Question 1

-Which one of the atoms shown would be most likely to form an anion with a charge of -1?

Accepted Answer

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

Question 2

Use the following figure to answer the questions below.
  
-How many electrons does an atom of sulphur have in its valence shell (see the figure above)?

Accepted Answer

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

Question 3

Which of the following correctly 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 4

Why is each element unique and different from other elements in chemical properties?

Accepted Answer

A) Each element has a unique atomic mass. 
B) Each element has a unique atomic weight. 
C) Each element has a unique number of protons in its nucleus. 
D) Each element has a unique number of neutrons in its nucleus. 
E) Each element has different radioactive properties. 
A) Each element has a unique atomic mass. 
B) Each element has a unique atomic weight. 
C) Each element has a unique number of protons in its nucleus. 
D) Each element has a unique number of neutrons in its nucleus. 
E) Each element has different radioactive properties.

Question 5

When two atoms are equally electronegative,they will interact to form

Accepted Answer

A) hydrogen bonds. 
B) van der Waals interactions. 
C) polar covalent bonds. 
D) nonpolar covalent bonds. 
E) ionic bonds. 
A) hydrogen bonds. 
B) van der Waals interactions. 
C) polar covalent bonds. 
D) nonpolar covalent bonds. 
E) ionic bonds.

Question 6

The atomic number of sulphur is 16.Sulphur combines with hydrogen by covalent bonding to form a compound,hydrogen sulfide.Based on the number of valence electrons in a sulphur atom,predict the molecular formula of the compound.

Accepted Answer

A) HS 
B) HS₂ 
C) H₂S 
D) H₃S₂ 
E) H₄S 
A) HS 
B) HS₂ 
C) H₂S 
D) H₃S₂ 
E) H₄S

Question 7

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 8

In comparing covalent bonds and ionic bonds,which of the following would you expect?

Accepted Answer

A) An atom can form covalent bonds with multiple partner atoms, but only a single ionic bond with a single partner atom. 
B) Covalent bonds and ionic bonds occupy opposite ends of a continuous spectrum, from nearly equal to completely unequal sharing of electrons. 
C) Both involve electrical attraction between the electrons of one atom and the nucleus of the other atom. 
D) Ionic interactions remain when covalent bonds are broken in water. Ionic bonds are much stronger than covalent bonds. 
A) An atom can form covalent bonds with multiple partner atoms, but only a single ionic bond with a single partner atom. 
B) Covalent bonds and ionic bonds occupy opposite ends of a continuous spectrum, from nearly equal to completely unequal sharing of electrons. 
C) Both involve electrical attraction between the electrons of one atom and the nucleus of the other atom. 
D) Ionic interactions remain when covalent bonds are broken in water. Ionic bonds are much stronger than covalent bonds.

Question 9

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 10

Two atoms appear to have the same mass number.These atoms

Accepted Answer

A) must have the same atomic number. 
B) must have the same number of electrons. 
C) must have the same chemical properties. 
D) must have the same number of protons + neutrons. 
E) must have the same atomic number, the same number of protons + neutrons, the same number of electrons, and the same chemical properties. 
A) must have the same atomic number. 
B) must have the same number of electrons. 
C) must have the same chemical properties. 
D) must have the same number of protons + neutrons. 
E) must have the same atomic number, the same number of protons + neutrons, the same number of electrons, and the same chemical properties.

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

We can represent atoms by listing the number of protons,neutrons,and electrons-for example,
2p⁺; 2n⁰; 2e⁻ for helium.Which of the following represents the ¹⁸O isotope of oxygen?

Accepted Answer

A) 6p⁺, 8n⁰, 6e⁻ 
B) 8p⁺, 10n⁰, 8e⁻ 
C) 9p⁺, 9n⁰, 9e⁻ 
D) 7p⁺, 2n⁰, 9e⁻ 
E) 10p⁺, 8n⁰, 9e⁻ 
A) 6p⁺, 8n⁰, 6e⁻ 
B) 8p⁺, 10n⁰, 8e⁻ 
C) 9p⁺, 9n⁰, 9e⁻ 
D) 7p⁺, 2n⁰, 9e⁻ 
E) 10p⁺, 8n⁰, 9e⁻

Question 13

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 14

An atom has 6 electrons in its outer shell.How many unpaired electrons does it have?

