Slide 1 / 42
1
In a single molecule of
water, the two hydrogen
atoms are bonded to a
single oxygen atom by
A
hydrogen bonds.
B
nonpolar covalent bonds.
C
polar covalent bonds.
D
ionic bonds.
E
van der Waals interactions.
Slide 2 / 42
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
E
a hydrophobic bond
Slide 3 / 42
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).
E
Mg and Cl in MgCl2.
+
-
Slide 4 / 42
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
the oxygen atom in a water molecule
has a weak positive charge.
E
each of the hydrogen atoms in a
water molecule is weakly negative in
charge.
Slide 5 / 42
5
What determines the
cohesiveness of water
molecules?
A
hydrophobic interactions
B
nonpolar covalent bonds
C
ionic bonds
D
hydrogen bonds
E
both A and C
Slide 6 / 42
6
What do cohesion, surface
tension, and adhesion
have in common with
reference to water?
A
All increase when temperature
increases.
B
All are produced by ionic bonding.
C
All are properties related to
hydrogen bonding.
D
All have to do with nonpolar covalent
bonds.
E
C and D only
Slide 7 / 42
7
Which of the following is
possible due to 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
Water can act as a solvent.
E
The pH of water remains exactly
neutral.
Slide 8 / 42
8
Which of the following is
true when an ice cube
cools a drink?
A
Molecule 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.
E
Evaporation of the water in the drink
increases.
Slide 9 / 42
9
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.
E
inability of water to dissipate heat
into dry air.
Slide 10 / 42
10 Which bonds must be
broken for water to
vaporize?
A
ionic bonds
B
nonpolar covalent bonds
C
polar covalent bonds
D
hydrogen bonds
E
covalent bonds
Slide 11 / 42
11 Ice is lighter and floats in
water because it is a
crystalline structure in
which each water
molecule is bonded to a
maximum of four other
water molecules by which
kind of bond?
A
ionic
B
hydrogen
C
covalent
D
A and C only
E
A, B, and C
Slide 12 / 42
12 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.
E
The crystalline lattice of ice causes it
to be denser than liquid water.
Slide 13 / 42
13 Based on your knowledge
of the polarity of water
molecules, the solute
molecule in the center of
the diagram is most likely
A
positively charged.
B
negatively charged.
C
without charge.
D
hydrophobic.
E
nonpolar.
Slide 14 / 42
14 Hydrophobic substances
such as vegetable oil are
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.
E
charged molecules that hydrogenbond with water molecules.
Slide 15 / 42
15 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
t he 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
Slide 16 / 42
16 How many molecules of
glucose (C6H12O6 molecular
mass =180 amu) would be
present in one mole of
glucose?
A
24
B
342
C
23 × 1014
D
180 × 10
E
6.02 × 1023
14
Slide 17 / 42
17 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 × 107
E
6.02 × 10
23
Slide 18 / 42
18 Recall that when 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 concentration of
particles (molecules or ions)?
A
0.5 M NaCl
B
0.5 M glucose
C
1.0 M NaCl
D
1.0 M glucose
E
1.0 M MgCl2
Slide 19 / 42
19
When 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
particles (molecules or ions)?
A
1 L of 0.5 M NaCl
B
1 L 0.5 M glucose
C
1 L of 1.0 M NaCl
D
1 L of 1.0 M glucose
E
C and D only
Slide 20 / 42
20 How many grams of the
molecule in the figure
would be equal to 1 mol of
the molecule?
(Carbon = 12, Oxygen = 16,
Hydrogen = 1)
A
B
C
29
D
E
150
342
30
60
Slide 21 / 42
21 Which of the following
ionizes completely in
solution and is considered
to be a strong acid?
A
NaOH
B HCl
C NH3
D
H2CO3
E
CH3COOH
Slide 22 / 42
22 Which of the following
ionizes completely in
solution and is considered
to be a strong base?
A NaCl
B HCl
C NH3
D H2CO3
E NaOH
Slide 23 / 42
23 A given solution contains
0.0001(10-4) moles of
hydrogen ions [H+] per liter.
Which of the following best
describes this solution?
A
B
+
acidic: H acceptor
basic: H+ acceptor
+
C
acidic: H donor
D
basic: H+ donor
E
neutral
Slide 24 / 42
24 A solution contains
0.0000001(10-7) moles of
hydroxide ions [OH-] per
liter. Which of the following
best describes this
solution?
+
A
acidic: H acceptor
B
basic: H+ acceptor
+
C
acidic: H donor
D
basic: H+ donor
E
neutral
Slide 25 / 42
25 What would be the pH of a
solution with a hydroxide
ion [OH-] concentration of
10-12 M?
A
pH 2
B
pH 4
C
pH 10
D
pH 12
E
pH 14
Slide 26 / 42
26 What would be the pH of a
solution with a hydrogen ion
[H+] concentration of 10-8 M?
