Question 1

A(n) inorganic compound is one that contains carbon. 
__________________

Accepted Answer

A) True 
 B)False  False

Question 2

Which event illustrates evaporative cooling?

Accepted Answer

A)  a tea kettle whistling 
B)  sweat evaporating from the skin 
C)  ice cubes floating in a glass of water 
D)  a fish not freezing in a pond covered with ice 
E)  salt dissolving in a pot of water full of potatoes 
A)  a tea kettle whistling 
B)  sweat evaporating from the skin 
C)  ice cubes floating in a glass of water 
D)  a fish not freezing in a pond covered with ice 
E)  salt dissolving in a pot of water full of potatoes B

Question 3

A solution having a pH of 8 is slightly acidic . 
__________________

Accepted Answer

A) True 
 B)False  False

Question 4

A substance that is resistant to changes in pH is called a(n) buffer . 
__________________

Accepted Answer

A) True 
 B)False

Question 5

When atoms react to form an ionic bond, electrons are shared between those atoms. 
__________________

Accepted Answer

A) True 
 B)False

Question 6

The atomic mass determines the type of element. 
__________________

Accepted Answer

A) True 
 B)False

Question 7

What is the purpose of a buffer?

Accepted Answer

A)  To convert an acid to a base 
B)  To minimize the change in pH 
C)  To measure the acidity of a solution 
D)  To form a stable bond between atoms 
E)  To maintain a constant internal temperature 
A)  To convert an acid to a base 
B)  To minimize the change in pH 
C)  To measure the acidity of a solution 
D)  To form a stable bond between atoms 
E)  To maintain a constant internal temperature

Question 8

The molecular mass of C6H12O6 is 180 amu. How much mass does 0.25 moles of this substance contain?

Accepted Answer

A)  1.8 g 
B)  45 g 
C)  180 g 
D)  45 daltons 
E)  180 daltons 
A)  1.8 g 
B)  45 g 
C)  180 g 
D)  45 daltons 
E)  180 daltons

Question 9

Figure 2-2   The type of bond illustrated in the accompanying diagram is a(n):

Accepted Answer

A)  ionic bond. 
B)  polar bond. 
C)  hydrogen bond. 
D)  single covalent bond. 
E)  double covalent bond. 
A)  ionic bond. 
B)  polar bond. 
C)  hydrogen bond. 
D)  single covalent bond. 
E)  double covalent bond.

Question 10

What is the OH −  concentration of a solution having a pH of 2?

Accepted Answer

A)  1 × 10 − 12 
B)  1 × 10 − 10 
C)  1 × 10 − 7 
D)  1 × 10 − 2 
E)  1 × 10 − 1 
A)  1 × 10 − 12 
B)  1 × 10 − 10 
C)  1 × 10 − 7 
D)  1 × 10 − 2 
E)  1 × 10 − 1

Question 11

Isotopes differ from each other with respect to the number of:

Accepted Answer

A)  protons only. 
B)  electrons only. 
C)  neutrons only. 
D)  both protons and electrons. 
E)  both neutrons and protons. 
A)  protons only. 
B)  electrons only. 
C)  neutrons only. 
D)  both protons and electrons. 
E)  both neutrons and protons.

Question 12

Nitrogen has five electrons in its valence shell. How many electrons does it need to gain to complete its valence shell?

Accepted Answer

A)  one 
B)  two 
C)  three 
D)  seven 
E)  eight 
A)  one 
B)  two 
C)  three 
D)  seven 
E)  eight

Question 13

An example of a(n) anion is K+. 
__________________

Accepted Answer

A) True 
 B)False

Question 14

What type of bond is formed if one atom is more electronegative than the other atom?

Accepted Answer

A)  covalent 
B)  hydrogen 
C)  polar covalent 
D)  van der Waals 
E)  nonpolar covalent 
A)  covalent 
B)  hydrogen 
C)  polar covalent 
D)  van der Waals 
E)  nonpolar covalent

Question 15

A stalk of celery is placed in a solution of blue colored dye. After one hour, the leaves have blue fluid in their veins. Which property of water is being demonstrated?

Accepted Answer

A)  surface tension 
B)  high specific heat 
C)  adhesion and cohesion 
D)  evaporation and cooling 
E)  lower density as a solid than as a liquid 
A)  surface tension 
B)  high specific heat 
C)  adhesion and cohesion 
D)  evaporation and cooling 
E)  lower density as a solid than as a liquid

Question 16

What is the difference between a stable isotope and a radioisotope?

Accepted Answer

A)  A stable isotope emits light. 
B)  A radioisotope emits radiation. 
C)  A stable isotope emits radiation. 
D)  A stable isotope absorbs radiation. 
E)  A radioisotope has an unequal number of protons and electrons. 
A)  A stable isotope emits light. 
B)  A radioisotope emits radiation. 
C)  A stable isotope emits radiation. 
D)  A stable isotope absorbs radiation. 
E)  A radioisotope has an unequal number of protons and electrons.

