Polyatomic Ions Flashcards
1
Q
Silver
A
Ag,+
2
Q
Zinc
A
Zn,2+
3
Q
Mercury(I)
A
Hg2,2+
4
Q
Ammonium
A
NH4,+
5
Q
Nitrite
A
NO2,-
6
Q
Nitrate
A
NO3,-
7
Q
Sulfite
A
SO3,2-
8
Q
Sulfate
A
SO4,2-
9
Q
Hydrogen Sulfate
A
HSO4,-
10
Q
Hydroxide
A
OH,-
11
Q
Cyanide
A
CN,-
12
Q
Phosphate
A
PO4,3-
13
Q
Hydrogen Phosphate
A
HPO4,2-
14
Q
Dihydrogen Phosphate
A
H2PO4,-
15
Q
Thiocyanate
A
NCS,-
16
Q
Carbonate
A
CO3,2-
17
Q
Hydrogen Carbonate
A
HCO3,-
18
Q
Hypochlorite
A
ClO,-
19
Q
Chlorite
A
ClO2,-
20
Q
Chlorate
A
ClO3,-
21
Q
Perchlorate
A
ClO4,-
22
Q
Hypobromite
A
BrO,-
23
Q
Bromite
A
BrO2,-
24
Q
Bromate
A
BrO3,-
25
Perbromate
BrO4,-
26
Hypoiodite
IO,-
27
Iodite
IO2,-
28
Iodate
IO3,-
29
Periodate
IO4,-
30
Acetate
C2H3O2,-
31
Permanganate
MnO4,-
32
Dichromate
Cr2O7,2-
33
Chromate
CrO4,2-
34
Peroxide
O2,2-
35
Oxalate
C2O4,2-
36
Amide
NH2,-
37
Borate
BO3,3-
38
Thiosulfate
S2O3,2-
39
RED CAT/ AN OX
Reduction takes place at the cathode, and oxidation takes place at the anode
40
OIL RIG
Oxidation is Losing electrons/ Reduction is gain electrons
41
The CAT gets FAT
A metallic cathode will always increase in mass
42
A/C
Electrons move through the wire from anode to cathode
43
Salt Bridge
Anions to anode, cations to cathode
44
Ions that are ALWAYS soluble in water
Na+, K+, NH4+, NO3-
45
The 7 strong acids
Hydrochloric Acid (HCl)
Hydrobromic Acid (HBr)
Hydroiodic Acid (HI)
Nitric Acid (HNO3)
Sulfuric Acid (H2SO4)
Chloric Acid (HClO3)
Perchloric Acid (HClO4)
46
The 8 strong bases
Lithium Hydroxide (LiOH)
Sodium Hydroxide (NaOH)
Potassium Hydroxide (KOH)
Rubidium Hydroxide (RbOH)
Cesium Hydroxide (CsOH)
Calcium Hydroxide (Ca(OH)2)
Strontium Hydroxide (Ca(OH)2)
Barium Hydroxide (Sr(OH)2)
47
5 Common weak acids
Hydrofluoric Acid (HF)
Acetic Acid (HC2H3O2)
Carbonic Acid (H2CO3)
Phosphoric Acid (H3PO4)
Hydrocyanic Acid (HCN)
48
2 common weak bases
Ammonia NH3
Conjugates of weak acids (NaC2H3O2, NaCN, NaHCO3, Na2CO3, etc.)
49
Strongest to weakest intramolecular forces
Network Covalent (C, Si, SiO2)
Ionic (metal/nonmetal, lattice energy based on magnitude of charge and ion size)
Metallic (Sea of electrons, malleability, conductivity, and luster)
Covalent (Sharing electrons, nonmetal/nonmetal combo)
50
Strongest to weakest intermolecular forces
Ion-Dipole (Interaction between an ion and a polar bond)
Hydrogen Bonding (Very polar bonds, H with O, N, or F)
Dipole-Dipole (2 polar molecules interacting)
London Dispersion Forces (temporary dipole moments, increases with atomic radius and mass because they are easily polarizable)
51
Linear
2 electron groups, 0 lone pairs, 180 degrees
52
Trigonal Planar
3 electron groups, 0 lone pairs, 120 degrees
53
Bent (3)
3 electron groups, 1 lone pair, <120 degrees
54
Tetrahedral
4 electron groups, 0 lone pairs, 109.5 degrees
55
Trigonal pyramidal
4 electron groups, 1 lone pair, ~107 degrees
56
Bent (4)
4 electron groups, 2 lone pairs, ~105 degrees
57
Trigonal Bipyramidal
5 electron groups, 0 lone pairs, 90 and 120 degrees
58
See-Saw
5 electron groups, 1 lone pair, <90 and <120 degrees
59
T-Structure
5 electron groups, 2 lone pairs, <90 degrees
60
Linear (5)
5 electron groups, 3 lone pairs, 180 degrees
61
Octahedral
6 electron groups, 0 lone pairs, 90 and 90 degrees
62
Square Pyramidal
6 electron groups, 1 lone pair, 90 and <90 degrees
63
Square Planar
6 electron groups, 2 lone pairs, 90 degrees
