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KLowe Chemistry And Physics Larmon > States Of Matter And Changes Of State > Flashcards

States Of Matter And Changes Of State Flashcards

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1
Q

Gases are well described by ___

A

Gas laws—no such laws exist for solids or liquids

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2
Q

Kinetic-molecular theory of matter attempts to describe…

A

All states of matter and conversion between states

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3
Q

Solids have a definite ___ and ___

A

Volume and shape

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4
Q

Molecules of solids are ___

A

Closely packed together

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5
Q

What holds molecules together in solids?

A

Intermolecular forces

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6
Q

Liquids have definite ___ but no definite ___

A

Definite volume, no definite shape

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7
Q

Liquids have the ability to ___

A

Flow

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8
Q

Molecules in liquids are ___

A

Very close together, but can flow past each other

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9
Q

Intermolecular forces of liquids are strong enough to ___; not strong enough to ___

A

Strong enough to hold molecules in a condensed phase; not strong enough to prevent molecules from sliding past each other

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10
Q

Gases have neither ___ nor ___

A

No definite shape or definite volume

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11
Q

A gaseous sample will expand to ___

A

Fill the available space

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12
Q

Intermolecular forces are ___ between gas molecules

A

Essentially zero

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13
Q

Transitions between states of matter:

A
  • Melting (S-L)
  • Freezing (L-S)
  • Vaporization (L-G)
  • Condensation (G-L)
  • Deposition (G-S)
  • Sublimation (S-G)
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14
Q

Deposition

A

Gas to solid

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15
Q

Sublimation

A

Solid to gas

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16
Q

What are intermolecular forces?

A

Chemical bonds hold atoms in molecules

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17
Q

Intermolecular forces determine how molecules ___

A

Interact

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18
Q

Intermolecular forces most directly impact ___

A

The macroscopic properties of a sample

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19
Q

Repulsion of intermolecular forces

A

Molecules, atoms, and oppositely charged ions are attracted to each other, but not too close

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20
Q

Intermolecular forces are ___ in nature

A

Electrostatic

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21
Q

Coulomb’s Law

A

States that intermolecular forces arise because of the attraction of opposite charges

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22
Q

The driving force in the formation of chemical bonds of all types is the ___

A

Octet rule

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23
Q

Octet rule

A

Atoms tend to add, remove, or share electrons so as to wind up with eight valence electrons

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24
Q

Valence electrons

A

Electrons in the highest energy, or valence shell

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25
Q

Noble gases each have a ___ valence shell

A

Filled, containing 8 electrons; located in group 8A

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26
Q

Ionic compounds are formed between ___ and ___

A

Metals and non metals

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27
Q

Metals don’t ___ their electrons very strongly; they are good ___; tend to form ___

A

Don’t hold onto their electrons very strongly; this is why they are good electrical conductors; tend to form cations

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28
Q

Nonmetals are much better at ___ electrons; tend to form ___

A

Attracting electrons; tend to form anions

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29
Q

Ionic bond

A

Results from coulombic attraction between oppositely charged ions

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30
Q

In the solid state, oppositely charged ions settle into a ___, in which every cation is attracted to every anion

A

Highly organized crystalline lattice

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31
Q

Ionic bonds are generally stronger than ___

A

Covalent bonds

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32
Q

Ionic compounds are (almost) always ___ under normal conditions

A

Solids

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33
Q

Example of an ionic compound:

A

NaCl

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34
Q

Valence bond theory—a covalent bond results from ___

A

Overlap of two electron clouds, electron sharing

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35
Q

Valence bond theory—electron is bound to the ___ because the negatively charged electron is attracted to the positively charged nucleus by Coulomb’s Law

A

Nucleus

This allows the electron on atom 1 to spend time around atom 2’s nucleus, and vice versa

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36
Q

VESPR Theory

A

The intermolecular forces that operate between the molecules in a sample, all of which are caused by how electrons are arranged in the molecule

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37
Q

Non-polar bond

A

If two atoms of identical electronegativity are bonded together

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38
Q

Polar bond

A

If two atoms of different electronegativity are bonded together; the electrons spend more time around the more electronegative atom; this creates partial charges

