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Chem 101 > Chapter 13 > Flashcards

Chapter 13 Flashcards

1
Q

Adhesive force

A

Force of attraction between a liquid and another surface

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2
Q

Allotropes

A

Different forms of the same element in the same physical state

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3
Q

Amorphous solid

A

A noncrystalline solid with no well-defined, ordered structure

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4
Q

Band

A

A series of very closely spaced, nearly continuous molecular orbitals that belong to the material as a whole

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5
Q

Band gap

A

An energy separation between an insulator’s highest filled electron energy band and the next higher-energy vacant band

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6
Q

Band theory of metals

A

A theory that accounts for the bonding and properties of metallic solids

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7
Q

Boiling point

A

The temperature at which the vapor pressure of a liquid is equal to the external pressure; also the condensation point

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8
Q

Capillary action

A

The drawing of a liquid up the inside of a small-bore tube when adhesive forces exceed adhesive forces

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9
Q

Cohesive forces

A

All the forces of attraction among particles of a liquid

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10
Q

Condensation

A

Liquefaction of vapor

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11
Q

Condensed phases

A

The liquid and solid phases; phases in which particles interact strongly

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12
Q

Conduction band

A

A partially filled band or band of vacant energy levels just higher in energy than a filled band; a band within which, or into which, electrons must be promoted to allow electrical conduction to occur in a solid

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13
Q

Coordination number

A

In describing crystals, the number of nearest neighbors of an atom or ion

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14
Q

Critical point

A

The combination of critical temperature and critical pressure of a substance

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15
Q

Critical pressure

A

The pressure required to liquefy a gas (vapor) at its critical temperature

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16
Q

Critical temperature

A

The temperature above which a gas cannot be liquefied; the temperature above which a substance cannot exhibit distinct gas and liquid phases

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17
Q

Crystal lattice

A

The pressure of arrangement of particles in a crystal

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18
Q

Crystalline solid

A

A solid characterized by a regular, ordered arrangement of particles

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19
Q

Deposition

A

The direct solidification of a vapor by cooling; the reverse of sublimation

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20
Q

Dipole-dipole interactions

A

Interactions between polar molecules, that is, between molecules with permanent dipoles

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21
Q

Dipole-induced dipole interaction

A

Very weak and very short-range attractive forces between short-lived temporary (induced) dipoles; also called London forces

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22
Q

Dispersion forces

A

Very weak and very short-range attractive forces between short-lived temporary (induced) dipoles; also called London forces

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23
Q

Distillation

A

The separation of a liquid mixture into its components on the basis of differences in boiling points

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24
Q

Dynamic equilibrium

A

A situation in which two (or more) processes occur at the same rate so that no net change occurs

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25
Enthalpy of fusion
The amount of heat required to melt a specific amount of a solid at its melting point with no change in temperature expressed in kJ/mol
26
Enthalpy of solidification
The amount of heat that must be removed from a specific amount of liquid at its freezing point to freeze it with no change in temperature; usually expressed in kJ/mol
27
Evaporation
Vaporization of a liquid below its boiling point
28
Freezing point
The temperature at which liquid and solid coexist in equilibrium
29
Heat of condensation
The amount of heat that must be removed from a specific amount of a vapor at its condensation point to condense the vapor with no change in temperature; usually expressed in J/g or kJ/mol; in the latter case it is called the *molar heat of condensation*
30
Heat of fusion
The amount of heat required to melt a specific amount of a solid at its melting point with no change in temperature; usually expressed in J/g or kJ/mol; in the latter case it is called the *molar heat of fusion*
31
Heat of solidification
The amount of heat that must be removed from a specific amount of liquid at its freezing point to freeze it with no change in temperature; usually expressed in J/g or kJ/mol; in the latter case it is called the molar heat of solidification
32
Heat of vaporization
The amount of heat required to vaporize a specific amount of a liquid at its boiling point with no change in temperature; usually expressed in J/g or kJ/mol; in the latter case it is called the *molar heat of vaporization*
33
Hydrogen bond
A fairly strong dipole-dipole interaction (but still considerably weaker than covalent or ionic bonds) between molecules containing hydrogen directly bonded to a small, highly electronegative ato, such as N, O, or F
34
Insulator
A poor conductor of electricity or heat
35
Intermolecular forces
Forces between individual particles (atoms, molecules, ions) of a substance
36
Intramolecular forces
Forces between atoms (or ions) *within* molecules (or formula units)
37
Isomorphous
Refers to crystals having the same atomic arrangement
38
LeChatelier's Principle
A system at equilibrium, or striving to attain equilbirum, respons in such a way as to counteract any stress placed upon it
39
London forces
Very weak and very short-range attractive forces between short-lived temporary (induced) dipoles; also called dispersion forces
40
Melting point
The temperature at which liquid and solid coexist in equilibrium, also the freezing point
41
Meniscus
The upper surface of a liquid in a cylindrical container
42
Metallic bonding
Bonding within metals due to the electrical attraction of positively charged metal ions for mobile electrons that belong to the crystal as a whole
43
Molar enthalpy of vaporization
The amount of heat required to vaporize a specific amount of a liquid at its boiling point with no change in temperature; usually expressed in kJ/mol
44
Molar heat capacity
The amount of heat necessary to raise the temperature of one mole of a substance one degree Celsius with no change in state; usually expressed in kJ/mol
45
Molar heat of condensation
The amount of heat that must be removed from one mole of a vapor at its condensation point to condense the vapor with no change in temperature; usually expressed in kJ/mol
46
Molar heat of fusion
The amount of heat required to melt one mole of a solid at its melting point with no change in temperature; usually expressed in kJ/mol
47
Molar heat of vaporiation
The amount of heat required to vaporize one mole of a liquid at its boiling point with no change in temperature; usually expressed in kJ/mol
48
Normal boiling point
The temperature at which the vapor pressure of a liquid is equal to one atmosphere pressure
49
Normal melting point
The melting (freezing) point at one atmosphere pressure
50
Phase diagram
A diagram that shows equilibrium temperature-pressure relationships for different phases of a substance
51
Polymorphous
Refers to substances that crystallie in more than one crystalline arrangement
52
Semiconductor
A substance that does not conduct electricity well at low temperatures but that does at higher temperatures
53
Specific heat
The amount of heat necessary to raise the temperature of a specific amount of a substance one degree Celsius with no change in state; usually expressed in J/g\*ºC
54
Sublimation
The direct vaporiation of a solid by heating without passing through the liquid state
55
Supercritical fluid
A substance at a temperature above its critical temperature. A supercritical fluid cannot be described as either a liquid or gas, but has the properties of both
56
Surface tension
The result of inward intermolecular forces of attraction among liquid particles that must be overcome to expand the surface area
57
Triple point
The point on a phase diagram that corresponds to the only pressure and temperature at which three phases (usually solid, liquid, and gas) of a substance can coexist at equilibrium
58
Unit cell
The smallest repeating unit showing all the structural characteristics of a crystal
59
Vapor pressure
The partial pressure of a vapor in equilibrium with its parent liquid or solid
60
Viscosity
The tendency of a liquid to resist flow; the inverse of its fluidity
61
Volatility
The ease with which a liquid vaporizes

Chem 101 (13 decks)

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