1. Lewis Dot Structure Rules:
Treat ions separately (e.g. NH4Cl)
Count only valence electrons
Assemble bonding framework
Fill up non-bonding electrons on
outer atoms
inner atoms

2. To do Lewis Structures:
Must be able to recognize
polyatomic ions
Must be able to identify
valence electrons
Must be able to construct
Bond framework
Periodic Table : Column numbers!
More complex: H outside
Formula hints
Acidic Hs bond to O atoms

3. Hints on Lewis Dot Structures
Octet “rule” is the most useful guideline.
Carbon forms 4 bonds.
Hydrogen can only form one bond.
Halogens will only form one bond
When multiple bonds are forming, they are usually between C, N, O or S.
Nonmetals can form single, double, and triple bonds, but not quadruple bonds.
Always account for single bonds and lone pairs before forming multiple bonds.
Look for resonance structures.

4. PCl3 5+(3*7)=26 e- Bonding Pairs Lone Pairs
(a.k.a. nonbonding electrons)

5. Covalent Bonding Multiple Bonds
It is possible for more than one pair of electrons to be shared between two atoms (multiple bonds):
One shared pair of electrons = single bond (e.g. H2);
Two shared pairs of electrons = double bond (e.g. O2);
Three shared pairs of electrons = triple bond (e.g. N2).
Generally, bond distances shorten with multiple bonding.
Octet in each case

6. Try Some Examples: Ozone (O3) CH3CH2NH2 H3PO4
NO2 vs. N2O vs. nitrate ion
SPENT LOTS O’ TIME PRACTICING…

9. Odd Number of Electrons…NO
Number of valence electrons = 11
Resonance occurs when more than one valid Lewis structure can be written for a particular molecule (i.e. rearrange electrons)
NO2
Number of valence electrons = 17
Molecules and atoms which are neutral (contain no formal charge) and with an unpaired electron are called Radicals O2

10. Beyond the Octet
Elements in the 3rd period or higher can have more than an octet if needed.
Atoms of these elements have valence d orbitals, which allow them to accommodate more than eight electrons.

11. More than an Octet…
Elements from the 3rd period and beyond, have ns, np and unfilled nd orbitals which can be used in bonding
P : (Ne) 3s2 3p3 3d0
Number of valence electrons = 5 + (5 x 7) = 40
PCl5
SF4
S : (Ne) 3s2 3p4 3d0
Number of valence electrons = 6 + (4 x 7) = 34
The Larger the central atom, the more atoms you can bond to it – usually small atoms such as F, Cl and O allow central atoms such as P and S to expand their valency.

12. Less than an Octet…
BCl3
Group 3A atom only has six electrons around it
However, Lewis acids “accept” a pair of electrons readily from Lewis bases to establish a stable octet