Question 1

About 25 of the 92 natural elements are known to be essential to life. Which four of these 25 elements make up approximately 96% of living matter?

Accepted Answer

A) carbon, sodium, hydrogen, nitrogen 
B) carbon, oxygen, phosphorus, hydrogen 
C) oxygen, hydrogen, calcium, nitrogen 
D) carbon, hydrogen, nitrogen, oxygen 
E) carbon, oxygen, nitrogen, calcium 
A) carbon, sodium, hydrogen, nitrogen 
B) carbon, oxygen, phosphorus, hydrogen 
C) oxygen, hydrogen, calcium, nitrogen 
D) carbon, hydrogen, nitrogen, oxygen 
E) carbon, oxygen, nitrogen, calcium

Question 2

Which of the following molecules contains the most polar covalent bond?

Accepted Answer

A) H₂ 
B) O₂ 
C) CO₂ 
D) H₂O 
E) CH₄ 
A) H₂ 
B) O₂ 
C) CO₂ 
D) H₂O 
E) CH₄

Question 3

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 4

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 5

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

Accepted Answer

A) They are isomers. 
B) They are polymers. 
C) They are isotopes. 
D) They contain 1 and 3 protons, respectively. 
E) They each contain 1 neutron. 
A) They are isomers. 
B) They are polymers. 
C) They are isotopes. 
D) They contain 1 and 3 protons, respectively. 
E) They each contain 1 neutron.

Question 6

Plants that are capable of thriving in serpentine soil can do so as a result of

Accepted Answer

A) natural selection. 
B) chance. 
C) chemical neutralization of contaminants. 
D) generating their own essential elements. 
E) serpentine soil poses no challenge to plants. 
A) natural selection. 
B) chance. 
C) chemical neutralization of contaminants. 
D) generating their own essential elements. 
E) serpentine soil poses no challenge to plants.

Question 7

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 8

A dalton is a unit of

Accepted Answer

A) distance. 
B) weight. 
C) mass. 
D) bond strength. 
E) energy. 
A) distance. 
B) weight. 
C) mass. 
D) bond strength. 
E) energy.

Question 9

Atoms whose outer electron shells contain 8 electrons tend to

Accepted Answer

A) form ions in aqueous solutions. 
B) form hydrogen bonds in aqueous solutions. 
C) be stable and chemically nonreactive, or inert. 
D) be gaseous at room temperature. 
E) be both chemically inert and gaseous at room temperature. 
A) form ions in aqueous solutions. 
B) form hydrogen bonds in aqueous solutions. 
C) be stable and chemically nonreactive, or inert. 
D) be gaseous at room temperature. 
E) be both chemically inert and gaseous at room temperature.

Question 10

The atomic number of each atom is given to the left of each of the elements below. Which of the atoms has the same valence as carbon (   )?

Accepted Answer

A) ₇N nitrogen 
B) ₉F fluorine 
C) ₁₀Ne neon 
D) ₁₂Mg magnesium 
E) ₁₄Si silicon 
A) ₇N nitrogen 
B) ₉F fluorine 
C) ₁₀Ne neon 
D) ₁₂Mg magnesium 
E) ₁₄Si silicon

Question 11

Use the following information to answer the questions below.
You are investigating how chemical reactions occur. You place two reactants together and measure the concentration of product at regular intervals. After a time, the amount of product becomes stable.
-Compared with ³¹P, the radioactive isotope ³²P has

Accepted Answer

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

Question 12

The combining of the metal, sodium, with the poisonous gas, chlorine, to produce an edible product, salt, is a good example of

Accepted Answer

A) essential elements. 
B) emergent properties. 
C) covalent interactions. 
D) Van der Waals interactions. 
E) chemical equilibrium. 
A) essential elements. 
B) emergent properties. 
C) covalent interactions. 
D) Van der Waals interactions. 
E) chemical equilibrium.

Question 13

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 14

If a salamander relied on hydrogen bonds to cling to surfaces, what type of surface would cause the most problems for this animal?

