Question 1

One liter of a solution of pH 2 has how many more hydrogen ions (H+) than 1 L of a solution of pH 6?

Accepted Answer

A)  4 times more 
B)  16 times more 
C)  40,000 times more 
D)  10,000 times more 
E)  100,000 times more 
A)  4 times more 
B)  16 times more 
C)  40,000 times more 
D)  10,000 times more 
E)  100,000 times more

Question 2

A dietary Calorie equals 1 kilocalorie. Which of the following statements correctly defines 1 kilocalorie?

Accepted Answer

A)  1,000 calories, or the amount of heat required to raise the temperature of 1 g of water by 1,000°C 
B)  100 calories, or the amount of heat required to raise the temperature of 100 g of water by 1°C 
C)  10,000 calories, or the amount of heat required to raise the temperature of 1 kg of water by 1°F 
D)  1,000 calories, or the amount of heat required to raise the temperature of 1 kg of water by 1°C 
E)  1,000 calories, or the amount of heat required to raise the temperature of 100 g of water by 100°C 
A)  1,000 calories, or the amount of heat required to raise the temperature of 1 g of water by 1,000°C 
B)  100 calories, or the amount of heat required to raise the temperature of 100 g of water by 1°C 
C)  10,000 calories, or the amount of heat required to raise the temperature of 1 kg of water by 1°F 
D)  1,000 calories, or the amount of heat required to raise the temperature of 1 kg of water by 1°C 
E)  1,000 calories, or the amount of heat required to raise the temperature of 100 g of water by 100°C

Question 3

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 (2X) 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 (0.01X) what it was at pH 5. 
E)  concentration of H+ is 100 times greater and the concentration of OH- is one-hundredth what they were at pH 5. 
A)  concentration of H+ is twice (2X) 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 (0.01X) what it was at pH 5. 
E)  concentration of H+ is 100 times greater and the concentration of OH- is one-hundredth what they were at pH 5.

Question 4

What is the maximum number of electrons in a single 2 p orbital of an atom?

Accepted Answer

A)  1 
B)  2 
C)  3 
D)  4 
E)  5 
A)  1 
B)  2 
C)  3 
D)  4 
E)  5

Question 5

Which of the following statements is true about buffer solutions?

Accepted Answer

A)  They maintain a constant pH when bases are added to them but not when acids are added to them. 
B)  They maintain a constant pH when acids are added to them but not when bases are added to them. 
C)  They maintain a relatively constant pH of approximately 7 when either acids or bases are added to them. 
D)  They maintain a relatively constant pH when either acids or bases are added to them. 
E)  They are found only in living systems and biological fluids. 
A)  They maintain a constant pH when bases are added to them but not when acids are added to them. 
B)  They maintain a constant pH when acids are added to them but not when bases are added to them. 
C)  They maintain a relatively constant pH of approximately 7 when either acids or bases are added to them. 
D)  They maintain a relatively constant pH when either acids or bases are added to them. 
E)  They are found only in living systems and biological fluids.

Question 6

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 7

Temperature usually increases when water condenses. Which behavior of water is most directly responsible for this phenomenon?

Accepted Answer

A)  the change in density when it condenses to form a liquid or solid 
B)  reactions with other atmospheric compounds 
C)  the release of heat by the formation of hydrogen bonds 
D)  the release of heat by the breaking of hydrogen bonds 
E)  the high surface tension of water 
A)  the change in density when it condenses to form a liquid or solid 
B)  reactions with other atmospheric compounds 
C)  the release of heat by the formation of hydrogen bonds 
D)  the release of heat by the breaking of hydrogen bonds 
E)  the high surface tension of water

Question 8

Figure 2.7
-What causes the shape of the molecule shown in Figure 2.7?

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 9

In what way are elements in the same column of the periodic table the same?

Accepted Answer

A)  They have the same number of protons. 
B)  They have the same number of neutrons. 
C)  They have the same number of electrons. 
D)  They have the same number of electrons in their valence shell. 
E)  They have the same number of electron shells. 
A)  They have the same number of protons. 
B)  They have the same number of neutrons. 
C)  They have the same number of electrons. 
D)  They have the same number of electrons in their valence shell. 
E)  They have the same number of electron shells.

Question 10

The molecular weight of water is 18 daltons. What is the molarity of 1 liter of pure water? (Hint: Note that 1 liter of pure water has a mass of 1 kg.)

Accepted Answer

A)  55.6 M 
B)  18 M 
C)  37 M 
D)  0.66 M 
E)  1.0 M 
A)  55.6 M 
B)  18 M 
C)  37 M 
D)  0.66 M 
E)  1.0 M

Question 11

Which of the following is (are) not considered to be a weak molecular interaction?

Accepted Answer

A)  a covalent bond 
B)  a van der Waals interaction 
C)  an ionic bond in the presence of water 
D)  a hydrogen bond 
E)  both a hydrogen bond and a covalent bond 
A)  a covalent bond 
B)  a van der Waals interaction 
C)  an ionic bond in the presence of water 
D)  a hydrogen bond 
E)  both a hydrogen bond and a covalent bond

Question 12

Which of the following effects is produced by the high surface tension of water?

