Deck 11: Crystals, Ions, and Solutions

Question 1

The strongest bonds are

A)ionic.
B)covalent.
C)metallic.
D)van der Waals.

Answer 1

covalent.

Question 2

The individual particles in an ionic solid are held together as a result of

A)electron transfer between adjacent molecules.
B)electron sharing between adjacent atoms.
C)the attraction of polar molecules.
D)a sea of freely moving electrons.

Answer 2

electron transfer between adjacent molecules.

Question 3

In general molecular solids

A)have fairly low melting points.
B)are good electrical conductors.
C)are good heat conductors.
D)are insoluble.

Answer 3

have fairly low melting points.

Question 4

An example of a molecular solid is

A)ice.
B)diamond.
C)table salt.
D)tin.

Question 5

Glass is

A)amorphous.
B)crystalline.
C)covalent.
D)polar.

Question 6

The individual particles in a metal are held together as a result of

A)electron transfer between adjacent atoms.
B)electron sharing between adjacent atoms.
C)the attraction of polar molecules.
D)a sea of freely moving electrons.

Question 7

Most solids are

A)amorphous.
B)crystalline.
C)covalent.
D)polar.

Question 8

The individual particles in a covalent solid are held together as a result of

A)electron transfer between adjacent atoms.
B)electron sharing between adjacent atoms.
C)the attraction of polar molecules.
D)a gas of freely moving electrons.

Question 9

The individual particles in a molecular solid are held together as a result of

A)electron transfer between adjacent atoms.
B)electron sharing between adjacent atoms.
C)the attraction of polar molecules.
D)a sea of freely moving electrons.

Question 10

An emulsion in which tiny oil droplets are dispersed in water is an example of

A)a colloid.
B)an aerosol.
C)a saturated solution.
D)a polar liquid.

Question 11

An example of a covalent solid is

A)ice.
B)diamond.
C)table salt.
D)tin.

Question 12

The weakest bonds are

A)ionic.
B)covalent.
C)metallic.
D)van der Waals.

Question 13

An insoluble solid that results from a chemical reaction is called

A)a solute.
B)a colloid.
C)an electrolyte.
D)a precipitate.

Question 14

An example of an ionic solid is

A)ice.
B)diamond.
C)table salt.
D)tin.

Question 15

All forms of solid carbon

A)are amorphous.
B)are crystalline.
C)are held together only by covalent bonds.
D)conduct electricity well.

Question 16

With increasing temperature, the solubility of a gas in a liquid

A)decreases.
B)increases.
C)remains the same.
D)Any of these choices could be correct, depending on the particular gas and liquid.

Question 17

With increasing temperature, the solubility of a solid in a liquid

A)decreases.
B)increases.
C)remains the same.
D)Any of these choices could be correct, depending on the particular solid and liquid.

Question 18

When a supersaturated solution is disturbed,

A)it may solidify.
B)it may boil.
C)some of its solute may crystallize out of solution.
D)a precipitate may form.

Question 19

A solid whose particles are irregularly arranged with no definite pattern is said to be

A)a van der Waals solid.
B)nonpolar.
C)amorphous.
D)unsaturated.

Question 20

A saturated solution contains

A)only ions.
B)only nonpolar molecules.
C)the maximum concentration of solute.
D)the maximum concentration of solvent.

Question 21

The symbol of the hydronium ion is

A)H₃O^-.
B)H₃O⁺.
C)OH^-.
D)OH⁺.

Question 22

An example of a weak acid is

A)nitric acid.
B)acetic acid.
C)sulfuric acid.
D)hydrochloric acid.

Question 23

When dissolved in water, which one or more of the following compounds gives rise to a basic solution?

A)calcium hydroxide, Ca(OH)₂
B)washing soda, Na₂CO₃
C)methanol, CH₃OH
D)copper sulfate, CuSO₄
E)Both A and B

Question 24

The average salinity of seawater is about

A)0.1 percent.
B)1.5 percent.
C)3.5 percent.
D)10 percent.

