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Molecular Geometry

Molecular Geometry. 6.5. Hybridization. Mixing of two or more atomic orbitals of similar E’s on the same atom to produce new hybrid atomic orbitals of = E Hybrid orbitals = orbitals of = E produced by the combination of 2 or more orbitals of the same atom. An Example. Methane (CH 4 )

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Molecular Geometry

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  1. Molecular Geometry 6.5

  2. Hybridization • Mixing of two or more atomic orbitals of similar E’s on the same atom to produce new hybrid atomic orbitals of = E • Hybrid orbitals = orbitals of = E produced by the combination of 2 or more orbitals of the same atom

  3. An Example • Methane (CH4) • All bonds b/t C and H are identical • C has a valence config of 2s2 2p2 (leaving 4 spaces for H to join) • In order for all 4 spaces to be =, the s and p orbitals hybridize  sp3 • __ __ __ __ sp3

  4. VSEPR Theory • Valence Shell Electron Pair Repulsion Theory – the shape of a molecule will be so that e-’s are as far apart as possible • Takes into account bonded atoms and lone pairs of __________.

  5. Determining Shapes • Look at steric number (how many things are around central atom). • Look at lone e- pairs • Use the sheet to help you determine geometry

  6. Polarity • Uneven distribution of electrical __________ in an atom • If one atom in a bond pulls e- better than the other and that pull is not balanced out you have a polar molecule • CH4 balances b/c of shape = non polar • NH3 does not balance b/c shape= polar • Try determining polarity on LS sheet 

  7. Intermolecular Forces • Vary in strength but are ___________ than bonds • Strongest IMF is b/t polar molecules • Dipole – created by equal but opposite charges that are separated by a short distance

  8. IMF • Dipole-Dipole Forces – b/t polar molec. • A short range force b/t nearby molec. • Look at the b.p. of I-Cl and Br-Br. • I-Cl – is 97°C and Br-Br is 59°C • This is due to the _______-_________ force between ____ and _____

  9. IMF • Dipole-Dipole induced dipole – a nonpolar molecule becomes a slight dipole b/c a ___________ molecule attracts it’s electrons • Weaker than dipole-dipole

  10. IMF • Hydrogen Bonding – a H atom bonded to a highly e-neg atom is attracted to an unshared pair of e-’s of an e-neg atom in a nearby molec. • Quite strong  responsible for _______ b.p.’s of some materials (H2O) • In dipoles

  11. IMF

  12. IMF • London Dispersion Forces – results from the constant motion of e-’s and the creation of instantaneous dipoles • Between __________ polar molecules

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