1. Chapter 8 Covalent Bonding 8.2 The Nature of Covalent Bonding
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. Complete Section 8.1 of the handout.
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Complete Section 8.1 of the handout.
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3. The Octet Rule in Covalent Bonding
Single Covalent Bond: atoms held together by sharing one pair of electrons
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4. The Octet Rule in Covalent Bonding
Structural Formula: represents the covalent bonds as dashes and shows the arrangement of covalently bonded atoms.
H:H H-H
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5. The Octet Rule in Covalent Bonding
Double Covalent Bond: a bond that involves two shared pairs of electrons
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6. The Octet Rule in Covalent Bonding
Triple Covalent Bond: a bond formed by sharing three pairs of electrons
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7. Bond Dissociation Energies
Bond Dissociation Energy: energy required to break the bond between two covalently bonded atoms.
Bond
Bond Dissociation Energy
(kJ/mol)
Bond Length
(pm)
C C
347
154
C = C
657
133
908
121
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8. The Octet Rule in Covalent Bonding
Drawing Lewis Dot Structures:
Determine # of valence electrons.
Determine # of “octet” electrons.
*Note*– Hydrogen gets 2
# bonds = (# valence e- - # octet e-) / 2
Arrange atoms with # bonds from step 3.
Add electron pairs until all atoms have the correct number of electrons around them
Recheck your answer to make sure you have the right # of bonds and electrons.
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9. The Octet Rule in Covalent Bonding
Draw Lewis Dot Structures for each molecular compound:
SiO2
HCl
H2O
HCN
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10. Here are some common molecular shapes.
Linear
Trigonal planar
Bent
Pyramidal
Tetrahedral
Trigonal
bipyramidal
Octahedral
Square
planar
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11. END OF 8.2
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