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Chapter 3 review



Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

 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 attractions.
e.
van der Waals (aka London Dispersion) interactions.
 

 2. 

What determines the cohesiveness of water molecules?
a.
hydrophobic interactions
b.
nonpolar covalent bonds
c.
ionic attractions
d.
hydrogen bonds
e.
both A and C
 

 3. 

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.
 

 4. 

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.
 

 5. 

The formation of ice during colder weather helps moderate the seasonal transition to winter. This is mainly because
a.
the breaking of hydrogen bonds absorbs heat.
b.
the formation of hydrogen bonds releases heat.
c.
the formation of hydrogen bonds absorbs heat.
d.
there is greater evaporative cooling of lakes.
e.
ice is denser than liquid water.
 

 6. 

At what temperature is water at its densest?
a.
0°C
b.
4°C
c.
32°C
d.
100°C
e.
212°C
 

 7. 

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.
 

 8. 

How many molecules of glucose (C6H2O6 molecular mass =180 daltons) would be present in one mole of glucose?
a.
24
b.
342
c.
23 chpt03_files/i0090000.jpg 1014
d.
180 chpt03_files/i0090001.jpg 1014
e.
6.02 chpt03_files/i0090002.jpg 1023
 

 9. 

The molecular mass of glucose (C6H12O6) is 180 g. To make a 0.5 M solution of glucose, you should do which of the following?
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.
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.
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.
d.
Dissolve 0.5 g of glucose in 1 L of water.
e.
Dissolve 180 g of glucose in 1 L of water.
 

 10. 

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
 

 11. 

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
 

 12. 

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
 

 13. 

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.
 



 
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