Deck 11: Crystals, Ions, and Solutions

Question 1

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.

Answer 1

a colloid.

Question 2

An example of an ionic solid is

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

Answer 2

table salt.

Question 3

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.

Answer 3

increases.

Question 4

All forms of solid carbon

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

Question 5

An amorphous solid

A) has its particles arranged in a regular pattern.
B) is held together by ionic bonds.
C) does not melt at a definite temperature but softens gradually.
D) consists of nonpolar molecules.

Question 6

Which solids are the best electrical conductors?

A) covalent
B) ionic
C) molecular
D) metallic

Question 7

The extremely strong material called graphene

A) consists of molecules in the form of cages made up of 60 carbon atoms.
B) consists of carbon nanotubes.
C) is a one-atom-thick sheet of carbon atoms.
D) is a thick sheet of carbon atoms.

Question 8

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 9

An example of a covalent solid is

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

Question 10

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 11

Which solids are the best heat conductors?

A) covalent
B) ionic
C) molecular
D) metallic

Question 12

The strongest bonds are

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

Question 13

Most solids are

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

Question 14

In general molecular solids

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

Question 15

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 16

The weakest bonds are

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

Question 17

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.

Question 18

Glass is

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

Question 19

An example of a molecular solid is

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

Question 20

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 21

Ocean water is acidic mainly because of

A) dissolved carbon dioxide
B) its salt content
C) pollution by agricultural chemicals
D) pollution by industrial chemicals

Question 22

A saturated solution contains

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

Question 23

The symbol of the hydronium ion is

A) H₃O^-.
B) H₃O⁺.
C) OH^-.
D) OH⁺.

Question 24

Pure water is not

A) polar.
B) a good solvent.
C) a compound.
D) saturated.

Question 25

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 26

Dissolving an electrolyte in water results in the formation of

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

Question 27

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 28

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

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

Question 29

The symbol of the hydroxide ion is

A) H₃O^-.
B) H₃O⁺.
C) OH^-.
D) OH⁺.

Question 30

Ionic crystals dissolve only in liquids that are

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

Question 31

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 32

Reverse osmosis

A) is used to replenish the oxygen content of bodies of water.
B) causes dead zones off the mouths of rivers.
C) is used to soften hard water.
D) is used to desalinate salt water.

Question 33

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 34

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 35

An insoluble solid that results from a chemical reaction is called

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

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 chief ions in seawater are

A) H⁺ and OH^-.
B) Na⁺ and Cl^-.
C) Ca²⁺ and Mg²⁺.
D) K⁺ and SO^2-.

Question 38

The chief use of freshwater in the world is in

A) agriculture.
B) industry.
C) mining.
D) domestic applications.

Question 39

An example of a weak acid is

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

Question 40

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 41

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 42

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 43

Which of the following has the highest pH?

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

Question 44

Which of the following has the lowest pH?

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

Question 45

Pure water has a pH of

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

Question 46

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 47

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 48

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 49

The formula for ironII) hydroxide is

A) FeOH.
B) Fe₂OH.
C) FeOH)₂.
D) Fe₂OH)₂.

Question 50

Pure water does not

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

Question 51

The fundamental reaction of neutralization is

A) H⁺ + H₂O → H₃O⁺.
B) H₂O → H⁺ + OH^-.
C) H⁺ + OH^- → H₂O.
D) H₂O + H₂O → H₃O⁺ + OH^-.

Question 52

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.