Question 1

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. 
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.

Question 2

We can be sure that a mole of table sugar and a mole of vitamin C are equal in their

Accepted Answer

A)  mass. 
B)  volume. 
C)  number of atoms. 
D)  number of molecules. 
A)  mass. 
B)  volume. 
C)  number of atoms. 
D)  number of molecules.

Question 3

In ammonium chloride salt (NH4Cl), the anion is a single chloride ion, Cl. What is the cation of NH4Cl?

Accepted Answer

A)  N, with a charge of +1 
B)  NH, with a charge of +1 
C)  H3, with a charge of +1 
D)  NH4, with a charge of +1 
E)  NH4, with a charge of +4 
A)  N, with a charge of +1 
B)  NH, with a charge of +1 
C)  H3, with a charge of +1 
D)  NH4, with a charge of +1 
E)  NH4, with a charge of +4

Question 4

Fluorine has an atomic number of 9 and a mass number of 19. How many electrons are needed to complete the valence shell of a fluorine atom?

Accepted Answer

A)  1 
B)  3 
C)  0 
D)  7 
E)  9 
A)  1 
B)  3 
C)  0 
D)  7 
E)  9

Question 5

Figure 2.3
-Which drawing in Figure 2.3 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 6

Figure 2.8
-How many grams of the compound in Figure 2.8 would be required to make 2.5 L of a 1 M solution?
(carbon = 12, oxygen = 16, hydrogen = 1)

Accepted Answer

A)  29 
B)  30 
C)  60 
D)  150 
E)  342 
A)  29 
B)  30 
C)  60 
D)  150 
E)  342

Question 7

If the pH of a solution is increased from pH 5 to pH 7, it means that the

Accepted Answer

A)  concentration of H+ is twice (2×) what it was at pH 5. 
B)  concentration of H+ is one-half (1/2) what it was at pH 5. 
C)  concentration of OH- is 100 times greater than what it was at pH 5. 
D)  concentration of OH- is one-hundredth (0.01×) what it was at pH 5. 
E)  concentration of H+ is 100 times greater than what it was at pH 5. 
A)  concentration of H+ is twice (2×) what it was at pH 5. 
B)  concentration of H+ is one-half (1/2) what it was at pH 5. 
C)  concentration of OH- is 100 times greater than what it was at pH 5. 
D)  concentration of OH- is one-hundredth (0.01×) what it was at pH 5. 
E)  concentration of H+ is 100 times greater than what it was at pH 5.

Question 8

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

Accepted Answer

A)  The concentration of the reactants equals the concentration of the products. 
B)  The rate of the forward reaction is equal to the rate of the reverse reaction. 
C)  All of the reactants have been converted to the products of the reaction. 
D)  All of the products have been converted to the reactants of the reaction. 
A)  The concentration of the reactants equals the concentration of the products. 
B)  The rate of the forward reaction is equal to the rate of the reverse reaction. 
C)  All of the reactants have been converted to the products of the reaction. 
D)  All of the products have been converted to the reactants of the reaction.

Question 9

What is the hydrogen ion (H+) concentration of a solution of pH 8?

Accepted Answer

A)  8 M 
B)  8 × 10-6 M 
C)  0.01 M 
D)  10-8 M 
E)  10-6 M 
A)  8 M 
B)  8 × 10-6 M 
C)  0.01 M 
D)  10-8 M 
E)  10-6 M

Question 10

Figure 2.6
-Which 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 11

Oxygen has an atomic number of 8 and a mass number of 16. What is the atomic mass of an oxygen atom?

Accepted Answer

A)  approximately 8 grams 
B)  approximately 8 daltons 
C)  approximately 16 grams 
D)  approximately 16 daltons 
E)  approximately 24 grams 
A)  approximately 8 grams 
B)  approximately 8 daltons 
C)  approximately 16 grams 
D)  approximately 16 daltons 
E)  approximately 24 grams

Question 12

Which bond or interaction would be most difficult to disrupt when compounds are put into water?

