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Chemistry > Test 2 > Flashcards

Test 2 Flashcards

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1
Q

surface tension

A

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

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2
Q

capillarity

A

A property that results in a liquid rising through a narrow space against the pull of gravity

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3
Q

viscosity

A

A measure of the resistance of liquid to flow

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4
Q

crystalline solid

A

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

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5
Q

amorphous solid

A

A solid that has a poorly defined shape because it lacks extensive molecular-level ordering of its particles.

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6
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

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7
Q

unit cell

A

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

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8
Q

coordination number

A

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

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9
Q

simple cubic unit cell

A

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

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10
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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11
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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12
Q

packing efficiency

A

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

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13
Q

hexagonal closet packing

A

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

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14
Q

cubic closet 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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15
Q

x-ray diffraction analysis

A

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

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16
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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17
Q

molecular solid

A

A solid held together by intermolecular forces between individual molecules.

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18
Q

ionic solid

A

A solid whose unit cell contains cations and anions

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19
Q

metallic solid

A

A solid whose individual atoms are held together by metallic bonding

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20
Q

network covalent solid

A

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

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21
Q

electron-sea model

A

A qualitative description of metallic bonding proposing that metal atoms pool their valence electrons into a delocalized “sea” of electrons in which the metal cores are submerged in an orderly array.

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22
Q

band theory

A

An extension of molecular orbital theory that explains many properties of metals and other solids, in particular, the differences in electrical conductivity of conductors, semiconductors, and insulators.

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23
Q

valence band

A

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

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24
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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25
Q

conductor

A

A substance that conducts an electric current well.

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26
Q

semiconductor

A

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

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27
Q

insulator

A

A substance that does not conduct an electric current.

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28
Q

superconductivity

A

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

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29
Q

solute

A

The substance that dissolves in the solvent

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30
Q

solvent

A

The substance in which the solute dissolves.

31
Q

miscible

A

Soluble in any proportion

32
Q

solubility

A

The maximum amount of solute that dissolves in a fixed quantity of a particular solvent at a specific temperature

33
Q

like-dissolves-like rule

A

An empirical observation stating that substances having similar kinds of intermolecular forces dissolve in each other

34
Q

hydration shell

A

The oriented cluster of water molecules that surrounds an ion in aqueous solution

35
Q

ion-induced dipole force

A

The attractive force between an ion and the dipole it induces in the electron cloud of a nearby non polar molecule

36
Q

dipole-induced dipole force

A

The intermolecular attraction between a polar molecule and the oppositely charged pole it induces in a nearby molecule

37
Q

alloy

A

A mixture of elements with metallic properties that is typically a solid-solid solution.

38
Q

heat of solution

A

The enthalpy change occurring when a solution forms from solute and solvent

39
Q

solvation

A

The process of surrounding a solute particle with solvent particles

40
Q

hydration

A

Solvation in water

41
Q

heat of hydration

A

The enthalpy change occurring when 1mol of a gaseous species is hydrated

42
Q

charge density

A

The ratio of the charge of an ion to its volume

43
Q

entropy

A

A thermodynamic quantity related to the number of ways the energy of a system can be dispersed through the motions of its particles

44
Q

saturated solution

A

A solution that contains the maximum amount of dissolved solute at a given temperature

45
Q

unsaturated solution

A

A solution in which more solute can be dissolved at a given temperature

46
Q

supersaturated solution

A

An unstable solution in which more solute is dissolved than in a saturated solution

47
Q

Henry’s Law

A

A law stating that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid

48
Q

molality

A

A concentration term expressed as number of moles of solute dissolved in 1000g of solvent.

49
Q

mass percent

A

The fraction by mass expressed as a percentage

50
Q

volume percent

A

A concentration term defined as the volume of solute in 100 volumes of solution.

51
Q

mole fraction

A

A concentration term expressed as the ratio of moles of one component of a mixture to the total moles present.

52
Q

colligative property

A

A property of a solution that depends on the number, not the identity, of solute particles.

53
Q

electrolyte

A

A substance that conducts a current when it dissolves in water.

54
Q

non electrolyte

A

A substance whose aqueous solution does not conduct an electric current

55
Q

vapor pressure lowering

A

The decrease in the vapor pressure of a solvent caused by the presence of dissolved solute particles.

56
Q

Raoul’s law

A

A low stating the the vapor pressure of solvent above a solution equals the mole fraction of solvent times the vapor pressure of pure solvent.

57
Q

ideal solution

A

A solution whose vapor pressure equals the mole fraction of the solvent times the vapor pressure of the pure solvent.

58
Q

boiling point elevation

A

The increase int he boiling point of a solvent caused by the presence of dissolved solute

59
Q

freezing point depression

A

The lowering of the freezing point of a solved caused by the presence of dissolved solute particles.

60
Q

semipermeable membrane

A

A membrane that allows solvent, but not solute, to pass through.

61
Q

osmosis

A

The process by which solvent flows through a semipermeable membrane from a dilute to a concentrated solution.

62
Q

osmotic pressure

A

The pressure that results from the ability of solvent, but not solute, particles to cross a semipermeable membrane. The pressure required to prevent the net movement of solvent across the membrane

63
Q

ionic atmosphere

A

A cluster of ions of net opposite charge surrounding a given ion in solution.

64
Q

chemical kinetics

A

The study of the rates and mechanism of reactions.

65
Q

reaction rate

A

The change in the concentrations of reactants with time.

66
Q

average rate

A

The change in concentration of reactant divided by a finite time period.

67
Q

instantaneous rate

A

The reaction rate at a particular, given by the slope of a tangent to a plot of reactant concentration vs. time.

68
Q

initial rate

A

The instantaneous rat occurring as soon as the reactants are mixed,, that is, at t=0.

69
Q

rate law

A

An equation that expresses the rate of a reaction as a function of reactant concentrations

70
Q

rate constant

A

The proportionality constant that relates reaction to rate to reactant concentrations.

71
Q

reaction orders

A

The exponent of a reactant concentration in a rate law that shows how the rate is affected by changes in that concentration

72
Q

integrated rate law

A

A mathematical expression for reactant concentration a s a function of time.

73
Q

half-life

A

In chemical processes, the time required for half the initial reactant concentration to be consumed.

Chemistry (25 decks)

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