Campbell Biology 2nd Canadian Edition Plus Mastering Biology 2nd Edition By Jane B. Reece – Test Bank
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Sample Test
Campbell Biology, Cdn. Ed., 2e (Reece et al.)
Chapter 3 Water and Life
1) In a single molecule of water, two hydrogen atoms are bonded
to a single oxygen atom by
1. A)
hydrogen bonds.
2. B)
nonpolar covalent bonds.
3. C)
polar covalent bonds.
4. D)
ionic bonds.
5. E)
van der Waals interactions.
Answer: C
Type: MC
Topic: Concept 3.1
Skill: Knowledge/Comprehension
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?
1. A) a
covalent bond
2. B) a
hydrogen bond
3. C) an
ionic bond
4. D) a
hydrophilic bond
5. E) a
van der Waals interaction
Answer: B
Type: MC
Topic: Concept 3.1
Skill: Knowledge/Comprehension
3) The partial negative charge in a molecule of water occurs
because
1. A)
the oxygen atom acquires an additional electron.
2. B)
the electrons shared between the oxygen and hydrogen atoms spend more time
around the oxygen atom nucleus than around the hydrogen atom nucleus.
3. C)
the oxygen atom has two pairs of electrons in its valence shell that are not
neutralized by hydrogen atoms.
4. D) the
oxygen atom forms hybrid orbitals that distribute electrons unequally around
the oxygen nucleus.
5. E)
one of the hydrogen atoms donates an electron to the oxygen atom.
Answer: B
Type: MC
Topic: Concept 3.1
Skill: Knowledge/Comprehension
4) Sulphur is in the same column of the periodic table as
oxygen, but has electronegativity similar to carbon. Compared to water
molecules, molecules of H2S
1. A)
will ionize more readily.
2. B)
will have greater cohesion to other molecules of H2S.
3. C)
will have a greater tendency to form hydrogen bonds with each other.
4. D)
will have a higher capacity to absorb heat for the same change in temperature.
5. E)
will not form hydrogen bonds with each other.
Answer: E
Type: MC
Topic: Concept 3.1
Skill: Synthesis/Evaluation
5) Water molecules are able to form hydrogen bonds with
1. A)
compounds that have polar covalent bonds.
2. B)
oils.
3. C)
oxygen gas (O2) molecules.
4. D)
chloride ions.
5. E)
any compound that is not soluble in water.
Answer: A
Type: MC
Topic: Concept 3.1
Skill: Application/Analysis
6) Which of the following effects is produced by the high
surface tension of water?
1. A)
Lakes don’t freeze solid in winter, despite low temperatures.
2. B) A
water strider can walk across the surface of a small pond.
3. C)
Organisms resist temperature changes, although they give off heat due to
chemical reactions.
4. D)
Evaporation of sweat from the skin helps to keep people from overheating.
5. E)
Water flows upward from the roots to the leaves in plants.
Answer: B
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
7) Which of the following takes place as an ice cube cools a
drink?
1. A)
Molecular collisions in the drink increase.
2. B)
Kinetic energy in the drink decreases.
3. C) A
calorie of heat energy is transferred from the ice to the water of the drink.
4. D)
The specific heat of the water in the drink decreases.
5. E)
Evaporation of the water in the drink increases.
Answer: B
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
8) A dietary calorie equals 1 kilocalorie. Which of the following
statements correctly defines 1 kilocalorie?
1. A)
1000 calories, or the amount of heat required to raise the temperature of 1 g
of water by 1000°C
2. B)
100 calories, or the amount of heat required to raise the temperature of 100 g
of water by 1°C
3. C) 10
000 calories, or the amount of heat required to raise the temperature of 1 kg
of water by 1°F
4. D)
1000 calories, or the amount of heat required to raise the temperature of 1 kg
of water by 1°C
5. E)
1000 calories, or the amount of heat required to raise the temperature of 100 g
of water by 100°C
Answer: D
Type: MC
Topic: Concept 3.2
Skill: Knowledge/Comprehension
9) The nutritional information on a cereal box shows that one
serving of a dry cereal has 200 kilocalories. If one were to burn one serving
of the cereal, the amount of heat given off would be sufficient to raise the
temperature of 20 kg of water how many degrees Celsius?
1. A)
0.2°C
2. B)
1.0°C
3. C)
2.0°C
4. D)
10.0°C
5. E)
20.0°C
Answer: D
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
10) Which of the following can be attributed to water’s high
specific heat?
1. A)
Oil and water do not mix well.
2. B) A
lake heats up more slowly than the air around it.
3. C)
Ice floats on water.
4. D)
Sugar dissolves in hot tea faster than in iced tea.
5. E) We
experience a cooling effect when we sweat.
Answer: B
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
11) Which type of bond must be broken for water to vaporize?
1. A)
ionic bonds
2. B)
both hydrogen bonds and ionic bonds
3. C)
polar covalent bonds
4. D)
hydrogen bonds
5. E)
both polar covalent bonds and hydrogen bonds
Answer: D
Type: MC
Topic: Concept 3.2
Skill: Knowledge/Comprehension
12) Temperature usually increases when water condenses. Which
behaviour of water is most directly responsible for this phenomenon?
1. A)
the change in density when it condenses to form a liquid or solid
2. B)
reactions with other atmospheric compounds
3. C)
the release of heat by the formation of hydrogen bonds
4. D)
the release of heat by the breaking of hydrogen bonds
5. E)
the high surface tension of water
Answer: C
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
13) Why does evaporation of water from a surface cause cooling
of the surface?
1. A)
The breaking of bonds between water molecules absorbs heat.
2. B)
The water molecules with the most heat energy evaporate more readily.
3. C)
The solute molecules left behind absorb heat.
4. D)
Water molecules absorb heat from the surface in order to acquire enough energy
to evaporate.
5. E)
The expansion of water vapor extracts heat from the surface.
