1. VSEPR What does VSEPR stand for?
What is the basis of the theory-assumptions?
Definitions: A (central atom)
X (bonding e- pr = e- domain)
E (non bonding e- pr)
CN (X + E around A)
For each formula, give CN, # bonding and nonbonding domains
AX2 AX AX2E AX4E2

2. CN 1-2 Possible VSEPR notations Examples?
Shape, bond angle, polar/nonpolar?

3. CN 3 Possible VSEPR notations Examples?
Shape, bond angle, polar/nonpolar?

4. CN 4 Possible VSEPR notations Examples?
Shape, bond angle, polar/nonpolar?

5. CN 5 Possible VSEPR notations Examples?
Shape, bond angle, polar/nonpolar?

6. CN 6 Possible VSEPR notations Examples?
Shape, bond angle, polar/nonpolar?

7. Polarity from Shape If symmetrical base structure = np
If asymmetrical = polar
Lone pairs on A = polar

8. Shapes of Larger Molecules
Ethane
Glycine (simplest amino acid)

9. 3 Types of Orbitals Atomic Orbitals (s, p, d, f)
belong to an atom and are described by quantum numbers
When atomic orbitals overlap to make covalent bonds, create new orbitals
Hybrid Orbitals and Molecular Orbitals

10. Molecular Orbitals (MO)
Hybrid Orbitals
described by Valence Bond Theory (VBT)
when atomic orbitals overlap, they “blob” together to make hybrid orbitals (sp, sp2, sp3, dsp3, d2sp3)
helps explain geometry and location of lone pairs in 3-D
Molecular Orbitals (MO)
described by MO Theory
when atomic orbitals overlap, they can make MO (, *, , *) (we will only do  and )
helps explain excitation, bond order, and magnetism (we will not cover this)

11. Hybridization
How does HCl make covalent bond? What orbitals are available for bonding?
What about BeF2 (if draw as covalent)?
# atomic orbitals that combine = # hybrid orbitals made

12. Look at BH3, CH4, PCl5, SF6

13. What is the hybridization scheme around central atom in
NH NH SO32-
Glycine? What about H-CC-COH?

14. Molecular Orbitals Help explain excitation, bond order, magnetism
Describe orbitals within molecules (not on atom like atomic orbitals)
Like atomic orbitals, described by , follow Pauli, have a definite Energy
Like hybrid orbitals, # atomic orbitals that combine = # MO that form
Instead of “blobbing” get constructive and destructive combination (not covering this)

15. MO Theory When atomic orbitals overlap can do so in one of two ways
Head to Head collision
Side to Side collision
Head on →  bond (s+s, s+p, p+p, sp3 + s)
Side to Side →  bond (p+p, p+d, d+d)

16. Describing Bonding
Methane: what is the hybridization scheme around C? Any sigma or pi bonds? Describe the bonding. O
What about H-C-H?
What about ethene? ethyne?
Acetonitrile (CH3CN)? 

17. Which have delocalized  bonds?
SO3 SO32- H2CO O3 NH4+

18. Side Note

20. Suspension of Liquid Oxygen between Magnets (paramagnetic)