Question 1

The partial negative charge in a molecule of water occurs because

Accepted Answer

A) the oxygen atom acquires an additional electron. 
B) the electrons shared between the oxygen and hydrogen atoms spend more time around the oxygen atom nucleus than around the hydrogen atom nucleus. 
C) the oxygen atom has two pairs of electrons in its valence shell that are not neutralized by hydrogen atoms. 
D) the oxygen atom forms hybrid orbitals that distribute electrons unequally around the oxygen nucleus. 
E) one of the hydrogen atoms donates an electron to the oxygen atom. 
A) the oxygen atom acquires an additional electron. 
B) the electrons shared between the oxygen and hydrogen atoms spend more time around the oxygen atom nucleus than around the hydrogen atom nucleus. 
C) the oxygen atom has two pairs of electrons in its valence shell that are not neutralized by hydrogen atoms. 
D) the oxygen atom forms hybrid orbitals that distribute electrons unequally around the oxygen nucleus. 
E) one of the hydrogen atoms donates an electron to the oxygen atom.

Question 2

The slight negative charge at one end of one water molecule is attracted to the slight positive charge of another water molecule.What is this attraction called?

Accepted Answer

A) a covalent bond 
B) a hydrogen bond 
C) an ionic bond 
D) a hydrophilic bond 
E) a van der Waals interaction 
A) a covalent bond 
B) a hydrogen bond 
C) an ionic bond 
D) a hydrophilic bond 
E) a van der Waals interaction

Question 3

What is the pH of a 1 millimolar NaOH solution?

Accepted Answer

A) pH 3 
B) pH 8 
C) pH 9 
D) pH 10 
E) pH 11 
A) pH 3 
B) pH 8 
C) pH 9 
D) pH 10 
E) pH 11

Question 4

One idea to mitigate the effects of burning fossil fuels on atmospheric CO₂ concentrations is to pipe liquid CO₂ into the ocean at depths of 2500 feet or greater.At the high pressures at such depths,CO₂ is heavier than water.What potential effects might result from implementing such a scheme?

Accepted Answer

A) increased photosynthetic carbon fixation because of the increased dissolved carbon dioxide in the deep water 
B) increased carbonate concentrations in the deep waters 
C) reduced growth of corals from a change in the carbonate-bicarbonate equilibrium 
D) no effect because carbon dioxide is not soluble in water 
E) both increased acidity of the deep waters and changes in the growth of bottom-dwelling organisms with calcium carbonate shells 
A) increased photosynthetic carbon fixation because of the increased dissolved carbon dioxide in the deep water 
B) increased carbonate concentrations in the deep waters 
C) reduced growth of corals from a change in the carbonate-bicarbonate equilibrium 
D) no effect because carbon dioxide is not soluble in water 
E) both increased acidity of the deep waters and changes in the growth of bottom-dwelling organisms with calcium carbonate shells

Question 5

The cities of Vancouver,Canada,and Regina,Saskatchewan,are at about the same latitude,but Regina has much hotter summers and much colder winters than Vancouver.Why?

Accepted Answer

A) They are not at the same exact latitude. 
B) The ocean near Vancouver moderates the temperature. 
C) Fresh water is more likely to freeze than salt water. 
D) Regina is much windier, due to its location in Canada. 
E) Vancouver experiences more chinook winds. 
A) They are not at the same exact latitude. 
B) The ocean near Vancouver moderates the temperature. 
C) Fresh water is more likely to freeze than salt water. 
D) Regina is much windier, due to its location in Canada. 
E) Vancouver experiences more chinook winds.

Question 6

A solution contains 0.0000001 (10⁻⁷)moles of hydroxyl ions [OH⁻] per litre.Which of the following best describes this solution?

