1. Read Section 6.3 After Quiz Lewis Structures & Molecular Geometries

2. Lewis Dot Diagrams Represent the valence e- for an atom using dots.
Start at the top and place e- on each side going clockwise. Once there are e- on each side, begin to pair them up.
Sodium
1 valence e-
Magnesium
2 valence e-

3. Aluminum
3 valence e-
Silicon
4 valence e-
Phosphorus
5 valence e-
Sulfur
6 valence e-
Chlorine
7 valence e-
Argon
8 valence e-

4. Elements in the same family have the same number of valence e- and the same Lewis dot arrangement

5. Bonding Using Lewis Dot Diagrams
Share a pair of e- to form
and
So that each atom has a full outer energy level
A pair of shared e- can also be represented with a dashed line.

6. Exceptions to the Octet Rule
In covalent bonds, atoms always share e- to reach a full valence shell of 8 valence e-…except…
Hydrogen only needs 2 e- in its outer energy level.
Boron only needs 6 e- in its outer energy level.
Some elements can form an expanded octet using empty d-orbitals to form bonds and have more than 8 valence e-.

7. 5 Steps for Drawing Lewis Structures
Count the total number of valence electrons for all atoms.
Attach each atom to the central atom with a single bond (single bond = 2 shared electrons)
Complete the octet for the attached atoms by adding pairs of non-bonding electrons.
Complete the octet for the central atom by adding pairs of non-bonding electrons

8. 5. Count the total number of electrons in your structure and compare to step one.
If the number of e- is the same, it is correct.
If you used too many e-, add double bond(s) and check your total again (usually add one double bond for each two electrons that you are over the total).
If there are extra electrons left over, add them as non-bonding electrons on the central atom. This is called an expanded octet.

9. Valence Shell Electron Pair Repulsion Theory
Abbreviated “VSEPR”
Pairs of e- around an atom repel each other and will form an arrangement that minimizes this repulsion (i.e. spread as far apart from each other as possible). As a result, molecules tend to form predictable shapes.
Lone pairs of non-bonding e- have greater repulsion than bonded pairs of e-.

10. Basic VSEPR Geometries
Molecular Geometry
ABE Notation
Atoms bonded to the central atom
Non-bonding pairs on the central atom
Tetrahedral
AB4 4
Trigonal Pyramid
AB3E 3 1
Bent
AB2E2 or AB2E 2
1 or 2
Linear
AB2
Trigonal Planar
AB3

11. Expanded Octet Geometries
Molecular Geometry
ABE Notation
Atoms bonded to the central atom
Non-bonding pairs on the central atom
Octahedral
AB6 6
Square Pyramid
AB5E 5 1
Square Planar
AB4E2 4 2
Trigonal Bipyramid
AB5
Seesaw
AB4E
T-Shaped
AB3E2 3
Linear
AB2E4