Question 1

Figure 2.4
-Based on electron configuration, which of the elements in Figure 2.4 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 2

Which of the following are the strongest molecular interactions?

Accepted Answer

A)  van der Waals interactions 
B)  van der Waals interactions in a nonpolar environment 
C)  ionic bonds in an aqueous environment 
D)  covalent bonds 
E)  hydrogen bonds 
A)  van der Waals interactions 
B)  van der Waals interactions in a nonpolar environment 
C)  ionic bonds in an aqueous environment 
D)  covalent bonds 
E)  hydrogen bonds

Question 3

Figure 2.3
-Which drawing in Figure 2.3 depicts the electron configuration of an atom capable of forming three covalent bonds with other atoms?

Accepted Answer

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

Question 4

Why does ice float in liquid water?

Accepted Answer

A)  The high surface tension of liquid water keeps the ice on top. 
B)  The ionic bonds between the molecules in ice prevent the ice from sinking. 
C)  Ice always has air bubbles that keep it afloat. 
D)  Hydrogen bonds stabilize and keep the molecules of ice farther apart than the water molecules of liquid water. 
E)  The crystalline lattice of ice causes it to be denser than liquid water. 
A)  The high surface tension of liquid water keeps the ice on top. 
B)  The ionic bonds between the molecules in ice prevent the ice from sinking. 
C)  Ice always has air bubbles that keep it afloat. 
D)  Hydrogen bonds stabilize and keep the molecules of ice farther apart than the water molecules of liquid water. 
E)  The crystalline lattice of ice causes it to be denser than liquid water.

Question 5

How many electron pairs are shared between carbon atoms in a molecule that has the formula C2H6?

Accepted Answer

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

Question 6

Approximately what percentage of human-generated atmospheric CO₂ is absorbed by the oceans?

Accepted Answer

A)  1% 
B)  5% 
C)  25% 
D)  60% 
E)  95% 
A)  1% 
B)  5% 
C)  25% 
D)  60% 
E)  95%

Question 7

You have two beakers. One contains a solution of HCl at pH = 1.0. The other contains a solution of NaOH at pH = 13. Into a third beaker, you slowly and cautiously pour 20 mL of the HCl and 20 mL of the NaOH. After complete stirring, the pH of the mixture will be

Accepted Answer

A)  2.0. 
B)  12.0. 
C)  7.0. 
D)  5.0. 
E)  9.0. 
A)  2.0. 
B)  12.0. 
C)  7.0. 
D)  5.0. 
E)  9.0.

Question 8

If a salamander clings to surfaces through hydrogen bonds, it would have the most difficulty clinging to which of the following surfaces?

Accepted Answer

A)  a surface coated with a thin film of water 
B)  a surface coated with a thin film of vinegar (acetic acid) 
C)  a surface coated with a thin film of vegetable oil 
D)  a surface coated with a thin film of ammonia (NH3) 
A)  a surface coated with a thin film of water 
B)  a surface coated with a thin film of vinegar (acetic acid) 
C)  a surface coated with a thin film of vegetable oil 
D)  a surface coated with a thin film of ammonia (NH3)

Question 9

Hydrophobic substances such as vegetable oil are

Accepted Answer

A)  nonpolar substances that repel water molecules. 
B)  nonpolar substances that have an attraction for water molecules. 
C)  polar substances that repel water molecules. 
D)  polar substances that have an affinity for water. 
E)  charged molecules that hydrogen-bond with water molecules. 
A)  nonpolar substances that repel water molecules. 
B)  nonpolar substances that have an attraction for water molecules. 
C)  polar substances that repel water molecules. 
D)  polar substances that have an affinity for water. 
E)  charged molecules that hydrogen-bond with water molecules.

Question 10

How many glucose molecules are contained in one liter of a 0.1 M solution of glucose in water?

Accepted Answer

A)  6.02 × 1023 
B)  3.01 × 1023 
C)  6.02 × 1024 
D)  12.04 × 1023 
E)  6.02 × 1022 
A)  6.02 × 1023 
B)  3.01 × 1023 
C)  6.02 × 1024 
D)  12.04 × 1023 
E)  6.02 × 1022

Question 11

Carbon dioxide (CO₂) is readily soluble in water, according to the equation CO₂ + H₂O ↔ H2CO3. Carbonic acid (H2CO3) is a weak acid. Respiring cells release CO₂ into the bloodstream. What will be the effect on the pH of blood as that blood first comes in contact with respiring cells?

