1. Covalent Bonding Formation of hydrogen chloride: Cl ® Cl H H +
Lone pairs, valence electrons not involved in covalent bond
Formation of hydrogen chloride:
· · Cl
· · Cl
· · H H +
® H - Cl
· ·
· ·
Covalent bond, shared electrons
Structural Formula: H-Cl (lone pairs are not drawn)

2. + Lewis Structures H H2: ® H H or H H Cl + ® Cl Cl Cl2: or Cl Cl+
H2:
® H H
or H H Cl
· · +
® Cl Cl
· ·
Cl2:
or Cl Cl
· ·
Structural Formula: Cl-Cl

3. Double and Triple Bonds
Atoms can share 4 electrons to form a double bond or 6 electrons to form a triple bond. =
O O
· ·
O2:
· ·
N N 
N2:
The number of shared electron pairs (covalent bonds) that an atom can form is the
bonding capacity.

4. Multiple Covalent Bonds• • N • •• •• N • • N •• • • N • •• N ••

5. Multiple Covalent Bonds• • • C O • ••
• • O • C • • • O
• •
• • •
• • • C O •• C O ••

6. Drawing Lewis Structures
Arrange the element symbols.
Central atoms are generally those with the highest bonding capacity.
Carbon atoms are always central atoms
Hydrogen atoms are always peripheral atoms
Add up the number of valence electrons from all atoms.
Add one electron for each negative charge and subtract one for each positive charge.
Draw a skeleton structure with atoms attached by single bonds.
Complete the octets of peripheral atoms.
Place extra electrons on the central atom.
If the central atom doesn’t have an octet, try forming multiple bonds by moving lone pairs.

7. Strategy for Writing Lewis Structures

8. Structural Formula
From the Lewis structure, remove dots representing lone pairs
Replace bond dots with a dash
H can only accommodate two electrons
H and O are common exceptions to rule 2
Organic compounds are not compact nor symmetrical.

9. or H F HF: H F H O H or H O H H2O: H N H H or H N H H NH3: H C H H
Draw Lewis structures and the structural formula for:
· ·
or H F
· ·
HF:
H F
· ·
· ·
· ·
H O H
· ·
or H O H
· ·
H2O:
H N H H
· ·
or H N H H
· ·
NH3:
H C H H
· ·
or H C H H
CH4:

10. For NF3 : : : : : : : : : : N = 5e- F F N F = 7e- X 3 = 21e-
Molecular formula
For NF3
Atom placement : :
N = 5e- : F : : F : :
Sum of valence e- N
F = 7e-
X 3 = 21e-
Total e- : F : :
Remaining valence e-
Zero: NF3 is uncharged
Lewis structure

11. SAMPLE PROBLEM 10.1
Writing Lewis Structures for Molecules with One Central Atom
PROBLEM:
Write a Lewis structure for CCl2F2, one of the compounds responsible for the depletion of stratospheric ozone.
SOLUTION: Cl
Step 1: Carbon has the highest bonding capacity and is the central atom.
The other atoms are placed around it. Cl C F F
Steps 2-4:
C has 4 valence e-, Cl and F each have 7. The sum is 4 + 4(7) = 32 valence e-. : C Cl F : :
Make bonds and fill in remaining valence electrons placing 8e- around each atom. :

12. H : H C O H : H SAMPLE PROBLEM 10.2
Writing Lewis Structure for Molecules with More than One Central Atom
PROBLEM:
Write the Lewis structure for methanol (molecular formula CH4O), an important industrial alcohol that is being used as a gasoline alternative in car engines.
SOLUTION:
Hydrogen can have only one bond so C and O must be next to each other with H filling in the bonds.
There are 4(1) = 14 valence e-.
C has 4 bonds and O has 2. O has 2 pair of nonbonding e-. H : H C O H : H

13. : C C H H : : : SAMPLE PROBLEM 10.3
Writing Lewis Structures for Molecules with Multiple Bonds.
PROBLEM:
Write Lewis structures for the following:
(a) Ethylene (C2H4), the most important reactant in the manufacture of polymers
(b) Nitrogen (N2), the most abundant atmospheric gas
PLAN:
For molecules with multiple bonds, there is a Step 5 which follows the other steps in Lewis structure construction. If a central atom does not have 8e-, an octet, then e- can be moved in to form a multiple bond.
SOLUTION:
(a) There are 2(4) + 4(1) = 12 valence e-. H can have only one bond per atom. C H : C H
(b) N2 has 2(5) = 10 valence e-. Therefore a triple bond is required to make the octet around each N. N : . N : . N :

14. Polyatomic Ions
Many compounds contain a combination of covalent and ionic bonds.
E.g. NaOH
OH- is a polyatomic ion with a covalent bond between O and H
Ionic bond between Na+ and OH-

15. Coordinate Covalent Bonds
A covalent bond in which both of the shared electrons come from the same atom.
E.g. NH3 (ammonia) and H+ (hydrogen ion) to form NH4 (ammonium)

16. Practice Problems
p #1-15

17. Drawing Lewis Structures
· ·
Cl C Cl O
· ·
· ·
COCl2
24 ve’s
· ·
· ·
· ·
· ·
· ·
· ·
· ·
· ·
HOCl
14 ve’s
H O Cl
· ·
· ·
· · 
· ·
O Cl O O
· ·
· ·
· ·
· ·
ClO3
26 ve’s
· ·
· ·
· ·
· ·
· ·
H C O H H
· ·
CH3OH
14 ve’s
· ·