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General Chemistry I > [VOCAB] Chapter 12: Intermolecular Forces: Liquids, Solids, and Phase Changes > Flashcards

[VOCAB] Chapter 12: Intermolecular Forces: Liquids, Solids, and Phase Changes Flashcards

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1
Q

Amorphous Solid

A

A solid that has a poorly defined shape because its particles do not have an orderly arrangement throughout a sample

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2
Q

Atomic Solid

A

A solid consisting of individual atoms held together by dispersion forces; the frozen noble gases are the only examples

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3
Q

Band Theory

A

An extension of molecular orbital (MO) theory that explains many properties of metals and other solids—in particular, the differences in conductivity of metals, metalloids, and nonmetals

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4
Q

Body-Centered Cubic Unit Cell

A

A unit cell in which a particle lies at each corner and in the center of a cube

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5
Q

Boiling Point

A

The temperature at which the vapor pressure inside bubbles forming in a liquid equals the external (atmospheric) pressure

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6
Q

Branch

A

A side chain appended to a polymer backbone or to the longest sequence of atoms in an organic compound

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7
Q

Capillarity

A

(also capillary action) The rising of a liquid through a narrow space against the pull of gravity

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8
Q

Ceramic

A

A nonmetallic, nonpolymeric solid that is hardened by heating it to high temperatures and, in most cases, consists of silicate microcrystals suspended in a glassy cementing medium

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9
Q

Clausius-Clapeyron Equation

A

An equation that expresses the linear relationship between vapor pressure P of a liquid and temperature T; in two-point form, it is

In(P^2)/(P1) = (-change of Hvap)/(R)

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10
Q

Condensation

A

The process of a gas changing into a liquid

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11
Q

Conduction Band

A

In band theory, the empty, higher energy portion of the band of molecular orbitals into which electrons move when conducting heat and electricity

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12
Q

Conductor

A

A substance (usually a metal) that conducts an electric current well

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13
Q

Coordination Number

A

In a crystal, the number of nearest neighbors surrounding a particle. In a complex ion, the number of ligand atoms bonded to the central metal ion

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14
Q

Copolymer

A

A polymer that consists of two or more types of monomer

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15
Q

Critical Point

A

The point on a phase diagram above which the vapor cannot be condensed to a liquid; the end of the liquid-gas curve

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16
Q

Crosslink

A

A branch that covalently joins one polymer chain to another

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17
Q

Crystal Defect

A

Any of a variety of disruptions in the regularity of a crystal structure

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18
Q

Crystalline Solid

A

A solid with a well-defined shape because of the orderly arrangement of the atoms, molecules, or ions

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19
Q

Cubic Closest Packing

A

A crystal structure based on the face-centered cubic unit cell in which the layers have an abcabc . . . pattern

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20
Q

Degree of Polymerization (n)

A

The number of repeat units in a polymer chain

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21
Q

Deposition

A

The process of changing directly from a gas to a solid

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22
Q

Dipole-Dipole Force

A

The intermolecular attraction between oppositely charged poles of nearby polar molecules

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23
Q

dispersion force

A

(also London force) The intermolecular attraction between all particles as a result of instantaneous polarizations of their electron clouds; the intermolecular force primarily responsible for the condensed states of nonpolar substances

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24
Q

Doping

A

Adding small amounts of other elements into the crystal structure of a semiconductor to enhance a specific property, usually conductivity

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25
Q

Elastomer

A

A polymeric material that can be stretched and springs back to its original shape when released

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26
Q

Face-Centered Cubic Unit Cell

A

A unit cell in which a particle occurs at each corner and in the center of each face of a cube

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27
Q

Freezing

A

The process of cooling a liquid until it solidifies

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28
Q

Heat of Fusion (ΔH°fus)

A

(also enthalpy of fusion) The enthalpy change occurring when 1 mol of a solid substance melts; designated (change of H degree_fus) at the standard state

29
Q

Heat of Sublimation

A

(also enthalpy of sublimation) The enthalpy change occurring when 1 mol of a solid substance changes directly to a gas. The sum of the heats of fusion and vaporization; designated (change of H degree_subl) at the standard state

30
Q

Heat of Vaporization

A

(also enthalpy of vaporization) The enthalpy change occurring when 1 mol of a liquid substance vaporizes; designated (change of H degree_vap) at the standard state

31
Q

Heating-Cooling Curve

A

A plot of temperature vs. time for a sample when heat is absorbed or released at a constant rate

