lattice 
E)  hydrogen bonding configurations between the carbon and hydrogen atoms 
A)  the configuration of the 2 p orbitals in the carbon atom 
B)  the configuration of the 1 s orbital in the carbon atom 
C)  the configuration of the sp hybrid orbitals of the electrons shared between the carbon and hydrogen atoms 
D)  the packing of the carbon and hydrogen atoms in a crystal lattice 
E)  hydrogen bonding configurations between the carbon and hydrogen atoms

Question 8

What is the atomic number of the cation formed in the reaction illustrated above?

Accepted Answer

A)  1 
B)  8 
C)  10 
D)  11 
E)  16 
A)  1 
B)  8 
C)  10 
D)  11 
E)  16

Question 9

The atomic number of each atom is given to the left of each of the elements below. Which of the atoms has the same valence as carbon (   )?

Accepted Answer

A)  ₇N nitrogen 
B)  ₉F flourine 
C)  ₁₀Ne neon 
D)  ₁₂Mg magnesium 
E)  ₁₄Si silicon 
A)  ₇N nitrogen 
B)  ₉F flourine 
C)  ₁₀Ne neon 
D)  ₁₂Mg magnesium 
E)  ₁₄Si silicon

Question 10

-Which drawing in the figure above depicts the most electronegative atom?

Accepted Answer

A)  A 
B)  B 
C)  C 
D)  D 
E)  E 
A)  A 
B)  B 
C)  C 
D)  D 
E)  E

Question 11

-Refer to the figure above (first three rows of the periodic table). If life arose on a planet where carbon is absent, which element might fill the role of carbon?

Accepted Answer

A)  boron 
B)  silicon 
C)  nitrogen 
D)  aluminum 
E)  phosphorus 
A)  boron 
B)  silicon 
C)  nitrogen 
D)  aluminum 
E)  phosphorus

Question 12

Which of the following correctly describes chemical equilibrium?

Accepted Answer

A)  Forward and reverse reactions continue with no effect on the concentrations of the reactants and products. 
B)  Concentrations of products are higher than the concentrations of the reactants. 
C)  Forward and reverse reactions have stopped so that the concentration of the reactants equals the concentration of the products. 
D)  Reactions stop only when all reactants have been converted to products. 
E)  There are equal concentrations of reactants and products, and the reactions have stopped. 
A)  Forward and reverse reactions continue with no effect on the concentrations of the reactants and products. 
B)  Concentrations of products are higher than the concentrations of the reactants. 
C)  Forward and reverse reactions have stopped so that the concentration of the reactants equals the concentration of the products. 
D)  Reactions stop only when all reactants have been converted to products. 
E)  There are equal concentrations of reactants and products, and the reactions have stopped.

Question 13

Atoms whose outer electron shells contain 8 electrons tend to

Accepted Answer

A)  form ions in aqueous solutions. 
B)  form hydrogen bonds in aqueous solutions. 
C)  be stable and chemically nonreactive, or inert. 
D)  be gaseous at room temperature. 
E)  be both chemically inert and gaseous at room temperature. 
A)  form ions in aqueous solutions. 
B)  form hydrogen bonds in aqueous solutions. 
C)  be stable and chemically nonreactive, or inert. 
D)  be gaseous at room temperature. 
E)  be both chemically inert and gaseous at room temperature.

Question 14

Which of the following is true for this reaction?
3 H₂ + N₂ ↔ 2 NH₃

Accepted Answer

A)  The reaction is nonreversible. 
B)  Hydrogen and nitrogen are the reactants of the reverse reaction. 
C)  Hydrogen and nitrogen are the products of the forward reaction. 
D)  Ammonia is being formed and decomposed. 
E)  Hydrogen and nitrogen are being decomposed. 
A)  The reaction is nonreversible. 
B)  Hydrogen and nitrogen are the reactants of the reverse reaction. 
C)  Hydrogen and nitrogen are the products of the forward reaction. 
D)  Ammonia is being formed and decomposed. 
E)  Hydrogen and nitrogen are being decomposed.

Question 15

What factors are most important in determining which elements are most common in living matter?

Accepted Answer

A)  the relative abundances of the elements in Earth's crust and atmosphere 
B)  the emergent properties of the simple compounds made from these elements 
C)  the reactivity of the elements with water 
D)  the chemical stability of the elements 
E)  both the relative abundances of the elements and the emergent properties of the compounds made from these elements 
A)  the relative abundances of the elements in Earth's crust and atmosphere 
B)  the emergent properties of the simple compounds made from these elements 
C)  the reactivity of the elements with water 
D)  the chemical stability of the elements 
E)  both the relative abundances of the elements and the emergent properties of the compounds made from these elements

Question 16

-In the figure above, how many unpaired electrons does phosphorus have in its valence shell?