Accepted Answer

A)  Blood pH will decrease slightly. 
B)  Blood pH will increase slightly. 
C)  Blood pH will remain unchanged. 
D)  Blood pH will first increase, then decrease as CO₂ combines with hemoglobin. 
A)  Blood pH will decrease slightly. 
B)  Blood pH will increase slightly. 
C)  Blood pH will remain unchanged. 
D)  Blood pH will first increase, then decrease as CO₂ combines with hemoglobin.

Question 12

What coefficients must be placed in the following blanks so that all atoms are accounted for in the products?
C₆H₁₂O₆ → ________ C2H6O + ________ CO₂

Accepted Answer

A)  1; 2 
B)  3; 1 
C)  1; 3 
D)  2; 2 
A)  1; 2 
B)  3; 1 
C)  1; 3 
D)  2; 2

Question 13

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 14

If the cytoplasm of a cell is at pH 7, and the mitochondrial matrix is at pH 8, this means that

Accepted Answer

A)  the concentration of hydrogen ions is tenfold higher in the cytoplasm than in the mitochondrial matrix. 
B)  the concentration of hydrogen ions is tenfold higher in the mitochondrial matrix than in the cytoplasm. 
C)  the concentration of hydrogen ions in the cytoplasm is 7/8 the concentration in the mitochondrial matrix. 
D)  the mitochondrial matrix is more acidic than the cytoplasm. 
E)  the concentration of hydrogen ions in the cytoplasm is 8/7 the concentration in the mitochondrial matrix. 
A)  the concentration of hydrogen ions is tenfold higher in the cytoplasm than in the mitochondrial matrix. 
B)  the concentration of hydrogen ions is tenfold higher in the mitochondrial matrix than in the cytoplasm. 
C)  the concentration of hydrogen ions in the cytoplasm is 7/8 the concentration in the mitochondrial matrix. 
D)  the mitochondrial matrix is more acidic than the cytoplasm. 
E)  the concentration of hydrogen ions in the cytoplasm is 8/7 the concentration in the mitochondrial matrix.

Question 15

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)  The concentrations of the products are higher than the concentrations of the reactants. 
C)  Forward and reverse reactions have stopped so that the concentrations of the reactants and products remain constant. 
D)  Reactions stop only when all reactants have been converted to products. 
A)  Forward and reverse reactions continue with no effect on the concentrations of the reactants and products. 
B)  The concentrations of the products are higher than the concentrations of the reactants. 
C)  Forward and reverse reactions have stopped so that the concentrations of the reactants and products remain constant. 
D)  Reactions stop only when all reactants have been converted to products.

Question 16

The molar mass of glucose (C₆H₁₂O₆) is 180 g/mol. Which of the following procedures should you carry out to make a 0.5 M solution of glucose?

Accepted Answer

A)  Dissolve 0.5 g of glucose in a small volume of water, and then add more water until the total volume of the solution is 1 L. 
B)  Dissolve 90 g of glucose in a small volume of water, and then add more water until the total volume of the solution is 1 L. 
C)  Dissolve 180 g of glucose in a small volume of water, and then add more water until the total volume of the solution is 1 L. 
D)  Dissolve 0.5 g of glucose in 1 L of water. 
E)  Dissolve 180 g of glucose in 0.5 L of water. 
A)  Dissolve 0.5 g of glucose in a small volume of water, and then add more water until the total volume of the solution is 1 L. 
B)  Dissolve 90 g of glucose in a small volume of water, and then add more water until the total volume of the solution is 1 L. 
C)  Dissolve 180 g of glucose in a small volume of water, and then add more water until the total volume of the solution is 1 L. 
D)  Dissolve 0.5 g of glucose in 1 L of water. 
E)  Dissolve 180 g of glucose in 0.5 L of water.

Question 17

Which of the following takes place as an ice cube cools a drink?

Accepted Answer

A)  Molecular collisions in the drink increase. 
B)  Kinetic energy in the drink decreases. 
C)  A calorie of heat energy is transferred from the ice to the water of the drink. 
D)  The specific heat of the water in the drink decreases. 
E)  Evaporation of the water in the drink increases. 
A)  Molecular collisions in the drink increase. 
B)  Kinetic energy in the drink decreases. 
C)  A calorie of heat energy is transferred from the ice to the water of the drink. 
D)  The specific heat of the water in the drink decreases. 
E)  Evaporation of the water in the drink increases.

Question 18

Nitrogen (N) is much more electronegative than hydrogen (H). Which of the following statements about the atoms in ammonia (NH3) is correct?