32
Q

Hexagonal Closest Packing

A

A crystal structure based on the hexagonal unit cell in which the layers have an abab . . . pattern

33
Q

Hydrogen Bond (H bond)

A

A type of dipole-dipole force that arises between molecules that have an H atom bonded to a small, highly electronegative atom with lone pairs, usually N, O, or F

34
Q

Insulator

A

A substance (usually a nonmetal) that does not conduct an electric current

35
Q

Intermolecular Forces

A

(also interparticle forces) The attractive and repulsive forces among the particles—molecules, atoms, or ions—in a sample of matter

36
Q

Ion-Dipole Force

A

The intermolecular attractive force between an ion and a polar molecule (dipole)

37
Q

Ionic Solid

A

A solid whose unit cell contains cations and anions

38
Q

Lattice

A

The three-dimensional arrangement of points created by choosing each point to be at the same location within each particle of a crystal; thus, the lattice consists of all points with identical surroundings

39
Q

Liquid Crystal

A

A substance that flows like a liquid but packs like a crystalline solid at the molecular level

40
Q

Melting

A

(also fusion) The change of a substance from a solid to a liquid

41
Q

Melting Point

A

The temperature at which the solid and liquid forms of a substance are at equilibrium

42
Q

Metallic Solid

A

A solid whose individual atoms are held together by metallic bonding

43
Q

Molecular Solid

A

A solid held together by intermolecular forces between individual molecules

44
Q

Monomer

A

A small molecule, linked covalently to others of the same or similar type to form a polymer; the repeat unit of the polymer

45
Q

Nanotechnology

A

The science and engineering of nanoscale systems (size range of 1–100 nm)

46
Q

Network Covalent Solid

A

A solid in which all the atoms are bonded covalently so that individual molecules are not present

47
Q

Packing Efficiency

A

The percentage of the total volume occupied by atoms, ions, or molecules in a unit cell

48
Q

Phase

A

A physically distinct and homogeneous part of a system

49
Q

Phase Change

A

A physical change from one phase to another, usually referring to a change in physical state

50
Q

Phase Diagram

A

A diagram used to describe the stable phases and phase changes of a substance as a function of temperature and pressure

51
Q

Plastic

A

A material that, when deformed, retains its new shape

52
Q

Polarizability

A

The ease with which a particle’s electron cloud can be distorted

53
Q

Polymer

A

(also macromolecule) An extremely large molecule that results from the covalent linking of many simpler molecular units (monomers)

54
Q

Radius of Gyration (Rg)

A

A measure of the size of a coiled polymer chain, expressed as the average distance from the center of mass of the chain to its outside edge

55
Q

Random Coil

A

The shape adopted by most polymer chains and caused by random rotation about the bonds joining the repeat units

56
Q

Scanning Tunneling Microscopy

A

An instrumental technique that uses electrons moving across a minute gap to observe the topography of a surface on the atomic scale

57
Q

Semiconductor

A

A substance whose electrical conductivity is poor at room temperature but increases significantly with rising temperature

58
Q

Simple Cubic Unit Cell

A

A unit cell in which a particle occupies each corner of a cube

59
Q

Sublimation

A

The process by which a solid changes directly into a gas

60
Q

Superconductivity

A

The ability to conduct a current with no loss of energy to resistive heating

61
Q

Surface Tension

A

The energy required to increase the surface area of a liquid by a given amount

62
Q

Triple Point

A

The pressure and temperature at which three phases of a substance are in equilibrium. In a phase diagram, the point at which three phase-transition curves meet

63
Q

Unit Cell

A

The smallest portion of a crystal that, if repeated in all three directions, yields the crystal

64
Q

Valence Band

A

In band theory, the lower energy portion of the band of molecular orbitals, which is filled with valence electrons

65
Q

Van der Waals Radius

A

One-half of the closest distance between the nuclei of identical nonbonded atoms

66
Q

Vapor Pressure

A

(also equilibrium vapor pressure) The pressure exerted by a vapor at equilibrium with its liquid in a closed system

67
Q

Vaporization

A

The process of changing from a liquid to a gas

68
Q

Viscosity

A

A measure of the resistance of a fluid to flow

69
Q

X-ray Diffraction Analysis

A

An instrumental technique used to determine dimensions of a crystal structure by measuring the diffraction patterns caused by x-rays impinging on the crystal

General Chemistry I (12 decks)

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