Answer: B
Type: MC
Topic: Concept 3.2
Skill: Knowledge/Comprehension
14) Why does ice float in liquid water?
1. A)
The high surface tension of liquid water keeps the ice on top.
2. B)
The ionic bonds between the molecules in ice prevent the ice from sinking.
3. C)
Ice always has air bubbles that keep it afloat.
4. D)
Hydrogen bonds stabilize and keep the molecules of ice farther apart than the
water molecules of liquid water.
5. E)
The crystalline lattice of ice causes it to be denser than liquid water.
Answer: D
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
15) Hydrophobic substances such as vegetable oil are
1. A)
nonpolar substances that repel water molecules.
2. B)
nonpolar substances that have an attraction for water molecules.
3. C)
polar substances that repel water molecules.
4. D)
polar substances that have an affinity for water.
5. E)
charged molecules that hydrogen-bond with water molecules.
Answer: A
Type: MC
Topic: Concept 3.2
Skill: Knowledge/Comprehension
16) One mole (mol) of glucose (molecular mass = 180 daltons) is
1. A)
180 × 1023 molecules of glucose.
2. B) 1
kg of glucose dissolved in 1 L of solution.
3. C)
the largest amount of glucose that can be dissolved in 1 L of solution.
4. D)
180 kilograms of glucose.
5. E)
both 180 grams of glucose and 6.02 × 1023 molecules of glucose.
Answer: E
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
17) How many molecules of glucose (C6H12O6 molecular mass = 180
daltons) would be present in 90 grams of glucose?
1. A) 90
× 1023
2. B)
(6.02/180) × 1023
3. C)
(6.02/90) × 1023
4. D)
(90 × 6.02) × 1023
5. E)
(90/180) × 6.02 × 1023
Answer: E
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
18) How many molecules of glycerol would be present in 1 L of a
1 M glycerol solution?
1. A) 1
× 106
2. B) 14
× 6.02 × 1023
3. C) 92
× 6.02 × 1023
4. D)
6.02 × 1026
5. E)
6.02 × 1023
Answer: E
Type: MC
Topic: Concept 3.2
Skill: Knowledge/Comprehension
19) 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)?
1. A) 1
L of 0.5 M NaCl
2. B) 1
L of 0.5 M glucose
3. C) 1
L of 1.0 M NaCl
4. D) 1
L of 1.0 M glucose
5. E) 1
L of 1.0 M NaCl and 1 L of 1.0 M glucose will contain equal numbers of solute
particles.
Answer: C
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
20) The molar mass of glucose is 180 g/mol. Which of the
following procedures should you carry out to make a 1 M solution of glucose?
1. A)
Dissolve 1 g of glucose in 1 L of water.
2. B)
Dissolve 180 g of glucose in 1 L of water.
3. C)
Dissolve 180 g of glucose in 180 g of water.
4. D)
Dissolve 180 milligrams (mg) of glucose in 1 L of water.
5. E)
Dissolve 180 g of glucose in 0.8 L of water, and then add more water until the
total volume of the solution is 1 L.
Answer: E
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
21) The molar mass of glucose is 180 g/mol. Which of the
following procedures should you carry out to make a 0.5 M solution of glucose?
1. A)
Dissolve 0.5 g of glucose in a small volume of water, and then add more water
until the total volume of solution is 1 L.
2. B)
Dissolve 90 g of glucose in a small volume of water, and then add more water
until the total volume of the solution is 1 L.
3. C)
Dissolve 180 g of glucose in a small volume of water, and then add more water
until the total volume of the solution is 1 L.
4. D)
Dissolve 0.5 g of glucose in 1 L of water.
5. E)
Dissolve 180 g of glucose in 0.5 L of water.
Answer: B
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
22) You have a freshly prepared 0.1 M solution of glucose in
water. Each litre of this solution contains how many glucose molecules?
6. A)
6.02 × 1023
7. B)
3.01 × 1023
8. C)
6.02 × 1024
9. D)
12.04 × 1023
10.
E) 6.02 × 1022
Answer: E
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
23) The molecular weight of water is 18 daltons. What is the
molarity of 1 litre of pure water? (Hint: What is the mass of 1 litre of pure
water?)
55.
A) 55.6 M
56.
B) 18 M
57.
C) 37 M
58.
D) 0.66 M
59.
E) 1.0 M
Answer: A
Type: MC
Topic: Concept 3.2
Skill: Synthesis/Evaluation
24) You have a freshly prepared 1 M solution of glucose in
water. You carefully pour out a 100 mL sample of that solution. How many
glucose molecules are included in that 100 mL sample?
6. A)
6.02 × 1023
7. B) 3.01
× 1023
8. C)
6.02 × 1024
9. D)
12.04 × 1023
10.
E) 6.02 × 1022
Answer: E
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
25) A strong acid like HCl
1. A)
ionizes completely in an aqueous solution.
2. B)
increases the pH when added to an aqueous solution.
3. C)
reacts with strong bases to create a buffered solution.
4. D) is
a strong buffer at low pH.
5. E)
both ionizes completely in aqueous solutions and is a strong buffer at low pH.
Answer: A
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
26) Which of the following ionizes completely in solution and is
considered to be a strong base (alkali)?
1. A)
NaCl
2. B)
HCl
3. C)
NH3
4. D)
H2CO3
5. E)
NaOH
Answer: E
Type: MC
Topic: Concept 3.3
Skill: Knowledge/Comprehension
27) A 0.01 M solution of a substance has a pH of 2. What can you
conclude about this substance?
1. A) It
is a strong acid that ionizes completely in water.
2. B) It
is a strong base that ionizes completely in water.
3. C) It
is a weak acid.
4. D) It
is a weak base.
5. E) It
is neither an acid nor a base.
Answer: A
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
28) In living systems molecules involved in hydrogen bonding
almost always contain either oxygen or nitrogen or both. How do you explain
this phenomenon?
1. A) Oxygen
and nitrogen are elements found in both nucleic acids and proteins.