Accepted Answer

A)  Each hydrogen atom has a partial positive charge; the nitrogen atom has a partial negative charge. 
B)  The nitrogen atom has a full positive charge; each hydrogen atom has a full positive charge. 
C)  Each hydrogen atom has a partial negative charge; the nitrogen atom has a full positive charge. 
D)  The nitrogen atom has a partial positive charge; each hydrogen atom has a partial negative charge. 
E)  There are nonpolar covalent bonds between the hydrogen atoms and polar covalent bonds between each hydrogen atom and the nitrogen atom. 
A)  Each hydrogen atom has a partial positive charge; the nitrogen atom has a partial negative charge. 
B)  The nitrogen atom has a full positive charge; each hydrogen atom has a full positive charge. 
C)  Each hydrogen atom has a partial negative charge; the nitrogen atom has a full positive charge. 
D)  The nitrogen atom has a partial positive charge; each hydrogen atom has a partial negative charge. 
E)  There are nonpolar covalent bonds between the hydrogen atoms and polar covalent bonds between each hydrogen atom and the nitrogen atom.

Question 19

Glucose has a molecular mass of 180 g/mol. How many glucose molecules are present in 90 grams of glucose?

Accepted Answer

A)  90 × 1023 
B)  (6.02/180) × 1023 
C)  (6.02/90) × 1023 
D)  (90 × 6.02) × 1023 
E)  (90/180) × 6.02 × 1023 
A)  90 × 1023 
B)  (6.02/180) × 1023 
C)  (6.02/90) × 1023 
D)  (90 × 6.02) × 1023 
E)  (90/180) × 6.02 × 1023

Question 20

Figure 2.6
-  Figure 2.7
Based on your knowledge of the polarity of water molecules, the solute molecule depicted in Figure 2.7 is most likely

Accepted Answer

A)  positively charged. 
B)  negatively charged. 
C)  without charge. 
D)  hydrophobic. 
E)  nonpolar. 
A)  positively charged. 
B)  negatively charged. 
C)  without charge. 
D)  hydrophobic. 
E)  nonpolar.

Exam 2: The Chemical Context of Life

Figure 2.4 -Based on electron configuration, which of the elements in Figure 2.4 would exhibit a chemical behavior most like that of oxygen?

Which of the following are the strongest molecular interactions?

Figure 2.3 -Which drawing in Figure 2.3 depicts the electron configuration of an atom capable of forming three covalent bonds with other atoms?

Why does ice float in liquid water?

How many electron pairs are shared between carbon atoms in a molecule that has the formula C2H6?

Approximately what percentage of human-generated atmospheric CO₂ is absorbed by the oceans?

You have two beakers. One contains a solution of HCl at pH = 1.0. The other contains a solution of NaOH at pH = 13. Into a third beaker, you slowly and cautiously pour 20 mL of the HCl and 20 mL of the NaOH. After complete stirring, the pH of the mixture will be

If a salamander clings to surfaces through hydrogen bonds, it would have the most difficulty clinging to which of the following surfaces?

Hydrophobic substances such as vegetable oil are

How many glucose molecules are contained in one liter of a 0.1 M solution of glucose in water?

Carbon dioxide (CO₂) is readily soluble in water, according to the equation CO₂ + H₂O ↔ H2CO3. Carbonic acid (H2CO3) is a weak acid. Respiring cells release CO₂ into the bloodstream. What will be the effect on the pH of blood as that blood first comes in contact with respiring cells?

What coefficients must be placed in the following blanks so that all atoms are accounted for in the products? C₆H₁₂O₆ → ________ C2H6O + ________ CO₂

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

If the cytoplasm of a cell is at pH 7, and the mitochondrial matrix is at pH 8, this means that

Which of the following correctly describes chemical equilibrium?

The molar mass of glucose (C₆H₁₂O₆) is 180 g/mol. Which of the following procedures should you carry out to make a 0.5 M solution of glucose?

Which of the following takes place as an ice cube cools a drink?

Nitrogen (N) is much more electronegative than hydrogen (H). Which of the following statements about the atoms in ammonia (NH3) is correct?

Glucose has a molecular mass of 180 g/mol. How many glucose molecules are present in 90 grams of glucose?

Figure 2.6 - Figure 2.7 Based on your knowledge of the polarity of water molecules, the solute molecule depicted in Figure 2.7 is most likely

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

Filters

What coefficients must be placed in the following blanks so that all atoms are accounted for in the products? C₆H₁₂O₆ → C2H6O + CO₂