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Molecular (Covalent) Bonding

Molecular (Covalent) Bonding. Chemistry Level ___ Chapter ____. 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 Level ___ Chapter ____

  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. Shapes: • CO2 linear 180° • CH4 tetrahedral 109.5° • NH3 pyramidal 107° • H2O bent 105° • BF3trigonal planar120°

  6. Polarity: • Bonds HCl H2O • Molecules CO2 H2O • Electronegativity differences indicate polarity: • Nonpolar covalent, Polar covalent, Ionic

  7. Resonance: • O3 (ozone)

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

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

  10. Quiz Review: • Electron dot structures for a molecule • Shape • Bond angle • Polar? • Resonance? • Polar/nonpolar/ionic • Electronegativity difference • Bond dissociation energy

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