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Chem > General Zumdahl Vocab > Flashcards

General Zumdahl Vocab Flashcards

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1
Q

1/12 of the mass of an atom of 12C

A

Atomic mass unit(u)

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2
Q

synonymous with atomic mass unit

A

Dalton

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3
Q

formula for a salt

A

formula unit

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4
Q

contains the relative amounts of reactants that match the numbers in the balanced equation.

A

Stoichiometric mixture

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5
Q

solutions where concentration is known

A

Standard solutions

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6
Q

procedure where you find the concentration of a solution

A

Standardizing a solution

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7
Q

solutions in concentrated form

A

Stock Solutions

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8
Q

reaction where same element is oxidized and reduced

A

Disproportionation

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9
Q

measures atmospheric pressure

A

Barometer

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10
Q

unit equal to one mm Hg

A

Torr

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11
Q

Molar mass of specific gas relative to molar mass of air

A

Vapor density

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12
Q

law where if pressure and temperature remain the same, the total volume of a gaseous mixture will be the sum of the partial volumes of the gasses

A

Amagat’s law

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13
Q

Calculates vapor pressure from temperature

A

Clausius Clapeyron Equation

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14
Q

the average distance a particle travels between collisions

A

Mean free path

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15
Q

system that blows powdered limestone to remove sulfur

A

Scrubber

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16
Q

thick suspension produced after lime is injected into exhaust gases

A

Slurry

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17
Q

in going from a particular set of reactants to a particular set of products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps

A

Hess’s Law

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18
Q

the energy that needs to be added for the homolytic or symmetrical cleavage of a bond in the gas phase

A

Bond enthalpy

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19
Q

heats petroleum to break kerosene bonds to form more gasoline

A

Pyrolytic cracking

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20
Q

hydrogen and carbon monoxide mixture produced by coal gasification

A

Syngas

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21
Q

fuel produced by coal pulverized and mixed with water

A

Coal slurry

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22
Q

Alcohol - gasoline mixture

A

Gasohol

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23
Q

As protons are added one by one to the nucleus to build up the elements, electrons are added to hydrogen-like orbitals.

A

Aufbau principle

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24
Q

Chromium Electron Config

A

[Ar] 4s(1)3d(5)

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25
Q

Copper Electron Config

A

[Ar] 4s(1)3d(10)

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26
Q

The lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals.

A

Hund’s rule

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27
Q

used to determine ionization energy. High energy photons are directed at the sample and the kinetic energies of the ejected electrons are measured.

A

Photoelectron spectroscopy

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28
Q

rules that allow you to calculate effective nuclear charge on an electron

A

Slater’s rules

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29
Q

Coinage Metals

A

gold, silver, and copper

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30
Q

metals highly resistant to heat and wear

A

Refractory metals

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31
Q

energy required to break a chemical bond

A

Bond Energy

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32
Q

unit of dipole moment

A

Debyes

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33
Q

molecules composed of two identical atoms

A

Homonuclear diatomic molecules

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34
Q

surface of the electron sea at absolute zero where no electrons will have enough energy to rise above the surface

A

Fermi level

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35
Q

Alloy where atoms replace each other

A

substitutional

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36
Q

Alloy where atoms fit between each other

A

interstitial

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37
Q

temperature graph of a substance when energy is added as heat at a constant rate

A

Heating curve

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38
Q

Once a bubble forms in a superheated liquid, it accumulates vapor much faster than normal and cause burst and splash liquid out of the container

A

Bumping

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39
Q

meant to prevent bumping; bits of porous ceramic material containing trapped air that escapes on heating, forming tiny bubbles that act as “starters” for vapor bubble formation

A

Boiling chips

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40
Q

static pressure of a liquid reduces to below the liquid’s vapor pressure, leading to the formation of small vapor-filled cavities in the liquid

A

Cavitation

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41
Q

Since melting point decreases with pressure for water, applying pressure can melt ice

