VSEPR and CARBON CHEMISTRY

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Presentation transcript:

VSEPR and CARBON CHEMISTRY Unit 3

VSEPR (Valence Shell Electron Pair Repulsion 2 Rules Govern VSEPR: Regions of high electron concentration repel one another. to minimize these repulsions these regions move as far away from each other as possible. We do not distinguish between single and multiple bonds. **Remember VSEPR simply extends Lewis’s theory of bonding to account for molecular shapes by adding rules that account for bond angles. ***When naming a shape we only consider the position of atoms not lone pairs.

Linear Geometry. Simple arragnement Notice the bond angle is 180° AX2 CO2 AX H2 AXE CN- Notice the bond angle is 180°

Angular/ Bent Geometry Simple Arrangement AX2E H2O AX2E2 SeBr2 AXE3 Cl2 Notice the bond angle is 104°

Trigonal Planar Geometry Simple arrangement: AX3 AlBr3 BF3 COCl2 The bond angles will be 120°

Trigonal Pyrimidal Geometry Simple arrangement: AX3E NH3 Bond angles are 109.5°

Tetrahedral Geometry Simple arrangement: The bond angles are 109.5° AX4 CH4 CH3Cl The bond angles are 109.5°

Trigonal Bipyramidal Simple Arrangement Bond angles are 90° and 120° AX5 PCl5 Bond angles are 90° and 120°

Octahedral Geometry Simple Arrangement: Bond anlges are all 90° AX6 SF6 Bond anlges are all 90°

Sigma and Pi Bonds A single bond has a a σ-bond. A σ-bond is the merging of two atomic orbitals by overlap.

Sigma and Pi Bonds A double bond is a σ-bond plus one π-bond. A π-bond is formed when electron is p-orbitals overlap to share electrons.

Sigma and Pi bonds A triple bond consists of a σ-bond plus two π-bonds.

Carbon Chemistry single bonds between carbons end in -ane. (Alkanes) Double bonds between carbons end in -ene. (Alkenes) Triple Bonds between carbons end in -yne. (Alkynes)

Arenes (Aromatic Carbon Compounds “Rings”) Aromatic Benzene