Question 25

The chloride ion Cl^- is

A)less reactive than the chlorine molecule Cl₂.
B)more reactive than the chlorine molecule Cl₂.
C)equal in reactivity to the chlorine molecule Cl₂.
D)Any of these choices could be correct, depending on the temperature.

Question 26

Dissolving an electrolyte in water results in the formation of

A)polar molecules.
B)covalent molecules.
C)ions.
D)a precipitate.

Question 27

Which of the following would you expect to be a strong electrolyte in solution?

A)NaCl
B)AgCl
C)acetic acid
D)soap

Question 28

Bases do not

A)taste bitter.
B)turn red litmus to blue.
C)liberate H₂ when mixed with an active metal.
D)produce OH^- ions in water solution.

Question 29

The symbol of the hydroxide ion is

A)H₃O^-.
B)H₃O⁺.
C)OH^-.
D)OH⁺.

Question 30

When a strong acid is added to water,

A)more of it dissolves than in the case of a weak acid.
B)more of it dissociates than in the case of a weak acid.
C)more of it forms hydroxide ions than in the case of a weak acid.
D)less of it forms hydronium ions than in the case of a weak acid.

Question 31

Fertilizers do not contain

A)sodium.
B)potassium.
C)phosphorus.
D)nitrogen.

Question 32

A solution of carbon dioxide, CO₂, in water is

A)acidic.
B)basic.
C)neutral.
D)Any of these choices could be correct, depending on the concentration.

Question 33

Ionic crystals dissolve only in liquids that are

A)polar.
B)nonpolar.
C)saturated.
D)supersaturated.

Question 34

At room temperature and atmospheric pressure, ammonia is a

A)gas whose formula is NH₃.
B)liquid whose formula is NH₃.
C)gas whose formula is NH₄.
D)liquid whose formula is NH₄.

Question 35

Polar molecules behave as though they

A)contain tiny magnets.
B)have a positive charge at both ends.
C)have a negative charge at both ends.
D)have a positive charge at one end and a negative charge at the other.

Question 36

Acids do not

A)neutralize bases.
B)taste sour.
C)combine with active metals to give off H₂.
D)liberate OH^- ions when dissolved in water.

Question 37

The formula for iron(II) hydroxide is

A)FeOH.
B)Fe₂OH.
C)Fe(OH)₂.
D)Fe₂(OH)₂.

Question 38

A solution of ammonia, NH₃, in water is

A)acidic.
B)basic.
C)neutral.
D)Any of these choices could be correct, depending on the concentration.

Question 39

Pure acids in the liquid state consist of

A)neutral molecules.
B)H⁺ ions and neutral molecules.
C)H⁺ ions and negative ions.
D)H⁺ and OH^- ions.

Question 40

A solution of table salt, NaCl, in water is

A)acidic.
B)basic.
C)neutral.
D)Any of these choices could be correct, depending on the concentration.

Question 41

When an acid is added to a basic solution, the pH of the solution

A)increases.
B)decreases.
C)is unchanged.
D)Any of these choices could be correct, depends on the natures of the acid and base.

Question 42

Which of the following has the highest pH?

A)pure water
B)concentrated sugar solution
C)concentrated sodium hydroxide solution
D)gastric fluid

Question 43

Pure water has a pH of

A)0.
B)1.
C)7.
D)10.

Question 44

When equivalent amounts of a strong acid and a strong base react, the resulting solution is

A)acidic.
B)basic.
C)neutral.
D)pure water.

Question 45

The fundamental reaction of neutralization is

A)H⁺ + H₂O $\rarr$ H₃O⁺.
B)H₂O $\rarr$ H⁺ + OH^-.
C)H⁺ + OH^- $\rarr$ H₂O.
D)H₂O + H₂O $\rarr$ H₃O⁺ + OH^-.

Question 46

Pure water does not

A)contain H⁺ ions.
B)contain OH^- ions.
C)contain polar molecules.
D)form ionic crystals when it freezes.

Question 47

Which of the following has the lowest pH?

A)pure water
B)concentrated sugar solution
C)concentrated sodium hydroxide solution
D)gastric fluid