Question 1

The atomic number of neon is 10. Therefore, which of the following is correct about an atom of neon?

Accepted Answer

A) It has 8 electrons in its outer electron shell. 
B) It is inert. 
C) It has an atomic mass of 10 daltons. 
D) A and B only 
E) A, B, and C are correct. 
A) It has 8 electrons in its outer electron shell. 
B) It is inert. 
C) It has an atomic mass of 10 daltons. 
D) A and B only 
E) A, B, and C are correct.

Question 2

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 3

Which of the following results from a transfer of electron(s)between atoms?

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 4

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 +3 
B) H, with a charge of +1 
C) H₂ with a charge of +4 
D) NH₄ with a charge of +1 
E) NH₄ with a charge of +4 
A) N, with a charge of +3 
B) H, with a charge of +1 
C) H₂ with a charge of +4 
D) NH₄ with a charge of +1 
E) NH₄ with a charge of +4

Question 5

Use the information extracted from the periodic table in Figure 2.2 to answer the following questions.

-How many electrons would be expected in the outermost electron shell of an atom with atomic number 12?

Accepted Answer

A) 1 
B) 2 
C) 4 
D) 6 
E) 8 
A) 1 
B) 2 
C) 4 
D) 6 
E) 8

Question 6

Electrons exist only at fixed levels of potential energy. However, if an atom absorbs sufficient energy, a possible result is that

Accepted Answer

A) an electron may move to an electron shell farther out from the nucleus. 
B) an electron may move to an electron shell closer to the nucleus. 
C) the atom may become a radioactive isotope. 
D) the atom would become a positively charged ion, or cation. 
E) the atom would become a negatively charged ion, or anion. 
A) an electron may move to an electron shell farther out from the nucleus. 
B) an electron may move to an electron shell closer to the nucleus. 
C) the atom may become a radioactive isotope. 
D) the atom would become a positively charged ion, or cation. 
E) the atom would become a negatively charged ion, or anion.

Question 7

Three or four of the following statements are True and correct. Which one, if any, is False? If all the statements are True, choose answer E.

Accepted Answer

A) Carbon, hydrogen, oxygen, and nitrogen make up approximately 96% of living matter. 
B) The trace element iodine is required only in very small quantities by vertebrates. 
C) Virtually all organisms require the same elements in the same quantities. 
D) Iron is an example of an element needed by all organisms. 
E) All of the other statements are True and correct. 
A) Carbon, hydrogen, oxygen, and nitrogen make up approximately 96% of living matter. 
B) The trace element iodine is required only in very small quantities by vertebrates. 
C) Virtually all organisms require the same elements in the same quantities. 
D) Iron is an example of an element needed by all organisms. 
E) All of the other statements are True and correct.

Question 8

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 9

Which of the following best describes chemical equilibrium?

Accepted Answer

A) Forward and reverse reactions continue with no effect on the concentrations of the reactants and products. 
B) Concentrations of 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) Concentrations of 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 10

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 11

What is the approximate atomic mass of an atom with 16 neutrons, 15 protons, and 15 electrons?

Accepted Answer

A) 15 daltons 
B) 16 daltons 
C) 30 daltons 
D) 31 daltons 
E) 46 daltons 
A) 15 daltons 
B) 16 daltons 
C) 30 daltons 
D) 31 daltons 
E) 46 daltons

Question 12

The following questions refer to Figure 2.3.

-What is the atomic number of the cation formed in the reaction illustrated in Figure 2.3?

Accepted Answer

A) 1 
B) 8 
C) 10 
D) 11 
E) 16 
A) 1 
B) 8 
C) 10 
D) 11 
E) 16

Question 13

Which of the following 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 14

Use the information extracted from the periodic table in Figure 2.2 to answer the following questions.

-What is the maximum number of electrons in the 1s 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 15

Compared with 31P, the radioactive isotope ³²P has

Accepted Answer

A) a different atomic number. 
B) one more neutron. 
C) one more proton. 
D) one more electron. 
E) a different charge. 
A) a different atomic number. 
B) one more neutron. 
C) one more proton. 
D) one more electron. 
E) a different charge.

Question 16

Nitrogen (N)is much more electronegative than hydrogen (H). Which of the following statements is correct about the atoms in ammonia (NH₃)?

Accepted Answer

A) Each hydrogen atom has a partial positive charge. 
B) The nitrogen atom has a strong positive charge. 
C) Each hydrogen atom has a slight negative charge. 
D) The nitrogen atom has a partial positive charge. 
E) There are covalent bonds between the hydrogen atoms. 
A) Each hydrogen atom has a partial positive charge. 
B) The nitrogen atom has a strong positive charge. 
C) Each hydrogen atom has a slight negative charge. 
D) The nitrogen atom has a partial positive charge. 
E) There are covalent bonds between the hydrogen atoms.

Question 17

Use the information extracted from the periodic table in Figure 2.2 to answer the following questions.

-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 18

The atomic number of carbon is 6. Carbon-14 is heavier than carbon-12 because the atomic nucleus of carbon-14 contains _____ neutrons.

