Question 1

Two atoms appear to have the same mass number. These atoms

Accepted Answer

A)  must have the same atomic number. 
B)  must have the same number of electrons. 
C)  must have the same chemical properties. 
D)  must have the same number of protons + neutrons. 
E)  must have the same atomic number, the same number of protons + neutrons, the same number of electrons, and the same chemical properties. 
A)  must have the same atomic number. 
B)  must have the same number of electrons. 
C)  must have the same chemical properties. 
D)  must have the same number of protons + neutrons. 
E)  must have the same atomic number, the same number of protons + neutrons, the same number of electrons, and the same chemical properties.

Question 2

If the pH of a solution is decreased from 9 to 8, it means that the

Accepted Answer

A)  concentration of H+ has decreased to one-tenth (1/10) what it was at pH 9. 
B)  concentration of H+ has increased tenfold (10X) compared to what it was at pH 9. 
C)  concentration of OH- has increased tenfold (10X) compared to what it was at pH 9. 
D)  concentration of OH- has decreased to one-tenth (1/10) what it was at pH 9. 
E)  concentration of H+ has increased tenfold (10X) and the concentration of OH- has decreased to one-tenth (1/10) what they were at pH 9. 
A)  concentration of H+ has decreased to one-tenth (1/10) what it was at pH 9. 
B)  concentration of H+ has increased tenfold (10X) compared to what it was at pH 9. 
C)  concentration of OH- has increased tenfold (10X) compared to what it was at pH 9. 
D)  concentration of OH- has decreased to one-tenth (1/10) what it was at pH 9. 
E)  concentration of H+ has increased tenfold (10X) and the concentration of OH- has decreased to one-tenth (1/10) what they were at pH 9.

Question 3

The molar mass of glucose is 180 g/mol. Which of the following procedures should you carry out to make a 1 M solution of glucose?

Accepted Answer

A)  Dissolve 1 g of glucose in 1 L of water. 
B)  Dissolve 180 g of glucose in 1 L of water. 
C)  Dissolve 180 g of glucose in 180 g of water. 
D)  Dissolve 180 milligrams (mg) of glucose in 1 L of water. 
E)  Dissolve 180 g of glucose in 0.8 L of water, and then add more water until the total volume of the solution is 1 L. 
A)  Dissolve 1 g of glucose in 1 L of water. 
B)  Dissolve 180 g of glucose in 1 L of water. 
C)  Dissolve 180 g of glucose in 180 g of water. 
D)  Dissolve 180 milligrams (mg) of glucose in 1 L of water. 
E)  Dissolve 180 g of glucose in 0.8 L of water, and then add more water until the total volume of the solution is 1 L.

Question 4

Figure 2.3
-Which drawing in Figure 2.3 is of the electron configuration of a sodium 11Na+ ion?

Accepted Answer

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

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 2.4
-In Figure 2.4, 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 7

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)  one of the atoms has absorbed more energy than the other atom. 
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)  one of the atoms has absorbed more energy than the other atom. 
E)  the two atoms sharing electrons are different elements.

Question 8

Which of the following solutions would require the greatest amount of base to be added to bring the solution to neutral pH?

Accepted Answer

A)  gastric juice at pH 2 
B)  vinegar at pH 3 
C)  tomato juice at pH 4 
D)  black coffee at pH 5 
E)  household bleach at pH 12 
A)  gastric juice at pH 2 
B)  vinegar at pH 3 
C)  tomato juice at pH 4 
D)  black coffee at pH 5 
E)  household bleach at pH 12

Question 9

A solution contains 0.0000001(10-7) moles of hydroxyl ions (OH-) per liter. Which of the following best describes this solution?

Accepted Answer

A)  acidic: H+ acceptor 
B)  basic: H+ acceptor 
C)  acidic: H+ donor 
D)  basic: H+ donor 
E)  neutral 
A)  acidic: H+ acceptor 
B)  basic: H+ acceptor 
C)  acidic: H+ donor 
D)  basic: H+ donor 
E)  neutral

Question 10

How many molecules of glucose (C6H12O6 molecular mass = 180 daltons) would be 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 11

If an atom of sulfur (atomic number 16) were allowed to react with atoms of hydrogen (atomic number 1), which of the following molecules would be formed?

Accepted Answer

A)  S-H 
B)  H-S-H 
C) 
  
D) 
  
E)  H = S = H 
A)  S-H 
B)  H-S-H 
C) 
  
D) 
  
E)  H = S = H

Question 12

In comparing covalent bonds and ionic bonds, which of the following would you expect?

Accepted Answer

A)  An atom can form covalent bonds with multiple partner atoms, but only a single ionic bond with a single partner atom. 
B)  Covalent bonds and ionic bonds occupy opposite ends of a continuous spectrum, from nearly equal to completely unequal sharing of electrons. 
C)  Both involve electrical attraction between the electrons of one atom and the nucleus of the other atom. 
D)  Ionic interactions remain when covalent bonds are broken in water. Ionic bonds are much stronger than covalent bonds. 
A)  An atom can form covalent bonds with multiple partner atoms, but only a single ionic bond with a single partner atom. 
B)  Covalent bonds and ionic bonds occupy opposite ends of a continuous spectrum, from nearly equal to completely unequal sharing of electrons. 
C)  Both involve electrical attraction between the electrons of one atom and the nucleus of the other atom. 
D)  Ionic interactions remain when covalent bonds are broken in water. Ionic bonds are much stronger than covalent bonds.