Accepted Answer

A)  covalent bond 
B)  hydrogen bond 
C)  van der Waals interaction 
D)  ionic bond 
A)  covalent bond 
B)  hydrogen bond 
C)  van der Waals interaction 
D)  ionic bond

Question 13

A covalent bond is likely to be polar when

Accepted Answer

A)  one of the atoms sharing electrons is much more electronegative than the other atom. 
B)  the two atoms sharing electrons are equally electronegative. 
C)  oxygen is one of the two atoms sharing electrons. 
D)  the two atoms sharing electrons are the same element. 
E)  the two atoms sharing electrons are different elements. 
A)  one of the atoms sharing electrons is much more electronegative than the other atom. 
B)  the two atoms sharing electrons are equally electronegative. 
C)  oxygen is one of the two atoms sharing electrons. 
D)  the two atoms sharing electrons are the same element. 
E)  the two atoms sharing electrons are different elements.

Question 14

Which of the following is primarily responsible for the unique chemical properties of each element?

Accepted Answer

A)  Each element has a unique atomic mass. 
B)  Each element has a unique atomic number. 
C)  Each element has a unique number of protons. 
D)  Each element has a unique number of neutrons. 
E)  Each element has unique radioactive properties. 
A)  Each element has a unique atomic mass. 
B)  Each element has a unique atomic number. 
C)  Each element has a unique number of protons. 
D)  Each element has a unique number of neutrons. 
E)  Each element has unique radioactive properties.

Question 15

Figure 2.6
-What is the atomic number of the cation formed in the reaction illustrated in Figure 2.6?

Accepted Answer

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

Question 16

What type of bonding or interaction is most likely to occur among a broad array of molecules with various physical properties (polar, nonpolar, hydrophilic, hydrophobic)?

Accepted Answer

A)  covalent bonding 
B)  polar covalent bonding 
C)  ionic bonding 
D)  hydrogen bonding 
E)  van der Waals interactions 
A)  covalent bonding 
B)  polar covalent bonding 
C)  ionic bonding 
D)  hydrogen bonding 
E)  van der Waals interactions

Question 17

Identical heat lamps are arranged to shine on identical containers of water and methanol (wood alcohol) so that each liquid absorbs the same amount of energy minute by minute. The covalent bonds of methanol molecules are nonpolar, so there are no hydrogen bonds among methanol molecules. Which of the following graphs correctly describes what will happen to the temperature of the water and the methanol?

Accepted Answer

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

Question 18

When an ionic compound such as sodium chloride (NaCl) is placed in water, the component atoms of the NaCl crystal dissociate into individual sodium ions (Na+) and chloride ions (Cl-). In contrast, the atoms of covalently bonded molecules (e.g., glucose, sucrose, glycerol) do not generally dissociate when placed in aqueous solution. Which of the following solutions would be expected to contain the greatest number of solute particles (molecules or ions)?

Accepted Answer

A)  1 L of 0.5 M NaCl 
B)  1 L of 0.5 M glucose 
C)  1 L of 1.0 M NaCl 
D)  1 L of 1.0 M glucose 
E)  2 L of 0.5 M glucose. 
A)  1 L of 0.5 M NaCl 
B)  1 L of 0.5 M glucose 
C)  1 L of 1.0 M NaCl 
D)  1 L of 1.0 M glucose 
E)  2 L of 0.5 M glucose.

Question 19

The most stable interaction between magnesium (atomic number 12) and chlorine (atomic number 17) forms

Accepted Answer

A)  MgCl, in which atoms are joined by covalent bonds. 
B)  MgCl, in which atoms are joined by ionic bonds. 
C)  Mg2Cl, in which atoms are joined by ionic bonds. 
D)  MgCl2, in which atoms are joined by covalent bonds. 
E)  MgCl2, in which atoms are joined by ionic bonds. 
A)  MgCl, in which atoms are joined by covalent bonds. 
B)  MgCl, in which atoms are joined by ionic bonds. 
C)  Mg2Cl, in which atoms are joined by ionic bonds. 
D)  MgCl2, in which atoms are joined by covalent bonds. 
E)  MgCl2, in which atoms are joined by ionic bonds.

