Chapter 3 Simple Bonding Theory

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Presentation transcript:

Chapter 3 Simple Bonding Theory Lewis Dot Structures Resonance Formal Charge VSEPR: the subtle effects

Lewis Dot Structures 1. Count valence electrons 2. Arrange atoms 3. Add bonds 4. Add lone pairs 5. Convert lone pairs to bonding pairs (octet rule and exceptions)

Lewis Dot Structures Examples: CO2 SO3 N2O XeF4 ClF3 PCl6–

Why does the octet rule work?

More complex NO2 NO

= Group # - #unshared electrons on atom - # bonds to atom Formal Charge = Group # - #unshared electrons on atom - # bonds to atom Example: O3

Resonance Example: SO3

Resonance and Formal Charge Example: SCN-

Resonance and Formal Charge Example: SCN-

Octet Rule vs. Pi Bonding Trends BeF2 and BF3

Octet Rule vs. Formal Charge Always follow octet rule Exceptions? SO42-

VSEPR Maximize “personal space” CO2, SO3, SO42–, PCl5, SF6 Lone pairs vs. bonding pairs? Single bonds vs. multiple bonds? Electronegativity effects

VSEPR

Lone Pair Effects

Pi Bonds vs. Lone Pairs: Guess these bond angles.

Pi Bonds vs. Lone Pairs: Guess these bond angles.

Pi Bonds vs. Lone Pairs

Pi Bonds vs. Lone Pairs Which take up more room: lone pairs or a pi bond?

Electronegativity Effects

Electronegativity Effects Molecule X-P-X Angle o PF3 97.8 PCl3 100.3 PBr3 101 Explain this trend.

Electronegativity Effects Molecule X-P-X Angle o PF3 97.8 PCl3 100.3 PBr3 101 Terminal Atom Effects: F: Electron density of the bond pairs is mostly near the F. Electron density near the central atom is less, which decreases bond pair – bond pair repulsion near the P.

Electronegativity Effects Molecule H-X-H Angle o H2O 104.4 H2S 92.1 H2Se 90.6 Explain this trend.

Electronegativity Effects Molecule H-X-H Angle o H2O 104.4 H2S 92.1 H2Se 90.6 Explain this trend. Central atom effects: O: as O pulls more electron density toward it, bonds have more electron density near the central atom. This causes greater bond pair – bond pair repulsions.

Electronegativity Effects Molecule X-As-X Angle o AsF3 AsCl3 AsBr3 Predict this trend.

Predicting Positions of Different Atoms PF3Cl2 Are Cl atoms axial or equatorial?

Homework Chapter 3 7, 9 acde, 11, 12,14,29,30a