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39
Q

The greater the difference in electronegativity between two atoms, the more ___ the bond

A

Polar

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40
Q

Intermolecular forces are attractive forces between ___ or ___ or ___

A

Molecules or atoms or ions

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41
Q

Intermolecular forces are immensely important because these forces hold…

A

DNA molecules in a helix and are the mechanism for DNA transcription

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42
Q

Three main varieties of IM forces:

A
  • Dipolar
  • Hydrogen bonding
  • London forces
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43
Q

Dipole-dipole attraction

A

This is the attraction between the opposite (partial) charges of polar molecules

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44
Q

Dipolar attractions occur only between

A

Polar molecules

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45
Q

Hydrogen bonding

A

Hydrogen bonds

46
Q

London forces are generally the ___ of the three intermolecular forces

A

Weakest

47
Q

All common matter experiences ___

A

London forces

48
Q

A London force is the result of…

A

An instantaneous dipole that is created wherever electrons in a molecule are unevenly distributed

49
Q

___ molecules show more London forces because ___ molecules have more ___

A

Larger molecules because large molecules have more electrons

50
Q

London forces are AKA

A

Van der waals forces

51
Q

More intermolecular forces mean— ___ boiling and melting points; ___ heats of fusion and vaporization; ___ vapor pressure; ___ viscous liquids

A

Higher boiling and melting points; higher heats of fusion and vaporization; lower vapor pressure; more viscous liquids

52
Q

IM forces also affect ___

A

Solubility—“like dissolves like”

53
Q

Substances with greater intermolecular attractions have ___ surface tensions

A

Greater

54
Q

What is surface tension?

A

Molecules in the liquid state are attracted to all neighboring molecules by intermolecular forces

A molecule near the surface experiences attractive forces to all of the surrounding surface molecules and with the molecules below it in the liquid

Unbalanced forces create a “skin” on the surface of a liquid

The attractive strength of this skin is called the surface tension

55
Q

LaPlace’s law—surface tension on a blood vessel wall will depend on the ___ of the vessel

A

Radius

56
Q

LaPlace’s Law—the tension on the surface of the blood vessel is directly proportional to the ___ of the vessel

A

Radius

57
Q

Aneurysms

A

Spherical

Represent a dangerous physical means for lowering the surface tension on a blood vessel

58
Q

Tension for cylinders (LaPlace’s Law)

A

T = Pr

T = wall tension, P = pressure of fluid within the cylinder, r = radius

59
Q

Tension for spheres (LaPlace’s Law)

A

T = Pr/2

60
Q

Surfactants improve a solvent’s ability to be a solvent by reducing the ___

A

Surface tension of the solvent

61
Q

Surfactant =

A

Surface active agent; commonly known as soaps or detergents

62
Q

Soaps are derived directly from ___ or ___ through a chemical process called

A

Fats or oils (triglycerides) through a chemical process called saponification

63
Q

A triglyceride is a triester derived from ___ and three ___

A

Glycerin and 3 fatty acids

64
Q

A fatty acid is a long-chained carboxylic acid having ___ to ___ carbon atoms

A

12 to 18

65
Q

Heating a fat or oil with excess sodium hydroxide gives 3 moles of a ___ plus 1 mole of ___

A

3 moles of a fatty acid salt, plus 1 mole of glycerin

66
Q

A soap is the ___

A

Salt of a fatty acid

67
Q

Detergent

A

Chemically synthesized, most commonly from soaps

Molecular structure can be tweaked to optimize the physical properties of the detergent

Can be positively or negatively charged, or uncharged

68
Q

Surfactant molecules stick their polar heads onto ___ while their greasy tails ___

A

Polar heads onto water; greasy tails stick out of the surface of the water

69
Q

Bilayer

A

Basic structure of cell membranes

Tails of surfactant molecules can dissolve in each other to form a double layer

Non polar tails interact with each other, with the polar heads on the outside interacting with the water molecules

70
Q

Micelles

A

Tails can dissolve in each other forming a sphere; this creates a non-polar micro environment in the water

71
Q

Viscosity is a measure of…

A

A fluid’s resistance to flow

72
Q

Viscosity increases with ___

A

Increasing intermolecular forces

73
Q

Substances having greater intermolecular forces have ___ vapor pressures

A

Lower

74
Q

What is vapor pressure?