2. B)
Oxygen and nitrogen are elements with very high attractions for their
electrons.
3. C)
Oxygen and nitrogen are elements found in fats and carbohydrates.
4. D)
Oxygen and nitrogen were both components of gases that made up the early
atmosphere on Earth.
5. E)
Oxygen and nitrogen have valence electrons.
Answer: B
Type: MC
Topic: Concept 3.1
Skill: Application/Analysis
29) A solution contains 0.0000001 (10-7) moles of hydroxyl ions
[OH-] per litre. Which of the following best describes this solution?
1. A)
acidic: H+ acceptor
2. B)
basic: H+ acceptor
3. C)
acidic: H+ donor
4. D)
basic: H+ donor
5. E)
neutral
Answer: E
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
30) What is the pH of a solution with a hydroxyl ion [OH-]
concentration of 10-12 M?
1. A) pH
2
2. B) pH
4
3. C) pH
10
4. D) pH
12
5. E) pH
14
Answer: A
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
31) What is the pH of a 1 millimolar NaOH solution?
1. A) pH
3
2. B) pH
8
3. C) pH
9
4. D) pH
10
5. E) pH
11
Answer: E
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
32) Which of the following solutions would require the greatest
amount of base to be added to bring the solution to neutral pH?
1. A)
gastric juice at pH 2
2. B)
vinegar at pH 3
3. C)
tomato juice at pH 4
4. D)
black coffee at pH 5
5. E)
household bleach at pH 12
Answer: A
Type: MC
Topic: Concept 3.3
Skill: Knowledge/Comprehension
33) What is the hydrogen ion [H+] concentration of a solution of
pH 8?
1. A) 8
M
2. B) 8
x 10-6 M
3. C)
0.01 M
4. D) 10-8
M
5. E)
10-6 M
Answer: D
Type: MC
Topic: Concept 3.3
Skill: Knowledge/Comprehension
34) If the pH of a solution is decreased from 9 to 8, it means
that the
9. A)
concentration of H+ has decreased to one-tenth (1/10) what it was at pH 9.
10.
B) concentration of H+ has increased tenfold (10X) compared to
what it was at pH 9.
11.
C) concentration of OH- has increased tenfold (10X) compared to
what it was at pH 9.
12.
D) concentration of OH- has decreased to one-tenth (1/10) what
it was at pH 9.
13.
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.
Answer: E
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
35) If the pH of a solution is increased from pH 5 to pH 7, it
means that the
5. A)
concentration of H+ is twice (2X) what it was at pH 5.
6. B)
concentration of H+ is one-half (1/2) what it was at pH 5.
7. C)
concentration of OH- is 100 times greater than what it was at pH 5.
8. D)
concentration of OH- is one-hundredth (0.01X) what it was at pH 5.
9. E)
concentration of H+ is 100 times greater and the concentration of OH- is
one-hundredth what they were at pH 5.
Answer: C
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
36) One litre of a solution of pH 2 has how many more hydrogen
ions (H+) than 1 L of a solution of pH 6?
1. A) 4
times more
2. B) 16
times more
3. C) 40
000 times more
4. D) 10
000 times more
5. E)
100 000 times more
Answer: D
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
37) One litre of a solution of pH 9 has how many more hydroxyl
ions (OH-) than 1 L of a solution of pH 4?
1. A) 5
times more
2. B) 32
times more
3. C) 50
000 times more
4. D) 10
000 times more
5. E)
100 000 times more
Answer: E
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
38) Which of the following statements is true about buffer
solutions?
1. A)
They maintain a constant pH when bases are added to them but not when acids are
added to them.
2. B)
They maintain a constant pH when acids are added to them but not when bases are
added to them.
3. C)
They maintain a relatively constant pH of approximately 7 when either acids or
bases are added to them.
4. D)
They maintain a relatively constant pH when either acids or bases are added to
them.
5. E)
They are found only in living systems and biological fluids.
Answer: D
Type: MC
Topic: Concept 3.3
Skill: Knowledge/Comprehension
39) Buffers are substances that help resist shifts in pH by
1. A)
releasing H+ to a solution when acids are added.
2. B)
donating H+ to a solution when bases are added.
3. C)
releasing OH- to a solution when bases are added.
4. D)
accepting H+ from a solution when acids are added.
5. E)
both donating H+ to a solution when bases are added, and accepting H+ when
acids are added.
Answer: E
Type: MC
Topic: Concept 3.3
Skill: Knowledge/Comprehension
40) One of the buffers that contribute to pH stability in human
blood is carbonic acid (H2CO3). Carbonic acid is a weak acid that dissociates
into a bicarbonate ion (HCO3-) and a hydrogen ion (H+). Thus,
H2CO3 ↔ HCO3- + H+
If the pH of the blood drops, one would expect
1. A) a
decrease in the concentration of H2CO3 and an increase in the concentration of
HCO3-.
2. B)
the concentration of hydroxide ion (OH-) to increase.
3. C)
the concentration of bicarbonate ion (HCO3-) to increase.
4. D)
the HCO3- to act as a base and remove excess H+ with the formation of H2CO3.
5. E)
the HCO3- to act as an acid and remove excess H+ with the formation of H2CO3.
Answer: D
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
41) One of the buffers that contributes to pH stability in human
blood is carbonic acid (H2CO3). Carbonic acid is a weak acid that, when placed
in an aqueous solution, dissociates into a bicarbonate ion (HCO3-) and a
hydrogen ion (H+). Thus, H2CO3 ↔ HCO3- + H+
If the pH of the blood increases, one would expect
1. A) a
decrease in the concentration of H2CO3 and an increase in the concentration of
HCO3-.
2. B) an
increase in the concentration of H2CO3 and a decrease in the concentration of
HCO3-.
3. C) a
decrease in the concentration of HCO3- and an increase in the concentration of
H+.
4. D) an
increase in the concentration of HCO3- and a decrease in the concentration of
OH-.
