Chapter Quiz

Chapter 3: Water and the Fitness of the Environment

Chapter Quiz

Chapter Quiz

1 .

Cells are surrounded by water, and cells themselves consist of about 70% to 95% water. As a result _____. (Concept 3.1

) [Hint]

the temperature of living things tends to change relatively slowly

a variety of nutrient molecules are readily available as dissolved solutes

waste products produced by cell metabolism can be easily removed

dissolved substances can be easily transported within a cell or between cells in multicellular organisms

all of the above

2 .

Water is a polar molecule. This means that _____. (Concept 3.1

) [Hint]

the opposite ends of the molecule have opposite electrical charges

water molecules are linear, like a pole

water is one of the many hydrophobic molecules

the atoms in water have equal electronegativities

all of the above are correct

3 .

The tendency of water molecules to stay close to each other as a result of hydrogen bonding _____. (Concept 3.2

) [Hint]

provides the surface tension that allows leaves to float on water

is called cohesion

keeps water moving through the vessels in a tree trunk

acts to moderate temperature

all of the above

4 .

In a group of water molecules, hydrogen bonds form between _____. (Concept 3.1

) [Hint]

two hydrogen atoms in different water molecules

the oxygen atoms in different water molecules

the oxygen atom in one water molecule and a hydrogen atom in another water molecule

the hydrogen atoms in a single water molecule

none of the above

5 .

What do cohesion, surface tension, and adhesion have in common with reference to water? (Concept 3.2

) [Hint]

All are results of the structure of the hydrogen atom.

All are produced by covalent bonding.

All are properties related to hydrogen bonding.

All have to do with ionic interactions.

All are aspects of a crystalline structure.

6 .

Most of water's unique features (for example, its versatility as a solvent, ability to moderate temperature, and cohesive behavior) result from the fact that _____. (Concept 3.1

) [Hint]

hydrogen is the only element without any neutrons

oxygen attracts electrons more than hydrogen does

oxygen has only one stable isotope, but hydrogen has three

oxygen has two unfilled electron shells

More than one of the above is correct.

7 .

The partial charges on a water molecule occur because of _____. (Concept 3.1

) [Hint]

the unequal sharing of electrons between the hydrogen and the oxygen atoms of a water molecule

the achievement of a stable configuration by one atom of a bond but not by the other partner

covalent bonding

widespread ionization

the high electronegativity of hydrogen

8 .

The ability of water molecules to form hydrogen bonds with other water molecules and water's ability to dissolve substances that have charges or partial charges are _____. (Concept 3.2

) [Hint]

both caused by water's ability to form covalent bonds with hydrophobic substances

due to water's partial charges and low molecular mass, respectively

both caused by water's partial charges

both caused by water's two electron shells and the opposite spins of those shells

both due to water's low molecular mass

9 .

The phenomenon responsible for the maintenance of a column of water as it moves upward through a vessel is _____. (Concept 3.2

) [Hint]

cohesion

adhesion

surface tension

evaporation

heat of vaporization

10 .

Adhesion is best described as _____. (Concept 3.2

) [Hint]

a property of water that helps moderate Earth's temperature

the process by which a crystalline lattice forms

the process that contributes to the transport of water and dissolved nutrients in plants by causing water molecules to tug on other water molecules

the clinging of one substance to another substance

none of the above

11 .

You can fill a glass of water to just slightly above the rim without it spilling over the glass. What property of water best explains this phenomenon? (Concept 3.2

) [Hint]

surface tension

adhesion

its polarity

evaporative cooling

none of the above

12 .

Which action would involve the greatest transfer of heat? (Concept 3.2

) [Hint]

changing the temperature of 1 g of water from 10°C to 90°C

cooling 10 g of water from 80°C to 40°C

evaporating 1 g of water at 25°C

condensing 5 g of steam to liquid water

raising the temperature of 10 g of ethyl alcohol by 25°C

13 .

Which example is not an effect of water's high specific heat? (Concept 3.2

) [Hint]

Organisms are able to resist changes in their own temperatures.

Inland regions generally have milder climates than coastal regions.

Ocean temperatures are stabilized.

A large body of water can store a huge amount of heat from the sun, but only warm up a few degrees.

None of the above.

14 .

The amount of heat required to change the temperature of 1 g of any substance by 1°C is defined as _____. (Concept 3.2

) [Hint]

the specific heat of that substance

1 calorie

the heat of vaporization of that substance

1 kilocalorie

molecular cohesion

15 .

The amount of heat required to convert 1 g of any substance from the liquid to the gaseous state is defined as _____. (Concept 3.2

) [Hint]

the specific heat of that substance

1 calorie

the heat of vaporization of that substance

the heat of fusion of that substance

molecular cohesion

16 .

The reason that coastal climates are more moderate than inland climates is due primarily to water's high _____. (Concept 3.2

) [Hint]

heat of fusion

surface tension

heat of vaporization

specific heat

density

17 .

Sweating has a cooling effect because of water's high _____. (Concept 3.2

) [Hint]

heat of fusion

surface tension

heat of vaporization

specific heat

density

18 .

Water molecules have _____ than molecules of similar size, such as ammonia and methane. (Concept 3.2

) [Hint]

lower specific heat

a higher boiling point

a lower melting point

lower heat of fusion

less surface tension

19 .

Because molecules of water are farther apart in ice than in liquid water, _____. (Concept 3.2

) [Hint]

ice floats

ice is denser than liquid water

ice expands when it melts

ice vaporizes before liquid water does

all of the above

20 .

