2AB things to memorize Flashcards
(52 cards)
1
Q
diatomic element & phase: Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, Iodine
A
H2(g), N2(g), O2(g), F2(g), Cl2(g), Br2(l), I2(s)
2
Q
monatomic ions with fixed charge (+1)
A
H+, Li+, Na+, K+, Cs+, Ag+
3
Q
monatomic ions with fixed charge (+2)
A
Be2+, Mg2+, Ca2+, Sr2+, Ba2+, Zn2+
4
Q
monatomic ions with fixed charge (+3)
A
Al3+
5
Q
Hydride, Fluoride, Chloride, Bromide, Iodide
A
H-, F-, Cl-, Br-, I-
6
Q
Oxide, Sulfide, Nitride, Phosphide
A
O2- , S2-, N3-, P3-
7
Q
Fe3+
A
Ferric
8
Q
Fe2+
A
Ferrous
9
Q
Cu2+
A
Cupric
10
Q
Cu+
A
Cuprous
11
Q
Co3+
A
Cobaltic
12
Q
Co2+
A
Cobaltous
13
Q
Hg2+
A
Mercuric
14
Q
(Hg2)2+
A
Mercurous
15
Q
Sn4+
A
Stannic
16
Q
Sn2+
A
Stannous
17
Q
Pb4+
A
Plumbic
18
Q
Pb2+
A
Plumbous
19
Q
ammonium
A
NH4+
20
Q
Hydronium
A
H3O+
21
Q
Nitrite
A
NO2-
22
Q
Nitrate
A
NO3-
23
Q
Sulfite
A
SO32-
24
Q
Sulfate
A
SO42-
25
Hydrogen Sulfate
HSO4-
26
Cyanide
CN-
27
Phosphite
PO33-
28
Phosphate
PO43-
29
Hydrogen Phosphate
HPO42-
30
Dihydrogen Phosphate
H2PO4-
31
Carbonate
CO32-
32
Hydrogen Carbonate
HCO3-
33
Permanganate
MnO4-
34
Dichromate
Cr2O7 2-
35
Chromate
CrO4 2-
36
Peroxide
O2 2-
37
Hypochlorite
ClO-
38
Chlorite
ClO2-
39
Chlorate
ClO3 -
40
Hydroxide
OH-
41
Acetate
C2H3O2-
42
Perchlorate
ClO4-
43
Strong Acids
HCl, HBr, HI, HClO4, HClO3, HNO3, H2SO4
44
Strong Bases
LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Mg(OH)2, Sr(OH)2, Ba(OH)2
45
Weak base
NH3
46
Rules for Assigning Oxidation States
1. O.S. = 0 for elemental compounds
2. Monatomic ions have O.S. = to their charge (see above for fixed charge monatomic ions)
3. The sum of oxidations states in a compound = the overall charge of that compound
4. Five reliable groups can be used for assigning atoms with variable oxidations states:
Groups I and II have the charge of their group number.
F = -1 (exception = F2)
H is almost always +1 (exceptions: H2, metal hydrides)
O is almost always -2 (exceptions: O2, O3, peroxides)
Halides (Cl, Br, I) are -1 except when bonded to O or F
47
LINEAR Electron and Molecular Geometry
bond angles: 180, spatial geometry: linear electron pair geometry: (sp)
48
TRIGONAL PLANAR Electron and Molecular Geometry
bond angles: 120 spatial geometry: trigonal planar electron pair geometry: (sp2) lone pair substitutions: BENT
49
TETRAHEDRAL Electron and Molecular Geometry
bond angles: 109.5 spatial geometry: tetrahedral electron pair geometry: (sp3) lone pair substitutions: TRIGONAL PYRAMIDAL, BENT
50
TRIGONAL BIPYRAMIDAL Electron and Molecular Geometry
bond angles: 90,120 spatial geometry: trigonal bipyramidal electron pair geometry: (dsp3) lone pair substitutions: SAWHORSE, T-SHAPED, LINEAR
51
OCTAHEDRAL Electron and Molecular Geometry
bond angles: 90 spatial geometry: octahedral electron pair geometry: (d2sp3) lone pair substitutions: SQUARE PYRAMIDAL, SQUARE PLANAR, T-SHAPED, LINEAR
52
oxalate
C2O4 2-
