Common Polyatomic Ions Flashcards
1
Q
Acetate
A
C2H3O2-
2
Q
Carbonate
A
CO3 2-
3
Q
Hydrogencarbonate (bicarbonate)
A
HCO3-
4
Q
Hydroxide
A
OH-
5
Q
Nitrate
A
NO3-
6
Q
Nitrite
A
NO2-
7
Q
Chromate
A
CrO4 2-
8
Q
Dichromate
A
Cr2O7 2-
9
Q
Ammonium
A
NH4+
10
Q
Hypochlorite
A
ClO-
11
Q
Chlorite
A
ClO2
12
Q
Chlorate
A
ClO3 -
13
Q
Perchlorate
A
ClO4 -
14
Q
Sulfate
A
SO4 2-
15
Q
Sulfite
A
SO3 2-
16
Q
Hydrogen sulfate
A
HSO4 -
17
Q
Hydrogen sulfite
A
HSO3 -
18
Q
C2H3O2 -
A
Acetate
19
Q
CO3 2-
A
Carbonate
20
Q
HCO3 -
A
Hydrgencarbonate
21
Q
OH-
A
Hydroxide
22
Q
NO3 -
A
Nitrate
23
Q
NO2 -
A
Nitrite
24
Q
CrO4 2-
A
Chromate
25
Cr2O7 2-
Dichromate
26
NH4 +
Ammonium
27
ClO-
Hypochlorite
28
ClO2 -
Chlorite
29
ClO3 -
Chlorate
30
ClO4 -
Perchlorate
31
SO4 2-
Sulfate
32
SO3 2-
Sulfite
33
HSO4 -
Hydrogen sulfate
34
HSO3 -
Hydrogen sulfite
35
Lattice energies are large when distance is (small or large?) and charges are (small or large?)
Distance - small (small atomic radii)
| Charges - large
36
```
Properties of alkali metals:
Bright or dull?
Brittle or malleable?
Good conductor of electricity or bad?
Melting point: high or low?
```
```
Properties of alkali metals:
Bright
malleable?
Good conductor of electricity
Melting point: low?
```
37
```
Properties of alkaline earth metals:
Bright or dull?
Brittle or malleable?
Good conductor of electricity or bad?
Melting point: high or low?
```
```
Properties of alkaline earth metals:
Bright
malleable (but less than group 1)
Good conductor of electricity
Melting point: low (but higher than 1)
```
38
VSEPR: 2 groups - 2 bonds, 0 lone pairs
Linear
39
VSEPR: 3 groups - 3 bonds, no lone pairs
Trigonal planar
40
VSEPR: 3 groups - 2 bonds, 1 lone pair
Bent
41
VSEPR: 4 groups - 4 bonds, 0 lone pairs
Tetrahedral
42
VSEPR: 4 groups - 3 bonds, 1 lone pair
Trigonal pyramidal
43
VSEPR: 4 groups - 2 bonds, 2 lone pairs
Bent
44
VSEPR: 5 groups - 5 bonds, 0 lone pairs
Trigonal bipyramidal
45
VSEPR: 5 groups - 4 bonds, 1 lone pair
See-saw
46
VSEPR: 5 groups - 3 bonds, 2 lone pairs
T-shaped
47
VSEPR: 5 groups - 2 bonds, 3 lone pairs
Linear
48
VSEPR: 6 groups - 6 bonds, 0 lone pairs
Octahedron
49
VSEPR: 6 groups - 5 bonds, 1 lone pair
Square pyramidal
50
VSEPR: 6 groups - 4 bonds, 2 lone pairs
Square planar
51
These molecular bonds result from head to head overlap.
Sigma bonds
52
Will a molecular bonds with greater overlap be stronger or weaker?
Stronger
53
Explain hybrid atomic orbitals.
When an s orbital combines with 3 p orbitals, it creates four equivalent hybrid orbitals, called sp3 orbitals.
54
This type of hybrid orbital results from one s orbital combining with 3 p orbitals.
sp3
55
This type of hybrid orbital results from the combination of one a orbital with 2 p orbitals
sp2
56
This type of molecular bond occurs when orbitals form a bond in a parallel manner (rather than head on)
Pi bonds
57
Hybrid orbitals: atoms with 4 charge clouds will form what type of hybrid orbitals?
Sp3
58
Hybrid orbitals: atoms with 3 charge clouds will combine to make what type of hybrid orbitals?
Sp2
59
Hybrid orbitals: atoms with 2 charge clouds will combine to make what kind of hybrid orbital?
Sp
60
Molecular orbital theory: this is the type of orbital interaction (1 of 2) that results in a roughly egg shaped orbital.
Additive or bonding molecular orbital, denoted sigma
61
Molecular orbital theory - this type of orbital interaction (1 of 2) results in a molecular orbital with a node in the middle.
Subtractive or antibonding, denoted Sigma star
62
MO theory: a molecule has 2 bonding and 1 anti bonding electrons. What is it's bond order? Is it stable?
Bond order = 1/2. It is stable because it's not zero.
63
MO theory: what has higher energy: bonding or anti bonding electrons?
Antibonding
64
MO theory: what goes on top of a MO diagram: bonding or anti bonding electrons?
Anti bonding
65
What is lattice energy?
The measure or electrostatic interaction energies between ions in a solid - essentially a measure of the strength of its bonds. It has a + value since it's technically the amount of energy required to break the bond.
