1. Chapter 8 Covalent Bonding 8.3 Bonding Theories
8.1 Molecular Compounds
8.2 The Nature of Covalent Bonding
8.3 Bonding Theories
8.4 Polar Bonds and Molecules
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2. Log in to Google Classroom
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Begin working on Molecule Shapes simulation.
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3. Valence Shell Electron Pair Repulsion Theory
VSEPR Theory
VSEPR Theory
Valence Shell Electron Pair Repulsion Theory
Explains 3 dimensional shape of molecules.
Repulsion of electron pairs causes molecular shapes to adjust so valence electron pairs are as far apart as possible.
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4. 2 atoms bonded to central atom
VSEPR Theory
Linear
2 atoms bonded to central atom
No unshared electron pairs on central atom.
Bond angle is 180°
Carbon dioxide (CO2)
No unshared
electron pairs
on carbon
180°
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5. 2 atoms bonded to central atom 1 or 2 unshared electron pairs
VSEPR Theory
Bent
2 atoms bonded to central atom
1 or 2 unshared electron pairs
With two unshared pairs, the bond angle is ~105°
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6. 3 atoms bonded to central atom
VSEPR Theory
Trigonal Planar
3 atoms bonded to central atom
No unshared electron pairs.
Bond angle is120°
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7. 3 atoms bonded to central atom
VSEPR Theory
Trigonal Pyramidal
3 atoms bonded to central atom
1 unshared electron pair that strongly repels the bonding pairs, pushing the bonding electrons together.
Bond angle is 107°
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8. 4 atoms bonded to the central atom
VSEPR Theory
Tetrahedral
4 atoms bonded to the central atom
No unshared electron pairs.
Bond angles are 109.5°
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9. Here are some common molecular shapes.
VSEPR Theory
Here are some common molecular shapes.
Linear
Trigonal planar
Bent
Trigonal
Pyramidal
Tetrahedral
bipyramidal
Octahedral
Square
planar
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10. Molecular Shape Summary
VSEPR Theory
Molecular Shape Summary
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11. Do Now
Draw Lewis structures for each molecule below. Then use VSEPR theory to predict their shapes.
SiCl4
SCl2 CO
CH2O
PH3
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12. END OF 8.3
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13. Draw Lewis Structures for the following molecules.
Do Now
Draw Lewis Structures for the following molecules.
a) Br2
b) HF
c) NF3
d) H2O2
e) CO
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