1

Let’s get it on!!!!!!

2

Name the geometry and give the bond angles?

3

Name the geometry and give the bond angles?

trigonal pyramidal

107.3

4

Define covalent bond.

5

Define covalent bond.

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

6

List ALL the common diatomic molecules.

7

List ALL the common diatomic molecules.

H2 hydrogen

N2 nitrogen

O2 oxygen

F2 fluorine

Cl2 chlorine

Br2 bromine

I2 iodine

8

Draw the Lewis structure and the structural formula for water.

9

Draw the Lewis structure and the structural formula for water.

H O H OH H

StructuralLewis

10

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

11

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

12

The green line refers to a molecules ____________.

Distance

ENERGY

13

The green line refers to a molecules ____________.

Distance

ENERGY

BONDDISSOCIATIONENERGY

14

The arrow is pointing to a

15

The arrow is pointing to a

σ sigma bond

16

What is the relationship between bond length and bond strength?

17

What is the relationship between bond length and bond strength?

The shorter the bond the stronger it is!!!

18

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

19

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

20

List the rules for naming simple binary molecules

21

List the rules for naming simple binary molecules

1) Left to Right2) “-ide” be back!3) Junkies need their PRE-fix

a. EXCLUDE MONO on first element

22

Name this H3PO3

23

Name this H3PO3

phosphorous acid

PO33- phosphite ion

24

Define resonance. Draw O3 showing resonance.

25

Define resonance. Draw O3 showing resonance.

A structure has resonance when one or more correct Lewis structures can be draw to show the sharing of electrons.

OO

O

26

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

27

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

mono - 1di - 2tri - 3tetra - 4penta - 5

hexa - 6hepta - 7octa - 8nona - 9 deca - 10

28

List all 3 exceptions to the octet rule we discussed.

29

List all 3 exceptions to the octet rule we discussed.

I. Odd number of e-

II. Fewer than 8 e-

III. Expanded Octet

30

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

31

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

NO2

BH3

SF6

O N O

H B H

H

SF

FF

F

F

F

32

Define bonding orbital.

33

Define bonding orbital.

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

34

What does VESPR stand for and what does it mean?

35

What does VSEPR stand for and what does it mean?

V alence

S hell

E lectron

P air

R epulsion

The VSPER model states that atoms will arrange themselves into molecules in such a way as to minimize the repulsion between pairs of electrons

36

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

37

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

109.5

38

Name all of these molecular structure models.

39

Name all of these molecular structure models.

Stick

Space Filling

Ball & Stick

40

Name and describe all IMF discussed in class.

41

Name and describe all IMF discussed in class.

Dispersion Forces

Attraction between non-polar molecules

Electrons move and create small partial charges allowing for attraction

Dipole Dipole Forces

Attraction between polar molecules

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

42

According to the chart what is the bond character ratio of N2?

43

According to the chart what is the bond character ratio of N2?

100:0 covalent:ionic

N=3.04 3.04-3.04=0.00

44

Which Molecule is polar and why?

45

Which Molecule is polar and why?

F

F F

F

C H N H

O

46

Which Molecule is polar and why?

F

F F

F

C

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.

H N H

O

47

Draw the Lewis structure of sulfate.

48

Draw the Lewis structure of sulfate.

S O

O

O

O

2-

S O

O

O

O

2-

49

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

50

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 B

H

H

N

H

H

H