Chapter 3: Water and the Fitness of the Environment
1) In a single molecule of water, two hydrogen atoms are bonded to a single
oxygen atom by :
A) hydrogen bonding b) nonpolar covalent bonds . c) polar covalent bonds
d)van der Waals interactions. E) ionic bonds.
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?
A) a covalent bond B) a hydrogen bond C) an ionic bond D) a hydrophilic bond
3) An example of a hydrogen bond is the bond between:
A) C and H in methane (CH4).
B) the H of one water molecule and the O of another water molecule.
C) Na+and Cl- in salt.
D) the two hydrogen atoms in a molecule of hydrogen gas (H2).
4) Water is able to form hydrogen bonds because
A) oxygen has a valence of 2.
B) the water molecule is shaped like a tetrahedron.
C) the bonds that hold together the atoms in a water molecule are polar covalent bonds.
D) each of the hydrogen atoms in a water molecule is weakly negative in charge.
5) What gives rise to the cohesiveness of water molecules?
A) hydrophobic interactions B) nonpolar covalent bonds C) ionic bonds D) hydrogen bonds
6) Which of the following effects is produced by the high surface tension
of water?
A) Lakes don’t freeze solid in winter, despite low temperatures.
B) A water strider can walk across the surface of a small pond.
C) Organisms resist temperature changes, although they give off heat due to chemical reactions.
D) The pH of water remains exactly neutral.
7) Which of the following takes place as an ice cube cools a drink?
A) Molecular collisions in the drink increase.
B) Kinetic energy in the drink decreases.
C) A calorie of heat energy is transferred from the ice to the water of the drink.
D) The specific heat of the water in the drink decreases.
Page 1
,8) Which of the following statements correctly defines a kilocalorie?
A) the amount of heat required to raise the temperature of 1 g of water by 1°C
B) the amount of heat required to raise the temperature of 1 kg of water by 1°F
C) the amount of heat required to raise the temperature of 1 kg of water by 1°C
D) the amount of heat required to raise the temperature of 1,000 g of water by 1°F
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?
A)1.0°C B) 2.0°C C) 20.0°C D)10.0°C
Answer: D
10) Water’s high specific heat is mainly a consequence of the
A) small size of the water molecules.
B) high specific heat of oxygen and hydrogen atoms.
C) absorption and release of heat when hydrogen bonds break and form.
D) fact that water is a poor heat conductor.
11) Which type of bond must be broken for water to vaporize?
A)ionic bonds B)nonpolar covalent bonds C)polar covalent bonds D)hydrogen bonds
12) Temperature usually increases when water condenses. Which behavior of water is most
directly responsible for this phenomenon?
A) the change in density when it condenses to form a liquid or solid
B) reactions with other atmospheric compounds
C) the release of heat by the formation of hydrogen bonds
D) the release of heat by the breaking of hydrogen bonds
13) At what temperature is water at its densest?
A)0°C B)4°C C)32°C D)100°C
14) Why does ice float in liquid water?
A) The liquid water molecules have more kinetic energy and thus support the ice.
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.
15) Based on your knowledge of the polarity of water molecules, the solute molecule is most
likely
A) positively charged. B) negatively charged. C)without charge. D) nonpolar.
16) Hydrophobic substances such as vegetable oil are
A) nonpolar substances that repel water molecules.
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, 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.
17) One mole (mol) of a substance is
A) 6.02 × 1023 molecules of the substance.
B) 1 g of the substance dissolved in 1 L of solution.
C) the largest amount of the substance that can be dissolved in 1 L of solution.
D) the molecular mass of the substance expressed in grams.
E) A and D only
18) How many molecules of glucose (C6H2O6 molecular mass =180 daltons) would be present
in one mole of glucose?
A) 24 B)23 × 10^14 C)180 × 10^14 D) 6.02 × 10^23
19) How many molecules of glycerol (C3H8O3) would be present in 1 L of a 1 M glycerol
solution?
A)1 B) 14 C)92 D)1 × 10^7 E)6.02 × 10^23
20) How many grams of the molecule in Figure would be equal to 1 mol of the molecule? (Carbon
= 12, Oxygen = 16, Hydrogen = 1)
A) 29 B) 30 C) 60 D)150
21) How many grams of the molecule in Figure 3.2 would be required to make 1 L of a 0.5 M
solution of the molecule? (Carbon = 12, Oxygen = 16, Hydrogen = 1)
A)29 B)30 C) 60 D) 150
22)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?
A) waterʹs change in density when it condenses
B) waterʹs ability to dissolve molecules in the air
C) the release of heat by the formation of hydrogen bonds
D) the absorption of heat by the breaking of hydrogen bonds
23) The bonds that are broken when water vaporizes are
A) ionic bonds.
B) hydrogen bonds between water molecules.
C) covalent bonds between atoms within water molecules.
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, 24) Which of the following is a hydrophobic material?
A) Paper B) table salt C) wax D) sugar
25) We can be sure that a mole of table sugar and a mole of vitamin C are equal in their:
A) mass in daltons. B) mass in grams. C) number of molecules. D) number of atoms. E) volume
اإلجابة الصحيحة رقم السؤال
C 1
B 2
B 3
C 4
D 5
B 6
B 7
D 8
D 9
C 10
D 11
C 12
B 13
D 14
A 15
A 16
E 17
D 18
E 19
C 20
B 21
D 22
B 23
C 24
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1) In a single molecule of water, two hydrogen atoms are bonded to a single
oxygen atom by :
A) hydrogen bonding b) nonpolar covalent bonds . c) polar covalent bonds
d)van der Waals interactions. E) ionic bonds.
