Exam 2 (ch 4-5) Flashcards
1
Q
Binary Compounds (Ionic)
A
cation+anion-ide
2
Q
Name Al2O3
A
Aluminum Oxide
3
Q
Multivalent Cations
A
cation (charge)+anion-ide
4
Q
Name CuO
A
Copper (II) Oxide or -ous=lower, -ic=higher
5
Q
Oxyanions
A
Hypo-ite, -ite, -ate, Per-ate
2nd row (C, N) predict charge to O, -ate=O3
3rd row (P, S) predict to [Ar], -ate=O4
6
Q
Molecular Compounds
A
pre(1st)+pre(2nd)-ide
Higher atomic no. goes 1st
7
Q
Oxyacid
A
(HXO) = ate=ic, ite=ous
No O = Hydro(element)-ide
8
Q
Acetate
A
C2H3O2 -
9
Q
Carbonate
A
CO3 2-
10
Q
Hydrogen carbonate/bicarbonate
A
HCO3 -
11
Q
hydroxide
A
OH -
12
Q
nitrite
A
NO2 -
13
Q
nitrate
A
NO3 -
14
Q
chromate
A
CrO4 2-
15
Q
dichromate
A
Cr2O7 2-
16
Q
phosphate
A
PO4 3-
17
Q
Hydrogen phosphate
A
HPO4 2-
18
Q
dihydrogen phosphate
A
H2PO4 -
19
Q
Ammonium
A
NH4 +
20
Q
Permanganate
A
MnO4 -
21
Q
Sulfite
A
SO3 2-
22
Q
hydrogen sulfite/bisulfite
A
HSO3 -
23
Q
sulfate
A
SO4 2-
24
Q
cyanide
A
CN-
25
Peroxide
O2 2-
26
Binary Acids
2 elements (H+X), Hydro+nonmetal-ic+acid
27
Lewis Structure Rules (4)
8 electrons per atom
lowest FC
atoms 3rd row and below may have more than 8 electrons
puts a negative charge on most electronegative atom
28
reasonance
more than one possible Lewis Structure
29
exceptions to octet rule
ions/molecules with:
- odd no. electrons
- less than octet
- expanded octet
* H = 2
* B = 6
30
Name H3PO3
Phosphorous acid
31
Name H2CO3
Carbonic acid
32
Chromic acid chemical formula
H2CrO4
33
Acetic acid chemical formula
C2H4O2 or CH2O
34
How to determine the molecular formula of a compound (acids)
1. count back to the noble gas to find ionic charge
2. butterfly with O
3. add H to make even with O or add 2H and 1O
35
2 e- areas, 0 lone pairs
EDG = linear
MG = linear
Angle = 180
36
3 e- areas, 0 lone pairs
EDG= trigonal planar
MG= trigonal planar
Angle= 120
37
3 e-, 1 lone pair
EDG= trigonal planar
MG= bent
Angle= <120
38
4 e-, 0 lone pairs
EDG= tetrahedral
MG= tetrahedral
Angle= 109.5
39
4 e-, 1 lone pair
EDG= tetrahedral
MG= trigonal pyramidal
Angle= <109.5
40
4 e-, 2 lone pair
EDG= tetrahedral
MG= bent
Angle= <<109.5
41
5 e-, 0 lone pairs
EDG= trigonal bipyramidal
MG= trigonal bipyramidal
Angle= 90, 120
42
5 e-, 1 lone pair
EDG= trigonal bipyramidal
MG= seesaw
Angle= <90, <120
*never take from axis
43
5 e-, 2 lone pair
EDG= trigonal bipyramidal
MG= T-shape
Angle= <90
44
5 e-, 3 lone pairs
EDG= trigonal bipyramidal
MG= linear
Angle= 180
45
6 e-, 0 lone pairs
EDG= octahedral
MG= octahedral
Angle= 90
46
6 e-, 1 lone pair
*take from axis
EDG= octahedral
MG= square pyramidal
Angle= <90
47
6 e-, 2 lone pairs
*take from axis
EDG= octahedral
MG= square planar
Angle= 90
48
6 e-, 3 lone pairs
*don't take from axis
EDG= octahedral
MG= T-shaped
Angle= <90
49
6 e-, 4 lone pairs
EDG= octahedral
MG= linear
Angle= 180
50
How to determine polarity
use vectors to show electronegativity
(point towards most electronegative atom)
51
nonpolar molecule
net dipole = 0
pulled equally in all directions = canceled
52
Polar molecule
permanent dipole moment
unsymmetrical EDG
53
VSEPR theory
best geometric arrangement
predicts shape and bond angles
54
Valence bond theory
localized electron model
chemical bond = overlapped e- orbitals
hybridization
55
hybridization
mixing of atomic orbitals
s to sp3d5 depending on no. of things going on
electrons get promoted from ground state to allow to be shared and bonded
56
sigma bonds
head to head overlap
1 per bond
cylindrical symmetry about internuclear axis
57
Pi bonds
side to side overlap
the rest of the bonds
e- density above/below internuclear axis
58
Hypochlorite
ClO -
59
Chlorite
ClO2 -
60
Chlorate
ClO3 -
61
Perchlorate
ClO4 -
62
Difference between VSEPR and Valence bond theory
VBT describes chemical bonding of an atom while VSEPR describes the molecular shape based on electron clouds
63
bond rotation, single bond
free rotation
64
bond rotation, double
restricted
65
bond rotation, same on each side
cis
66
bond rotation, mixed
trans
67
difference between VSEPR and VBT
VSEPR = shape and angles
VBT = chemical bonding
68
Lewis theory prob: bond angles
VSEPR
69
Lewis theory prob: resonance, chem bond
VBT, hybridization
70
Lewis theory prob: magnetic behavior
molecular orbital theory (MO)
71
diamagnetic
repelled, all bonded/paired e- or bond=unbond
72
paramagnetic
unbonded e-
73
bond strength
Hi Bond Order
shorter bonds
- Hi number of bonds
- hi difference in EN