Accepted Answer

A) a surface coated with a thin film of water 
B) a surface made with carbon and hydrogen atoms covalently bonded together 
C) a surface made with carbon, hydrogen, and oxygen atoms covalently bonded together 
D) a surface made with carbon, hydrogen, nitrogen, and oxygen atoms covalently bonded together 
E) a surface made with silicon and oxygen atoms covalently bonded together 
A) a surface coated with a thin film of water 
B) a surface made with carbon and hydrogen atoms covalently bonded together 
C) a surface made with carbon, hydrogen, and oxygen atoms covalently bonded together 
D) a surface made with carbon, hydrogen, nitrogen, and oxygen atoms covalently bonded together 
E) a surface made with silicon and oxygen atoms covalently bonded together

Question 15

Use the following information to answer the questions below.
You are investigating how chemical reactions occur. You place two reactants together and measure the concentration of product at regular intervals. After a time, the amount of product becomes stable.
-This solution has

Accepted Answer

A) used up all the reactants, so no more product can be made. 
B) used up all the product, so no more reaction is occurring. 
C) reached equilibrium, where there is no more formation of the product. 
D) reached equilibrium, where the net formation of both product and reactants is neutral. 
E) become saturated. 
A) used up all the reactants, so no more product can be made. 
B) used up all the product, so no more reaction is occurring. 
C) reached equilibrium, where there is no more formation of the product. 
D) reached equilibrium, where the net formation of both product and reactants is neutral. 
E) become saturated.

Question 16

Which of the following pairs of atoms would be most likely to form a polar covalent bond?

Accepted Answer

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

Question 17

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) sulphur-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) sulphur-32 (atomic number 16) 
E) the conversion of the phosphorus-32 atom into pure energy

Question 18

Chemical bond/interaction strength appears in what order?

Accepted Answer

A) Hydrogen > covalent > ionic > VanderWaals. 
B) Covalent > ionic > hydrogen > VanderWaals. 
C) Covalent > hydrogen > ionic > VanderWaals. 
D) VanderWaals > hydrogen > ionic > covalent. 
E) Ionic > hydrogen > VanderWaals > covalent. 
A) Hydrogen > covalent > ionic > VanderWaals. 
B) Covalent > ionic > hydrogen > VanderWaals. 
C) Covalent > hydrogen > ionic > VanderWaals. 
D) VanderWaals > hydrogen > ionic > covalent. 
E) Ionic > hydrogen > VanderWaals > covalent.

Question 19

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 20

Use the following information to answer the questions below.
You are investigating how chemical reactions occur. You place two reactants together and measure the concentration of product at regular intervals. After a time, the amount of product becomes stable.
-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.

Exam 2: The Chemical Context of Life

About 25 of the 92 natural elements are known to be essential to life. Which four of these 25 elements make up approximately 96% of living matter?

Which of the following molecules contains the most polar covalent bond?

Van der Waals interactions result when

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

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

Plants that are capable of thriving in serpentine soil can do so as a result of

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

A dalton is a unit of

Atoms whose outer electron shells contain 8 electrons tend to

The atomic number of each atom is given to the left of each of the elements below. Which of the atoms has the same valence as carbon ( )?

The combining of the metal, sodium, with the poisonous gas, chlorine, to produce an edible product, salt, is a good example of

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

If a salamander relied on hydrogen bonds to cling to surfaces, what type of surface would cause the most problems for this animal?

Use the following information to answer the questions below. You are investigating how chemical reactions occur. You place two reactants together and measure the concentration of product at regular intervals. After a time, the amount of product becomes stable. -This solution has

Which of the following pairs of atoms would be most likely to form a polar covalent bond?

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?

Chemical bond/interaction strength appears in what order?

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)?

Use the following information to answer the questions below. You are investigating how chemical reactions occur. You place two reactants together and measure the concentration of product at regular intervals. After a time, the amount of product becomes stable. -The reactivity of an atom arises from

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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