Accepted Answer

A) 0 
B) 2 
C) 4 
D) 6 
E) 2 or 4 
A) 0 
B) 2 
C) 4 
D) 6 
E) 2 or 4

Question 15

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 16

What factors are most important in determining which elements are most common in living matter?

Accepted Answer

A) the relative abundances of the elements in Earth's crust and atmosphere 
B) the emergent properties of the simple compounds made from these elements 
C) the reactivity of the elements with water 
D) the chemical stability of the elements 
E) both the relative abundances of the elements and the emergent properties of the compounds made from these elements 
A) the relative abundances of the elements in Earth's crust and atmosphere 
B) the emergent properties of the simple compounds made from these elements 
C) the reactivity of the elements with water 
D) the chemical stability of the elements 
E) both the relative abundances of the elements and the emergent properties of the compounds made from these elements

Question 17

Which bond or interaction would be difficult to disrupt when compounds are put into water?

Accepted Answer

A) covalent bond 
B) hydrogen bond 
C) van der Waals interaction 
D) ionic bond 
E) either covalent bonds or ionic bonds 
A) covalent bond 
B) hydrogen bond 
C) van der Waals interaction 
D) ionic bond 
E) either covalent bonds or ionic bonds

Question 18

A covalent bond is likely to be polar when

Accepted Answer

A) one of the atoms sharing electrons is much more electronegative than the other atom. 
B) the two atoms sharing electrons are equally electronegative. 
C) oxygen is one of the two atoms sharing electrons. 
D) one of the atoms has absorbed more energy than the other atom. 
E) the two atoms sharing electrons are different elements. 
A) one of the atoms sharing electrons is much more electronegative than the other atom. 
B) the two atoms sharing electrons are equally electronegative. 
C) oxygen is one of the two atoms sharing electrons. 
D) one of the atoms has absorbed more energy than the other atom. 
E) the two atoms sharing electrons are different elements.

Question 19

Use the following figure to answer the questions below.
  
-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 20

Use the following figure to answer the questions below.
  
-In the figure above,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

Exam 2: The Chemical Context of Life

-Which one of the atoms shown would be most likely to form an anion with a charge of -1?

Use the following figure to answer the questions below. -How many electrons does an atom of sulphur have in its valence shell (see the figure above)?

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

Why is each element unique and different from other elements in chemical properties?

When two atoms are equally electronegative,they will interact to form

The atomic number of sulphur is 16.Sulphur combines with hydrogen by covalent bonding to form a compound,hydrogen sulfide.Based on the number of valence electrons in a sulphur atom,predict the molecular formula of the compound.

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

In comparing covalent bonds and ionic bonds,which of the following would you expect?

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

Two atoms appear to have the same mass number.These atoms

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

We can represent atoms by listing the number of protons,neutrons,and electrons-for example, 2p⁺; 2n⁰; 2e⁻ for helium.Which of the following represents the ¹⁸O isotope of oxygen?

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

An atom has 6 electrons in its outer shell.How many unpaired electrons does it have?

Which statement is true of all atoms that are anions?

What factors are most important in determining which elements are most common in living matter?

Which bond or interaction would be difficult to disrupt when compounds are put into water?

A covalent bond is likely to be polar when

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

Use the following figure to answer the questions below. -In the figure above,how many electrons does nitrogen have in its valence shell?

Introduction: Evolution and Themes of Biology

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

DNA Tools and 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 Signalling

Nervous Systems

Sensory and Motor Mechanisms

Animal Behaviour

An Introduction to Ecology and the Biosphere

Population Ecology

Community Ecology

Ecosystems and Restoration Ecology

Conservation Biology and Global Change

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