1. Covalent Bonding

2. Illustration of the formation of the Covalent bond between Hydrogen and Chlorine
HCl

3. Hydrogen(H) Hydrogen is a gas.
Hydrogen has only 1 electron in its outer shell 1P 0N
Hydrogen
H= 1,1

4. Chlorine (Cl) Chlorine is a poisonous gas.
It has 7 electrons in the outside shell and is not stable.
18N
17P
Chlorine
= 2,8,7

5. Neither Hydrogen nor Chlorine are stable, since both have less than 8 electrons in their outside shell. However this can easily be achieved by combining H and Cl together.
Watch how! 1P
0 N
17P
18N H Cl

6. A covalent bond will be formed between H and Cl by sharing a pair of electrons ….
A Hydrogen atom has only 1 electron which it cannot lose. Therefore , the only type of bond H can form is a covalent bond 1P 0N
17P
18N H Cl

7. HCl
1 atom of Hydrogen has combined with 1 atom of Chlorine. Both H and Cl are now in a stable state - each with a full outer shell. 1P 0N
17P
18N H Cl

8. Satisfying the Octet Rule…..
The Octet rule is simply a rule which helps us to understand bonding
Atoms bond together so that each atom attains an electron arrangement of 8 electrons in its outermost shell.

9. To satisfy the Octet Rule, atoms tend to gain, lose or share electrons
H and Cl shared one pair of electrons
The H began with 1 electron in its outer shell - It needed 2.
The Cl atom began with 7 electrons in its outer shell - It needed 8.
By sharing the pair of electrons, both atoms are now in a stable state.
H has 2 electrons in its outer shell and Cl has 8 in its outer shell.

10. Other examples of Covalent Bonds2 H
1 atom of Hydrogen has combined with 1 atom of Hydrogen. Both Hydrogens are now in a stable state - each with a full outer shell. 1P 0N 1P 0N H H

11. The Water molecule H O 2 1P 0N H 8P 8N H 1P 0N O

12. X O B. Lewis Structures 2s 2p Electron Dot Diagrams
show valence e- as dots
distribute dots like arrows in an orbital diagram
4 sides = 1 s-orbital, 3 p-orbitals
EX: oxygen X 2s 2p O

13. Ne B. Lewis Structures Octet Rule
Most atoms form bonds in order to obtain 8 valence e-
Full energy level stability ~ Noble Gases Ne

14. B. Lewis Structures - + Nonpolar Covalent - no charges
Polar Covalent - partial charges + -

15. C. Molecular Nomenclature
The Seven Diatomic Elements
Br2 I2 N2 Cl2 H2 O2 F2 H N O F Cl Br I