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ap chem > unit 4 > Flashcards

unit 4 Flashcards

1
Q

gases

A

low density
indefinite shape
indefinite volume
weak IMF

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2
Q

liquids

A

high density
indefinite shape
definite volume
moderate IMF

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3
Q

solid

A

high density
definite shape
definite volume
strong IMF

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4
Q

kinetic molecular theory

A

explains the states of matter, and is based on the idea that matter is composed of tiny particles that are always in motion

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5
Q

stronger attractive forces between particles =

A

more they resist moving

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6
Q

solids melt when

A

heated

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7
Q

gases can be condensed by

A

decreasing temp
increasing pressure

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8
Q

attractive forces and boiling/melting point relation

A

stronger attractive forces = higher melting/boiling point

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9
Q

charge and attraction relation

A

larger charge = stronger attraction

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10
Q

distance and attraction relation

A

longer distance = weaker attraction

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11
Q

boiling point and IMF relation

A

higher boiling point = stronger IMF

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12
Q

unequal electron distribution gives

A

temporary polarity

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13
Q

permanent dipole adds to the

A

attractive forces between molecules

raises boiling and melting point

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14
Q

polar substances dissolve in

A

polar substances

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15
Q

non polar substances dissolve in

A

non polar substances

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16
Q

strongest type of IMF

A

hydrogen

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17
Q

ion-dipole attraction

A

ions are attracted to the dipole of polar molecules

strength determines solubility of ionic compounds in water

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18
Q

London dispersion forces are present in

A

all molecules

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19
Q

dipole-dipole forces are present in

A

polar molecules

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20
Q

Hydrogen bonding forces are present in

A

molecules with H bonded to F, O, or N

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21
Q

ion dipole forces are present in

A

mixtures of ionic compounds and polar compounds

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22
Q

surface tension

A

Property of liquids that results from the tendency of liquids to minimize their surface area

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23
Q

are molecules more or less stable than molecules in the interior

A

less

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24
Q

IMF and surface tension relation

A

stronger IMF = higher surface tension

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25
Q

temperature and surface tension relation

A

increasing temp = less suface tension

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26
Q

viscosity

A

resistance of a liquid to flow

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27
Q

IMF and viscosity relation

A

larger IMF = larger viscosity

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28
Q

IMF and viscosity relation

A

stronger IMF = higher viscosity

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29
Q

temp and viscosity relation

A

increasing temp = less viscosity

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30
Q

capillary action

A

ability of a liquid to flow up a thin tube against the influence of gravity

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31
Q

capillary action forces

A

cohesive: hold liquid molecules together

adhesive: attracts outer liquid molecules to the tube’s surface

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32
Q

when does capillary action stop?

A

until gravity counteracts the capillary action forces

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33
Q

What factors cause transitions between the solid and liquid state?

A

-temperature
-pressure
-heating/cooling

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34
Q

What factors cause transitions between the gas and liquid state?

A

-temperature
-pressure
-heating/cooling

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35
Q

Describe the relationship between the state of a substance, its temperature, and the strength of its intermolecular forces

A

solid: as temp increases, they become liquids. strongest IMF.

liquid: as temp increases, they become gases. strong IMF.

gas: lowest IMF

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36
Q

From what kinds of interactions do intermolecular forces originate?

A

interactions between charges, partial charges and temporary charges on molecules, atoms or ions

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37
Q

Why are intermolecular forces generally much weaker than bonding forces?

A

Bonding forces are the result of large charges acting over small distances

IMF are the result of smaller charges acting over large distances

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38
Q

What is the dispersion force?

A

result of fluctuations in electron distribution within molecules or atoms

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39
Q

How is the miscibility of two liquids related to their polarity?

A

Polar liquids are miscible with other polar liquids, but are not miscible with nonpolar liquids.
Nonpolar liquids are miscible with other nonpolar liquids

40
Q

what does viscosity depend on?

A

-temp
-molecular shape
-molar mass

41
Q

avg. kinetic energy and temperature proportion

42
Q

surface area and evaporation proportion

43
Q

vapor

A

gas form of a liquid

44
Q

temp and evaporation proportion

45
Q

opposite of vaporization

A

condensation

46
Q

attractive forces and evaporation relation

A

weaker attractive forces = faster rate of evaporation

47
Q

volatile

A

vaporizes easily

48
Q

nonvolatile

A

doesn’t evaporate easily

49
Q

is vaporization endothermic or exothermic?

