Question 1

You have a freshly prepared 0.1 M solution of glucose in water. Each liter of this solution contains how many glucose molecules?

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 E

Question 2

What results from an unequal sharing of electrons between atoms?

Accepted Answer

A)  a nonpolar covalent bond 
B)  a polar covalent bond 
C)  an ionic bond 
D)  radioactive decay 
E)  a hydrophobic interaction 
A)  a nonpolar covalent bond 
B)  a polar covalent bond 
C)  an ionic bond 
D)  radioactive decay 
E)  a hydrophobic interaction B

Question 3

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. 
E)  Blood pH will first decrease, then increase sharply 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. 
E)  Blood pH will first decrease, then increase sharply as CO2 combines with hemoglobin. A

Question 4

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 5

Consider two solutions: solution X has a pH of 4; solution Y has a pH of 7. From this information, we can reasonably conclude that

Accepted Answer

A)  solution Y has no free hydrogen ions (H+). 
B)  the concentration of hydrogen ions in solution X is 30 times as great as the concentration of hydrogen ions in solution Y. 
C)  the concentration of hydrogen ions in solution Y is 1,000 times as great as the concentration of hydrogen ions in solution X. 
D)  the concentration of hydrogen ions in solution X is 3 times as great as the concentration of hydrogen ions in solution Y. 
E)  the concentration of hydrogen ions in solution X is 1,000 times as great as the concentration of hydrogen ions in solution Y. 
A)  solution Y has no free hydrogen ions (H+). 
B)  the concentration of hydrogen ions in solution X is 30 times as great as the concentration of hydrogen ions in solution Y. 
C)  the concentration of hydrogen ions in solution Y is 1,000 times as great as the concentration of hydrogen ions in solution X. 
D)  the concentration of hydrogen ions in solution X is 3 times as great as the concentration of hydrogen ions in solution Y. 
E)  the concentration of hydrogen ions in solution X is 1,000 times as great as the concentration of hydrogen ions in solution Y.

Question 6

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 7

The partial negative charge in a molecule of water occurs because

Accepted Answer

A)  the oxygen atom acquires an additional electron. 
B)  the electrons shared between the oxygen and hydrogen atoms spend more time around the oxygen atom's nucleus than around the hydrogen atom's nucleus. 
C)  the oxygen atom has two pairs of electrons in its valence shell that are not neutralized by hydrogen atoms. 
D)  the oxygen atom forms hybrid orbitals that distribute electrons unequally around the oxygen nucleus. 
E)  one of the hydrogen atoms donates an electron to the oxygen atom. 
A)  the oxygen atom acquires an additional electron. 
B)  the electrons shared between the oxygen and hydrogen atoms spend more time around the oxygen atom's nucleus than around the hydrogen atom's nucleus. 
C)  the oxygen atom has two pairs of electrons in its valence shell that are not neutralized by hydrogen atoms. 
D)  the oxygen atom forms hybrid orbitals that distribute electrons unequally around the oxygen nucleus. 
E)  one of the hydrogen atoms donates an electron to the oxygen atom.

Question 8

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 9

What is the difference between covalent bonds and ionic bonds?

Accepted Answer

A)  Covalent bonds are formed between atoms to form molecules; ionic bonds are formed between atoms to form compounds. 
B)  Covalent bonds involve the sharing of pairs of electrons between atoms; ionic bonds involve the sharing of single electrons between atoms. 
C)  Covalent bonds involve the sharing of electrons between atoms; ionic bonds involve the electrical attraction between atoms. 
D)  Covalent bonds involve the sharing of electrons between atoms; ionic bonds involve the sharing of protons between atoms. 
E)  Covalent bonds involve the transfer of electrons between atoms; ionic bonds involve the sharing of electrons between atoms. 
A)  Covalent bonds are formed between atoms to form molecules; ionic bonds are formed between atoms to form compounds. 
B)  Covalent bonds involve the sharing of pairs of electrons between atoms; ionic bonds involve the sharing of single electrons between atoms. 
C)  Covalent bonds involve the sharing of electrons between atoms; ionic bonds involve the electrical attraction between atoms. 
D)  Covalent bonds involve the sharing of electrons between atoms; ionic bonds involve the sharing of protons between atoms. 
E)  Covalent bonds involve the transfer of electrons between atoms; ionic bonds involve the sharing of electrons between atoms.

Question 10

Figure 2.4
-How many neutrons are present in the nucleus of a phosphorus-32 (32P) atom (see Figure 2.4)?

Accepted Answer

A)  5 
B)  15 
C)  16 
D)  17 
E)  32 
A)  5 
B)  15 
C)  16 
D)  17 
E)  32

Question 11

Why is each element unique and different from other elements with respect to its chemical properties?

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 different 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 different radioactive properties.

Question 12

Which of the following molecules contains the most polar covalent bond?

Accepted Answer

A)  H2 
B)  O2 
C)  CO2 
D)  H2O 
E)  CH4 
A)  H2 
B)  O2 
C)  CO2 
D)  H2O 
E)  CH4

Question 13

Which of the following statements is false?

