Question 1

Figure 2.5
-Figure 2.5 shows a representation of formic acid. A formic acid molecule

Accepted Answer

A)  will form hydrogen bonds with water molecules. 
B)  has a tetrahedral configuration of hybrid electron orbitals for the carbon atom. 
C)  consists of largely nonpolar covalent bonds. 
D)  is held together by hydrogen bonds. 
E)  has a tetrahedral shape and will form hydrogen bonds with water molecules. 
A)  will form hydrogen bonds with water molecules. 
B)  has a tetrahedral configuration of hybrid electron orbitals for the carbon atom. 
C)  consists of largely nonpolar covalent bonds. 
D)  is held together by hydrogen bonds. 
E)  has a tetrahedral shape and will form hydrogen bonds with water molecules.

Question 2

Van der Waals interactions result when

Accepted Answer

A)  hybrid orbitals overlap. 
B)  electrons are not symmetrically distributed in a molecule. 
C)  molecules held by ionic bonds react with water. 
D)  two polar covalent bonds react. 
E)  a hydrogen atom loses an electron. 
A)  hybrid orbitals overlap. 
B)  electrons are not symmetrically distributed in a molecule. 
C)  molecules held by ionic bonds react with water. 
D)  two polar covalent bonds react. 
E)  a hydrogen atom loses an electron.

Question 3

How many electron pairs are shared between carbon atoms in a molecule that has the formula C2H4?

Accepted Answer

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

Question 4

A covalent chemical bond is one in which

Accepted Answer

A)  electrons are removed from one atom and transferred to another atom so that the two atoms become oppositely charged. 
B)  protons and neutrons are shared by two atoms so as to satisfy the requirements of both atoms. 
C)  outer-shell electrons of two atoms are shared so as to satisfactorily fill the outer electron shells of both atoms. 
D)  outer-shell electrons of one atom are transferred to fill the inner electron shell of another atom. 
E)  an electron occupies a hybrid orbital located between the nuclei of two atoms. 
A)  electrons are removed from one atom and transferred to another atom so that the two atoms become oppositely charged. 
B)  protons and neutrons are shared by two atoms so as to satisfy the requirements of both atoms. 
C)  outer-shell electrons of two atoms are shared so as to satisfactorily fill the outer electron shells of both atoms. 
D)  outer-shell electrons of one atom are transferred to fill the inner electron shell of another atom. 
E)  an electron occupies a hybrid orbital located between the nuclei of two atoms.

Question 5

Sulfur is in the same column of the periodic table as oxygen, but has electronegativity similar to carbon. Compared to water molecules, molecules of H2S will

Accepted Answer

A)  ionize more readily. 
B)  have greater cohesion to other molecules of H2S. 
C)  have a greater tendency to form hydrogen bonds with each other. 
D)  have a higher capacity to absorb heat for the same change in temperature. 
E)  not form hydrogen bonds with each other. 
A)  ionize more readily. 
B)  have greater cohesion to other molecules of H2S. 
C)  have a greater tendency to form hydrogen bonds with each other. 
D)  have a higher capacity to absorb heat for the same change in temperature. 
E)  not form hydrogen bonds with each other.

Question 6

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 7

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. 
E)  Both the forward and the reverse reactions have stopped with no net effect on the concentration of the reactants and the products. 
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. 
E)  Both the forward and the reverse reactions have stopped with no net effect on the concentration of the reactants and the products.

Question 8

The atomic number of nitrogen is 7. Nitrogen-15 is heavier than nitrogen-14 because the atomic nucleus of nitrogen-15 contains how many neutrons?

Accepted Answer

A)  6 
B)  7 
C)  8 
D)  12 
E)  14 
A)  6 
B)  7 
C)  8 
D)  12 
E)  14

Question 9

Many mammals control their body temperature by sweating. Which property of water is most directly responsible for the ability of sweat to lower body temperature?

Accepted Answer

A)  water's change in density when it condenses 
B)  water's ability to dissolve molecules in the air 
C)  the release of heat by the formation of hydrogen bonds 
D)  the absorption of heat by the breaking of hydrogen bonds 
E)  water's high surface tension 
A)  water's change in density when it condenses 
B)  water's ability to dissolve molecules in the air 
C)  the release of heat by the formation of hydrogen bonds 
D)  the absorption of heat by the breaking of hydrogen bonds 
E)  water's high surface tension

Question 10

Figure 2.6
-What results from the chemical reaction illustrated in Figure 2.6?

Accepted Answer

A)  a cation with a net charge of +1 
B)  a cation with a net charge of -1 
C)  an anion with a net charge of +1 
D)  an anion with a net charge of -1 
E)  a cation with a net charge of +1 and an anion with a net charge of -1 
A)  a cation with a net charge of +1 
B)  a cation with a net charge of -1 
C)  an anion with a net charge of +1 
D)  an anion with a net charge of -1 
E)  a cation with a net charge of +1 and an anion with a net charge of -1

Question 11

One mole (mol) of glucose (molecular mass = 180 daltons) is

Accepted Answer

A)  180 × 1023 molecules of glucose. 
B)  1 kg of glucose dissolved in 1 L of solution. 
C)  the largest amount of glucose that can be dissolved in 1 L of solution. 
D)  180 kilograms of glucose. 
E)  both 180 grams of glucose and 6.02 × 1023 molecules of glucose. 
A)  180 × 1023 molecules of glucose. 
B)  1 kg of glucose dissolved in 1 L of solution. 
C)  the largest amount of glucose that can be dissolved in 1 L of solution. 
D)  180 kilograms of glucose. 
E)  both 180 grams of glucose and 6.02 × 1023 molecules of glucose.

