1. Warm-up  Draw the following in VSEPR a) Butane b) Cyclopropane c) Dichloromethane d) 2-Bromopropane

2. Carbon Hybridization

3. Atomic Orbitals of Carbon  Valence e- have different energy levels!!! 2 e- in 2s 2 e- in 2p  This cannot create 4 equal bonds!

4. Atomic vs Bonding Orbital Atomic Orbitals  Distinct s, p, d, and f orbitals  explains the spectra of individual atoms Bonding Orbitals  Elements will fuse half filled orbitals to make Hybrid Orbitals  Fusion of s and p orbitals creates sp hybrid orbital

5. What is a Bonding Orbital?  Bonding orbitals are half-filled orbitals s-bonding p-bonding orbital

6. sp 3 Hybridization 1. e- transfer: 2s 2 to empty pz 2. Fusion: 1 s-orbital with all 3 p-orbitals 3. Hybridization: creation of 4 x sp 3 hybrid orbitals

7. Orbital shapes  Will arrange themselves in a tetrahedral arrangement

8. Sigma bonds (single covalent bond)  Formed by a ‘head-on’ or axial overlapping of half filled orbitals  The electron cloud formed is cylindrically symmetrical around the inter nuclear axis

10. Methane – CH 4  4 sigma bonds  Created by 4 x sp3 - s-orbital overlap

11. Practice: draw the orbital model of ethane, name the bonds 6 sigma bonds C-H (sp3/s overlap) 1 sigma bond C-C (sp3/sp3 overlap)

12. Prctice  Draw Butane in VSEPR and Orbital model