5. E) a
decrease in the concentration of HCO3- and an increase in the concentration of
both H2CO3 and H+.
Answer: A
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
42) 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?
1. A) 1
× 10-10 mol of hydroxyl ion per litre of lake water
2. B) 1
× 10-4 mol of hydroxyl ion per litre of lake water
3. C)
10.0 M with regard to hydroxyl ion concentration
4. D)
4.0 M with regard to hydroxyl ion concentration
5. E) 1
× 10-4 mol of hydroxyl ion per litre of lake water and 4.0 M with regard to
hydrogen ion concentration
Answer: A
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
43) Research indicates that acid precipitation can damage living
organisms by
1. A)
buffering aquatic systems such as lakes and streams.
2. B) decreasing
the H+ concentration of lakes and streams.
3. C)
increasing the OH- concentration of lakes and streams.
4. D)
washing away certain mineral ions that help buffer soil solution and are
essential nutrients for plant growth.
5. E)
both decreasing the H+ concentration of lakes and streams and increasing the
OH- concentration of lakes and streams.
Answer: D
Type: MC
Topic: Concept 3.3
Skill: Knowledge/Comprehension
44) 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
1. A)
solution Y has no free hydrogen ions (H+).
2. B)
the concentration of hydrogen ions in solution X is 30 times as great as the
concentration of hydrogen ions in solution Y.
3. C)
the concentration of hydrogen ions in solution Y is 1000 times as great as the
concentration of hydrogen ions in solution X.
4. D)
the concentration of hydrogen ions in solution X is 3 times as great as the
concentration of hydrogen ions in solution Y.
5. E)
the concentration of hydrogen ions in solution X is 1000 times as great as the
concentration of hydrogen ions in solution Y.
Answer: E
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
45) If a solution has a pH of 7, this means that
1. A)
there are no H+ ions in the water.
2. B)
this is a solution of pure water.
3. C)
the concentration of H+ ions in the water equals the concentration of OH- ions
in the water.
4. D)
this is a solution of pure water, and the concentration of H+ ions in the water
is 10-7 M.
5. E)
this is a solution of pure water, and the concentration of H+ ions equals the
concentration of OH- ions in the water.
Answer: C
Type: MC
Topic: Concept 3.3
Skill: Knowledge/Comprehension
46) Carbon dioxide (CO2) is readily soluble in water, according
to the equation CO2 + H2O ↔ H2CO3. Carbonic acid (H2CO3) is a weak acid.
Respiring cells release CO2 into the bloodstream. What will be the effect on pH
of blood as that blood first comes in contact with respiring cells?
1. A)
Blood pH will decrease slightly.
2. B)
Blood pH will increase slightly.
3. C)
Blood pH will remain unchanged.
4. D)
Blood pH will first increase, then decrease as CO2 combines with hemoglobin.
5. E)
Blood pH will first decrease, then increase sharply as CO2 combines with
hemoglobin.
Answer: A
Type: MC
Topic: Concept 3.3
Skill: Synthesis/Evaluation
47) A beaker contains 100 mL of NaOH solution at pH = 13. A
technician carefully pours into the beaker 10 mL of HCl at pH = 1. Which of the
following statements correctly describes the results of this mixing?
1. A)
The concentration of Na+ ion rises.
2. B)
The concentration of Cl- ion will be 0.1 M.
3. C)
The concentration of undissociated H2O molecules remains unchanged.
4. D)
The pH of the beaker’s contents will be neutral.
5. E)
The pH of the beaker’s contents falls.
Answer: E
Type: MC
Topic: Concept 3.3
Skill: Synthesis/Evaluation
48) Equal volumes (5 mL) of vinegar from a freshly opened bottle
are added to each of the following solutions. After complete mixing, which of
the mixtures will have the highest pH?
1. A)
100 mL of pure water
2. B) 100
mL of freshly brewed coffee
3. C)
100 mL of household cleanser containing 0.5 M ammonia
4. D)
100 mL of freshly squeezed orange juice
5. E)
100 mL of tomato juice
Answer: C
Type: MC
Topic: Concept 3.3
Skill: Synthesis/Evaluation
49) Increased atmospheric CO2 concentrations might have what
effect on sea water?
1. A)
Sea water will become more acidic, and bicarbonate concentrations will
decrease.
2. B)
Sea water will become more alkaline, and carbonate concentrations will
decrease.
3. C)
There will be no change in the pH of sea water, because carbonate will turn to
bicarbonate.
4. D)
Sea water will become more acidic, and carbonate concentrations will decrease.
5. E)
Sea water will become more acidic, and carbonate concentrations will increase.
Answer: D
Type: MC
Topic: Concept 3.3
Skill: Knowledge/Comprehension
50) How would acidification of sea water affect marine
organisms?
1. A)
Acidification would increase dissolved carbonate concentrations and promote
faster growth of corals and shell-building animals.
2. B) Acidification
would decrease dissolved carbonate concentrations and promote faster growth of
corals and shell-building animals.
3. C)
Acidification would increase dissolved carbonate concentrations and hinder
growth of corals and shell-building animals.
4. D) Acidification
would decrease dissolved carbonate concentrations and hinder growth of corals
and shell-building animals.
5. E)
Acidification would increase dissolved bicarbonate concentrations, and cause
increased calcification of corals and shellfish.
Answer: D
Type: MC
Topic: Concept 3.3
Skill: Knowledge/Comprehension
51) 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?
1. A)
increased photosynthetic carbon fixation because of the increased dissolved
carbon dioxide in the deep water
2. B)
increased carbonate concentrations in the deep waters
3. C)
reduced growth of corals from a change in the carbonate-bicarbonate equilibrium
4. D) no
effect because carbon dioxide is not soluble in water
5. E)
both increased acidity of the deep waters and changes in the growth of
bottom-dwelling organisms with calcium carbonate shells
Answer: E
Type: MC
Topic: Concept 3.3
Skill: Synthesis/Evaluation
52) If the cytoplasm of a cell is at pH 7, and the mitochondrial
matrix is at pH 8, this means that
1. A)
the concentration of H+ ions is tenfold higher in the cytoplasm than in the
mitochondrial matrix.
