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Bettelheim and Chang > Gases, Liquids and Solids > Flashcards

Gases, Liquids and Solids Flashcards

1
Q

When all the molecules
of a system become motionless and line up perfectly, we achieve
the greatest possible order.

A

entropy

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2
Q

Kinetic energy increases with
increasing temperature.

A

true

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3
Q

At high temperatures, molecules possess a high kinetic energy and move
so fast that the attractive forces between them are too weak to hold them
together. This situation is called the

A

gaseous state

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4
Q

At lower temperatures,
molecules move more slowly, to the point where the forces of attraction
between them become important. When the temperature is low enough, a gas
condenses to form a

A

liquid state

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5
Q

When the temperature is even lower, molecules no longer have enough
velocity to move past each other.

A

solid state

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6
Q

each molecule has a certain number of nearest neighbors, and these neighbors do not change

A

solid state

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7
Q

Typically a solid,
when heated to a sufficiently high temperature, melts and becomes a liquid.
The temperature at which this change takes place is called the

A

melting point

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8
Q

Further heating causes the temperature to rise to the point at which
the liquid boils and becomes a gas. This temperature is called the

A

boiling point

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9
Q

The force per unit area
exerted against a surface

A

pressure

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10
Q

Instrument used to measure atmospheric pressure

A

barometer

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11
Q

Pressure is most commonly measured in

A

mmHg

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12
Q

Pressure is also measure in torr, a unit named in honor of

A

Evangelista Torricelli

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13
Q

At sea level, the average pressure of the
atmosphere is

A

760 mmHg

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14
Q

A barometer is adequate for measuring the pressure of the atmosphere,
but to measure the pressure of a gas in a container, we use a simpler instrument called a

A

manometer

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15
Q

states that for a fixed mass of gas at a constant temperature, the
volume of the gas is inversely proportional to the pressure.

A

Boyle’s Law

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16
Q

P1V1 = P2V2

A

Boyle’s Law

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17
Q

states that the volume of a fixed mass of gas at a constant
pressure is directly proportional to the temperature in kelvins (K).

A

Charles’ Law

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18
Q

(V1/T1) = (V2/T2)

A

Charles’ Law

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19
Q

states that, for a fixed mass of a gas at constant volume,
the pressure is directly proportional to the temperature in kelvins (K)

A

Gay-Lussac’s Law

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20
Q

(P1/T1) = (P2/T2)

A

Gay-Lussac’s Law

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21
Q

The three gas laws can be combined and expressed by a mathematical
equation called the

A

Combined gas law

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22
Q

(P1V1/T1) = (P2V2/T2)

A

Combined gas law

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23
Q

Equal volumes
of gases at the same temperature
and pressure contain the same
number of molecules

A

Avogadro’s Law

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24
Q

Standard pressure

A

1atm

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25
Q

Standard Temperature

A

0°C

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26
Q

Avogadro’s law allows us to write a gas law that is valid not only for any
pressure, volume, and temperature, but also for any quantity of gas. This
law, called

A

ideal gas law

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27
Q

states that the total
pressure, PT, of a mixture of gases is the sum of the partial pressures of each
individual gas

A

Dalton’s law of partial pressure

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28
Q

is the pressure that the gas would exert if it were alone in the container

A

Partial pressure

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29
Q

The relationship between the observed behavior of gases and the behavior of individual gas molecules within the gas can be explained by the

A

kinetic molecular theory

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30
Q

Assumptions of kinetic molecular theory

A
  1. Gases consist of particles, either atoms or molecules, constantly moving
    through space in straight lines, in random directions, and with various
    speeds.
    2.The average kinetic energy of gas particles is proportional to the temperature in kelvins.
  2. Molecules collide with each other but the total kinetic energy of the gas sample remains the same.
  3. Gas particles have no volume.
  4. There are no attractive forces between gas particles.
  5. Molecules collide with the walls of the container, and these collisions
    constitute the pressure of the gas. The greater the number of collisions
    per unit time, the greater the pressure.
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31
Q

change from a gas to a
liquid

A

condensation

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32
Q

change from a liquid to a solid

A

solidification

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33
Q

three types of intermolecular forces

A

London
dispersion forces, dipole–dipole interactions, and hydrogen bonding

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34
Q

Extremely weak attractive forces
between atoms or molecules
caused by the electrostatic
attraction between temporary
induced dipoles

A

London dispersion forces

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35
Q

He first explained the London dispersion forces

A

Fritz London

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36
Q

The attraction
between the positive end of one dipole and the negative end of another
dipole is called a

A

dipole-dipole interaction

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37
Q

These interactions can exist
between two identical polar molecules or between two different polar molecules

A

dipole-dipole interaction

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38
Q

When
the positive end of one dipole is a hydrogen atom bonded to an O or N and the negative end of the other
dipole is an O or N atom, the attractive interaction between dipoles is particularly strong and is given a special name:

A

hydrogen bond

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39
Q

is directly related to the
strength of the intermolecular attraction between its molecules.

