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AP Chemistry > Chapter 11: Liquids and Solids > Flashcards

Chapter 11: Liquids and Solids Flashcards

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1
Q

liquids and solids are …, in which matter occupies a large fraction of the …, causing the characteristic high … and low …

A

condensed states; sample volume; densities; compressibilities

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2
Q

solids and liquids are held together by

A

intermolecular forces

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3
Q

intramolecular forces are chemical bonds that hold

A

atoms and ions together in compounds

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4
Q

intermolecular forces affect the behavior of substances only when the molecules are

A

quite close together

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5
Q

the physical state of any sample of matter depends on the …. and the average … of the molecules

A

strengths of the intermolecular attractions; kinetic energy

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6
Q

the strengths of intermolecular attractions do not change much with

A

temperature

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7
Q

at any instant, some molecules have kinetic energies greater than the … and others have kinetic energies ..

A

average; less than the average

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8
Q

for gases energy of attraction is … kinetic energy of molecules

A
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9
Q

for liquids, energy of attraction is …. kinetic energy of molecules

A

=

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10
Q

for solids, energy of attraction is …. kinetic energy of molecules

A

> >

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11
Q

at a given temp, a solid has … intermolecular attractions than a liquid, whereas a liquid has … intermoleular attractions than a gas

A

stronger; stronger

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12
Q

the concept of distribution of energies also applies to molecules in the liquid state and is an important factor in evaporation, the conversion of molecules from the

A

liquid to the gas phase

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13
Q

to escape from a liquid, a molecule must have a kinetic energy that is sufficient to …

A

overcome the forces of attraction from the other molecules

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14
Q

for any temperature at which the liquid state is stable, only a small fraction of the moleules possess enough energy to evaporate, or vaporize– that is, have enough energy to

A

escape from the surface of the liquid

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15
Q

rate of evaporation depends on the

A

temperature of the liquid

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16
Q

the greater the temp, the greater the fraction of molecules that have …, and the faster the …

A

enough en ergy to evaorate; evaporation

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17
Q

condensation: conversion of a

A

gas to a liquid

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18
Q

the greater the number of gaseous molecules, the greater the rate of

A

condensation

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19
Q

when the rate of condensation equals the rate of evaporation, the pressure in the vessel …, the constant pressure that is achieved is called the … of the liquid

A

no longer changes; vapor pressure

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20
Q

a state of dynamic equilibrium is one in which two opposing changes occur

A

at equal rates (no net change is apparent)

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21
Q

at equilibrium, both … continue to occur

A

opposing processes

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22
Q

vapor pressure changes as the … changes

A

temperature

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23
Q

rate of evaporation and the equilibrium vapor presure … with increasing temperature

A

increase

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24
Q

boiling point of a liquid is the temperature at which the vapor pressure is

A

equal to the surrounding pressure

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25
Q

vapor pressure is the pressure at which the rate of

A

evaporation equals the rate of condensation

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26
Q

the boiling point is a function of the surrounding pressure– at lower surrounding pressures, a lower temperature is needed for the vapor pressure to

A

equal that pressure

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27
Q

the normal boiling point of a liquid is the temperature at which its equilibrium vapor pressure

A

equals one atmosphere

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28
Q

the stronger the intermolecular forces of attraction, the … the boiling point

A

greater

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29
Q

vaporization is an … process

A

endothermic

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30
Q

enthalpy of vaporization is the enthalpy change that accompanies the conversion of one mole of a substance from the

A

liquid state to the gaseous state at constant temp.

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31
Q

the higher the vapor pressure at a given temperature, the … the intermolecular forces

A

weaker

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32
Q

enthalpy of vaporization is

A

endothermic

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33
Q

the larger the enthalpy of vaporization, the … the intermolecular forces

A

greater

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34
Q

the enthalpy of vaporization of a liquid is the energy needed to separate the molecules by

A

overcoming the intermolecular attractions

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35
Q

the vapor pressure and rate of evaporation are low and the boiling point is high for a liquid with … intermolecular forces

A

strong

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36
Q

critical temperature is the maximum temperature at which a substance can

A

exist in the liquid state

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37
Q

above its critical temp., no matter how high the applied pressure, a substance has only

A

one phase that completely occupies the volume of the vessel.