2. B)
the concentration of H+ ions is tenfold higher in the mitochondrial matrix than
in the cytoplasm.
3. C)
the concentration of H+ ions in the cytoplasm is 7/8 the concentration in the
mitochondrial matrix.
4. D)
the mitochondrial matrix is more acidic than the cytoplasm.
5. E)
the concentration of H+ ions in the cytoplasm is 8/7 the concentration in the
mitochondrial matrix.
Answer: A
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
53) The only common substance on earth, which occurs naturally
in all three physical states, is
1. A)
oxygen.
2. B)
carbon.
3. C)
nitrogen.
4. D)
sodium chloride.
5. E)
water.
Answer: E
Type: MC
Topic: Introduction to Chapter 3
Skill: Knowledge/Comprehension
54) Plants transport water through their vascular system
utilizing what property of water?
1. A)
Hydrogen bonds allowing for surface tension.
2. B)
Hydrogen bonds allowing for increased structure of water.
3. C)
Hydrogen bonds allowing for adhesion and cohesion of molecules.
4. D)
Evaporative cooling.
5. E)
Its ability to function as a solvent.
Answer: C
Type: MC
Topic: Concept 3.2
Skill: Knowledge/Comprehension
55) Hydrogen bonding in water is a result of
1. A)
the electronegativity of hydrogen atoms.
2. B)
the electronegativity of oxygen creating partially positive hydrogen atoms.
3. C)
the single electron in hydrogen, allowing for covalent bonds with other
molecules.
4. D)
the linear shape of the water molecule.
5. E)
the ionic charge of water.
Answer: B
Type: MC
Topic: Concept 3.2
Skill: Knowledge/Comprehension
56) Coastal regions tend to have more moderate climates than
land-locked areas due to the
1. A)
high specific heat of water.
2. B)
heat of vaporization of water.
3. C)
amount of solutes in ocean water.
4. D)
high thermal energy in the atmosphere.
5. E)
latitude on which it is dependent; landmass has no effect.
Answer: A
Type: MC
Topic: Concept 3.2
Skill: Knowledge/Comprehension
57) The reason water has a high specific heat is that
1. A)
the adhesive property of water resists heat absorption.
2. B)
ionic bonds require a lot of energy to be broken.
3. C) a
lot of heat needs to be absorbed to disrupt hydrogen bonds.
4. D)
the covalent bonds resist splitting.
5. E)
water cools very quickly.
Answer: C
Type: MC
Topic: Concept 3.2
Skill: Knowledge/Comprehension
58) Water is densest at
1. A)
-4°C.
2. B)
0°C.
3. C)
2°C.
4. D)
4°C.
5. E)
8°C.
Answer: D
Type: MC
Topic: Concept 3.2
Skill: Knowledge/Comprehension
59) What is the major area of biological concern regarding
acidification of the oceans?
1. A)
They will become too acidic for life.
2. B)
There will not be enough carbonate available for organisms to make calcium
carbonate.
3. C)
There will be too much bicarbonate, making the oceans basic.
4. D)
There will be too much CO2 released back into the atmosphere.
5. E)
They will become too polluted for human use.
Answer: B
Type: MC
Topic: Concept 3.3
Skill: Knowledge/Comprehension
60) The biological significance of water being its densest at
4°C is that
1. A)
bodies of water do not freeze solid.
2. B) floating
ice allows for a solid surface in open water.
3. C)
ice functions as a protective barrier in ponds and lakes.
4. D)
organisms are best adapted to 4°C.
5. E)
oceans are never colder than 4°C.
Answer: A
Type: MC
Topic: Concept 3.2
Skill: Knowledge/Comprehension
61) Based on your knowledge of the polarity of water molecules,
the solute molecule depicted here is most likely
1. A)
positively charged.
2. B)
negatively charged.
3. C)
without charge.
4. D)
hydrophobic.
5. E)
nonpolar.
Answer: A
Type: MC
Topic: Concept 3.1
Skill: Application/Analysis
Use the following figure to answer the questions below.
62) How many grams would be equal to 1 mol of the compound shown
in the figure above?
(carbon = 12, oxygen = 16, hydrogen = 1)
1. A) 29
2. B) 30
3. C) 60
4. D)
150
5. E)
342
Answer: C
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
63) How many grams of the compound in the figure above would be
required to make 1 L of a 0.5 M solution?
(carbon = 12, oxygen = 16, hydrogen = 1)
1. A) 29
2. B) 30
3. C) 60
4. D)
150
5. E) 342
Answer: B
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
64) How many grams of the compound in the figure above would be
required to make 2.5 L of a 1 M solution?
(carbon = 12, oxygen = 16, hydrogen = 1)
1. A) 29
2. B) 30
3. C) 60
4. D)
150
5. E)
342
Answer: D
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
65) 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?
1. A)
2092 joules per gram of wax burned
2. B) 20
920 joules per gram of wax burned
3. C) 41
840 joules per gram of wax burned
4. D) 83
680 joules per gram of wax burned
5. E)
209 200 joules per gram of wax burned
Answer: A
Type: MC
Topic: Concept 3.2
Skill: Synthesis/Evaluation
66) Identical heat lamps are arranged to shine on identical
containers of water and methanol (wood alcohol), so that each liquid absorbs
the same amount of energy minute by minute. The covalent bonds of methanol
molecules are nonpolar, so there are no hydrogen bonds among methanol
molecules. Which of the following graphs correctly describes what will happen
to the temperature of the water and the methanol?
A)
B)
C)
D)
E)
Answer: B
Type: MC
Topic: Concept 3.2
Skill: Synthesis/Evaluation
67) Which of these molecules would be soluble in water?