Accepted Answer

A)  Lakes don't freeze solid in winter, despite low temperatures. 
B)  A water strider can walk across the surface of a small pond. 
C)  Organisms resist temperature changes, although they give off heat due to chemical reactions. 
D)  Evaporation of sweat from the skin helps to keep people from overheating. 
E)  Water flows upward from the roots to the leaves in plants. 
A)  Lakes don't freeze solid in winter, despite low temperatures. 
B)  A water strider can walk across the surface of a small pond. 
C)  Organisms resist temperature changes, although they give off heat due to chemical reactions. 
D)  Evaporation of sweat from the skin helps to keep people from overheating. 
E)  Water flows upward from the roots to the leaves in plants.

Question 13

Figure 2.4
-In Figure 2.4, how many electrons does nitrogen have in its valence shell?

Accepted Answer

A)  2 
B)  5 
C)  7 
D)  8 
E)  14 
A)  2 
B)  5 
C)  7 
D)  8 
E)  14

Question 14

Figure 2.3
-Which drawing in Figure 2.3 depicts an atom with a valence of 2?

Accepted Answer

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

Question 15

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

Accepted Answer

A)  mass in daltons. 
B)  mass in grams. 
C)  volume. 
D)  number of atoms. 
E)  number of molecules. 
A)  mass in daltons. 
B)  mass in grams. 
C)  volume. 
D)  number of atoms. 
E)  number of molecules.

Question 16

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 17

Which bond or interaction would be 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 
E)  either covalent bond or ionic bond 
A)  covalent bond 
B)  hydrogen bond 
C)  van der Waals interaction 
D)  ionic bond 
E)  either covalent bond or ionic bond

Question 18

Figure 2.9
  
-Based on your knowledge of the polarity of water molecules, the solute molecule depicted in Figure 2.9 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.

Question 19

Molybdenum has an atomic number of 42. Several common isotopes exist, with mass numbers of 92, 94, 95, 96, 97, 98, and 100. Therefore, which of the following can be true?

Accepted Answer

A)  Molybdenum atoms can have between 50 and 58 neutrons. 
B)  The isotopes of molybdenum have different electron configurations. 
C)  The isotopes of molybdenum can have between 50 and 58 protons. 
D)  The isotopes of molybdenum have between 50 and 58 neutrons and have different electron configurations. 
E)  The isotopes of molybdenum have between 50 and 58 protons and have different electron configurations. 
A)  Molybdenum atoms can have between 50 and 58 neutrons. 
B)  The isotopes of molybdenum have different electron configurations. 
C)  The isotopes of molybdenum can have between 50 and 58 protons. 
D)  The isotopes of molybdenum have between 50 and 58 neutrons and have different electron configurations. 
E)  The isotopes of molybdenum have between 50 and 58 protons and have different electron configurations.

Question 20

Carbon dioxide (CO2) is readily soluble in water, according to the equation CO2 + H2O ↔ H2CO3. Carbonic acid (H2CO3) is a weak acid. If CO2 is bubbled into a beaker containing pure, freshly distilled water, which of the following graphs correctly describes the results?

Accepted Answer

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

Exam 2: The Chemical Context of Life

One liter of a solution of pH 2 has how many more hydrogen ions (H+) than 1 L of a solution of pH 6?

A dietary Calorie equals 1 kilocalorie. Which of the following statements correctly defines 1 kilocalorie?

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

What is the maximum number of electrons in a single 2 p orbital of an atom?

Which of the following statements is true about buffer solutions?

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

Temperature usually increases when water condenses. Which behavior of water is most directly responsible for this phenomenon?

Figure 2.7 -What causes the shape of the molecule shown in Figure 2.7?

In what way are elements in the same column of the periodic table the same?

The molecular weight of water is 18 daltons. What is the molarity of 1 liter of pure water? (Hint: Note that 1 liter of pure water has a mass of 1 kg.)

Which of the following is (are) not considered to be a weak molecular interaction?

Which of the following effects is produced by the high surface tension of water?

Figure 2.4 -In Figure 2.4, how many electrons does nitrogen have in its valence shell?

Figure 2.3 -Which drawing in Figure 2.3 depicts an atom with a valence of 2?

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

Why does ice float in liquid water?

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

Figure 2.9 -Based on your knowledge of the polarity of water molecules, the solute molecule depicted in Figure 2.9 is most likely

Molybdenum has an atomic number of 42. Several common isotopes exist, with mass numbers of 92, 94, 95, 96, 97, 98, and 100. Therefore, which of the following can be true?

Carbon dioxide (CO2) is readily soluble in water, according to the equation CO2 + H2O ↔ H2CO3. Carbonic acid (H2CO3) is a weak acid. If CO2 is bubbled into a beaker containing pure, freshly distilled water, which of the following graphs correctly describes the results?

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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