Word Splash – Write a few sentences about how the following terms are related

Hybrid orbitals

Lewis Structures

Bonding

Hybridization

Additional Notes

Structure and Bonding – sp3 orbitals

• Look at methane, CH4

• We must take a look at the 2s and 2p orbitals of carbon

• Carbon has two core electrons, and 4 valence• Look at the ground state electron

configuration

Structure and Bonding - sp3 orbitals

Structure and Bonding - sp3 orbitals

• Using the ground state configuration, carbon should only form two bonds

• Bc there are only two unpaired electrons:

• This is NOT STABLE! NO OCTET!• Does not work!

Structure and Bonding - sp3 orbitals• Second possibility: with energy, promote an electron in 2s to the

empty 2p orbital

• Still not good description! This means carbon would form two types of bonds: 3 bonds with the 2p orbitals and 1 bond with the 2s orbital

Structure and Bonding - sp3 orbitals

• Evidence shows that the four bonds in methane are identical

• We do not use pure s and pure p orbitals, instead we use hybrid of the two types of orbitals

Structure and Bonding – sp3 orbitals

• Hybridization of the 2s and three 2p orbitals produced four hybrid orbitals:

Structure and Bonding – sp3 orbitals

• Each bond in CH4 is formed by an overlap of one sp3 orbital of carbon with a 1s orbital from hydrogen

Structure and Bonding - sp2 orbitals

• One 2s orbital and two 2p orbitals form three sp2 hybrid orbitals, leaving one of the 2p orbitals unhybridized

Structure and Bonding - sp2 orbitals

• Let’s look at ethene, C2H4

Structure and Bonding – sp orbitals

• Let’s look at ethyne, C2H2

Summary

Summary