A)
B)
C)
D)
1. E)
Both of these molecules
Answer: B
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
68) 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?
A)
B)
C)
D)
E)
Answer: B
Type: MC
Topic: Concept 3.3
Skill: Synthesis/Evaluation
69) You have two beakers. One contains pure water; the other
contains pure methanol (wood alcohol). The covalent bonds of methanol molecules
are nonpolar, so there are no hydrogen bonds among methanol molecules. You pour
crystals of table salt (NaCl) into each beaker. Predict what will happen.
1. A)
Equal amounts of NaCl crystals will dissolve in both water and methanol.
2. B)
NaCl crystals will NOT dissolve in either water or methanol.
3. C)
NaCl crystals will dissolve readily in water but will not dissolve in methanol.
4. D)
NaCl crystals will dissolve readily in methanol but will not dissolve in water.
5. E)
When the first crystals of NaCl are added to water or to methanol, they will
not dissolve; but as more crystals are added, the crystals will begin to
dissolve faster and faster.
Answer: C
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
70) You have two beakers. One contains a solution of HCl at pH =
1.0. The other contains a solution of NaOH at pH = 13. Into a third beaker, you
slowly and cautiously pour 20 mL of the HCl and 20 mL of the NaOH. After
complete stirring, the pH of the mixture will be
2. A)
2.0.
3. B)
12.0.
4. C)
7.0.
5. D)
5.0.
6. E)
9.0.
Answer: C
Type: MC
Topic: Concept 3.3
Skill: Synthesis/Evaluation
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.
71) The best explanation for this difference is that
1. A)
your climate is moderated by the Atlantic Ocean.
2. B) it
is just much colder in the middle of the country.
3. C) it
rains more in central Canada.
4. D)
your friend just doesn’t adjust well to changes in temperature.
5. E)
she must be at a higher latitude.
Answer: A
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
72) This phenomenon is due to
1. A)
solar energy at different latitudes.
2. B)
evolutionary adaptation to different climates.
3. C)
rate of vaporization.
4. D)
land freezing before water and thus land masses are colder.
5. E)
specific heat of water.
Answer: E
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
73) Many mammals control their body temperature by sweating.
Which property of water is most directly responsible for the ability of sweat
to lower body temperature?
1. A)
water’s change in density when it condenses
2. B)
water’s ability to dissolve molecules in the air
3. C)
the release of heat by the formation of hydrogen bonds
4. D)
the absorption of heat by the breaking of hydrogen bonds
5. E)
water’s high surface tension
Answer: D
Type: MC
Topic: End-of-Chapter Questions
Skill: Knowledge/Comprehension
74) The bonds that are broken when water vaporizes are
1. A)
ionic bonds.
2. B)
hydrogen bonds between water molecules.
3. C)
covalent bonds between atoms within water molecules.
4. D)
polar covalent bonds.
5. E)
nonpolar covalent bonds.
Answer: B
Type: MC
Topic: End-of-Chapter Questions
Skill: Knowledge/Comprehension
75) Which of the following is a hydrophobic material?
1. A)
paper
2. B)
table salt
3. C)
wax
4. D)
sugar
5. E)
pasta
Answer: C
Type: MC
Topic: End-of-Chapter Questions
Skill: Knowledge/Comprehension
76) We can be sure that a mole of table sugar and a mole of
vitamin C are equal in their
1. A)
mass in daltons.
2. B)
mass in grams.
3. C)
volume.
4. D)
number of atoms.
5. E)
number of molecules.
Answer: E
Type: MC
Topic: End-of-Chapter Questions
Skill: Knowledge/Comprehension
77) Measurements show that the pH of a particular lake is 4.0.
What is the hydrogen ion concentration of the lake?
4. A)
4.0 M
5. B)
10-10 M
6. C)
10-4 M
7. D)
104 M
8. E) 4%
Answer: C
Type: MC
Topic: End-of-Chapter Questions
Skill: Knowledge/Comprehension
78) Measurements show that the pH of a particular lake is 4.0.
What is the hydroxide ion concentration of the lake?
1. A)
10-10 M
2. B)
10-4 M
3. C)
10-7 M
4. D)
10-14 M
5. E) 10
M
Answer: A
Type: MC
Topic: End-of-Chapter Questions
Skill: Knowledge/Comprehension
79) A slice of pizza has 2092 kJ. If we could burn the pizza and
use all the heat to warm a 50-L container of cold water, what would be the
approximate increase in the temperature of the water? (Note: A litre of cold
water weighs about 1 kg.)
1. A)
50°C
2. B)
5°C
3. C)
1°C
4. D)
100°C
5. E)
10°C
Answer: E
Type: MC
Topic: End-of-Chapter Questions
Skill: Application/Analysis
80) How many grams of acetic acid (C2H4O2) would you use to make
10 L of a 0.1 M aqueous solution of acetic acid? (Note: The atomic masses, in
daltons, are approximately 12 for carbon, 1 for hydrogen, and 16 for oxygen.)
1. A) 10
g
2. B)
0.1 g
3. C)
6.0 g
4. D) 60
g
5. E)
0.6 g
Answer: D
Type: MC
Topic: End-of-Chapter Questions
Skill: Application/Analysis
81) Which of the following is a property of liquid water? Liquid
water ________.
1. A) is
less dense than ice
2. B)
has a specific heat that is lower than that for most other substances
3. C)
has a heat of vaporization that is higher than that for most other substances
4. D) is
nonpolar
5. E) is
ionic
Answer: C
Type: MC
Topic: Concept 3.2
Skill: Knowledge/Comprehension
82) Rank, from low to high, the pH of blood, stomach acid, and
urine.
1. A)
blood, urine, and stomach acid
2. B) stomach
acid, blood, and urine
3. C)
urine, blood, stomach acid
4. D)
stomach acid, urine, blood
5. E)
stomach acid, urine and blood have a similar neutral pH
Answer: D
Type: MC
Topic: Concept 3.3
Skill: Knowledge/Comprehension
83) 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?