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38
Q

critical pressure is the minimum pressure needed to … at the critical temperature

A

liquefy the substance

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39
Q

the single phase that exists above the critical temp and pressure is sometimes called a

A

supercritical fluid

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40
Q

the melting point of a substance is the temperature at which the

A

solid and liquid phases are in equilibrium

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41
Q

normal melting point is the temperature at which the solid and liquid phases are in equilibrium when the pressure is

A

1 atm

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42
Q

enhalpy of fusion is the enthalpy change that occurs when one mole of solid is converted to

A

liquid at a constant temperature

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43
Q

fusion is

A

endothermic

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44
Q

for any substance, the enthalpy of fusion is considerably … than the enthalpy of vaporization

A

smaller

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45
Q

the energy required for melting overcomes some of the intermolecular attractions, giving the molecules greater freedom of motion but much less freedom than they

A

would have in the vapor phase

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46
Q

solidification (freezing) is reverse of fusion, so it has the same … but different ..

A

magnitude; sign

47
Q

supercooling is the cooling of liquid below its

A

melting pt without forming solid

48
Q

a supercooled liquid is an … state, and stirring or adding a small crystal of the substance causes the rapid …

A

unstable; formation of the solid

49
Q

solid too has

A

vapor pressure

50
Q

sublimation is the direct conversion of a substance from

A

the solid state to the gaseous state

51
Q

the reverse of sublimation, deposition, is the conversion of the gas

A

directly to the solid state

52
Q

the opposing hanges of sublimation and deposiition lead to a state of dynamic equilibrium at an applied pressure equal to the

A

vapor pressure of the solid

53
Q

enthalpy of sublimation is the enthalpy change for conversion of one mole of a solid to the

A

gaseous state

54
Q

sublimation is

A

endothermic

55
Q

enthalpy of sublimation=

A

enthalpy of fusion + enthalpy of vaporization

56
Q

a phase diagram is a graph of … versus … that shows the region of stability for each of the …

A

pressure; temperature; physical states

57
Q

three line segments show the combination of temp and pressure at which any two phases exist in

A

equilibrium

58
Q

the line that separates the liquid from the gas is the

A

vapor pressure curve

59
Q

the triple point is a unique combination of temperature and pressure at which

A

all three phases are in a dynamic equilibrium

60
Q

the liquid-gas equilibrium line ends at the …, which indicates the … and …

A

critical point; critical temp; critical pressure

61
Q

if two phases are in equilibrium and the pressure increases, a decrease in volume results by formation of the

A

denser phase

62
Q

all intermolecular attractions depend on …, the attraction between charges of …

A

electrostatic interactions; opposite sign

63
Q

dipole-dipole attractions are the intermolecular forces that arise from the electrostatic attractions between the

A

molecular dipoles

64
Q

in general, the larger the dipole moment of a molecule, the

A

stronger the dipole-dipole attraction

65
Q

dipoles exist due to the partial positive and negative charges on atoms produced by

A

unequal sharing of electrons

66
Q

electrical charges or polar molecules close to a non-polar molecule can distort the nonpolar molecule’s electron cloud and produce an

A

induced dipole moment

67
Q

the intermolelcular force that exists between a permanent and induced dipole is called

A

dipole-induced dipole attraction

68
Q

an instantaneous dipole is the result of an unequal … within a molecule, caused by the … of the electrons

A

charge distribution; motion

69
Q

the very small charges of an instantaeous dipole in one nonpolar molecule can induce a dipole in a

A

nearby nonpolar molecule

70
Q

london dispersion forces arise from the attractions between .. and …

A

instantaneous and induced dipoles

71
Q

polarizabilityrefers to the ease with which the electron cloud of a molecule can be

A

distorted by a nearby charge

72
Q

the greater the polarizability, the greater the … and the magnitude of the …

A

induced dipole; electrostatic attraction

73
Q

because molar mass increases with the size of the electron cloud, the strengths of intermolecular attractios usually increase with