Accepted Answer

A) acidic: H⁺ acceptor 
B) basic: H⁺ acceptor 
C) acidic: H⁺ donor 
D) basic: H⁺ donor 
E) neutral 
A) acidic: H⁺ acceptor 
B) basic: H⁺ acceptor 
C) acidic: H⁺ donor 
D) basic: H⁺ donor 
E) neutral

Question 7

Use the following information to answer the questions below.
You live in Atlantic Canada and you are Skyping a friend in Manitoba.You are both complaining about the weather as both regions are being subjected to the same arctic air mass.As you discuss it,however,it becomes clear that she is experiencing a bitter cold that you are not.You realize that you had pretty much the same conversation last summer when it was much hotter in Manitoba than at home.
-The best explanation for this difference is that

Accepted Answer

A) your climate is moderated by the Atlantic Ocean. 
B) it is just much colder in the middle of the country. 
C) it rains more in central Canada. 
D) your friend just doesn't adjust well to changes in temperature. 
E) she must be at a higher latitude. 
A) your climate is moderated by the Atlantic Ocean. 
B) it is just much colder in the middle of the country. 
C) it rains more in central Canada. 
D) your friend just doesn't adjust well to changes in temperature. 
E) she must be at a higher latitude.

Question 8

When an ionic compound such as sodium chloride (NaCl)is placed in water,the component atoms of the NaCl crystal dissociate into individual sodium ions (Na⁺)and chloride ions (Cl⁻).In contrast,the atoms of covalently bonded molecules (e.g.,glucose,sucrose,glycerol)do not generally dissociate when placed in aqueous solution.Which of the following solutions would be expected to contain the greatest number of solute particles (molecules or ions)?

Accepted Answer

A) 1 L of 0.5 M NaCl 
B) 1 L of 0.5 M glucose 
C) 1 L of 1.0 M NaCl 
D) 1 L of 1.0 M glucose 
E) 1 L of 1.0 M NaCl and 1 L of 1.0 M glucose will contain equal numbers of solute particles. 
A) 1 L of 0.5 M NaCl 
B) 1 L of 0.5 M glucose 
C) 1 L of 1.0 M NaCl 
D) 1 L of 1.0 M glucose 
E) 1 L of 1.0 M NaCl and 1 L of 1.0 M glucose will contain equal numbers of solute particles.

Question 9

Water molecules are able to form hydrogen bonds with

Accepted Answer

A) compounds that have polar covalent bonds. 
B) oils. 
C) oxygen gas (O₂)molecules. 
D) chloride ions. 
E) any compound that is not soluble in water. 
A) compounds that have polar covalent bonds. 
B) oils. 
C) oxygen gas (O₂)molecules. 
D) chloride ions. 
E) any compound that is not soluble in water.

Question 10

Rank,from low to high,the pH of blood,stomach acid,and urine.

Accepted Answer

A) blood, urine, and stomach acid 
B) stomach acid, blood, and urine 
C) urine, blood, stomach acid 
D) stomach acid, urine, blood 
E) stomach acid, urine and blood have a similar neutral pH 
A) blood, urine, and stomach acid 
B) stomach acid, blood, and urine 
C) urine, blood, stomach acid 
D) stomach acid, urine, blood 
E) stomach acid, urine and blood have a similar neutral pH

Question 11

Carbon dioxide (CO₂)is readily soluble in water,according to the equation CO₂ + H₂O ↔ H₂CO₃.Carbonic acid (H₂CO₃)is a weak acid.If CO₂ is bubbled into a beaker containing pure,freshly distilled water,which of the following graphs correctly describes the results?

Accepted Answer

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

Question 12

Why does ice float in liquid water?

Accepted Answer

A) The high surface tension of liquid water keeps the ice on top. 
B) The ionic bonds between the molecules in ice prevent the ice from sinking. 
C) Ice always has air bubbles that keep it afloat. 
D) Hydrogen bonds stabilize and keep the molecules of ice farther apart than the water molecules of liquid water. 
E) The crystalline lattice of ice causes it to be denser than liquid water. 
A) The high surface tension of liquid water keeps the ice on top. 
B) The ionic bonds between the molecules in ice prevent the ice from sinking. 
C) Ice always has air bubbles that keep it afloat. 
D) Hydrogen bonds stabilize and keep the molecules of ice farther apart than the water molecules of liquid water. 
E) The crystalline lattice of ice causes it to be denser than liquid water.

