Question 1

Why is a steam burn more severe than a hot water burn?

Accepted Answer

A)  Burns caused by liquids are always milder. 
B)  Steam can penetrate into the skin. 
C)  Steam contains more energy than water. 
D)  Water evaporates and leaves the surface faster and helps in cooling. 
A)  Burns caused by liquids are always milder. 
B)  Steam can penetrate into the skin. 
C)  Steam contains more energy than water. 
D)  Water evaporates and leaves the surface faster and helps in cooling.

Question 2

Liquid water ________.

Accepted Answer

A)  is less dense than ice 
B)  has a specific heat lower than that of most other substances 
C)  has a heat of vaporisation higher than that of most other substances 
D)  is nonpolar 
A)  is less dense than ice 
B)  has a specific heat lower than that of most other substances 
C)  has a heat of vaporisation higher than that of most other substances 
D)  is nonpolar

Question 3

What is the hydroxyl ion (OH-) concentration of a solution of pH 8?

Accepted Answer

A)  8 M 
B)  8 × 10-6 M 
C)  10-8 M 
D)  10-6 M 
A)  8 M 
B)  8 × 10-6 M 
C)  10-8 M 
D)  10-6 M

Question 4

Low humidity in the atmosphere on a hot day ________.

Accepted Answer

A)  helps in cooling because skin absorbs water from the atmosphere 
B)  does not help in cooling because water evaporates from the skin faster 
C)  helps in cooling because water evaporates from the skin faster 
D)  does not help in cooling because skin absorbs water from the atmosphere 
A)  helps in cooling because skin absorbs water from the atmosphere 
B)  does not help in cooling because water evaporates from the skin faster 
C)  helps in cooling because water evaporates from the skin faster 
D)  does not help in cooling because skin absorbs water from the atmosphere

Question 5

Assume that acid rain has lowered the pH of a particular river to pH 5.0. What is the hydroxide ion concentration of this river?

Accepted Answer

A)  1 × 10-9 mol of hydroxide ions per litre of river water 
B)  1 × 10-5 mol of hydroxide ions per litre of river water 
C)  5.0 M hydroxide ion 
D)  5.0 × 10-5 mol of hydroxide ions per litre of river water 
A)  1 × 10-9 mol of hydroxide ions per litre of river water 
B)  1 × 10-5 mol of hydroxide ions per litre of river water 
C)  5.0 M hydroxide ion 
D)  5.0 × 10-5 mol of hydroxide ions per litre of river water

Question 6

In a single molecule of water, two hydrogen atoms are bonded to a single oxygen atom by ________.

Accepted Answer

A)  hydrogen bonds 
B)  nonpolar covalent bonds 
C)  polar covalent bonds 
D)  ionic bonds 
A)  hydrogen bonds 
B)  nonpolar covalent bonds 
C)  polar covalent bonds 
D)  ionic bonds

Question 7

Increased atmospheric CO₂ concentrations might have what effect on seawater?

Accepted Answer

A)  Seawater will become more alkaline, and carbonate concentrations will decrease. 
B)  There will be no change in the pH of seawater, because carbonate will turn to bicarbonate. 
C)  Seawater will become more acidic, and carbonate concentrations will decrease. 
D)  Seawater will become more acidic, and carbonate concentrations will increase. 
A)  Seawater will become more alkaline, and carbonate concentrations will decrease. 
B)  There will be no change in the pH of seawater, because carbonate will turn to bicarbonate. 
C)  Seawater will become more acidic, and carbonate concentrations will decrease. 
D)  Seawater will become more acidic, and carbonate concentrations will increase.

Question 8

One mole (mol) of glucose (molecular mass = 180 daltons) is ________.

Accepted Answer

A)  180 × 1023 molecules of glucose 
B)  1 kilogram of glucose dissolved in 1 litre of solution 
C)  180 mL of dissolved glucose 
D)  180 grams of glucose 
A)  180 × 1023 molecules of glucose 
B)  1 kilogram of glucose dissolved in 1 litre of solution 
C)  180 mL of dissolved glucose 
D)  180 grams of glucose

Question 9

Carbon dioxide in the atmosphere dissolves with the raindrops. The pH of raindrops is ________.

