1 In a single molecule of water, the two hydrogen atoms are bonded - - PowerPoint PPT Presentation

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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

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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

• f hydrogen gas (H2).

E

Mg+and Cl- in MgCl2.

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4 Water is able to form hydrogen bonds because

A

• xygen 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.

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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

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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

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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.

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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

• f the drink.

D The specific heat of the water in the drink decreases. E Evaporation of the water in the drink increases.

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9 Water's high specific heat is mainly a consequence

• f 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.

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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

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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

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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.

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13 Based on your knowledge

• f 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.

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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 hydrogen- bond with water molecules.

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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

• f 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

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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 × 1014

E

6.02 × 1023

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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 × 1023

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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

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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

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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

29

B

30 C 60

D

150

E

342

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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

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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

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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

acidic: H+ acceptor

B

basic: H+ acceptor

C acidic: H+ donor D basic: H+ donor

E neutral

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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

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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

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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

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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

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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

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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.

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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 OH- is 100 times less than what they were at pH 5.

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31 One liter of a solution of pH 2 has how many more hydrogen ions (H+) than 1 L

• f 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

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32 One liter of a solution pH 9 has how many more hydroxide ions (OH-) than 1 L

• f 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

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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.

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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

• f lake water

B

1 × 10-4 mol of hydroxide ion per liter

• f lake water

C 10.0 M with regard to hydroxide ion concentration D 4.0 M with regard to hydroxide ion concentration

E

both B and D

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36 Water's surface tension and heat storage capacity is accounted for by its

A

• rbitals.

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

• ne 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

10-10 M

C

10-4 M

D 104 M

E

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