A

Regelation

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42
Q

Enthalpy of breaking intermolecular bonds in the pure solvent and creating interactions between the solute and solvent

A

Enthalpy of hydration

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43
Q

concentration of gas in solvent is proportional to its partial pressure

A

Henry’s law

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44
Q

coating of insoluble calcium carbonate on industrial boilers and tea kettles and that can block pipes and decrease heat transfer

A

Boiler scale

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45
Q

Solution vapor pressure is the weighted average of their vapor pressures

A

Raoult’s law

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46
Q

a mixture of two or more liquids whose proportions cannot be altered or changed by simple distillation

A

Azeotrope

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47
Q

properties that depend only on the number, and not on the identity, of the solute particles in an ideal solution

A

Colligative

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48
Q

light scattered by colloids makes them blue

A

Tyndall Effect

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49
Q

suspensions of tiny particles in a medium

A

Colloid

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50
Q

Colloids dispersed in gas

A

aerosols

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51
Q

Colloids gas dispersed in liquid

A

foam

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52
Q

Colloids gas dispersed in solid

A

solid foam

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53
Q

Colloids liquid dispersed in liquid

A

emulsion

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54
Q

Colloids solid dispersed in liquid

A

sol

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55
Q

Colloids solid dispersed in solid

A

solid sol

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56
Q

Colloids liquid dispersed in solid

A

solid emulsion

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57
Q

equation gives change in equilibrium constant for a change in temperature

A

Van’t Hoff’s Equation

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58
Q

acid where proton is attached to an oxygen atom

A

oxyacid

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59
Q

can behave as an acid or a base

A

amphoteric

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60
Q

molecules regularly transfering protons between each other

A

autoionization

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61
Q

having both hydrophilic and hydrophobic parts

A

amphipathic

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62
Q

All acids tend to become indistinguishable in strength when dissolved in strongly basic solvents

A

Leveling effect

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63
Q

Equilibrium constant for water autoionization

A

Ion product constant

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64
Q

Calcium Hydroxide common name

A

slaked lime

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65
Q

a compound or mixture that contains a Lewis acid and a Lewis base which, because of steric hindrance, cannot combine to form a classical adduct.

A

Frustrated Lewis Pair

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66
Q

The shift in equilibrium position that occurs because of the addition of an ion already involved in the equilibrium reaction

A

Common Ion Effect

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67
Q

determining the amount of a certain substance by doing a titration

A

Volumetric Analysis

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68
Q

solution added to solution to be analyzed in a titration

A

titrant

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69
Q

solution analyzed during titration

A

analyte

70
Q

point when the two solutions react exactly in a titration

A

equivalence point

71
Q

point when the indicator actually changes color in a titration

A

endpoint

72
Q

equilibrium constant for salt dissolution

A

Ksp - solubility product constant

73
Q

water molecules taken out of the environment(like water vapor) to be adsorbed or absorbed into a material

A

Hygroscopy

74
Q

take so much water out of the environment they form an aqueous solution that dissolves itself

A

Deliquescent material

75
Q

migration of a salt to the surface of a porous material, where it forms a coating

A

Efflorescence

76
Q

basically reaction quotient for salts

A

Ion product

77
Q

using a reagent whose anion forms a precipitate with only one or a few of the metal ions in the mixture

A

Selective Precipitation

78
Q

determining ions in a solution through selective precipitation

A

Qualitative Analysis

79
Q

number of ligands attached to a metal ion

A

coordination number

80
Q

equilibrium constant describing the addition of a ligand to a metal ion

A

formation constant

81
Q

mixture of HCl(acid + ligand) and HNO3(acid + oxidizer of sulfur) to dissolve HgS and Gold

A

Aqua Regia

82
Q

system can’t have matter leave, but energy can leave

A

Closed System

83
Q

system can’t have matter or energy leave

A

Isolated System

84
Q

In plane bending of bonds in opposite directions

A

scissoring

85
Q

In plane bending of bonds in the same direction

A

rocking

86
Q

out of plane bending of bonds in opposite directions

A

twisting

87
Q

out of plane bending of bonds in the same direction

A

wagging

88
Q

an effective attractive force that arises between large colloidal particles that are suspended in a dilute solution of depletants, which are smaller solutes that are preferentially excluded from the vicinity of the large particles.