Question 17

The covalent bond between a hydrogen atom and the oxygen atom in water is formed when:

Accepted Answer

A)  hydrogen gains an electron from oxygen. 
B)  hydrogen and oxygen share an electron pair. 
C)  hydrogen and oxygen both lose electrons from their outer shells. 
D)  hydrogen and oxygen both gain electrons in their outer shells. 
A)  hydrogen gains an electron from oxygen. 
B)  hydrogen and oxygen share an electron pair. 
C)  hydrogen and oxygen both lose electrons from their outer shells. 
D)  hydrogen and oxygen both gain electrons in their outer shells.

Question 18

How can we identify a particular element?

Accepted Answer

A)  By its number of protons 
B)  By its number of electrons 
C)  By its number of neutrons 
D)  By its shape of valence shells 
E)  By its amount of energy levels 
A)  By its number of protons 
B)  By its number of electrons 
C)  By its number of neutrons 
D)  By its shape of valence shells 
E)  By its amount of energy levels

Question 19

Figure 2-1   What is the difference between the two atoms in the accompanying figure?

Accepted Answer

A)  Their electrical charge 
B)  The number of electrons 
C)  The number of protons 
D)  The number of neutrons 
E)  The number of valence shells 
A)  Their electrical charge 
B)  The number of electrons 
C)  The number of protons 
D)  The number of neutrons 
E)  The number of valence shells

Question 20

Explain the role of carbon dioxide in maintaining blood pH levels.

Accepted Answer

Concepts to Consider

Exam 2: Atoms and Molecules the Chemical Basis of Life

A(n) inorganic compound is one that contains carbon. __________________

Which event illustrates evaporative cooling?

A solution having a pH of 8 is slightly acidic . __________________

A substance that is resistant to changes in pH is called a(n) buffer . __________________

When atoms react to form an ionic bond, electrons are shared between those atoms. __________________

The atomic mass determines the type of element. __________________

What is the purpose of a buffer?

The molecular mass of C6H12O6 is 180 amu. How much mass does 0.25 moles of this substance contain?

Figure 2-2 The type of bond illustrated in the accompanying diagram is a(n):

What is the OH − concentration of a solution having a pH of 2?

Isotopes differ from each other with respect to the number of:

Nitrogen has five electrons in its valence shell. How many electrons does it need to gain to complete its valence shell?

An example of a(n) anion is K+. __________________

What type of bond is formed if one atom is more electronegative than the other atom?

A stalk of celery is placed in a solution of blue colored dye. After one hour, the leaves have blue fluid in their veins. Which property of water is being demonstrated?

What is the difference between a stable isotope and a radioisotope?

The covalent bond between a hydrogen atom and the oxygen atom in water is formed when:

How can we identify a particular element?

Figure 2-1 What is the difference between the two atoms in the accompanying figure?

Explain the role of carbon dioxide in maintaining blood pH levels.

A View of Life

The Chemistry of Life Organic Compounds

Organization of the Cell

Biological Membranes

Cell Communication

Energy and Metabolism

How Cells Make Atp Energy-Releasing Pathways

Photosynthesis Capturing Light Energy

Chromosomes, Mitosis, and Meiosis

The Basic Principles of Heredity

Dna the Carrier of Genetic Information

Gene Expression

Gene Regulation

Dna Technology and Genomics

Human Genetics and the Human Genome

Developmental Genetics

Introduction to Darwinian Evolution

Evolutionary Change in Populations

Speciation and Macroevolution

The Origin and Evolutionary History of Life

The Evolution of Primates

Understanding Diversity Systematics

Viruses and Subviral Agents

Bacteria and Archaea

Protists

Seedless Plants

Seed Plants

The Fungi

An Introduction to Animal Diversity

Sponges, Cnidarians, Ctenophores, and Protostomes

The Deuterostomes

Plant Structure Growth and Development

Leaf Structure and Function

Stem Structure and Transport

Roots and Mineral Nutrition

Reproduction in Flowering Plants

Plant Developmental Responses to External and Internal Signals

Animal Structure and Function an Introduction

Protection Support and Movement

Neural Signaling

Neural Regulation

Sensory Systems

Internal Transport

The Immune System Internal Defense

Gas Exchange

Processing Food and Nutrition

Osmoregulation and Disposal of Metabolic Wastes

Endocrine Regulation

Reproduction

Animal Development

Animal Behavior

Introduction to Ecology Population Ecology

Community Ecology

Ecosystems and the Biosphere

Ecology and the Geography of Life

Biological Diversity and Conservation Biology

Filters

The molecular mass of C₆H₁₂O₆ is 180 amu. How much mass does 0.25 moles of this substance contain?

What is the OH⁻ concentration of a solution having a pH of 2?

An example of a(n) anion is K⁺. __________________