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Chem 101 > Chapter 13 > Flashcards

Chapter 13 Flashcards

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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
Q

Enthalpy of fusion

A

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
Q

Enthalpy of solidification

A

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
Q

Evaporation

A

Vaporization of a liquid below its boiling point

28
Q

Freezing point

A

The temperature at which liquid and solid coexist in equilibrium

29
Q

Heat of condensation

A

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
Q

Heat of fusion

A

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
Q

Heat of solidification

A

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
Q

Heat of vaporization

A

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
Q

Hydrogen bond

A

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
Q

Insulator

A

A poor conductor of electricity or heat

35
Q

Intermolecular forces

A

Forces between individual particles (atoms, molecules, ions) of a substance

36
Q

Intramolecular forces

A

Forces between atoms (or ions) within molecules (or formula units)

37
Q

Isomorphous

A

Refers to crystals having the same atomic arrangement

38
Q

LeChatelier’s Principle

A

A system at equilibrium, or striving to attain equilbirum, respons in such a way as to counteract any stress placed upon it

39
Q

London forces

A

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

40
Q

Melting point

A

The temperature at which liquid and solid coexist in equilibrium, also the freezing point

41
Q

Meniscus

A

The upper surface of a liquid in a cylindrical container

42
Q

Metallic bonding

A

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
Q

Molar enthalpy of vaporization

A

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
Q

Molar heat capacity

A

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
Q

Molar heat of condensation

A

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
Q

Molar heat of fusion

A

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
Q

Molar heat of vaporiation

A

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
Q

Normal boiling point

A

The temperature at which the vapor pressure of a liquid is equal to one atmosphere pressure

49
Q

Normal melting point

A

The melting (freezing) point at one atmosphere pressure

50
Q

Phase diagram

A

A diagram that shows equilibrium temperature-pressure relationships for different phases of a substance

51
Q

Polymorphous

A

Refers to substances that crystallie in more than one crystalline arrangement

52
Q

Semiconductor

A

A substance that does not conduct electricity well at low temperatures but that does at higher temperatures

53
Q

Specific heat

A

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
Q

Sublimation

A

The direct vaporiation of a solid by heating without passing through the liquid state

55
Q

Supercritical fluid

A

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
Q

Surface tension

A

The result of inward intermolecular forces of attraction among liquid particles that must be overcome to expand the surface area

57
Q

Triple point

A

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
Q

Unit cell

A

The smallest repeating unit showing all the structural characteristics of a crystal

59
Q

Vapor pressure

A

The partial pressure of a vapor in equilibrium with its parent liquid or solid

60
Q

Viscosity

A

The tendency of a liquid to resist flow; the inverse of its fluidity

61
Q

Volatility

A

The ease with which a liquid vaporizes

Chem 101 (13 decks)

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