A

surface tension

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40
Q

An important property of liquids is their tendency to evaporate.

A

vapor pressure

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41
Q

A condition in which
two opposing physical forces are
equal

A

equilibrium

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42
Q

The pressure of a
gas in equilibrium with its liquid
form in a closed container

A

vapor pressure

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43
Q

is the temperature at which its vapor pressure is equal to the pressure of the atmosphere in contact with its surface

A

boiling point

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44
Q

The boiling point when the atmospheric pressure is 1 atm is called the

A

normal boiling point

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45
Q

the boiling point of covalent compounds depends primarily on three factor

A
  1. Intermolecular forces
  2. Number of sites for intermolecular interaction
  3. Molecular shape
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46
Q

Formation of a solid from a liquid is called

A

solidification or crystallization

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47
Q

Types of solids

A

Ionic, Molecular, Polymeric, Network and Amorphous

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48
Q

Solids made up of ions in a crystal lattice

A

Ionic

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49
Q

Solids made up of molecules in a crystal lattice

A

Molecular

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50
Q

Solids made up of giant molecules; can be crystalline, semi-crystalline or amorphous

A

Polymeric

51
Q

Solids made up of a very large number of atoms connected by covalent bonds

A

Network

52
Q

Solids made up of randomly arranged atoms or molecules

A

Amorphous

53
Q

is the fifth form of solid carbon

A

Soot

54
Q

A change from
one physical state (gas, liquid,
or solid) to another

A

Phase change

55
Q

is any part
of a system that looks uniform (homogeneous) throughout

A

phase

56
Q

The heat necessary to melt 1.0 g of
any solid is called its

A

Heat of fusion

57
Q

The heat of fusion of ice is

A

80 cal/g

58
Q

The specific heat of liquid water is

A

1 cal/g °C

59
Q

The amount of heat necessary to vaporize 1.0 g of a liquid at its normal boiling point is called its

A

heat of vaporization

60
Q

Heat of vaporization of water

A

540 cal/g

61
Q

The specific heat of steam

A

0.48 cal/g

62
Q

The data for
heating 1.0 g of water from 220°C to 120°C can be shown in a graph called

A

heating curve

63
Q

A transition from the solid state directly into the vapor state without
going through the liquid state is called

A

sublimation

64
Q

We can show all phase changes for any substance on a

A

phase diagram

65
Q

At a unique point (A) on the phase diagram, called the ______, all three phases coexist.

A

triple point

66
Q

We live at the bottom of an ocean of air whose composition by volume is roughly ___ N2, _____ O2, and ______ other gases, including CO2

A

78%, 21%, 1%

67
Q

the nature and magnitude of the attractive forces among the molecules

A

intermolecular forces

68
Q

Characteristics of gases

A
  • Gases assume the volume and shape of their containers.
  • Gases are the most compressible of the states of matter.
  • Gases will mix evenly and completely when confined to the same container.
  • Gases have much lower densities than liquids and solids.
69
Q

is defined as the change in distance with elapsed time

A

velocity

70
Q

is the change in velocity with time

A

Acceleration

71
Q

The second law of motion, formulated by Sir Isaac Newton† in the late seventeenth century, defines another term, from which the units of pressure are derived

A

Force

72
Q

SI unit of force

A

Newton

73
Q

force applied per unit area

A

Pressure

74
Q

SI unit of pressure, defined as one newton per square meter

A

Pascal

75
Q

the pressure exerted by Earth’s atmosphere

A

Atmospheric pressure

76
Q

two types of manometer

A

Closed-tube manometer and open-tube manometer

77
Q

is normally used to measure pressures below atmospheric pressure

A

closed-tube manometer

78
Q

suited for measuring pressures equal to or greater
than atmospheric pressure

A

open-tube manometer

79
Q

Nearly all barometers and most manometers use ______ as the working fluid

A

mercury

80
Q

the proportionality constant

A

gas constant

81
Q

describes the relationship among the four variables
P, V, T, and n

A

ideal gas equation

82
Q

a hypothetical gas whose pressure-volume-temperature
behavior can be completely accounted for by the ideal gas equation

A

ideal gas

83
Q

a dimensionless
quantity that expresses the ratio of the number of moles of one component to the number of moles of all components present

A

mole fraction

84
Q

SI unit of energy

A

Joule

85
Q

a number of generalizations about gas behavior

A

Kinetic molecular theory of gases

86
Q

They found kinetic molecular theory of gases

A

Maxwell, Boltzmann and others

87
Q

is the result of collisions
between molecules and the walls of their container.