Question 13

If the pH of a solution is decreased from 9 to 8,it means that the

Accepted Answer

A) concentration of H⁺ has decreased to one-tenth (1/10)what it was at pH 9. 
B) concentration of H⁺ has increased tenfold (10X)compared to what it was at pH 9. 
C) concentration of OH⁻ has increased tenfold (10X)compared to what it was at pH 9. 
D) concentration of OH⁻ has decreased to one-tenth (1/10)what it was at pH 9. 
E) concentration of H⁺ has increased tenfold (10X)and the concentration of OH⁻ has decreased to one-tenth (1/10)what they were at pH 9. 
A) concentration of H⁺ has decreased to one-tenth (1/10)what it was at pH 9. 
B) concentration of H⁺ has increased tenfold (10X)compared to what it was at pH 9. 
C) concentration of OH⁻ has increased tenfold (10X)compared to what it was at pH 9. 
D) concentration of OH⁻ has decreased to one-tenth (1/10)what it was at pH 9. 
E) concentration of H⁺ has increased tenfold (10X)and the concentration of OH⁻ has decreased to one-tenth (1/10)what they were at pH 9.

Question 14

Plants transport water through their vascular system utilizing what property of water?

Accepted Answer

A) Hydrogen bonds allowing for surface tension. 
B) Hydrogen bonds allowing for increased structure of water. 
C) Hydrogen bonds allowing for adhesion and cohesion of molecules. 
D) Evaporative cooling. 
E) Its ability to function as a solvent. 
A) Hydrogen bonds allowing for surface tension. 
B) Hydrogen bonds allowing for increased structure of water. 
C) Hydrogen bonds allowing for adhesion and cohesion of molecules. 
D) Evaporative cooling. 
E) Its ability to function as a solvent.

Question 15

A solution with a pH of 7 has how many more protons in it than a solution with a pH of 9?

Accepted Answer

A) 2 times 
B) 5 times 
C) 10 times 
D) 100 times 
E) 1000 times 
A) 2 times 
B) 5 times 
C) 10 times 
D) 100 times 
E) 1000 times

Question 16

A small birthday candle is weighed,then lighted and placed beneath a metal can containing 100 mL of water.Careful records are kept as the temperature of the water rises.Data from this experiment are shown on the graph.What amount of heat energy is released in the burning of candle wax?

Accepted Answer

A) 2092 joules per gram of wax burned 
B) 20 920 joules per gram of wax burned 
C) 41 840 joules per gram of wax burned 
D) 83 680 joules per gram of wax burned 
E) 209 200 joules per gram of wax burned 
A) 2092 joules per gram of wax burned 
B) 20 920 joules per gram of wax burned 
C) 41 840 joules per gram of wax burned 
D) 83 680 joules per gram of wax burned 
E) 209 200 joules per gram of wax burned

Question 17

Buffers are substances that help resist shifts in pH by

Accepted Answer

A) releasing H⁺ to a solution when acids are added. 
B) donating H⁺ to a solution when bases are added. 
C) releasing OH⁻ to a solution when bases are added. 
D) accepting H⁺ from a solution when acids are added. 
E) both donating H⁺ to a solution when bases are added, and accepting H⁺ when acids are added. 
A) releasing H⁺ to a solution when acids are added. 
B) donating H⁺ to a solution when bases are added. 
C) releasing OH⁻ to a solution when bases are added. 
D) accepting H⁺ from a solution when acids are added. 
E) both donating H⁺ to a solution when bases are added, and accepting H⁺ when acids are added.

Question 18

Assume that acid rain has lowered the pH of a particular lake to pH 4.0.What is the hydroxyl ion concentration of this lake?

