Valence-Shell Electron-Pair Repulsion Theory

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Presentation transcript:

Valence-Shell Electron-Pair Repulsion Theory VSEPR Notes Valence-Shell Electron-Pair Repulsion Theory

VSEPR Theory VSEPR Theory states that molecules adjust their shapes so that the valence electron pairs are as far apart as possible.

Shape Table Bonding directions Lone pairs Shape name picture example 2 linear bent 3 trigonal planar 1 pyramidal 4 tetrahedral 5 trigonal bipyramidal

Linear Linear—angles are 180°-will be linear if you only have two atoms in the molecule & no lone e- pairs on central atom. Example—HCl or CO2

Bent Bent—2 unshared pairs of e- strongly repels the covalent bonding pairs. All angles are 105°. Example—H2O Water is NOT linear-- the two lone pairs actually bend the hydrogen atoms away from the oxygen atom!

Trigonal planar Trigonal-Planar—three pairs separate as much as possible, no lone e- pairs on central atom. Example—BF3

Pyramidal Trigonal-Pyramidal—1 unshared pair of e- on central atom strongly repels the covalent bonding pairs, pushing them closer together. All angles are 107 °. Example—NH3

Tetrahedral Tetrahedal—four faced—all angles are 109.5°, no lone e- pairs on central atom. Example—CH4

Trigonal bipyramidal Trigonal Bipyramidal — five pairs separate as much as possible, no lone e- pairs on central atom. Example—PCl5

Now you build them!