Question 1

For elements in the first three rows of the periodic table, the position of an element in the row indicates which of the following?

Accepted Answer

A)  the total number of electrons in the element 
B)  the total number of protons in the element 
C)  the total number of neutrons in the element 
D)  the number of electron orbitals in the element 
E)  the number of electrons in the valence shell 
A)  the total number of electrons in the element 
B)  the total number of protons in the element 
C)  the total number of neutrons in the element 
D)  the number of electron orbitals in the element 
E)  the number of electrons in the valence shell E

Question 2

From the atomic mass, one can deduce the number of ________ in each atom of an element.

Accepted Answer

A)  protons 
B)  neutrons 
C)  electrons 
D)  protons plus electrons 
E)  protons plus neutrons 
A)  protons 
B)  neutrons 
C)  electrons 
D)  protons plus electrons 
E)  protons plus neutrons E

Question 3

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 E

Question 4

The molar mass of water is 18 g/mol. What is the molarity of 1 liter of pure water? (Hint: One 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 5

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 6

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 7

A small birthday candle is weighed. It is then lighted and placed beneath a metal can containing 100 mL of water. Careful records are kept as the temperature of the water rises. Data from this experiment are shown on the graph. What amount of heat energy is released in the burning of candle wax? (Note that 1 liter of pure water has a mass of 1 kg.)   Figure 2.9

Accepted Answer

A)  0.5 kilocalorie per gram of wax burned 
B)  5 kilocalories per gram of wax burned 
C)  10 kilocalories per gram of wax burned 
D)  20 kilocalories per gram of wax burned 
E)  50 kilocalories per gram of wax burned 
A)  0.5 kilocalorie per gram of wax burned 
B)  5 kilocalories per gram of wax burned 
C)  10 kilocalories per gram of wax burned 
D)  20 kilocalories per gram of wax burned 
E)  50 kilocalories per gram of wax burned

Question 8

A beaker contains 100 mL of NaOH solution at pH = 13. A technician carefully pours into the beaker 10 mL of HCl at pH = 1. Which of the following statements correctly describes the results of this mixing?

Accepted Answer

A)  The concentration of Na+ ion will rise. 
B)  The concentration of Cl- ion will be 0.1 M. 
C)  The concentration of undissociated H₂O molecules will remain unchanged. 
D)  The pH of the beaker's contents will be neutral. 
E)  The pH of the beaker's contents will decrease. 
A)  The concentration of Na+ ion will rise. 
B)  The concentration of Cl- ion will be 0.1 M. 
C)  The concentration of undissociated H₂O molecules will remain unchanged. 
D)  The pH of the beaker's contents will be neutral. 
E)  The pH of the beaker's contents will decrease.

Question 9

Measurements show that the pH of a particular lake is 4.0. What is the hydrogen ion concentration of the lake?

Accepted Answer

A)  4.0 M 
B)  10−4 M 
C)  104 M 
D)  10−10 M 
A)  4.0 M 
B)  10−4 M 
C)  104 M 
D)  10−10 M

Question 10

Figure 2.4
-  Figure 2.5
Figure 2.5 shows a representation of formic acid. A formic acid molecule

Accepted Answer

A)  will dissociate in water, thus increasing the pH. 
B)  will dissociate in water, thus decreasing the pH. 
C)  contains primarily nonpolar covalent bonds. 
D)  is held together by hydrogen bonds. 
E)  has a tetrahedral shape. 
A)  will dissociate in water, thus increasing the pH. 
B)  will dissociate in water, thus decreasing the pH. 
C)  contains primarily nonpolar covalent bonds. 
D)  is held together by hydrogen bonds. 
E)  has a tetrahedral shape.

Question 11

How many molecules of glycerol (C3H8O3; molecular mass = 92) are present in 0.5 L of a 1 M glycerol solution?

Accepted Answer

A)  1 × 1023 
B)  0.5 × 6.02 × 1023 
C)  92/2 × 6.02 × 1023 
D)  0.5 × 6.02/92 × 1023 
E)  6.02 × 1023 
A)  1 × 1023 
B)  0.5 × 6.02 × 1023 
C)  92/2 × 6.02 × 1023 
D)  0.5 × 6.02/92 × 1023 
E)  6.02 × 1023

Question 12

What is the pH of a solution with a hydroxyl ion (OH-) concentration of 10-12 M?

