Chemistry Flashcards
(183 cards)
1
Q
the Mulliken scale averages electron affinity and ionization energy to find this
A
electronegativity
2
Q
highest value is fluorine with 4.0 (Pauling scale)
A
electronegativity
3
Q
difference between atoms determines bond polarity
A
electronegativity
4
Q
high values for this quantity increase the chemical shift of adjacent protons in the field effect
A
electronegativity
5
Q
high values for this quantity increase acidity in the inductive effect
A
electronegativity
6
Q
the effective nuclear charge over the square of the covalent radius (Allred-Rochow scale)
A
electronegativity
7
Q
formal charge is more positive than the oxidation state at high values
A
electronegativity
8
Q
an atom’s ability to attract electrons
A
electronegativity
9
Q
Van Deemter equation is used to figure out the height of a theoretical column
A
chromatography
10
Q
thin-layer form of this process uses a silica plate inside a beaker
A
chromatography
11
Q
compounds are separated by their size through a stationary phase
A
chromatography
12
Q
uses stationary and mobile phases to separate mixtures
A
chromatography
13
Q
ion exchange and size exclusion forms
A
chromatography
14
Q
substances can be characterized by their retention factor
A
chromatography
15
Q
the gas form is often paired with flame ionization detection (FID) or mass spectroscopy (MS)
A
chromatography
16
Q
relies on differences in partition coefficients between compounds
A
chromatography
17
Q
burettes are commonly used
A
titration
18
Q
lab technique is used to find an unknown substance’s concentration
A
titration
19
Q
phenolphthalein and bromothymol blue are often used in the acid-base form
A
titration
20
Q
the equivalence point is the inflection point on one of these curves
A
titration
21
Q
complexometric ones often use EDTA
A
titration
22
Q
Karl Fischer type uses electrolysis to determine water content
A
titration
23
Q
curves contain a buffer region
A
titration
24
Q
redox variety often uses permanganate
A
titration
25
a volatile substance is constantly boiling and condensing back into the reaction vessel
reflux
26
azeotropes cannot be separated by this process
distillation
27
often utilizes a Liebig or Vigreux condenser
distillation
28
the number of theoretical plates needed for this is predicted by the Fenske equation
distillation
29
the fractional type is used in oil refinement
distillation
30
theoretical plates are the optimal number of equilibrium stages in this technique
distillation
31
a sample is ionized, fragmented, then passed through electromagnetic fields to separate
mass spectroscopy (MS)
32
separates 'pieces' based on their mass-to-charge ratio (m/z)
mass spectroscopy (MS)
33
includes a base peak (the peak of highest intensity)
mass spectroscopy (MS)
34
matrix-assisted laser desorption/ionization (MALDI) or electrospray ionization (ESI) used
mass spectroscopy (MS)
35
proton and carbon-13 types are most common
nuclear magnetic resonance (NMR)
36
nuclei oscillate between spin states (Larmor precession)
nuclear magnetic resonance (NMR)
37
tetramethylsilane (TMS) used as a reference
nuclear magnetic resonance (NMR)
38
nuclei undergo chemical shift
nuclear magnetic resonance (NMR)
39
peaks can be “split” into several peaks due to J-coupling
nuclear magnetic resonance (NMR)
40
the theoretical basis for magnetic resonance imaging (MRI) in medicine
nuclear magnetic resonance (NMR)
41
involves vibrational modes called “stretching,” “wagging,” and “scissoring”
infrared spectroscopy (IR)
42
the carbonyl peak occurs at around 1700 cm-1
infrared spectroscopy (IR)
43
requires bonds to be polarizable
infrared spectroscopy (IR)
44
includes a fingerprint region below 1500 cm-1
infrared spectroscopy (IR)
45
aromatic hydrocarbon with formula C6H6
benzene
46
ortho, meta, and para position
benzene
47
phenol, aniline, toluene, and xylene are derivatives of this compound
benzene
48
the structure came to Auguste Kekulé in a dream (a snake eating its tail)
benzene
49
flat structure proven by Kathleen Lonsdale
benzene
50
substituents are added onto this compound in a Friedel-Crafts reaction
benzene
51
uses a Bunsen burner to view emission spectra
flame test
52
cobalt blue glass used to filter of the sodium D line
flame test
53
lithium = red