A

Depletion force

89
Q

the generation of electricity through chemical reactions

A

Galvanism

90
Q

device in which chemical energy is changed to electrical energy

A

Galvanic cell

91
Q

galvanic cell where both sides have the same components, but at different concentrations

A

concentration cell

92
Q

gives the relationship between the cell potential and the concentrations of the cell components

A

Nernst Equation

93
Q

Lead storage battery cathode and anode

A

lead as anode and lead coated in lead dioxide as the cathode

94
Q

Dry Acid Battery cathode and anode

A

anode is zinc inner case and cathode is carbon rod

95
Q

electrolyte in Dry Acid Battery

A

NH4Cl

96
Q

electrolyte in alkaline battery

A

KOH or NaOH

97
Q

Silver cell anode and cathode

A

anode is zinc and cathode is silver oxide

98
Q

Mercury cell anode and cathode

A

anode is zinc and cathode is mercury oxide

99
Q

Nickel-Cadmium battery anode and cathode

A

Anode is cadmium and cathode is nickel oxide

100
Q

battery where lithium ions move to cathode and electrons flow to balance it

A

Lithium ion battery

101
Q

metals oxidizing

A

corrosion

102
Q

coating steel with zinc

A

galvanizing steel

103
Q

created when gaseous or ionic metals are incorporated into the surface of a metal

A

Surface Alloys

104
Q

a more reactive anode metal connected to a metal that should be protected and the anode provides the electrons rather than the cathode, preventing rusting

A

Cathodic Protection

105
Q

uses electrical energy to produce chemical change

A

Electrolytic cell

106
Q

voltage needed above the expected value for an electrolytic cell

A

Overvoltage

107
Q

graphical representation of nernst equation

A

Pourbaix diagram

108
Q

neutrons and protons

A

Nucleons

109
Q

unique atom

A

Nuclide

110
Q

amount of energy released in forming the nucleus

A

binding energy per nucleon

111
Q

number of protons and neutrons in a nucleus is particularly stable

A

Magic numbers

112
Q

type of circular particle accelerator

A

Cyclotron

113
Q

elements beyond element 92

A

transuranic

114
Q

measures radioactivity based on measurement of ionization of matter

A

Geiger–Müller counter

115
Q

measures radioactivity based on zinc sulfide giving off light in response to radioactivity

A

scintillation counter

116
Q

radioactive nuclides that can be introduced into organisms in food or drugs and whose pathways can be traced by monitoring their radioactivity

A

radiotracers

117
Q

surrounds cylinders in reactor core to slow down neutrons and allow them to be more effectively captured

A

moderator

118
Q

made of substances that absorb neutrons; used to control power level of reactor

A

control rods

119
Q

fissionable material produced while reactor runs

A

Breeder reactors

120
Q

unit of energy of ionizing radiation

A

Rad

121
Q

unit of both the energy dose of the radiation and its effectiveness in causing biological damage

A

Roentgen

122
Q

attaining a metal from its ore

A

metallurgy

123
Q

resin or polymer that acts as a medium for ion exchange for water softening

A

ion exchange resin

124
Q

group name for boron

A

triels

125
Q

group name for carbon

A

Crystallogens/Adamantogens

126
Q

Tin crumbles away when exposed to low temperatures

A

tin disease

127
Q

deposition of an overlayer on a crystalline substrate, where the overlayer is in registry with the substrate

A

epitaxy

128
Q

Ozone can be used in water treatment

A

ozonolysis

129
Q

number of coordinate covalent bonds a ligand can form

A

Denticity

130
Q

ligands form two or more bonds to a metal ion where the bonds are on different atoms in the ligand molecule