A

Gas pressure

88
Q

the speed of the largest number of molecules

A

most probable speed

89
Q

an average molecular speed

A

root mean square speed

90
Q

the gradual mixing of molecules of one gas with molecules of another by virtue of their kinetic properties

A

Diffusion

91
Q

Buckminster Fuller (1895–1983) invented domes of a similar structure (he
called them geodesic domes), the C-60 substance was named

A

buckminsterfullerene or buckyball

92
Q

a homogeneous
part of the system in contact with other parts of the system but separated from them
by a well-defined boundary

A

phase

93
Q

attractive forces between molecules

A

intermolecular forces

94
Q

hold atoms together in
a molecule

A

intramolecular forces

95
Q

attractive forces between polar molecules

A

dipole-dipole forces

96
Q

attract an ion (either a cation
or an anion) and a polar molecule to each other

A

ion-dipole forces

97
Q

the separation of positive and negative charges in the
atom (or nonpolar molecule) is due to the proximity of an ion or a polar molecule

A

induced dipole

98
Q

attractive interaction between an ion and the induced dipole is called

A

ion-induced dipole interaction

99
Q

attractive interaction between a polar molecule and the induced dipole is called

A

dipole-induced dipole interaction

100
Q

At any instant it is likely that the atom has a dipole moment created
by the specific positions of the electrons. This dipole moment is called an

A

instantaneous dipole

101
Q

attractive forces that arise as a result of temporary dipoles induced in
atoms or molecules

A

dispersion forces

102
Q

A quantum mechanical interpretation of temporary dipoles was provided by

A

Fritz London

103
Q

special type of dipole-dipole interaction between the hydrogen atom in a polar bond, such as NOH, OOH, or FOH, and an electronegative O,
N, or F atom.

A

Hydrogen bond

104
Q

the amount of energy required to stretch or increase the surface of a liquid by a unit area

A

surface tension

105
Q

the intermolecular attraction between like molecules

A

cohesion

106
Q

an attraction between unlike molecules

A

adhesion

107
Q

a measure of a fluid’s resistance to flow

A

viscosity

108
Q

possesses rigid and long-range order; its atoms, molecules, or ions occupy specific positions

A

Crystalline solid

109
Q

basic repeating structural unit of a crystalline solid

A

unit cell

110
Q

Each sphere represents an atom, ion, or molecule and is called a

A

lattice point

111
Q

the number of atoms (or ions) surrounding an atom (or ion) in a crystal lattice

A

coordination number

112
Q

he most efficient arrangement
of spheres

A

closest packing

113
Q

the scattering of X rays by the units of a crystalline
solid

A

x-ray diffraction

114
Q

an optically transparent fusion product of inorganic materials that has cooled to a rigid
state without crystallizing

A

Glass

115
Q

process in which a liquid is transformed into a gas

A

Evaporation

116
Q

the rate of a forward process is exactly balanced by the rate of the reverse process, is reached when the rates of condensation and evaporation become equal

A

Dynamic equilibrium

117
Q

the vapor pressure measured when a dynamic equilibrium exists between condensation and
evaporation

A

equilibrium vapor pressure

118
Q

the energy (usually in kilojoules) required to vaporize
one mole of a liquid

A

molar heat of vaporization

119
Q

which its gas phase cannot be made to liquefy, no matter how great the applied pressure. This is also the highest temperature at which a substance can exist as a liquid

A

critical temperature

120
Q

the minimum pressure that must
be applied to bring about liquefaction at the critical temperature

A

critical pressure

121
Q

a liquid can be temporarily cooled to below its freezing point

A

supercooling

122
Q

molecules make the transition from vapor to solid directly

A

Deposition

123
Q

the energy (usually in kilojoules) required to sublime
one mole of a solid
= Hfusion + Hvaporization

A

Molar heat of sublimation

Bettelheim and Chang (7 decks)

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