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Chem > Ch 13 Section 1 > Flashcards

Ch 13 Section 1 Flashcards

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1
Q

solid compounds can be

A

ionic or molecular

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2
Q

in an ionic solid, a crystal structure is made up of .. held together by …

A

charged particles; ionic attractions

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3
Q

in a molecular solid, molecules are composed of

A

covalently bonded atoms

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4
Q

the solid is held togher by …, … forces

A

noncovalent; intermolecular

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5
Q

when they dissolve in water, ionic compounds and molecular compounds behave

A

differently

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6
Q

when a compound that is made of ions dissolves in water, the

A

ions separate from one another

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7
Q

this separation of ions that occurs when an ionic compound dissolves is called

A

dissociation

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8
Q

assuming 100% dissociation, a solution that contains 1 mol of sodium chloride contains .. of Na+ ions and … of Cl- ions

A

1 mol; 1 mol

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9
Q

a solution that contains 1 mol of calcium chloride contains .. of Ca2+ ions and … of Cl- ions

A

1 mol; 2 mol

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10
Q

although no ionic compound is completely insoluble, compounds of very low solubility can be considered … for most …

A

insoluble; practical purposes

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11
Q

it is difficult to write solubility rules that cover all

A

possible conditions

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12
Q

most sodium compounds are

A

soluble

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13
Q

most phosphates are

A

insoluble

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14
Q

dissociation equations cannot be written for

A

insoluble compounds

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15
Q

if the mixing results in a combination of ions that forms an insoluble compound, a … reaction and … will occur

A

double-displacement; precipitation

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16
Q

precipitation occurs when the attraction between the ions is greater than the attraction between the

A

ions and surrounding water molecules

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17
Q

to decide whether a precipitate can form, you must know the

A

solubilities of these two compounds

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18
Q

reactions of ions in aqueous solution are usually represented by … rather than…

A

net ionic equations; formula equations

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19
Q

a net ionic equation includes only those compounds and ions that undergo a

A

chemical change in a reaction in an aqueous solution

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20
Q

to write a net ionic equation, you first convert the chemical equation into an

A

overall ionic equation

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21
Q

all soluble ionic compounds are shown as

A

dissociated ions in solution

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22
Q

the precipitates are shown as

A

solids

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23
Q

ions that do not take part in a chemical reaction and are found in solution both before and after the reaction are

A

spectator ions

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24
Q

to convert an ionic equation into a net ionic equation, the … are … on both sides of the equation

A

spectator ions; canceled

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25
Q

some molecular compounds can also form

A

ions in solution (polar compounds)

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26
Q

ions are formed from solute molecules by the action of the solvent in a process called

A

ionization

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27
Q

the more general meaning of ionization is the creation of

A

ions where there were none

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28
Q

when n ionic compound dissolves, the ions that were already present

A

separate from one another

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29
Q

when a molecular compound dissolves and ionizes in a polar solvent, ions are formed where

A

non existed in the undissolved compound

30
Q

like all ions in aqueous solution, the ions formed by such a molecular solute are

A

hydrated

31
Q

the energy released as heat during the hydration of the ions provides the energy needed to

A

break the covalent bonds

32
Q

the extent to which a solute ionizes in solution depends on the strength of the bonds within the .. and the strength of attraction between the …

A

molecules of the solute; solute and solvent molecules

33
Q

if the strength of a bond within the solute molecule is weaker than the attractive forces of the solvent molecules, then the covalent bond of the solute … and the …

A

breaks; molecule is separated into ions

34
Q

HCl is a molecular compound that

A

ionizes in aqueous solution

35
Q

the attraction between a polar HCL molecule and the mpolar water molecules is strong enough to break the HCL bond, forming

A

hydrogen and chloride ions

36
Q

many molecular compounds contain a hydrogen atom bonded by a

A

polar covalent bon d

37
Q

some of these compounds ionize in an aqueous solution to release

A

H+

38
Q

the H+ ion attracts other molecules or ions so strongly that it does not normally

A

exist alone

39
Q

the ionization of hydrgoen chloride in water is better described a a chemical reaction in which a proton is transferred directly from HCl to awater molecule, where it becomes

A

covalently bonded to oxygen and forms H3O+

40
Q

the H3O+ ion is known as the

A

hydronium ion

41
Q

the reaction of the H+ ion to form the hydronium ion produces much of the energy needed to

A

ionize a molecular solute

42
Q

substances that yield ions and conduct an electric current in solution are

A

electroylytes

43
Q

substances that do not yield ions and do not conduct an electric current in solution are

A

nonelectrolytes

44
Q

the hydrogen halides are all molecular compounds with single

A

polar-covalent bonds

45
Q

all hydrogen halides are gases, all are very solubler in water, and all are

A

electrolytes

46
Q

HCl, hydrogen bromide, and HI strongly conduct an

A

electric current in an aqueous solution

47
Q

however, hydrogen fluoride only weakly conducts an electric current at the

A

same concentration

48
Q

the strength with which substances conduct an electric current is related to their

A

ability to form ions in solution

49
Q

HCL, hydrogen bromide, and hydrogen iodide are 100% ionized in

A

dilute aqueous solution

50
Q

a strong electrolyte is any compound whose dilute aqueous solutions

A

conduct electricity well

51
Q

the conductivity of strong electrolytes is due to the presence of all or almost all of the dissolved

A

compound in the form of ions

52
Q

HCL, hydrogen bromide, and HI are all

A

acids in aqueous solution

53
Q

these acids, several other acids, and all soluble ionic compounds are

A

strong electrolytes

54
Q

the distinguishing feature of strong electrolytes is that to whatever extent they dissolve in water, they

A

yield only ions

55
Q

for example, some strong electrolytes, such as NaCL, may be highly soluble in water and form

A

ions in solution

56
Q

others may not dissolve much, but the amount that does dissolve exists solely as

A

ions in solution

57
Q

some molecular compounds form aqueous solutions that contain not only dissolved ions but also some dissolved molecules that are not

A

ionized

58
Q

HF dissolves in water to give an acidic solution known as

A

hydrofluoric acid

59
Q

However, the HF bond is much stronger than the bonds between

A

hydrogen and other halogens

60
Q

when HF dissolves, some molecules

A

ionize

61
Q

but the reverse reaction–the transfer of H+ ions back to F- ions to form hydrogen fluoride molecules–

A

also takes place

62
Q

hydrogen fluoride is an example of a

A

weak electrolyte

63
Q

a weak electrolyte is any compound whose dilute aquous solutions conduct

A

electricity poorly

64
Q

the poor conductivity of weak electrolytes is due to the presence of a small amount of the

A

dissolved compound in the form of ions

65
Q

this is in contrast to a nonelectrolyte which dissolves but does not produce any

A

ions in solution

66
Q

another example of a weak electolyte is CH3COOH,

A

acetic acid

67
Q

the description of an electrolyte as strong or weak must not be confused with the description of a solution as

A

concentrated or dilute

68
Q

strong and weak electolytes differ in the degree of

A

ionization or dissociation

69
Q

concentrated and dilute solutions differ in the amount of

A

solute dissolved in a given quantity of a solvent

70
Q

hydrochloric acid is always a

A

strong electrolyte

71
Q

acetic acid is always considered a

A

weak electrolyte

Chem (54 decks)

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