A

The most energetic molecules in a liquid have sufficient kinetic energy to break intermolecular forces and escape into the gas phase; once the molecules are free as gases, they exert a pressure, known as the vapor pressure

75
Q

Vapor pressure and volatility of a liquid increases with ___ temperature

A

Increasing temperature

76
Q

At the surface of a liquid, the most energetic molecules can escape from the IM forces into the ___ phase

A

Gas

77
Q

Gas molecules near the surface of a liquid can be captured by IM forces into the ___ state

A

Liquid

78
Q

When there is a balance between vaporization and condensation, a state of ___ exists

A

Dynamic equilibrium

79
Q

Volatility is the tendency of a liquid to ___

A

Evaporate

80
Q

Does a more volatile liquid have a higher or lower vapor pressure?

A

Higher vapor pressure

81
Q

Does a more volatile liquid have a higher or lower boiling point?

A

Lower boiling point

82
Q

Boltzmann distribution

A

Explains why vapor pressure increases with increasing temperature

83
Q

Vapor pressures at 200C of common inhalational anesthetics—isoflurane

A

239 mm Hg

84
Q

Enflurane

A

175 mm Hg

85
Q

Halothane

A

243 mm Hg

86
Q

Desflurane

A

669 mm Hg

87
Q

Sevoflurane

A

157 mm Hg

88
Q

Solid to liquid

A

Melting

89
Q

Liquid to solid

A

Freezing

90
Q

Liquid to gas

A

Vaporization

91
Q

Gas to liquid

A

Condensation

92
Q

Solid to gas

A

Sublimation

93
Q

Gas to solid

A

Deposition

94
Q

Boiling point

A

The temperature at which the vapor pressure of a liquid equals the ambient pressure

95
Q

The normal boiling point is the temperature at which the vapor pressure of a liquid equals exactly ___

A

760 mm Hg

96
Q

Compounds with more intermolecular forces have ___ boiling points

A

Higher

97
Q

Molecules in the liquid state have sufficient intermolecular attractions to keep them from flying away from each other into the ___

A

Gas state

98
Q

Compounds with more intermolecular forces have ___ melting temperatures

A

Higher

99
Q

Melting point

A

The temperature at which the solid state reversibly passes into the liquid state

100
Q

Solid state is characterized by…

A

Definite shape and volume, which is due to strong intermolecular forces that lock the component molecules into a crystalline array

101
Q

Liquid state

A

Component molecules have sufficient intermolecular attractions to keep them from flying away from each other into the gas state, but the intermolecular forces are not strong enough to prevent the molecules from sliding around past each other

102
Q

Molar enthalpy of vaporization

A

The heat required to convert 1 mole of a liquid to a gas at its normal boiling point

103
Q

The molar enthalpy of vaporization is inherently ___, representing an amount of energy that must be added to the sample in order for the phase transition to occur

A

Endothermic

104
Q

Molar enthalpy of vaporization represents the energy needed to ___ intermolecular forces and allow molecules to escape into the ___ phase

A

Break intermolecular forces; allow molecules to escape into the gas phase

105
Q

Molar enthalpy of fusion

A

The heat necessary to convert 1 mole of a solid into a liquid at its normal melting point

106
Q

Fusion is an inherently ___ process

A

Endothermic

107
Q

Units for molar enthalpy of fusion

A

KJ/mole

108
Q

The heat of fusion represents the amount of energy necessary to overcome the intermolecular forces to the point that the molecules can start to ___

A

Move around each other

109
Q

A phase diagram shows combined effects of ___ and ___ on the state of matter

A

Temperature and pressure

110
Q

3 key points of phase diagrams:

A
  • Equilibrium lines between states
  • Triple point
  • Critical point

KLowe Chemistry And Physics Larmon (11 decks)

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