Untitled - Kelly Walsh High School

326 INDEX
atoms (Cont.):
nomenclature, 21–26
overview, 15–16
periodic table, 17–19
Aufbau principle, 111–113
Avogadro’s number, 34–35, 40–42
balanced chemical equations, 32–36, 41
band theory of conductivity, 283–284
base anhydrides, 284
base dissociation constant (K b), 225–226
bases, 219–233
acid-base equilibrium, 223–226
Brønsted-Lowery theory, 220
Lewis theory, 227
overview, 53–55, 219–220
pH scale, 222–223
properties of salts and oxides, 226
strength of, 220–221
water dissociation constant, 221–222
weak, 227–233
beta emission, 293, 295
bimolecular reactions, 198
binary acids, 26
biochemistry (see Organic chemistry)
Bohr, Niels, 109
boiling-point elevation, 178–179
bonds
chemical, 127–144
bond energy and length, 137
covalent bonds, 132–135
electronegativity, 130
Lewis structures, 137–144
Lewis symbols, 128–130
overview, 127–128
resonance, 136
hydrogen bonding, 160
valence bond theory, 149–151
(See also Ionic bonds)
Born-Haber cycle, 132
branches, 309
Brønsted-Lowery acid-base theory, 220, 232
buffers, 236–237, 249
C (molar heat capacity), 99–101
c (specific heat capacity), 99–101
cal (calories), 98
calories (cal), 98
calorimetry, 98–100, 103–105
capillary action, 161–162
carbohydrates, 314–315, 322
carboxylic acid groups, 314, 318–320
catalysis:
condensation reactions, 319
hydrogenation, 317
kinetics, 196–197, 201
and reaction rate, 189
saponification, 321
cathodes, 269, 274–276
cations:
aqueous solutions, 53, 61
ionic bonding, 131
ionization energy, 121–122
Lewis structures for, 135
metals as, 24, 283
overview, 20
salt, 55
transition metals as, 287
cell notation, 269–270
cells:
actual potential, 272–273
electrolytic, 273–274
galvanic (voltaic), 268–270
and nucleic acids, 315–316
standard reduction potentials of,
270–271
unit, 162
chelating ligands, 287
chemical bonds, 127–144
bond energy and bond length, 137
covalent bonds, 132–135
electronegativity, 130
ionic bonds and lattice energy,
131–132
Lewis structures, 137–141
Lewis symbols, 128–130
overview, 127–128
resonance, 136
chemical equilibria, 203–218, 235–250
acid-base equilibrium, 223–226
buffers and pH, 236–237
calculating, 209–216
common-ion effect, 236
complex ion formation constant, 241
equilibrium constants, 205–206
Le Châtelier’s principle, 207–209
overview, 203–205, 235–236
pH and titrations, 241–248
solubility product constant, 238–240
titrations and indicators, 237–238