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?
A) a covalent bond B) a hydrogen bond C) an ionic bond D) a hydrophilic bond
3) An example of a hydrogen bond is the bond between:
A) C and H in methane (CH4).
B) the H of one water molecule and the O of another water molecule.
C) Na+and Cl- in salt.
D) the two hydrogen atoms in a molecule of hydrogen gas (H2).
4) Water is able to form hydrogen bonds because
A) oxygen has a valence of 2.
B) the water molecule is shaped like a tetrahedron.
C) the bonds that hold together the atoms in a water molecule are polar covalent bonds.
D) each of the hydrogen atoms in a water molecule is weakly negative in charge.
5) What gives rise to the cohesiveness of water molecules?
A) hydrophobic interactions B) nonpolar covalent bonds C) ionic bonds D) hydrogen bonds
6) Which of the following effects is produced by the high surface tension
of water?
A) Lakes don’t freeze solid in winter, despite low temperatures.
B) A water strider can walk across the surface of a small pond.
C) Organisms resist temperature changes, although they give off heat due to chemical reactions.
D) The pH of water remains exactly neutral.
7) Which of the following takes place as an ice cube cools a drink?
A) Molecular collisions in the drink increase.
B) Kinetic energy in the drink decreases.
C) A calorie of heat energy is transferred from the ice to the water of the drink.
D) The specific heat of the water in the drink decreases.
Page 1
,8) Which of the following statements correctly defines a kilocalorie?
A) the amount of heat required to raise the temperature of 1 g of water by 1°C
B) the amount of heat required to raise the temperature of 1 kg of water by 1°F
C) the amount of heat required to raise the temperature of 1 kg of water by 1°C
D) the amount of heat required to raise the temperature of 1,000 g of water by 1°F
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?
A)1.0°C B) 2.0°C C) 20.0°C D)10.0°C
Answer: D
10) Water’s high specific heat is mainly a consequence of the
A) small size of the water molecules.
B) high specific heat of oxygen and hydrogen atoms.
C) absorption and release of heat when hydrogen bonds break and form.
D) fact that water is a poor heat conductor.
11) Which type of bond must be broken for water to vaporize?
A)ionic bonds B)nonpolar covalent bonds C)polar covalent bonds D)hydrogen bonds
12) Temperature usually increases when water condenses. Which behavior of water is most
directly responsible for this phenomenon?
A) the change in density when it condenses to form a liquid or solid
B) reactions with other atmospheric compounds
C) the release of heat by the formation of hydrogen bonds
D) the release of heat by the breaking of hydrogen bonds
13) At what temperature is water at its densest?
A)0°C B)4°C C)32°C D)100°C
14) Why does ice float in liquid water?
A) The liquid water molecules have more kinetic energy and thus support the ice.
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.
15) Based on your knowledge of the polarity of water molecules, the solute molecule is most
likely
A) positively charged. B) negatively charged. C)without charge. D) nonpolar.
16) Hydrophobic substances such as vegetable oil are
A) nonpolar substances that repel water molecules.
Page 2
, 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.
17) One mole (mol) of a substance is
A) 6.02 × 1023 molecules of the substance.
B) 1 g of the substance dissolved in 1 L of solution.
C) the largest amount of the substance that can be dissolved in 1 L of solution.
D) the molecular mass of the substance expressed in grams.
E) A and D only
18) How many molecules of glucose (C6H2O6 molecular mass =180 daltons) would be present
in one mole of glucose?
A) 24 B)23 × 10^14 C)180 × 10^14 D) 6.02 × 10^23
19) How many molecules of glycerol (C3H8O3) would be present in 1 L of a 1 M glycerol
solution?
A)1 B) 14 C)92 D)1 × 10^7 E)6.02 × 10^23
20) How many grams of the molecule in Figure would be equal to 1 mol of the molecule? (Carbon
= 12, Oxygen = 16, Hydrogen = 1)
A) 29 B) 30 C) 60 D)150
21) How many grams of the molecule in Figure 3.2 would be required to make 1 L of a 0.5 M
solution of the molecule? (Carbon = 12, Oxygen = 16, Hydrogen = 1)
A)29 B)30 C) 60 D) 150
22)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?
A) waterʹs change in density when it condenses
B) waterʹs ability to dissolve molecules in the air
C) the release of heat by the formation of hydrogen bonds
D) the absorption of heat by the breaking of hydrogen bonds
23) The bonds that are broken when water vaporizes are
A) ionic bonds.
B) hydrogen bonds between water molecules.
C) covalent bonds between atoms within water molecules.
Page 3
, 24) Which of the following is a hydrophobic material?
A) Paper B) table salt C) wax D) sugar
25) We can be sure that a mole of table sugar and a mole of vitamin C are equal in their:
A) mass in daltons. B) mass in grams. C) number of molecules. D) number of atoms. E) volume
اإلجابة الصحيحة رقم السؤال
C 1
B 2
B 3
C 4
D 5
B 6
B 7
D 8
D 9
C 10
D 11
C 12
B 13
D 14
A 15
A 16
E 17
D 18
E 19
C 20
B 21
D 22
B 23
C 24
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