Accepted Answer

A)  15 
B)  2 
C)  3 
D)  7 
E)  5 
A)  15 
B)  2 
C)  3 
D)  7 
E)  5

Question 17

Which of the following statements correctly describes any chemical reaction that has reached equilibrium?

Accepted Answer

A)  The concentrations of products and reactants are equal. 
B)  The reaction is now irreversible. 
C)  Both forward and reverse reactions have halted. 
D)  The rates of the forward and reverse reactions are equal. 
E)  No reactants remain. 
A)  The concentrations of products and reactants are equal. 
B)  The reaction is now irreversible. 
C)  Both forward and reverse reactions have halted. 
D)  The rates of the forward and reverse reactions are equal. 
E)  No reactants remain.

Question 18

What is the maximum number of covalent bonds an element with atomic number 8 can make with hydrogen?

Accepted Answer

A)  1 
B)  2 
C)  3 
D)  4 
E)  6 
A)  1 
B)  2 
C)  3 
D)  4 
E)  6

Question 19

What is the maximum number of hydrogen atoms that can be covalently bonded in a molecule containing two carbon atoms?

Accepted Answer

A)  2 
B)  3 
C)  4 
D)  6 
E)  8 
A)  2 
B)  3 
C)  4 
D)  6 
E)  8

Question 20

-Which drawing in the figure above depicts an atom with a valence of 3?

Accepted Answer

A)  A 
B)  B 
C)  C 
D)  D 
E)  E 
A)  A 
B)  B 
C)  C 
D)  D 
E)  E

Exam 2: The Chemical Context of Life

Which of the following would be regarded as compounds?

-Based on electron configuration, which of these elements in the figure above would exhibit a chemical behavior most like that of oxygen?

Which of the following explains most specifically the attraction of water molecules to one another?

-Which drawing in the figure above depicts the electron configuration of an atom that can form covalent bonds with two hydrogen atoms?

-How many electrons does an atom of sulfur have in its valence shell (see the figure above)?

Which one of the atoms shown would be most likely to form a cation with a charge of +1?

-What causes the shape of the molecule shown above?

What is the atomic number of the cation formed in the reaction illustrated above?

The atomic number of each atom is given to the left of each of the elements below. Which of the atoms has the same valence as carbon ( )?

-Which drawing in the figure above depicts the most electronegative atom?

-Refer to the figure above (first three rows of the periodic table). If life arose on a planet where carbon is absent, which element might fill the role of carbon?

Which of the following correctly describes chemical equilibrium?

Atoms whose outer electron shells contain 8 electrons tend to

Which of the following is true for this reaction? 3 H₂ + N₂ ↔ 2 NH₃

What factors are most important in determining which elements are most common in living matter?

-In the figure above, how many unpaired electrons does phosphorus have in its valence shell?

Which of the following statements correctly describes any chemical reaction that has reached equilibrium?

What is the maximum number of covalent bonds an element with atomic number 8 can make with hydrogen?

What is the maximum number of hydrogen atoms that can be covalently bonded in a molecule containing two carbon atoms?

-Which drawing in the figure above depicts an atom with a valence of 3?

Introduction: Themes in the Study of Life

Water and Life

Carbon and the Molecular Diversity of Life

The Structure and Function of Large Biological Molecules

A Tour of the Cell

Membrane Structure and Function

An Introduction to Metabolism

Cellular Respiration and Fermentation

Photosynthesis

Cell Communication

The Cell Cycle

Meiosis and Sexual Life Cycles

Mendel and the Gene Idea

The Chromosomal Basis of Inheritance

The Molecular Basis of Inheritance

From Gene to Protein

Regulation of Gene Expression

Viruses

Biotechnology

Genomes and Their Evolution

Descent with Modification: A Darwinian View of Life

The Evolution of Populations

The Origin of Species

The History of Life on Earth

Phylogeny and the Tree of Life

Bacteria and Archaea

Protists

Plant Diversity I: How Plants Colonized Land

Plant Diversity II: The Evolution of Seed Plants

Fungi

An Overview of Animal Diversity

An Introduction to Invertebrates

The Origin and Evolution of Vertebrates

Plant Structure, Growth, and Development

Resource Acquisition and Transport in Vascular Plants

Soil and Plant Nutrition

Angiosperm Reproduction and Biotechnology

Plant Responses to Internal and External Signals

Basic Principles of Animal Form and Function

Animal Nutrition

Circulation and Gas Exchange

The Immune System

Osmoregulation and Excretion

Hormones and the Endocrine System

Animal Reproduction

Animal Development

Neurons, Synapses, and Signaling

Nervous Systems

Sensory and Motor Mechanisms

Animal Behavior

An Introduction to Ecology and the Biosphere

Population Ecology

Community Ecology

Ecosystems and Restoration Ecology

Conservation Biology and Global Change

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