A

increasing molar masses in related series of substances

74
Q

london dispersion forces contribute to the attractions between

A

all molecules

75
Q

een in molecules with dipole moments, most of the energy of intermolecular attractio arises from the

A

dispersion forces

76
Q

van der Waals forces: collective term used to describe

A

dipole-dipole
dipole-induced dipole
instantaneous diple- induced dipole internations

77
Q

london forces increase with the … of the molecules

A

size

78
Q

for related series of molecules, london forces increase going

A

down any group in the periodic table

79
Q

hydrogen bonding occurs between a hydrogen atom that is bonded to a …. and a second …, …, or … on a neighboring atom

A

small, highly electronegative atom; nitrogen, oxygen, fluorine

80
Q

relative strength of forces (strongest on top)

A

covalent bonds
hydrogen bonding
dipole-dipole interactions
london forces

81
Q

small drops of liquids adopt a … due to intermolecular forces

A

spherical shape

82
Q

increasing the surface area of a liquid requires an expenditure of energy, because the number of surface molecules …, ad each molecule on the surface hs fewer … that attract it

A

increases; neighboring molecules

83
Q

surface tension is the energy required to increse the

A

surface area of a liquid

84
Q

surface tension is expressed in units of

A

J/m^2

85
Q

the greater the intermolcular forces, the greater the

A

surface tension

86
Q

a molecule in the interiro of a liquid is attrated by surrounding molecules

A

equally in all directions

87
Q

a molecule at the surface of a liquid has unbalanced forces of attraction toward the …, resulting in …

A

interior of the liquid; surface tension

88
Q

capillary action is the rising of water in a small diameter column against the forces of … de to intermolecular forces

A

gravity

89
Q

cohesion: is the attraction of molecules for

A

other molecules of the same substance

90
Q

adhesion: the attraction that molecules of one substance exert on

A

those of different substance

91
Q

the direction of curvature for the meniscus depends on the relative strengths of the

A

adhesive and cohesive forces

92
Q

viscosity is the resistance of a fluid to

A

flow

93
Q

the stronger the intermolecular forces between the molecules in a liquid, the more

A

viscous the liquid becomes

94
Q

viscosity is also infleunced by

A

structure, size, and shape of molecules

95
Q

solids can be … or …

A

crystalline; amorphous

96
Q

crystalline solids have units that are arraned in a very

A

regular repeating pattern

97
Q

crystalline solids are classified according to the types of … that hold the units together

A

intermolecular forces

98
Q

an amorphous solid lacks the order of

A

crystalline solids

99
Q

many amorphous solids consist of large molecules that cause the liquid state to become

A

viscous as temperature is reduced

100
Q

molecular solids are held together by

A

van der waals forces and/or hydrogen bonds

101
Q

physical properties of molecular solids vary considerably depedning on the strength of

A

intermolecular interactions

102
Q

covalent bonds hold the atoms together in the

A

molecules of molecular solids

103
Q

molecular solids are usually … substances with melting points <

A

soft; 300 C

104
Q

in a covalent network solid, all of the satoms are hld in place by

A

covalent bonds

105
Q

allotropes of carbon:

A

diamond (sp3), graphite (sp2)

106
Q

alltotropes: term refers to two or more molecules/crystalline forms of an element in the same physical state that exhibit

A

different physical and chemical properties

107
Q

many … are also covalent network solids

A

minerals

108
Q

ionic solids consist of oppositely charged … held together by … that are very strong

A

ions; electrostatic attractions

109
Q

ionic compounds generally have high … and are relatively … and …

A

melting points; hard; brittle

110
Q

metallic solids are solids formed by

A

metal atoms

111
Q

the metallic elements form crystalline solids that exhibit many unique properties such as

A

high thermal conductivity, good electrical conductivity, metallic luster

112
Q

a special kind of bonding called … accounts for properties of metallic soldids

A

metallic bonding

113
Q

strength of attraction in metallic solids varies greatly so there are a wide range of … for metallic substances

A

melting and boiling points

114
Q

“electron sea” model used to describe metallic bonding: a sea of electrons with

A

metal ions embedded in it

AP Chemistry (24 decks)

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