Question 12

The nucleus of a nitrogen atom contains 7 neutrons and 7 protons. Which of the following is a correct statement concerning nitrogen?

Accepted Answer

A)  The nitrogen atom has a mass number of approximately 7 and an atomic number of 14. 
B)  The nitrogen atom has a mass number of approximately 14 and an atomic number of 7. 
C)  The nitrogen atom has a mass number of approximately 14 and an atomic number of 14. 
D)  The nitrogen atom has a mass number of approximately 7 and an atomic number of 21. 
E)  The nitrogen atom has a mass number of approximately 14 and an atomic number of 21 
A)  The nitrogen atom has a mass number of approximately 7 and an atomic number of 14. 
B)  The nitrogen atom has a mass number of approximately 14 and an atomic number of 7. 
C)  The nitrogen atom has a mass number of approximately 14 and an atomic number of 14. 
D)  The nitrogen atom has a mass number of approximately 7 and an atomic number of 21. 
E)  The nitrogen atom has a mass number of approximately 14 and an atomic number of 21

Question 13

Figure 2.10
-How many grams would be equal to 1 mol of the compound shown in Figure 2.10? (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 14

The slight negative charge at one end of one water molecule is attracted to the slight positive charge of another water molecule. What is this attraction called?

Accepted Answer

A)  a covalent bond 
B)  a hydrogen bond 
C)  an ionic bond 
D)  a hydrophilic bond 
E)  a van der Waals interaction 
A)  a covalent bond 
B)  a hydrogen bond 
C)  an ionic bond 
D)  a hydrophilic bond 
E)  a van der Waals interaction

Question 15

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 16

The reactivity of an atom arises from

Accepted Answer

A)  the average distance of the outermost electron shell from the nucleus. 
B)  the existence of unpaired electrons in the valence shell. 
C)  the sum of the potential energies of all the electron shells. 
D)  the potential energy of the valence shell. 
E)  the energy differences between the electron shells. 
A)  the average distance of the outermost electron shell from the nucleus. 
B)  the existence of unpaired electrons in the valence shell. 
C)  the sum of the potential energies of all the electron shells. 
D)  the potential energy of the valence shell. 
E)  the energy differences between the electron shells.

Question 17

Liquid water's high specific heat is mainly a consequence of the

Accepted Answer

A)  small size of the water molecules. 
B)  high specific heat of oxygen and hydrogen atoms. 
C)  absorption and release of heat when hydrogen bonds break and form. 
D)  fact that water is a poor heat conductor. 
E)  higher density of liquid water than solid water (ice). 
A)  small size of the water molecules. 
B)  high specific heat of oxygen and hydrogen atoms. 
C)  absorption and release of heat when hydrogen bonds break and form. 
D)  fact that water is a poor heat conductor. 
E)  higher density of liquid water than solid water (ice).

Question 18

Based on electron configuration, which of these 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 19

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

Question 20

Figure 2.10
-How many grams of the compound in Figure 2.10 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

Exam 2: The Chemical Context of Life

Figure 2.5 -Figure 2.5 shows a representation of formic acid. A formic acid molecule

Van der Waals interactions result when

How many electron pairs are shared between carbon atoms in a molecule that has the formula C2H4?

A covalent chemical bond is one in which

Sulfur is in the same column of the periodic table as oxygen, but has electronegativity similar to carbon. Compared to water molecules, molecules of H2S will

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

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

The atomic number of nitrogen is 7. Nitrogen-15 is heavier than nitrogen-14 because the atomic nucleus of nitrogen-15 contains how many neutrons?

Many mammals control their body temperature by sweating. Which property of water is most directly responsible for the ability of sweat to lower body temperature?

Figure 2.6 -What results from the chemical reaction illustrated in Figure 2.6?

One mole (mol) of glucose (molecular mass = 180 daltons) is

The nucleus of a nitrogen atom contains 7 neutrons and 7 protons. Which of the following is a correct statement concerning nitrogen?

Figure 2.10 -How many grams would be equal to 1 mol of the compound shown in Figure 2.10? (carbon = 12, oxygen = 16, hydrogen = 1)

The slight negative charge at one end of one water molecule is attracted to the slight positive charge of another water molecule. What is this attraction called?

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

The reactivity of an atom arises from

Liquid water's high specific heat is mainly a consequence of the

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

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

Figure 2.10 -How many grams of the compound in Figure 2.10 would be required to make 2.5 L of a 1 M solution? (carbon = 12, oxygen = 16, hydrogen = 1)

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