Question 13

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 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

Which one of the atoms shown would be most likely to form an anion with a charge of -1?

Accepted Answer

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

Question 16

The atomic number of sulfur is 16. Sulfur combines with hydrogen by covalent bonding to form a compound, hydrogen sulfide. Based on the number of valence electrons in a sulfur atom, predict the molecular formula of the compound.

Accepted Answer

A)  HS 
B)  HS2 
C)  H2S 
D)  H3S2 
E)  H4S 
A)  HS 
B)  HS2 
C)  H2S 
D)  H3S2 
E)  H4S

Question 17

About 25 of the 92 natural elements are known to be essential to life. Which 4 of these 25 elements make up approximately 96% of living matter?

Accepted Answer

A)  carbon, sodium, hydrogen, nitrogen 
B)  carbon, oxygen, phosphorus, hydrogen 
C)  oxygen, hydrogen, calcium, nitrogen 
D)  carbon, hydrogen, nitrogen, oxygen 
E)  carbon, oxygen, nitrogen, calcium 
A)  carbon, sodium, hydrogen, nitrogen 
B)  carbon, oxygen, phosphorus, hydrogen 
C)  oxygen, hydrogen, calcium, nitrogen 
D)  carbon, hydrogen, nitrogen, oxygen 
E)  carbon, oxygen, nitrogen, calcium

Question 18

Figure 2.8
-In the methane molecule shown in Figure 2.8, bonds have formed that include both the s orbital valence electrons of the hydrogen atoms and the p orbital valence electrons of the carbon. The electron orbitals in these bonds are said to be

Accepted Answer

A)  double orbitals. 
B)  tetrahedral orbitals. 
C)  complex orbitals. 
D)  hybrid orbitals. 
E)  polar orbitals. 
A)  double orbitals. 
B)  tetrahedral orbitals. 
C)  complex orbitals. 
D)  hybrid orbitals. 
E)  polar orbitals.

Question 19

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 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)  The concentrations of the 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 20

One of the buffers that contributes to pH stability in human blood is carbonic acid (H2CO3). Carbonic acid is a weak acid that dissociates into a bicarbonate ion (HCO3-) and a hydrogen ion (H+). Thus, H2CO3 ↔ HCO3- + H+
If the pH of the blood drops, one would expect

Accepted Answer

A)  a decrease in the concentration of H2CO3 and an increase in the concentration of HCO3-. 
B)  the concentration of hydroxide ion (OH-) to increase. 
C)  the concentration of bicarbonate ion (HCO3-) to increase. 
D)  the HCO3- to act as a base and remove excess H+ with the formation of H2CO3. 
E)  the HCO3- to act as an acid and remove excess H+ with the formation of H2CO3. 
A)  a decrease in the concentration of H2CO3 and an increase in the concentration of HCO3-. 
B)  the concentration of hydroxide ion (OH-) to increase. 
C)  the concentration of bicarbonate ion (HCO3-) to increase. 
D)  the HCO3- to act as a base and remove excess H+ with the formation of H2CO3. 
E)  the HCO3- to act as an acid and remove excess H+ with the formation of H2CO3.

Exam 2: The Chemical Context of Life

Two atoms appear to have the same mass number. These atoms

If the pH of a solution is decreased from 9 to 8, it means that the

The molar mass of glucose is 180 g/mol. Which of the following procedures should you carry out to make a 1 M solution of glucose?

Figure 2.3 -Which drawing in Figure 2.3 is of the electron configuration of a sodium 11Na+ ion?

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

A covalent bond is likely to be polar when

Which of the following solutions would require the greatest amount of base to be added to bring the solution to neutral pH?

A solution contains 0.0000001(10-7) moles of hydroxyl ions (OH-) per liter. Which of the following best describes this solution?

How many molecules of glucose (C6H12O6 molecular mass = 180 daltons) would be present in 90 grams of glucose?

If an atom of sulfur (atomic number 16) were allowed to react with atoms of hydrogen (atomic number 1), which of the following molecules would be formed?

In comparing covalent bonds and ionic bonds, which of the following would you expect?

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

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

Which one of the atoms shown would be most likely to form an anion with a charge of -1?

The atomic number of sulfur is 16. Sulfur combines with hydrogen by covalent bonding to form a compound, hydrogen sulfide. Based on the number of valence electrons in a sulfur atom, predict the molecular formula of the compound.

About 25 of the 92 natural elements are known to be essential to life. Which 4 of these 25 elements make up approximately 96% of living matter?

Figure 2.8 -In the methane molecule shown in Figure 2.8, bonds have formed that include both the s orbital valence electrons of the hydrogen atoms and the p orbital valence electrons of the carbon. The electron orbitals in these bonds are said to be

Which of the following correctly describes chemical equilibrium?

One of the buffers that contributes to pH stability in human blood is carbonic acid (H2CO3). Carbonic acid is a weak acid that dissociates into a bicarbonate ion (HCO3-) and a hydrogen ion (H+). Thus, H2CO3 ↔ HCO3- + H+ If the pH of the blood drops, one would expect

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

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Ecosystems and Energy

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