1. A)
They are not at the same exact latitude.
2. B)
The ocean near Vancouver moderates the temperature.
3. C)
Fresh water is more likely to freeze than salt water.
4. D)
Regina is much windier, due to its location in Canada.
5. E)
Vancouver experiences more chinook winds.
Answer: B
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
84) To act as an effective coolant in a car’s radiator, a
substance has to have the capacity to absorb a great deal of heat. You have a
reference book with tables listing the physical properties of many liquids. In
choosing a coolant for your car, which table would you check first?
1. A) pH
2. B)
density at room temperature
3. C)
heat of vaporization
4. D)
specific heat
5. E)
volume
Answer: D
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
85) Water has many exceptional and useful properties. Which is
the rarest property among compounds?
1. A)
Water is a solvent.
2. B)
Solid water is less dense than liquid water.
3. C)
Water has a high heat capacity.
4. D)
Water has a high surface tension.
5. E)
Water has a high heat of evaporation.
Answer: B
Type: MC
Topic: Concept 3.2
Skill: Knowledge/Comprehension
86) A solution with a pH of 7 has how many more protons in it
than a solution with a pH of 9?
1. A) 2
times
2. B) 5
times
3. C) 10
times
4. D)
100 times
5. E)
1000 times
Answer: D
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
87) Consider the following reaction at equilibrium: What would
be the effect of adding additional H2CO3?
1. A) It
would drive the equilibrium dynamics to the right.
2. B) It
would drive the equilibrium dynamics to the left.
3. C)
Nothing would happen, because the reactants and products are in equilibrium.
4. D)
The amounts of CO2 and H2O would decrease.
5. E) H+
will form.
Answer: B
Type: MC
Topic: Concept 3.3
Skill: Application/Analysis
88) The loss of water from a plant by transpiration cools the
leaf. Movement of water in transpiration requires both adhesion to the
conducting walls and wood fibers of the plant and cohesion of the molecules to
each other. A scientist wanted to increase the rate of transpiration of a crop
species to extend its range into warmer climates. The scientist substituted a
nonpolar solution with an atomic mass similar to that of water for hydrating
the plants. What do you expect the scientist’s data will indicate from this
experiment?
1. A)
The rate of transpiration will be the same for both water and the nonpolar
substance.
2. B)
The rate of transpiration will be slightly lower with the nonpolar substance as
the plant will not have evolved with the nonpolar compound.
3. C)
Transpiration rates will fall to zero as nonpolar compounds do not have the
properties necessary for adhesion and cohesion.
4. D)
Transpiration rates will increase as nonpolar compounds undergo adhesion and
cohesion with wood fibers more readily than water.
5. E)
Transpiration will rise quickly, fall, and then reach an intermediate level as
the plants move from transpiring water to the non-polar solution.
Answer: C
Type: MC
Topic: Concept 3.3
Skill: Synthesis/Evaluation
89) Which of the following correctly describes the formation of
hydrogen bonds in water?
1. A)
Hydrogen bonds are almost as strong as a covalent bond.
2. B)
The hydrogen bonds organize water molecules into a higher level of structural
order.
3. C)
Each water molecule will tend to form hydrogen bonds repeatedly with the same
partner.
4. D)
Only a small fraction of the molecules in water molecules will be involved in
hydrogen bonds at any given instant.
5. E)
The hydrogen bonds that forms between adjacent water molecules remain intact
for several seconds.
Answer: B
Answer: B
Type: MC
Topic: Concept 3.1
Skill: Knowledge/Comprehension
90) Which of the following correctly describes thermal energy?
1. A)
Thermal energy is defined as temperature.
2. B)
Thermal energy is the controlled energy of motion.
3. C) Thermal
energy is the random movement of molecules.
4. D)
Thermal energy is not dependent on volume.
5. E)
Thermal energy is the energy possessed based on position relative to others.
Answer: C
Type: MC
Topic: Concept 3.2
Skill: Knowledge/Comprehension
91) Which of the following has the most thermal energy?
1. A) a
boiling cup of coffee
2. B) a
swimming pool at 28°C
3. C) a
hot tub at 37°C
4. D)
the Pacific ocean
5. E)
Lake Erie
Answer: D
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
92) When snow falls on Lake Superior how are the snow’s water
molecules impacted?
1. A)
They absorb thermal energy.
2. B)
They decrease their motion.
3. C)
They increase their potential energy.
4. D)
They release kinetic energy.
5. E)
They move less randomly.
Answer: A
Type: MC
Topic: Concept 3.2
Skill: Application/Analysis
Campbell Biology, Cdn. Ed., 2e (Reece et al.)
Chapter 4 Carbon and the Molecular Diversity of Life
1) The element present in all organic molecules is
1. A)
hydrogen.
2. B)
oxygen.
3. C)
carbon.
4. D)
nitrogen.
5. E) phosphorus.
Answer: C
Type: MC
Topic: Concept 4.1
Skill: Knowledge/Comprehension
2) The complexity and variety of organic molecules is due to
1. A)
the chemical versatility of carbon atoms.
2. B)
the variety of rare elements in organic molecules.
3. C)
the fact that they can be synthesized only in living organisms.
4. D)
their interaction with water.
5. E)
their tremendously large sizes.
Answer: A
Type: MC
Topic: Concept 4.1
Skill: Knowledge/Comprehension
3) The experimental approach taken in current biological
investigations presumes that
1. A)
simple organic compounds can be synthesized in the laboratory from inorganic
precursors, but complex organic compounds like carbohydrates and proteins can
only be synthesized by living organisms.
2. B) a
life force ultimately controls the activities of living organisms and this life
force cannot be studied by physical or chemical methods.
3. C)
although a life force, or vitalism, exists in living organisms, this life force
cannot be studied by physical or chemical methods.
4. D)
living organisms are composed of the same elements present in nonliving things,
plus a few special trace elements found only in living organisms or their
products.