Accepted Answer

A)  pH 2 
B)  pH 4 
C)  pH 10 
D)  pH 12 
E)  pH 14 
A)  pH 2 
B)  pH 4 
C)  pH 10 
D)  pH 12 
E)  pH 14

Question 13

Figure 2.6
-Which 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 14

Figure 2.4
-How many electrons does an atom of sulfur have in its valence shell (see Figure 2.4)?

Accepted Answer

A)  4 
B)  6 
C)  8 
D)  16 
E)  32 
A)  4 
B)  6 
C)  8 
D)  16 
E)  32

Question 15

A group of molecular biologists is trying to synthesize a new artificial compound to mimic the effects of a known hormone that influences sexual behavior. The biologists have turned to you for advice. Which of the following compounds is most likely to mimic the effects of the hormone?

Accepted Answer

A)  a compound with the same number of carbon atoms as the hormone 
B)  a compound with the same molecular mass (measured in daltons) as the hormone 
C)  a compound with the same three-dimensional shape as part of the hormone 
D)  a compound with the same number of valence electrons as the hormone 
E)  a compound with the same number of hydrogen and nitrogen atoms as the hormone 
A)  a compound with the same number of carbon atoms as the hormone 
B)  a compound with the same molecular mass (measured in daltons) as the hormone 
C)  a compound with the same three-dimensional shape as part of the hormone 
D)  a compound with the same number of valence electrons as the hormone 
E)  a compound with the same number of hydrogen and nitrogen atoms as the hormone

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. 
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.

Question 17

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

Question 18

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 grams of glucose. 
E)  180 grams of glucose dissolved in 1 L of solution. 
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 grams of glucose. 
E)  180 grams of glucose dissolved in 1 L of solution.

Question 19

How many molecules of glycerol (C3H8O3; molecular mass = 92) are present in 1 L of a 0.5 M glycerol solution?

Accepted Answer

A)  1 × 1023 
B)  0.5 × 6.02 × 1023 
C)  92/2 × 6.02 × 1023 
D)  0.5 × 6.02/92 × 1023 
E)  6.02 × 1023 
A)  1 × 1023 
B)  0.5 × 6.02 × 1023 
C)  92/2 × 6.02 × 1023 
D)  0.5 × 6.02/92 × 1023 
E)  6.02 × 1023

Question 20

The atomic number of chlorine is 17. The atomic number of calcium is 20. What is the chemical formula for calcium chloride?

Accepted Answer

A)  CaCl 
B)  CaCl2 
C)  Ca2Cl 
D)  Ca2Cl2 
E)  CaCl3 
A)  CaCl 
B)  CaCl2 
C)  Ca2Cl 
D)  Ca2Cl2 
E)  CaCl3

Exam 2: The Chemical Context of Life

For elements in the first three rows of the periodic table, the position of an element in the row indicates which of the following?

From the atomic mass, one can deduce the number of ________ in each atom of an element.

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

The molar mass of water is 18 g/mol. What is the molarity of 1 liter of pure water? (Hint: One liter of pure water has a mass of 1 kg.)

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

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?

A beaker contains 100 mL of NaOH solution at pH = 13. A technician carefully pours into the beaker 10 mL of HCl at pH = 1. Which of the following statements correctly describes the results of this mixing?

Measurements show that the pH of a particular lake is 4.0. What is the hydrogen ion concentration of the lake?

Figure 2.4 - Figure 2.5 Figure 2.5 shows a representation of formic acid. A formic acid molecule

How many molecules of glycerol (C3H8O3; molecular mass = 92) are present in 0.5 L of a 1 M glycerol solution?

What is the pH of a solution with a hydroxyl ion (OH-) concentration of 10-12 M?

Figure 2.6 -Which of the following pairs of atoms would be most likely to form ions and thus an ionic bond?

Figure 2.4 -How many electrons does an atom of sulfur have in its valence shell (see Figure 2.4)?

A group of molecular biologists is trying to synthesize a new artificial compound to mimic the effects of a known hormone that influences sexual behavior. The biologists have turned to you for advice. Which of the following compounds is most likely to mimic the effects of the hormone?

The reactivity of an atom arises from

What results from an unequal sharing of electrons between atoms?

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

How many molecules of glycerol (C3H8O3; molecular mass = 92) are present in 1 L of a 0.5 M glycerol solution?

The atomic number of chlorine is 17. The atomic number of calcium is 20. What is the chemical formula for calcium chloride?

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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