Accepted Answer

A) 1 × 10⁻¹⁰ mol of hydroxyl ion per litre of lake water 
B) 1 × 10⁻⁴ mol of hydroxyl ion per litre of lake water 
C) 10.0 M with regard to hydroxyl ion concentration 
D) 4)0 M with regard to hydroxyl ion concentration 
E) 1 × 10⁻⁴ mol of hydroxyl ion per litre of lake water and 4.0 M with regard to hydrogen ion concentration 
A) 1 × 10⁻¹⁰ mol of hydroxyl ion per litre of lake water 
B) 1 × 10⁻⁴ mol of hydroxyl ion per litre of lake water 
C) 10.0 M with regard to hydroxyl ion concentration 
D) 4)0 M with regard to hydroxyl ion concentration 
E) 1 × 10⁻⁴ mol of hydroxyl ion per litre of lake water and 4.0 M with regard to hydrogen ion concentration

Question 19

One litre of a solution of pH 9 has how many more hydroxyl ions (OH⁻)than 1 L of a solution of pH 4?

Accepted Answer

A) 5 times more 
B) 32 times more 
C) 50 000 times more 
D) 10 000 times more 
E) 100 000 times more 
A) 5 times more 
B) 32 times more 
C) 50 000 times more 
D) 10 000 times more 
E) 100 000 times more

Question 20

Use the following information to answer the questions below.
You live in Atlantic Canada and you are Skyping a friend in Manitoba.You are both complaining about the weather as both regions are being subjected to the same arctic air mass.As you discuss it,however,it becomes clear that she is experiencing a bitter cold that you are not.You realize that you had pretty much the same conversation last summer when it was much hotter in Manitoba than at home.
-This phenomenon is due to

Accepted Answer

A) solar energy at different latitudes. 
B) evolutionary adaptation to different climates. 
C) rate of vaporization. 
D) land freezing before water and thus land masses are colder. 
E) specific heat of water. 
A) solar energy at different latitudes. 
B) evolutionary adaptation to different climates. 
C) rate of vaporization. 
D) land freezing before water and thus land masses are colder. 
E) specific heat of water.

Exam 3: Water and Life

The partial negative charge in a molecule of water occurs because

The slight negative charge at one end of one water molecule is attracted to the slight positive charge of another water molecule.What is this attraction called?

What is the pH of a 1 millimolar NaOH solution?

One idea to mitigate the effects of burning fossil fuels on atmospheric CO₂ concentrations is to pipe liquid CO₂ into the ocean at depths of 2500 feet or greater.At the high pressures at such depths,CO₂ is heavier than water.What potential effects might result from implementing such a scheme?

The cities of Vancouver,Canada,and Regina,Saskatchewan,are at about the same latitude,but Regina has much hotter summers and much colder winters than Vancouver.Why?

A solution contains 0.0000001 (10⁻⁷)moles of hydroxyl ions [OH⁻] per litre.Which of the following best describes this solution?

Water molecules are able to form hydrogen bonds with

Rank,from low to high,the pH of blood,stomach acid,and urine.

Carbon dioxide (CO₂)is readily soluble in water,according to the equation CO₂ + H₂O ↔ H₂CO₃.Carbonic acid (H₂CO₃)is a weak acid.If CO₂ is bubbled into a beaker containing pure,freshly distilled water,which of the following graphs correctly describes the results?

Why does ice float in liquid water?

If the pH of a solution is decreased from 9 to 8,it means that the

Plants transport water through their vascular system utilizing what property of water?

A solution with a pH of 7 has how many more protons in it than a solution with a pH of 9?

A small birthday candle is weighed,then lighted and placed beneath a metal can containing 100 mL of water.Careful records are kept as the temperature of the water rises.Data from this experiment are shown on the graph.What amount of heat energy is released in the burning of candle wax?

Buffers are substances that help resist shifts in pH by

Assume that acid rain has lowered the pH of a particular lake to pH 4.0.What is the hydroxyl ion concentration of this lake?

One litre of a solution of pH 9 has how many more hydroxyl ions (OH⁻)than 1 L of a solution of pH 4?

Introduction: Evolution and Themes of Biology

The Chemical Context of 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

Filters