A

endothermic

50
Q

endothermic

A

requires energy

51
Q

exothermic

A

releases energy

52
Q

is condensation endothermic or exothermic?

A

exothermic

53
Q

heat of vaporization (Dh(vap))

A

amount of heat energy required to vaporize one mole of the liquid

54
Q

DH condensation =

A

DH vaporization

55
Q

DH vap is always

56
Q

dynamic equillibrium

A

rate of vaporization = rate of condensation

57
Q

vapor pressure

A

pressure exerted by the vapor when it is in dynamic equilibrium with its liquid

58
Q

attractive forces and vapor pressure proportion

59
Q

vapor pressure and volatility proportion

60
Q

temp and vapor pressure proportion

61
Q

boiling point

A

temp where vapor pressure = external pressure

62
Q

boiling

A

vapor bubbles form in the interior of a liquid

63
Q

normal boiling point

A

temp where vapor pressure = 1 atm

64
Q

external pressure and boiling point proportion

65
Q

what happens in the process of vaporization?

A

Molecules with highest kinetic energy will break free from the surface and enter the gas phase

66
Q

what happens in condensation?

A

Some of the water molecules in the gas phase have less energy than the average and may reenter the liquid phase

67
Q

Heat of vaporization (∆Hvap)

A

amount of heat needed to vaporize 1 mole of a liquid to a gas

68
Q

why is ∆Hvap useful?

A

-calculate the amount of energy needed to vaporize a given mass of -compare volatilities of two substances

69
Q

Which evaporates more quickly; 55 mL of water in a beaker with a diameter of 4.5 cm or 55 mL of water in a dish with a diameter of 12 cm? Is the vapor pressure of the water different in the two containers?

A

The beaker with a diameter of 12 cm as there is more surface area

70
Q

How is dynamic equilibrium related to vapor pressure?

A

Vapor pressure is the pressure of a gas in dynamic equilibrium with the liquid

71
Q

What happens to a system in dynamic equilibrium when it is disturbed in some way

A

The system responds in a way that reestablishes dynamic equilibrium

72
Q

fusion

A

phase transition from solid to liquid

73
Q

is fusion endothermic or exothermic?

A

endothermic

74
Q

Heat of fusion (∆Hfus)

A

amount of energy needed to melt 1 mol of a solid

75
Q

why is Heat of fusion (∆Hfus) important?

A

can be used to calculate the amount of heat energy needed to melt or freeze a given mass of a substance

76
Q

solid structure type

A

rigid crystal structures

77
Q

solid structures are defined by:

A

-their attractive forces
-arrangement of atoms

78
Q

metal crystals structure

A

rigid structure of metal nuclei and inner electrons

Valence electrons are mobile and act to bond metal atoms with varying degrees of force

79
Q

melting points of metallic crystals depend on

A

attractive forces

80
Q

substitutional alloy

A

Metal atoms are of similar size

One type of metal atom replaces another in the metallic crystal.

One metal substitutes a similar set of attractive forces with the other metal.

Properties of the alloy are between the properties of the two metals.

81
Q

interstitial alloy

A

One of the atoms is very small compared with the other.

The small atom fills spaces between the larger atoms.

Little change in volume so the added mass increases the density.

Added attractions-alloy is stronger and harder than original metals.

82
Q

ionic crystals

A

ionic compounds that are solids with rigid crystalline structures (crystal lattices)

83
Q

what is used to break ionic crystals?

A

large amount of lattice energy

84
Q

how do ionic crystals break?

A

a disruption causes cations to line up with anions, like charges repel each other

85
Q

molecular crystals and properties

A

held together by IMF, composed of nonmetal atoms or covalent molecules

soft
low boiling points

86
Q

network crystal

A

lattice structure

atoms covalently bonded

one large molecule

continuous network of covalent bonds

high melting and boiling points

87
Q

amorphous

A

do not form crystals

no defined melting point

88
Q

Explain why some metals, such as Hg have melting points that are below room temperature

A

Hg has weaker interatomic forces than other metals and it is easier to disrupt the metallic crystal structure.

89
Q

malleability

A

ability of a metal to be molded or shaped without breaking

90
Q

ductility

A

Ability of a metal to be drawn into a wire

91
Q

lattice energy

A

amount of energy needed to separate the ions in the crystal lattice of an ionic compound

92
Q

mole/Avogadros number

A

6.02 x 10^23

93
Q

representative particle

A

atom, ion, molecule, formula units

94
Q

molar mass

A

one mole of a substance

95
Q

formula mass

A

equal to Molar mass (amu)

ap chem (11 decks)

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