Hybridization

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Hybridization

• Explains how orbitals get rearranged when atoms
  form covalent bonds
• Describes how atoms are bonded

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Hybrid orbitals

• Orbitals of equal energy produced by the
  combining of two or more orbitals on the same
  atom
• The number of hybrid orbitals equals the number
  of orbitals they were made from

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Example Methane

• CH4
• To get 4 equal orbitals, the s and p orbitals
  combine.
• They form 4 sp3 orbitals

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Other hybrid orbitals
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Intermolecular forces

• The forces of attraction between molecules
• Usually weaker than covalent, ionic, and metallic
  bonds
• Can be measured by boiling point
• Higher boiling point means stronger
  intermolecular forces

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Dipole

• Equal but opposite charges separated by a short
  distance
• Direction is from the positive pole to the
  negative pole

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Dipole-dipole forces

• Forces of attraction between polar molecules
• Strongest intermolecular forces
• Only act over short distances

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More than two atoms

• Polarity of the molecule depends on the polarity
  and orientation of each bond

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Induced dipoles

• A polar molecule can induce a dipole in a
  nonpolar molecule by attracting its electrons.
• It is temporary

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Hydrogen bonding

• A hydrogen atom in a compound with a very
  electronegative atom is attracted to an unshared
  pair of electrons in a nearby molecule.
• Examples
• Water (H2O)
• Hydrogen fluoride (HF)
• Ammonia (NH3)

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Hydrogen bonding

• Causes higher boiling points

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Polarity and Hydrogen Bonding

• Polarity and Hydrogen Bonding

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London dispersion forces

• The intermolecular attractions caused by the
  constant motion of electrons and the creation of
  instantaneous dipoles
• Act between all atoms and molecules
• The only intermolecular forces among noble gas
  atoms and nonpolar molecules
• Low boiling points

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discuss

• What is the difference between intramolecular
  forces and intermolecular forces?
• What is a dipole? In what kind of molecule are
  dipoles common?
• What is hydrogen bonding?
• What are London dispersion forces?
• Molecular Geometry review