part 02 covalent bonding and covalent compounds
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Part 02 Covalent Bonding and Covalent Compounds. 1. Covalent Bonding - two or more non metals - two or more semi metals - share at least one pair of valence electrons - all the atoms get a stable octet or in the case of hydrogen, a duet

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Presentation Transcript
slide2
1. Covalent Bonding

- two or more nonmetals

- two or more semimetals

- share at least one pair of valence electrons

- all the atoms get a stable octet

or in the case of hydrogen, a duet

- a molecule is formed. The sharing of valence electrons holds the atoms together

slide3
2. Covalent Bonding Between Like Atoms:

The Diatomic Molecules

H

H

Lewis Dot Diagram

- shared pair belongs to both atoms

- each atom has a stable duet

slide4
H

H

Structural Diagram

- dash represents one shared pair of valence electrons

- a single covalent bond

- formula, H20

- no charges, no electrons lost or gained

- name, dihydrogen, or just hydrogen

- shape or molecular geometry, linear

slide5
Lewis Dot Diagram

F

F

- shared pair belongs to both atoms

- each atom has a stable octet

slide6
Nonbonding electrons

F

F

Structural Diagram

Bonding electrons

- a single covalent bond

- formula, F20

- no charges, no electrons lost or gained

- name, difluorine, or just fluorine

- shape or molecular geometry, linear

slide7
Nonbonding electrons

I

I

Structural Diagram

Bonding electrons

- all the other halogens bond the same way

- Cl2, Br2, I2 all with no charge

slide8
O

O

O

O

No octets!

Unpaired electrons!

O

O

Lewis Dot Diagram

slide9
O

O

Structural Diagram

- two dashes are two shared pairs of electrons, i.e., four electrons

- a double covalent bond

- all the other electrons are nonbonding electrons

slide10
O

O

Structural Diagram

- formula, O20

- no charge, no electrons lost or gained

- name, dioxygen or just oxygen

- shape or molecular geometry, linear

slide11
N

N

N

N

N

N

No octets!

Unpaired electrons!

N

N

No octets!

Unpaired electrons!

Lewis Dot Diagram

slide12
N

N

Structural Diagram

- three dashes are three shared pairs of electrons, i.e., six electrons

- a triple covalent bond

- all the other electrons are nonbonding electrons

slide13
N

N

Structural Diagram

- formula, N20

- no charge, no electrons lost or gained

- name, dinitrogen or nitrogen

- shape or molecular geometry, linear

slide14
3. Summary: The Diatomic Molecules

a. Single Covalent Bonds

1) Hydrogen, H2

2) Fluorine, F2

3) Chlorine, Cl2

4) Bromine, Br2

4) Iodine, I2

b. Double Bond, Oxygen, O2

c. Triple Bond, Nitrogen N2

Assignment: Read p236-240

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