Accepted Answer

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

Question 19

Which of the following statements is False?

Accepted Answer

A) Atoms of the various elements differ in their number of subatomic particles. 
B) All atoms of a particular element have the same number of protons in their nuclei. 
C) The neutrons and protons present in the nucleus of an atom are almost identical in mass; each has a mass of about 1 dalton. 
D) An atom is the smallest unit of an element that still retains the properties of the element. 
E) Protons and electrons are electrically charged particles. Protons have one unit of negative charge, and electrons have one unit of positive charge. 
A) Atoms of the various elements differ in their number of subatomic particles. 
B) All atoms of a particular element have the same number of protons in their nuclei. 
C) The neutrons and protons present in the nucleus of an atom are almost identical in mass; each has a mass of about 1 dalton. 
D) An atom is the smallest unit of an element that still retains the properties of the element. 
E) Protons and electrons are electrically charged particles. Protons have one unit of negative charge, and electrons have one unit of positive charge.

Question 20

Which of the following best describes the relationship between the atoms described below?
$\begin{array} { l l } 
\text { Atom 1 } & \text { Atom 2 } \
{ } _ { 15 } ^ { 13 } \mathrm { P } & { } _ { 15 } ^ { 33 } \mathrm { P }
\end{array}$

Accepted Answer

A) They contain 31 and 32 electrons, respectively. 
B) They are both phosphorus cations. 
C) They are both phosphorus anions. 
D) They are both isotopes of phosphorus. 
E) They contain 31 and 32 protons, respectively. 
A) They contain 31 and 32 electrons, respectively. 
B) They are both phosphorus cations. 
C) They are both phosphorus anions. 
D) They are both isotopes of phosphorus. 
E) They contain 31 and 32 protons, respectively.

Exam 2: The Chemical Context of Life

The atomic number of neon is 10. Therefore, which of the following is correct about an atom of neon?

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

Which of the following results from a transfer of electron(s)between atoms?

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

Use the information extracted from the periodic table in Figure 2.2 to answer the following questions. -How many electrons would be expected in the outermost electron shell of an atom with atomic number 12?

Electrons exist only at fixed levels of potential energy. However, if an atom absorbs sufficient energy, a possible result is that

Three or four of the following statements are True and correct. Which one, if any, is False? If all the statements are True, choose answer E.

Van der Waals interactions result when

Which of the following best describes chemical equilibrium?

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

What is the approximate atomic mass of an atom with 16 neutrons, 15 protons, and 15 electrons?

The following questions refer to Figure 2.3. -What is the atomic number of the cation formed in the reaction illustrated in Figure 2.3?

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

Use the information extracted from the periodic table in Figure 2.2 to answer the following questions. -What is the maximum number of electrons in the 1s orbital of an atom?

Compared with 31P, the radioactive isotope ³²P has

Nitrogen (N)is much more electronegative than hydrogen (H). Which of the following statements is correct about the atoms in ammonia (NH₃)?

Use the information extracted from the periodic table in Figure 2.2 to answer the following questions. -How many electrons does nitrogen have in its valence shell?

The atomic number of carbon is 6. Carbon-14 is heavier than carbon-12 because the atomic nucleus of carbon-14 contains _____ neutrons.

Which of the following statements is False?

Which of the following best describes the relationship between the atoms described below? Atom 1 Atom 2

Introduction: Themes in the Study of Life

Water and the Fitness of the Environment

Carbon and the Molecular Diversity of Life

The Structure and Function of Large Biological Molecules

A Tour of the Cell

Membrane Structure and Function

An Introduction to Metabolism

Cellular Respiration: Harvesting Chemical Energy

Photosynthesis

Cell Communication

The Cell Cycle

Meiosis and Sexual Life Cycles

Mendel and the Gene Idea

The Chromosomal Basis of Inheritance

The Molecular Basis of Inheritance

From Gene to Protein

Control of Gene Expression

Viruses

Biotechnology

Genomes and Their Evolution

Descent With Modification: a Darwinian View of Life

The Evolution of Populations

The Origin of Species

The History of Life on Earth

Phylogeny and the Tree of Life

Bacteria and Archaea

Protists

Plant Diversity I: How Plants Colonized Land

Plant Diversity Ii: the Evolution of Seed Plants

Fungi

An Introduction to Animal Diversity

Invertebrates

Vertebrates

Plant Structure, Growth, and Development

Transport in Vascular Plants

Soil and Plant Nutrition

Angiosperm Reproduction and Biotechnology

Plant Responses to Internal and External Signals

Basic Principles of Animal Form and Function

Animal Nutrition

Circulation and Gas Exchange

The Immune System

Osmoregulation and Excretion

Hormones and the Endocrine System

Animal Reproduction

Animal Development

Neurons, Synapses, and Signaling

Nervous Systems

Sensory and Motor Mechanisms

Animal Behavior

An Introduction to Ecology and the Biosphere

Population Ecology

Community Ecology

Ecosystems

Conservation Biology and Restoration Ecology

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