flame test
54
strontium = red
flame test
55
light purple (lilac) = potassium
flame test
56
barium = green
flame test
57
copper = blue/green
flame test
58
calculates the heat or enthalpy change of a chemical or physical process
calorimetry
59
coffee cups and bomb-type devices used
calorimetry
60
uses the equation q equals mc delta T
calorimetry
61
measures light absorbed by chromophores including a lambda-max
UV-Vis spectroscopy
62
cuvettes used in the technique
UV-Vis spectroscopy
63
used for Beer's law experiments
UV-Vis spectroscopy
64
Woodward-Fieser rules used to calculate lambda-max
UV-Vis spectroscopy
65
separates mixtures based on their relative solubilities in two immiscible solvents
liquid-liquid extraction
66
typically performed in a separatory funnel
liquid-liquid extraction
67
made of repeating monomers
polymers
68
nylon, rayon, teflon, kevlar are types of these
polymers
69
step-growth and chain-growth methods
polymers
70
AIBN is a radical initiator for chain-growth
polymers
71
equals internal energy plus pressure times volume
enthalpy
72
symbolized H
enthalpy
73
negative value = exothermic
enthalpy
74
positive value = endothermic
enthalpy
75
the change in this quantity for a reaction is independent of the number of steps according to Hess's Law
enthalpy
76
stays constant in the Joule-Thomson effect
enthalpy
77
the Born-Haber cycle can be used to calculate this for a lattice
enthalpy
78
k-sub-B times the natural log of the number of microstates according to Boltzmann
entropy
79
measure of a system’s disorder
entropy
80
values of zero for this quantity are defined by the third law of thermodynamics
entropy
81
is increasing according to the second law of thermodynamics
entropy
82
negative value = spontaneous
Gibbs free energy
83
positive value = nonspontaneous
Gibbs free energy
84
value of zero = equilibrium
Gibbs free energy
85
plotted with temperature in the Ellingham Diagram
Gibbs free energy
86
only depend on the number, not the type, of solute particles
colligative properties
87
include osmotic pressure, boiling point elevation and freezing point depression
colligative properties
88
examples of these substances include gels, aerosols, and emulsions
colloids
89
the scattering of light in these substances is known as the Tyndall effect
colloids
90
milk is an example
colloids
91
may sediment out via flocculation
colloids
92
the electrical potential at the double layers of these compounds is known as the zeta potential
colloids
93
gives a broad peak around 3300 cm-1 in IR spectroscopy
alcohols
94
reacted with carboxylic acids in Fischer esterification
alcohols
95
functional group symbolized -OH
alcohols
96
ranges from 0 to 14
pH
97
acids have a value less than 7
pH
98
bases have a value greater than 7
pH
99
buffers resist large changes in this value
pH
100
plotted against chemical potential in a Pourbaix diagram
pH
101
negative log of hydrogen ion concentration
pH
102
calculated by the Henderson-Hasselbalch equation (buffers)
pH
103
Arnold Beckman invented a device that uses a glass electrode to measure this
pH
104
reduce activation energy and speed up chemical reactions
catalyst
105
not consumed in a chemical reaction
catalyst
106
Iron oxide acts as one in the Haber-Bosch Process
catalyst
107
zeolites can behave like these materials during the refinement of petroleum
catalyst
108
can be 'poisoned' by adding sulphur
catalyst
109
ones named for Zeigler and Natta, Raney, Lindlar, Grubbs
catalyst
110
vanadium acts as one in the contact process
catalyst
111
consist of a regular repeating arrangement of atoms
crystal lattice
112
often grow around a “seed”
crystal lattice
113
characterized by x-ray diffraction according to Bragg's law
crystal lattice
114
symbolized uppercase K or Kc or Keq or Kp or Ksp
equilibrium constant
115
the rate of a forward reaction equals the rate of a backwards reaction
equilibrium
116
concentrations do not change
equilibrium
117
powers of RT convert between Kc and Kp
equilibrium constant
118
solids and liquids do not contribute to this
equilibrium constant
119
calculated by the law of mass action
equilibrium constant
120
will respond to stress according to Le Chatelier’s Principle
equilibrium constant
121
states that a system in chemical equilibrium will shift to counteract change