Accepted Answer

A)  slightly acidic 
B)  slightly basic 
C)  the same as pure water 
D)  depends on the altitude where rain drops are formed 
A)  slightly acidic 
B)  slightly basic 
C)  the same as pure water 
D)  depends on the altitude where rain drops are formed

Question 10

How does 0.5 M sucrose (molecular mass 342) solution compare to 0.5 M glucose (molecular mass 180) solution?

Accepted Answer

A)  Both have 6.02 × 1023 molecules. 
B)  Sucrose has 171 molecules, whereas glucose has 90. 
C)  Both have 3.01 × 1023 molecules. 
D)  Sucrose has 171 mg/L, whereas glucose has 90 mg/L. 
A)  Both have 6.02 × 1023 molecules. 
B)  Sucrose has 171 molecules, whereas glucose has 90. 
C)  Both have 3.01 × 1023 molecules. 
D)  Sucrose has 171 mg/L, whereas glucose has 90 mg/L.

Question 11

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

Question 12

How much of 0.5 M glucose (molecular mass 180) is needed to provide 100 mg of glucose?

Accepted Answer

A)  1.11 mL 
B)  0.11 mL 
C)  100 mL 
D)  10 mL 
A)  1.11 mL 
B)  0.11 mL 
C)  100 mL 
D)  10 mL

Question 13

Consider two solutions: solution X has a pH of 4; solution Y has a pH of 7. From this information, we can reasonably conclude that ________.

Accepted Answer

A)  solution Y has no free hydrogen ions (H⁺) 
B)  the concentration of hydrogen ions in solution Y is 1000 times as great as the concentration of hydrogen ions in solution X 
C)  the concentration of hydrogen ions in solution X is 3 times as great as the concentration of hydrogen ions in solution Y 
D)  the concentration of hydrogen ions in solution X is 1000 times as great as the concentration of hydrogen ions in solution Y 
A)  solution Y has no free hydrogen ions (H⁺) 
B)  the concentration of hydrogen ions in solution Y is 1000 times as great as the concentration of hydrogen ions in solution X 
C)  the concentration of hydrogen ions in solution X is 3 times as great as the concentration of hydrogen ions in solution Y 
D)  the concentration of hydrogen ions in solution X is 1000 times as great as the concentration of hydrogen ions in solution Y

Question 14

Hydrophobic substances such as vegetable oil are ________.

Accepted Answer

A)  nonpolar substances that repel water molecules 
B)  nonpolar substances that have an attraction for water molecules 
C)  polar substances that repel water molecules 
D)  polar substances that have an affinity for water 
A)  nonpolar substances that repel water molecules 
B)  nonpolar substances that have an attraction for water molecules 
C)  polar substances that repel water molecules 
D)  polar substances that have an affinity for water

Question 15

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)  Stable hydrogen bonds keep water molecules of ice farther apart than water molecules of liquid water. 
D)  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)  Stable hydrogen bonds keep water molecules of ice farther apart than water molecules of liquid water. 
D)  The crystalline lattice of ice causes it to be denser than liquid water.

Exam 3: Water and Life

Why is a steam burn more severe than a hot water burn?

Liquid water ________.

What is the hydroxyl ion (OH-) concentration of a solution of pH 8?

Low humidity in the atmosphere on a hot day ________.

Assume that acid rain has lowered the pH of a particular river to pH 5.0. What is the hydroxide ion concentration of this river?

In a single molecule of water, two hydrogen atoms are bonded to a single oxygen atom by ________.

Increased atmospheric CO₂ concentrations might have what effect on seawater?

One mole (mol) of glucose (molecular mass = 180 daltons) is ________.

Carbon dioxide in the atmosphere dissolves with the raindrops. The pH of raindrops is ________.

How does 0.5 M sucrose (molecular mass 342) solution compare to 0.5 M glucose (molecular mass 180) solution?

How much of 0.5 M glucose (molecular mass 180) is needed to provide 100 mg of glucose?

Consider two solutions: solution X has a pH of 4; solution Y has a pH of 7. From this information, we can reasonably conclude that ________.

Hydrophobic substances such as vegetable oil are ________.

Why does ice float in liquid water?

Evolution, the Themes of Biology, and Scientific Inquiry

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

Gene Expression: 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 Colonised 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

Vascular 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

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