5. E)
living organisms can be understood in terms of the same physical and chemical
laws that can be used to explain all natural phenomena.
Answer: E
Type: MC
Topic: Concept 4.1
Skill: Knowledge/Comprehension
4) Differences among organisms are caused by
1. A)
large differences in elemental composition from organism to organism.
2. B)
differences in the types and relative amounts of organic molecules synthesized
by each organism.
3. C)
differences in the elements that bond with carbon in each organism.
4. D)
differences in the sizes of the organic molecules in each organism.
5. E)
differences in inorganic compounds present in each organism.
Answer: B
Type: MC
Topic: Concept 4.1
Skill: Application/Analysis
5) Which of the following people was the first to synthesize an
organic compound, urea, from inorganic starting materials?
1. A)
Stanley Miller
2. B) Jakob
Berzelius
3. C)
Friedrich Wohler
4. D)
Hermann Kolbe
5. E)
August Kekulé
Answer: C
Type: MC
Topic: Concept 4.1
Skill: Knowledge/Comprehension
6) Stanley Miller’s 1953 experiments proved that
1. A)
life arose on Earth from simple inorganic molecules.
2. B)
organic molecules can be synthesized abiotically under conditions that may have
existed on early Earth.
3. C)
life arose on Earth from simple organic molecules, with energy from lightning
and volcanoes.
4. D)
the conditions on early Earth were conducive to the origin of life.
5. E)
the conditions on early Earth were conducive to the abiotic synthesis of
organic molecules.
Answer: B
Type: MC
Topic: Concept 4.1
Skill: Synthesis/Evaluation
7) Which of the following correctly describes ATP?
1. A)
ATP is hydrophobic.
2. B)
ATP is inorganic.
3. C)
ATP is unable to react with water.
4. D)
ATP has two covalently attached phosphates.
5. E)
ATP is able to store energy for the cell.
Answer: E
Type: MC
Topic: Concept 4.3
Skill: Knowledge/Comprehension
8) Stanley Miller’s 1953 experiments assumed that early Earth’s
atmosphere contained
1. A)
hydrogen cyanide, formaldehyde, hydrogen gas, and water vapour.
2. B)
ammonia, methane, hydrogen gas, and water vapour.
3. C)
ammonia, methane, oxygen gas, and water vapour.
4. D)
amino acids, methane, hydrogen cyanide, and water vapour.
5. E)
methane, formaldehyde, ammonia, and carbon dioxide.
Answer: B
Type: MC
Topic: Concept 4.1
Skill: Knowledge/Comprehension
9) When Stanley Miller applied heat and electrical sparks to a
mixture of simple inorganic compounds such as methane, hydrogen gas, ammonia,
and water vapour, what compounds were produced?
1. A)
mostly amino acids
2. B)
only simple organic compounds such as formaldehyde and cyanide
3. C)
mostly hydrocarbons
4. D)
only simple inorganic compounds
5. E)
both simple organic compounds and more complex organic compounds such as amino
acids and hydrocarbons
Answer: E
Type: MC
Topic: Concept 4.1
Skill: Knowledge/Comprehension
10) How many electron pairs does carbon share in order to complete
its valence shell?
1. A) 1
2. B) 2
3. C) 3
4. D) 4
5. E) 8
Answer: D
Type: MC
Topic: Concept 4.2
Skill: Knowledge/Comprehension
11) A carbon atom is most likely to form what kind of bond(s)
with other atoms?
1. A)
ionic
2. B)
hydrogen
3. C)
covalent
4. D)
covalent bonds and hydrogen bonds
5. E)
ionic bonds, covalent bonds, and hydrogen bonds
Answer: C
Type: MC
Topic: Concept 4.2
Skill: Knowledge/Comprehension
12) What is the key reason that often only one isomer of a pair
of enantiomers is biologically active?
1. A)
The functional groups in isomers may be found on the same or opposite sides of
a double bond.
2. B)
Isomers of an organic molecule may have either branched or linear structures.
3. C)
One isomer may take up more volume.
4. D)
One isomer may be more polar than the other.
5. E)
Only one isomer may bind to specific target molecules in an organism.
Answer: E
Type: MC
Topic: Concept 4.2
Skill: Knowledge/Comprehension
13) Why are hydrocarbons insoluble in water?
1. A)
The majority of their bonds are polar covalent carbon-to-hydrogen linkages.
2. B)
The majority of their bonds are nonpolar covalent carbon-to-hydrogen linkages.
3. C)
They are hydrophilic.
4. D)
They exhibit considerable molecular complexity and diversity.
5. E)
They are lighter than water.
Answer: B
Type: MC
Topic: Concept 4.2
Skill: Knowledge/Comprehension
14) How many structural isomers are possible for a substance
having the molecular formula C4H10?
1. A) 1
2. B) 2
3. C) 4
4. D) 3
5. E) 11
Answer: B
Type: MC
Topic: Concept 4.2
Skill: Application/Analysis
15) Which of the following statements correctly describes
cis-trans isomers?
1. A)
They have variations in arrangement around a double bond.
2. B)
They have an asymmetric carbon that makes them mirror images.
3. C)
They have the same chemical properties.
4. D)
They have different molecular formulas.
5. E)
Their atoms and bonds are arranged in different sequences.
Answer: A
Type: MC
Topic: Concept 4.2
Skill: Knowledge/Comprehension
16) Research indicates that ibuprofen, a drug used to relieve
inflammation and pain, is a mixture of two enantiomers, that is, molecules that
1. A)
have identical chemical formulas but differ in the branching of their carbon
skeletons.
2. B)
are mirror images of one another.
3. C)
exist in either linear chain or ring forms.
4. D)
differ in the location of their double bonds.
5. E)
differ in the arrangement of atoms around their double bonds.
Answer: B
Type: MC
Topic: Concept 4.2
Skill: Knowledge/Comprehension
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