Accepted Answer

A)  Carbon, hydrogen, oxygen, and nitrogen are the most abundant elements of living matter. 
B)  Some naturally occurring elements are toxic to organisms. 
C)  All organisms require the same elements in the same quantities. 
D)  Iron is an example of an element needed by all organisms. 
E)  Approximately one-quarter of the natural elements are essential elements. 
A)  Carbon, hydrogen, oxygen, and nitrogen are the most abundant elements of living matter. 
B)  Some naturally occurring elements are toxic to organisms. 
C)  All organisms require the same elements in the same quantities. 
D)  Iron is an example of an element needed by all organisms. 
E)  Approximately one-quarter of the natural elements are essential elements.

Question 14

Which one of the following pairs of atoms would be most likely to form ions and thus an ionic bond?

Accepted Answer

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

Question 15

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 16

Figure 2.1
-Which of the following best describes the relationship between the atoms described in Figure 2.1?

Accepted Answer

A)  They are isomers. 
B)  They are polymers. 
C)  They are isotopes. 
D)  They contain 1 and 3 protons, respectively. 
E)  They each contain 1 neutron. 
A)  They are isomers. 
B)  They are polymers. 
C)  They are isotopes. 
D)  They contain 1 and 3 protons, respectively. 
E)  They each contain 1 neutron.

Question 17

Phosphorus-32, a radioactive isotope of phosphorus-31 (atomic number 15), undergoes a form of radioactive decay whereby a neutron turns into a proton, which is retained in the nucleus, and emits radiation in the form of an electron. What is the product of such radioactive decay of phosphorus-32?

Accepted Answer

A)  phosphorus-31 
B)  a positively charged phosphorus-31 ion 
C)  a negatively charged phosphorus-32 ion 
D)  sulfur-32 (atomic number 16) 
E)  the conversion of the phosphorus-32 atom into pure energy 
A)  phosphorus-31 
B)  a positively charged phosphorus-31 ion 
C)  a negatively charged phosphorus-32 ion 
D)  sulfur-32 (atomic number 16) 
E)  the conversion of the phosphorus-32 atom into pure energy

Question 18

One idea to mitigate the effects of burning fossil fuels on atmospheric CO2 concentrations is to pipe liquid CO2 into the ocean at depths of 2,500 feet or greater. At the high pressures at such depths, CO2 is heavier than water. What potential effects might result from implementing such a scheme?

Accepted Answer

A)  increased photosynthetic carbon fixation because of the increased dissolved carbon dioxide in the deep water 
B)  increased carbonate concentrations in the deep waters 
C)  increased growth of corals from a change in the carbonate-bicarbonate equilibrium 
D)  no effect because carbon dioxide is not soluble in water 
E)  both increased acidity of the deep waters and changes in the growth of bottom-dwelling organisms with calcium carbonate shells 
A)  increased photosynthetic carbon fixation because of the increased dissolved carbon dioxide in the deep water 
B)  increased carbonate concentrations in the deep waters 
C)  increased growth of corals from a change in the carbonate-bicarbonate equilibrium 
D)  no effect because carbon dioxide is not soluble in water 
E)  both increased acidity of the deep waters and changes in the growth of bottom-dwelling organisms with calcium carbonate shells

Question 19

From its atomic number of 15, it is possible to predict that the phosphorus atom has

Accepted Answer

A)  15 neutrons. 
B)  15 protons. 
C)  15 electrons. 
D)  8 electrons in its outermost electron shell. 
E)  15 protons and 15 electrons. 
A)  15 neutrons. 
B)  15 protons. 
C)  15 electrons. 
D)  8 electrons in its outermost electron shell. 
E)  15 protons and 15 electrons.

Question 20

Figure 2.10
-How many grams of the compound in Figure 2.10 would be required to make 1 L of a 0.5 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

You have a freshly prepared 0.1 M solution of glucose in water. Each liter of this solution contains how many glucose molecules?

What results from an unequal sharing of electrons between atoms?

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?

Consider two solutions: solution X has a pH of 4; solution Y has a pH of 7. From this information, we can reasonably conclude that

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?

The partial negative charge in a molecule of water occurs because

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

What is the difference between covalent bonds and ionic bonds?

Figure 2.4 -How many neutrons are present in the nucleus of a phosphorus-32 (32P) atom (see Figure 2.4)?

Why is each element unique and different from other elements with respect to its chemical properties?

Which of the following molecules contains the most polar covalent bond?

Which of the following statements is false?

Which one of the following pairs of atoms would be most likely to form ions and thus an ionic bond?

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?

Figure 2.1 -Which of the following best describes the relationship between the atoms described in Figure 2.1?

Phosphorus-32, a radioactive isotope of phosphorus-31 (atomic number 15), undergoes a form of radioactive decay whereby a neutron turns into a proton, which is retained in the nucleus, and emits radiation in the form of an electron. What is the product of such radioactive decay of phosphorus-32?

One idea to mitigate the effects of burning fossil fuels on atmospheric CO2 concentrations is to pipe liquid CO2 into the ocean at depths of 2,500 feet or greater. At the high pressures at such depths, CO2 is heavier than water. What potential effects might result from implementing such a scheme?

From its atomic number of 15, it is possible to predict that the phosphorus atom has

Figure 2.10 -How many grams of the compound in Figure 2.10 would be required to make 1 L of a 0.5 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