A

Chelating Ligands

131
Q

two or more species have the same formula, but different properties

A

Isomerism

132
Q

isomer with different bonds

A

structural/constitutional

133
Q

isomer bonding through different atoms

A

linkage isomer

134
Q

complex isomer

A

coordination isomer

135
Q

for a structure with n asymmetric carbon atoms, there is a maximum of 2n different stereoisomers possible

A

Le Bel-van’t Hoff rule

136
Q

isomer with same bonds

A

stereoisomer

137
Q

non mirror image stereoisomer

A

diastereomer

138
Q

mirror image stereoisomer

A

enantiomer/optical isomer

139
Q

diastereomers that contain more than one chiral center but differ from each other in the absolute configuration at only one chiral center.

A

epimer

140
Q

hindered rotation about a single bond causes energy differences due to steric strain or other contributors create a barrier to rotation that is high enough to allow for isolation of individual conformers

A

Atropisomers

141
Q

diastereomer with same structural formula but with different shapes due to rotations about one or more bonds

A

Conformational isomer

142
Q

diastereomer with same structural formula, but different arrangement of atoms

A

Geometric/Cis Trans Isomer

143
Q

cyclic version of epimers

A

Anomers

144
Q

enantiomer that rotates light to the right

A

Dextrorotatory

145
Q

enantiomer that rotates light to the left

A

Levorotatory

146
Q

mixture of L and D enantiomers

A

Racemic mixture

147
Q

an attempt to account for the colors and magnetic properties of complex ions

A

Crystal Field Theory

148
Q

ranks ligands in their ability to produce d splitting

A

Spectrochemical series

149
Q

repels virtually all liquids

A

Omniphobic

150
Q

Saturated Hydrocarbons/Alkanes alternative name

A

Paraffins

151
Q

Alkenes alternative name

A

Olefins

152
Q

Alkynes alternative name

A

Acetylenes

153
Q

determines if a cyclic planar ring molecule is aromatic

A

Huckel’s rule

154
Q

polymer created from one type of monomer

A

Homopolymer

155
Q

polymer created from two types of monomer

A

Copolymer

156
Q

two monomers joined

A

Dimer

157
Q

covalent bonding between adjacent polymer chains

A

Crosslinking

158
Q

polymer when molded to a certain shape under high pressure and temperature cannot be softened again or dissolved

A

Thermoset polymer

159
Q

polymer that can be remelted after being molded

A

Thermoplastic polymer

160
Q

temperature change of a real gas or liquid when it is forced through a valve or porous plug while keeping it insulated so that no heat is exchanged with the environment

A

Joule Thompson Effect

161
Q

substance bombarded with infrared light and what is absorbed vs what is not is detected to allow us to figure out the structure of the molecule

A

Infrared Spectrometry

162
Q

technique that monitors color change in a reaction

A

Spectrophotometry

163
Q

Formula for absorbance

A

Beer’s Law

164
Q

the gradual deterioration and eventual cracking of a material by alternate heating and cooling during which free thermal expansion is partially or completely constrained.

A

Thermal Fatigue

165
Q

a part of a molecule that is given a name because it is identified as a part of other molecules as well

A

Moeity

166
Q

an achiral compound that has chiral centers

A

Meso compound

167
Q

the tendency of the two electrons in the outermost atomic s-orbital to remain unshared in compounds of post-transition metals

A

Inert Pair Effect

168
Q

any atom that is not carbon or hydrogen

A

Heteroatom

169
Q

alloy of mercury with another metal

A

Amalgam

170
Q

chemical that lowers surface tension

A

Surfactant

171
Q

the entropy of vaporization is almost the same value, about 85–88 J/(K·mol), for various kinds of liquids at their boiling points.

A

Trouton’s rule

172
Q

describes carbon chemicals that form chains and not rings

A

Aliphatic

Chem (12 decks)

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