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Molecular (Covalent) Bonding

Molecular (Covalent) Bonding. Chemistry. Covalent Bond = Share Electrons. H 2 single bond “shared pair” O 2 double bond bond pairs vs. lone pairs N 2 triple bond (diatomic elements). Lewis Dot Structures. HCCH PCl 3 HCN OH -1.

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Molecular (Covalent) Bonding

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  1. Molecular (Covalent) Bonding Chemistry

  2. Covalent Bond = Share Electrons • H2 single bond “shared pair” • O2 double bond bond pairs vs. lone pairs • N2 triple bond • (diatomic elements)

  3. Lewis Dot Structures • HCCH • PCl3 • HCN • OH-1

  4. Coordinate covalent bond = one atom donates both electrons for the bond pair • H+1 + NH3 → • Bond dissociation energy = energy required to break bond • − < = < ≡ • Bond length • − > = > ≡

  5. Resonance • O3

  6. Exceptions to the Octet Rule • Odd # of electrons • NO2 • Less than 8 • BF3 • Expanded Octet: More than 8 • SF6

  7. Diamagnetic • All electrons are paired • Repelled by magnetic field • Paramagnetic • Has an unpaired electron • Attracted to magnetic field

  8. Shapes

  9. Polarity

  10. Quiz Review

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