1. Warm Up #7
Draw the possible structures of the following: H2O, NH3, CO2
What is the name of CO2?
Explain what happens to the valence electrons in a covalent bond.
Why, given the octet rule, does this process differ from an ionic bond, where electrons are donated/received?

2. Covalent Bonds and Naming

3. Review Covalent Bond – SHARING electrons Lewis Dot Structures
Lone Pairs are NOT shared
Goal: 8 valence electrons (or 2)

4. Naming If dealing with TWO non-metals… PREFIXES are used
1 = mono 2 = di 3 = tri
4 = tetra 5 = penta 6 = hexa
7 = hepta 8 = octa 9 = nona
10 = deca

5. Naming Applied
Ex. CO2
If first non-metal has NO subscript…name stays same
Second non-metal = prefix ALWAYS
Carbon Dioxide
Ex. H20 (water)
If first non-metal HAS subscript, use prefixes
Dihydrogen Monoxide

6. Quick Quiz #2 yes, you should name these. SO3 N2O Cl2O8
N2O3 (watch out for the last two…)
BeO Cu2O

7. Types of Bonding
Single Bond – one electron on each element is shared (F-F)
Double Bond – two electrons on each element are shared (O = O)
Triple Bond – three electrons on each element are shared (N N)

8. Sigma and Pi Bonds Bonding affects shape of orbital (p-orbitals)
Sigma Bond (σ) – Single, double and triple bonds (1σ each)
Pi Bond (π) – Double (1π) and triple bonds (2π)
Ex. F – F (1σ)
Ex. O = O (1σ, 1π)
Ex. N N (1 σ, 2π)