Question 20

A slice of pizza has 500 kcal. If we could burn the pizza and use all the heat to warm a 50-L container of cold water, what would be the approximate increase in the temperature of the water? (Note: A liter of cold water weighs about 1 kg.)

Accepted Answer

A)  50°C 
B)  5°C 
C)  1°C 
D)  10°C 
A)  50°C 
B)  5°C 
C)  1°C 
D)  10°C

Exam 2: The Chemical Context of Life

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

We can be sure that a mole of table sugar and a mole of vitamin C are equal in their

In ammonium chloride salt (NH4Cl), the anion is a single chloride ion, Cl. What is the cation of NH4Cl?

Fluorine has an atomic number of 9 and a mass number of 19. How many electrons are needed to complete the valence shell of a fluorine atom?

Figure 2.3 -Which drawing in Figure 2.3 depicts the electron configuration of an atom that can form covalent bonds with two hydrogen atoms?

Figure 2.8 -How many grams of the compound in Figure 2.8 would be required to make 2.5 L of a 1 M solution? (carbon = 12, oxygen = 16, hydrogen = 1)

If the pH of a solution is increased from pH 5 to pH 7, it means that the

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

What is the hydrogen ion (H+) concentration of a solution of pH 8?

Figure 2.6 -Which of the atoms shown would be most likely to form a cation with a charge of +1?

Oxygen has an atomic number of 8 and a mass number of 16. What is the atomic mass of an oxygen atom?

Which bond or interaction would be most difficult to disrupt when compounds are put into water?

A covalent bond is likely to be polar when

Which of the following is primarily responsible for the unique chemical properties of each element?

Figure 2.6 -What is the atomic number of the cation formed in the reaction illustrated in Figure 2.6?

What type of bonding or interaction is most likely to occur among a broad array of molecules with various physical properties (polar, nonpolar, hydrophilic, hydrophobic)?

The most stable interaction between magnesium (atomic number 12) and chlorine (atomic number 17) forms

A slice of pizza has 500 kcal. If we could burn the pizza and use all the heat to warm a 50-L container of cold water, what would be the approximate increase in the temperature of the water? (Note: A liter of cold water weighs about 1 kg.)

Introduction: Evolution and the Foundations of Biology

Carbon and the Molecular Diversity of Life

A Tour of the Cell

Membrane Transport and Cell Signaling

An Introduction to Metabolism

Cellular Respiration and Fermentation

Photosynthesis

The Cell Cycle

Meiosis and Sexual Life Cycles

Mendel and the Gene Idea

The Chromosomal Basis of Inheritance

The Molecular Basis of Inheritance

Gene Expression: From Gene to Protein

Regulation of Gene Expression

Development, Stem Cells, and Cancer

Viruses

Genomes and Their Evolution

Descent With Modification

Phylogeny

The Evolution of Populations

The Origin of Species

Broad Patterns of Evolution

Early Life and the Diversification of Prokaryotes

The Origin and Diversification of Eukaryotes

The Colonization of Land by Plants and Fungi

The Rise of Animal Diversity

Plant Structure and Growth

Resource Acquisition, Nutrition, and Transport in Vascular Plants

Reproduction and Domestication of Flowering Plants

Plant Responses to Internal and External Signals

Homeostasis and Endocrine Signaling

Animal Nutrition

Circulation and Gas Exchange

The Immune System

Reproduction and Development

Neurons, Synapses, and Signaling

Nervous and Sensory Systems

Motor Mechanisms and Behavior

Population Ecology and the Distribution of Organisms

Species Interactions

Ecosystems and Energy

Global Ecology and Conservation Biology

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