Le Chatelier's principle
122
the van't Hoff equation applies this concept to thermodynamics
Le Chatelier's principle
123
different arrangements of atoms but the same molecular formula
isomers
124
glucose and fructose are “structural” types of these
isomers
125
cis' and 'trans' identify "stereo" forms of these
isomers
126
a molecule cannot be superimposed on its mirror image
chirality
127
derived from the Greek for “handedness”
chirality
128
use Cahn-Ingold-Prelog sequence rules
chirality
129
molecules with this property are designated as R or S
chirality
130
enantiomers exhibit this property
chirality
131
process which splits molecules using an electric current
electrolysis
132
used in the Castner-Kellner process and Hall-Heroult process
electrolysis
133
100 degrees celsius for water
boiling point
134
Duhring’s plot
boiling point
135
an increase in this quantity is related to molality by the ebullioscopic content
boiling point
136
used to calculate the pH of a buffer solution
Henderson-Hasselbalch equation
137
related to the Charlot equation
Henderson-Hasselbalch equation
138
relates pH to pKa for a weak acid
Henderson-Hasselbalch equation
139
regions in which electrons are most likely to be found
orbitals
140
split by ligands in crystal field theory (d specifically)
orbitals
141
s, p, d, and f forms
orbitals
142
molecular types have a HOMO and LUMO
orbitals
143
“hybrid” forms such as sp2 and sp3
orbitals
144
filling governed by the Aufbau principle, Pauli Exclusion principle, and Hund's rule
orbitals
145
head-on overlap forms sigma bonds
orbitals
146
side-on overlap forms pi bonds (p specifically)
orbitals
147
differ in azimuthal quantum numbers
orbitals
148
spherical orbital type
s orbitals
149
orbitals labeled x, y, and z
p orbitals
150
transition metals have partially filled orbitals of this type
d orbitals
151
split into t-sub-2g and e-sub-g by ligands
d orbitals
152
occurs when atomic orbitals combine to distribute their energy more evenly
hybridization
153
atomic orbitals mix to form bonds in this process
hybridization
154
kinetics equation that calculates reaction rate
Arrhenius equation
155
the product of steric factor and the collision frequency gives the pre-exponential factor which is multiplied by e to the minus E-a over RT
Arrhenius equation
156
responsible for the high specific heat of water, as well as its cohesive and adhesive nature
hydrogen bonds
157
solid, liquid, and gas exist at thermal equilibrium
triple point
158
demonstrates a nonlinear relationship between the temperature and vapor pressure of a system
Clausius-Clapeyron equation
159
the partial pressure of a gas is equal to its mole fraction times vapor pressure
Raoult's law
160
these mixtures cannot be separated by distillation
azeotropes
161
96% ethanol and 4% water forms the classic type of these
azeotropes
162
the endpoint of the liquid-gas boundary in a phase diagram
critical point
163
a substance is neither a liquid or a gas, but a homogenous mixture of both
critical point
164
a solid changes directly into gas
sublimation
165
phase change seen in dry ice
sublimation
166
allows iodine crystals to expose latent fingerprints
sublimation
167
“Cold finger” purification begins with this process
sublimation
168
zero celsius for water
melting point
169
phase transition directly from a gas to a solid
deposition
170
opposite of sublimation
deposition
171
used in a voltaic or galvanic cell to maintain charge balance
salt bridge
172
electrode where oxidation occurs
anode
173
electrode where reduction occurs
cathode
174
reaction in which electrons are lost
oxidation
175
reaction in which electrons are gained
reduction
176
eactions that involve the transfer of electrons
redox (oxidation-reduction)
177
nuclear process that emits a particle made of two protons and two neutrons
alpha decay
178
Americium-241 undergoes this process in smoke detectors
alpha decay
179
particle utilized by Rutherford (with Geiger and Marsden) to do the gold foil experiment
alpha
180
particle that is a helium nucleus
alpha
181
nuclear process that emits an electron
beta decay
182
nuclear process mediated by the weak nuclear force
beta decay
183
carbon-14 undergoes this type of radioactive decay
beta decay