A
pH 2
B
pH 4
C
pH 6
D
pH 8
E
pH 10
Slide 27 / 42
27 Which of the following
solutions has the greatest
concentration of hydrogen
ions [H+]?
A
gastric juice at pH 2
B
vinegar at pH 3
C
tomato juice at pH 4
D
black coffee at pH 5
E
household bleach at pH 12
Slide 28 / 42
28 Which of the following
solutions has the greatest
concentration of hydroxide
ions [OH-]?
A
lemon juice at pH 2
B
vinegar at pH 3
C
tomato juice at pH 4
D
urine at pH 6
E
seawater at pH 8
Slide 29 / 42
29 If the pH of a solution is
decreased from 9 to 8, it
means that the
A
concentration of H+ has decreased
10 times what it was at pH 9.
B
concentration of H+ has increased 10
times what it was at pH 9.
C
concentration of OH- has increased
10 times what it was at pH 9.
D
concentration of OH- has decreased
10 times what it was at pH 9.
E
B and D are correct.
Slide 30 / 42
30 If the pH of a solution is
increased from pH 5 to pH
7, it means that the
A
concentration of H+ is 2 times greater
than what it was at pH 5.
B
concentration of H+ is 2 times less
than what it was at pH 5.
C
concentration of OH- is 100 times
greater than what it was at pH 5.
D
concentration of OH- is 100 times less
than what it was at pH 5.
E
concentration of H+ is 100 times
greater and the concentration of OHis 100 times less than what they were
at pH 5.
Slide 31 / 42
31 One liter of a solution of pH
2 has how many more
hydrogen ions (H+) than 1 L
of a solution of pH 6?
A
4 times more
B
400 times more
C
4,000 times more
D
10,000 times more
E
100,000 times more
Slide 32 / 42
32 One liter of a solution pH 9
has how many more
hydroxide ions (OH-) than 1 L
of a solution of pH 4?
A
5 times more
B
100 times more
C
1,000 times more
D
10,000 times more
E
100,000 times more
Slide 33 / 42
33 Which of the following
statements is true about
buffer solutions?
A
They maintain a constant pH when
bases are added to them but not
when acids are added to them.
B
They maintain a constant pH when
acids are added to them but not
when bases are added to them.
C
They maintain a constant pH of
exactly 7 in all living cells and
biological fluids.
D
They maintain a relatively constant
pH.
E
They are found only in living systems
and biological fluids.
Slide 34 / 42
34 Buffers are substances that
help resist shifts in pH by
A
releasing H+ in acidic solutions.
B
donating H+ to a solution when they
have been depleted.
C
releasing OH in basic solutions.
D
accepting H when they are in excess.
E
-
+
both B and D
Slide 35 / 42
35 Assume that acid rain has
lowered the pH of a
particular lake to pH 4.0.
What is the hydroxide ion
concentration of this lake?
A
1 × 10-10 mol of hydroxide ion per liter
of lake water
B
1 × 10 mol of hydroxide ion per liter
of lake water
C
10.0 M with regard to hydroxide ion
concentration
D
4.0 M with regard to hydroxide ion
concentration
E
-4
both B and D
Slide 36 / 42
36 Water's surface tension
and heat storage capacity
is accounted for by its
A
orbitals.
B
weight.
C
hydrogen bonds.
D
mass.
E
size.
Slide 37 / 42
37 What property of water is
responsible for water
transport in plants?
A
moderation of temperature
B
insulation
C
its versatility as a solvent
D
cohesion
E
its role as a buffer
Slide 38 / 42
38 When does a hydronium
ion form?
A
when two water molecules bind
B
when a water molecule gains an
hydrogen ion from another water
molecule
C
as a product of evaporation
D
when a hydrogen ion binds with a
hydroxide ion
E
when a water molecule splits in half
Slide 39 / 42
39 In a neutral solution the
concentration of
A
hydrogen ions is equal to the
concentration of hydroxide ions.
B
water molecules is less than the
concentration of hydrogen ions.
C
hydrogen ions is less than the
concentration of hydroxide ions.
D
water molecules is less than the
concentration of hydroxide ions.
E
hydrogen ions is greater than the
concentration of hydroxide ions.
Slide 40 / 42
40 For two bodies of matter in
contact, heat always flows
from
A
the body with greater heat to the one
with less heat.
B
the body of higher temperature to the
one of lower temperature.
C
the denser body to the less dense
body.
D
the body with more water to the one
with less water.
E
the larger body to the smaller body.
Slide 41 / 42
41 Which of the following is
an example of a
hydrophobic material?
A
paper
B
table salt
C
wax
D
sugar
E
pasta
Slide 42 / 42
42 Acid precipitation has
lowered the pH of a
particular lake to 4.0. What
is the hydrogen ion
concentration of the lake?
A
4.0 M
B
10
C
10 M
D
104 M
E
4%
-10
M
-4