Question 1

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 2

-Which drawing in the figure above depicts the electron configuration of an element with chemical properties most similar to Helium (₂He)?

Accepted Answer

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

Question 3

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 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

Which of these systems is least likely to be at chemical equilibrium?

Accepted Answer

A)  a test tube of living cells 
B)  a test tube of organic molecules, kept in the freezer 
C)  a test tube of dry organic molecules, kept at room temperature 
D)  a test tube of organic molecules dissolved in water, kept at room temperature 
E)  a test tube of dead cells in water, kept at room temperature 
A)  a test tube of living cells 
B)  a test tube of organic molecules, kept in the freezer 
C)  a test tube of dry organic molecules, kept at room temperature 
D)  a test tube of organic molecules dissolved in water, kept at room temperature 
E)  a test tube of dead cells in water, kept at room temperature

Question 6

Phosphorus-32, a radioactive isotope of phosphorus-31 (atomic number 15), undergoes a form of radioactive decay whereby a neutron turns into a proton 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 7

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

Accepted Answer

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

Question 8

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 difference between the s and p orbitals. 
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 difference between the s and p orbitals.

Question 9

-Which drawing in the figure above 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 10

Which statement is true of all atoms that are anions?

Accepted Answer

A)  The atom has more electrons than protons. 
B)  The atom has more protons than electrons. 
C)  The atom has fewer protons than does a neutral atom of the same element. 
D)  The atom has more neutrons than protons. 
E)  The net charge is 1-. 
A)  The atom has more electrons than protons. 
B)  The atom has more protons than electrons. 
C)  The atom has fewer protons than does a neutral atom of the same element. 
D)  The atom has more neutrons than protons. 
E)  The net charge is 1-.

Question 11

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

Question 12

Molybdenum has an atomic number of 42. Several common isotopes exist, with mass numbers of 92, 94, 95, 96, 97, 98, and 100. Therefore, which of the following can be true?

Accepted Answer

A)  Molybdenum atoms can have between 50 and 58 neutrons. 
B)  The isotopes of molybdenum have different electron configurations. 
C)  The isotopes of molybdenum can have between 50 and 58 protons. 
D)  The isotopes of molybdenum have between 50 and 58 neutrons and have different electron configurations. 
E)  The isotopes of molybdenum have between 50 and 58 protons and have different electron configurations. 
A)  Molybdenum atoms can have between 50 and 58 neutrons. 
B)  The isotopes of molybdenum have different electron configurations. 
C)  The isotopes of molybdenum can have between 50 and 58 protons. 
D)  The isotopes of molybdenum have between 50 and 58 neutrons and have different electron configurations. 
E)  The isotopes of molybdenum have between 50 and 58 protons and have different electron configurations.

Question 13

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. They 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 orbital 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 orbital electrons as the hormone 
E)  a compound with the same number of hydrogen and nitrogen atoms as the hormone

Question 14

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

Question 15

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 16

What is the maximum number of electrons in a single 2 p 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 17

Carbon-12 is the most common isotope of carbon, and has an atomic mass of 12 daltons. A mole of carbon in naturally occurring coal, however, weighs slightly more than 12 grams. Why?

Accepted Answer

A)  The atomic mass does not include the mass of electrons. 
B)  Some carbon atoms in nature have an extra proton. 
C)  Some carbon atoms in nature have more neutrons. 
D)  Some carbon atoms in nature have a different valence electron distribution. 
E)  Some carbon atoms in nature have undergone radioactive decay. 
A)  The atomic mass does not include the mass of electrons. 
B)  Some carbon atoms in nature have an extra proton. 
C)  Some carbon atoms in nature have more neutrons. 
D)  Some carbon atoms in nature have a different valence electron distribution. 
E)  Some carbon atoms in nature have undergone radioactive decay.

Question 18

-In the methane molecule shown in the figure above, 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

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

Accepted Answer

A)  
  
B)  
  
C)  
  
D)

E)  
  
A)  
  
B)  
  
C)  
  
D)

E)

Question 20

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.

Exam 2: The Chemical Context of Life

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

-Which drawing in the figure above depicts the electron configuration of an element with chemical properties most similar to Helium (₂He)?

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?

A covalent chemical bond is one in which

Which of these systems is least likely to be at chemical equilibrium?

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

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

The reactivity of an atom arises from

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

Which statement is true of all atoms that are anions?

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

Molybdenum has an atomic number of 42. Several common isotopes exist, with mass numbers of 92, 94, 95, 96, 97, 98, and 100. Therefore, which of the following can be true?

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. They have turned to you for advice. Which of the following compounds is most likely to mimic the effects of the hormone?

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

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

What is the maximum number of electrons in a single 2 p orbital of an atom?

Carbon-12 is the most common isotope of carbon, and has an atomic mass of 12 daltons. A mole of carbon in naturally occurring coal, however, weighs slightly more than 12 grams. Why?

-In the methane molecule shown in the figure above, 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

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

Van der Waals interactions result when

Introduction: Themes in the Study of Life

Water and Life

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 and Fermentation

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

Regulation 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 Overview of Animal Diversity

An Introduction to Invertebrates

The Origin and Evolution of Vertebrates

Plant Structure, Growth, and Development

Resource Acquisition and 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 and Restoration Ecology

Conservation Biology and Global Change

Filters

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