Water is a very versatile solvent because water molecules are_____. (Concept 3.2

) [Hint]

polar

nonpolar

ionic

hydrophobic

volatile

21 .

Sodium chloride (NaCl) dissolves in water because water molecules _____. (Concept 3.2

) [Hint]

have a high specific heat

lose electrons

are polar

have a pH near 7

are less dense than NaCl molecules

22 .

Nonpolar molecules that cluster away from water molecules are called _____ molecules. (Concept 3.2

) [Hint]

ionic

hydrophilic

hydrophobic

saponified

none of the above

23 .

Hydrophilic substances, but not hydrophobic substances, _____. (Concept 3.2

) [Hint]

have charges and partial charges to which water molecules can adhere

have a higher bond energy than water

give up electrons to solvents

accept electrons from solvents

are repelled by water

24 .

A molecule that has all nonpolar covalent bonds would be _____. (Concept 3.2

) [Hint]

hydrophobic

hydrophilic

acidic

basic (alkaline)

ionic

25 .

Hydrophobic molecules are _____ water. (Concept 3.2

) [Hint]

attracted to

absorbed by

repelled by

neutralized by

polarized by

26 .

Some substances, such as oil and gasoline, will not dissolve in water because _____. (Concept 3.2

) [Hint]

their molecules are so large

their molecules have no charges or partial charges to which water molecules can adhere

they do not ionize

their electrons are so stable that they do not exchange atoms with water molecules

oil and gasoline are organic compounds

27 .

An acid is _____. (Concept 3.3

) [Hint]

any compound with a pH

any compound that accepts hydrogen ions

a material that resists changes in the pH of a solution

a compound that donates hydrogen ions to a solution

a solution with a pH between 7 and 14

28 .

Sucrose has a molecular mass of 342 daltons. To make a 2-molar (2 M) solution of sucrose, _____. (Concept 3.2

) [Hint]

stir 342 g of sucrose in water to dissolve the sugar, and then add enough water to bring the total volume of the solution to 1 L

stir 684 g of sucrose in water to dissolve the sugar, and then add enough water to bring the total volume of the solution up to 2 L

stir 684 g of sucrose in water to dissolve the sugar, and then add enough water to bring the total volume of the solution up to 0.5 L

stir 342 g of sucrose in water to dissolve the sugar, and then add enough water to bring the total volume of the solution up to 2 L

stir 342 g of sucrose in water to dissolve the sugar, and then add enough water to bring the total volume of the solution up to 0.5 L

29 .

A mole of ethyl alcohol weighs 46 g. How many grams of ethyl alcohol are needed to produce 1 L of a 2-millimolar (2 mM) solution? (Concept 3.2

) [Hint]

92 g

9.2 g

0.92 g

0.092 g

0.0092 g

30 .

Adding acid tends to ____ of a solution. (Concept 3.3

) [Hint]

increase the hydrogen ion concentration and raise the pH

increase the hydrogen ion concentration and lower the pH

decrease the hydrogen ion concentration and raise the pH

decrease the hydrogen ion concentration and lower the pH

either increase or decrease the pH, depending on the original acidity

31 .

Which of the following dissociations is that of an acid? (Concept 3.3

) [Hint]

H₂O → H⁺ + OH^-

NaOH → Na⁺ + OH^-

HF → H⁺ + F^-

NH₃ + H⁺ → NH₄⁺

KOH → K⁺ + OH^-

32 .

A glass of grapefruit juice, at pH 3, contains _____ H⁺ as a glass of tomato juice, at pH 4. (Concept 3.3

) [Hint]

one-tenth as much

half as much

twice as much

three times as much

ten times as much

33 .

A solution at pH 6 contains ____ than the same amount of solution at pH 8. (Concept 3.3

) [Hint]

2 times more H⁺

4 times more H⁺

100 times more H⁺

4 times less H⁺

100 times less H⁺

34 .

Adding a base tends to _____ of a solution. (Concept 3.3

) [Hint]

lower the hydrogen ion concentration and lower the pH

lower the hydrogen ion concentration and increase the pH

increase the hydrogen ion concentration and lower the pH

increase the hydrogen ion concentration and increase the pH

lower the hydroxide ion concentration and lower the pH

35 .

When the pH of a solution shifts from 7 to 3, how has the hydrogen ion concentration changed? (Concept 3.3

) [Hint]

It has increased by 4 times.

It has decreased by 4 times.

It has increased by 10,000 times.

It has decreased by 10,000 times.

It has not changed.

36 .

Pure water has a pH of 7. Why does uncontaminated rainwater have a pH of 5.6? (Concept 3.3

) [Hint]

formation of carbonic acid from carbon dioxide and water

presence of sulfuric acid

presence of nitric acid

burning of fossil fuels

none of the above

37 .

A substance that minimizes changes in the concentration of H⁺ and OH^- in a solution is a(n) ______. (Concept 3.3

) [Hint]

hydrocarbon

buffer

NaCl

strong acid

strong base

38 .

Which of the following statements does not correctly describe a buffer? (Concept 3.3

) [Hint]

A buffer can accept H⁺ ions when needed.

A buffer can donate H⁺ ions when needed.

A buffer resists changes in the pH of a solution.

A buffer is only partly dissociated.

None of the above (all the above statements correctly describe a buffer).

39 .

Which of the following statements is true about acid precipitation? (Concept 3.3

) [Hint]

It harms aquatic life, but has little effect on terrestrial life.

It washes away some minerals that are plant nutrients, while causing some toxic minerals to accumulate.

Automobile use is the leading contributor to acid rain.

Industrial areas are hit hardest by acid rain.

None of the above.

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