1

2

trigonal pyramidal
107.3
3

4

The electrostatic force between atoms that results in the sharing of one or more pairs of electrons
5

List ALL the common diatomic molecules.
6

List ALL the common diatomic molecules.
H2 hydrogen
N2
O2
F2
Cl2
Br2
I2 nitrogen oxygen fluorine chlorine bromine iodine
7

Draw the Lewis structure and the structural formula for water.
8

Draw the Lewis structure and the structural formula for water.
Structural
H O H
H
Lewis
O H
9

Name 3 ways to tell apart an oxyacid and a binary acid.
10

Name 3 ways to tell apart an oxyacid and a binary acid.
1. Binary H and usually a halogen
2. Oxyacids contain OXYANIONS
3. Binary start with prefix hydro-
4. Some Oxyacids end in –ous
5. Formula of Binary only has 2 capital letters
11

E
R
E
N
G
Y
The green line refers to a molecules ____________.
12

E
R
E
N
G
Y
The green line refers to a molecules ____________.
BOND
DISSOCIATION
ENERGY
13

14

15

What is the relationship between bond length and bond strength?
16

What is the relationship between bond length and bond strength?
17

Define endothermic! And explain the difference between endothemric and exothermic!!!
18

Define endothermic! And explain the difference between endothemric and exothermic!!!
Endothermic is used to describe a chemical reaction when you have to put more energy in to break the bonds then you get out when new bonds form!!!!
Endothermic- you put more energy in
Exothermic- you get more energy out
19

List the rules for naming simple binary molecules
20

List the rules for naming simple binary molecules
1) Left to Right
2) “-ide” be back!
3) Junkies need their PRE-fix a. EXCLUDE MONO on first element
21

3
3
22

3
3
3
3-
23

Define resonance. Draw O
3 showing resonance.
24

Define resonance. Draw O
3 showing resonance.
A structure has resonance when one or more correct Lewis structures can be draw to show the sharing of electrons.
O
O O
25

List the prefixes used in naming covalent molecules for 1-10.
26

List the prefixes used in naming covalent molecules for 1-10.
mono di
- 1
- 2 tri - 3 tetra - 4 penta - 5 hexa hepta octa nona deca
- 6
- 7
- 8
- 9
- 10
27

List all 3 exceptions to the octet rule we discussed.
28

List all 3 exceptions to the octet rule we discussed.
I. Odd number of e -
II. Fewer than 8 e -
III.Expanded Octet
29

Give an example of each of the exceptions to the octet rule.
30

Give an example of each of the exceptions to the octet rule.
NO
2
O N O
BH
3
H B H
H
SF
6
F
F
F
S
F
F
F
31

32

The region where shared electrons are most likely to be found.
33

What does VESPR stand for and what does it mean?
34

What does VSEPR stand for and what does it mean?
V alence
S hell
E lectron
P air
The VSPER model states that atoms will arrange themselves into molecules in such a way as to minimize the repulsion between pairs of electrons
R epulsion
35

A molecule that is sp3 hybridized with no lonepairs on the central atom would have bond angles of?
36

A molecule that is sp3 hybridized with no lonepairs on the central atom would have bond angles of?
109.5
37

Name all of these molecular structure models.
38

Name all of these molecular structure models.
Stick
Space Filling
Ball &
Stick
39

Name and describe all IMF discussed in class.
40

Name and describe all IMF discussed in class.
Dipole Dipole Forces
Dispersion Forces
Attraction between non-polar molecules
Attraction between polar molecules
Electrons move and create small partial charges allowing for attraction
The negative end of a polar molecule is attracted to the positive end of another polar molecule and vice-versa
Hydrogen bonding
Attractive force between a H on one molecule and the N, F, or O of another molecule
41

According to the chart what is the bond character ratio of N
2
?
42

According to the chart what is the bond character ratio of N
2
?
100:0 covalent:ionic
N=3.04 3.04-3.04=0.00
43

Which Molecule is polar and why?
44

Which Molecule is polar and why?
F
F C F
H N H
F
O
45

Which Molecule is polar and why?
F
F C F
H N H
F
O
Oxygen is the most electronegative atom in the molecule and will pull all electrons toward itself.
F is more electronegative than C but the geometry cancels out the pull of each F.
46

Draw the Lewis structure of sulfate.
47

Draw the Lewis structure of sulfate.
2-
O
O
S O
O
O
O
S O
O
2-
48

Explain a coordinate covalent bond and give an example of one.
49

Explain a coordinate covalent bond and give an example of one.
A coordinate covalent bond occurs when on atom donates both electrons that are involved in making a bond.
H
H B
H
H
N
H
H
50