​Hybridization

• ​VSEPR Theory is useful for explaining the shapes of molecules, but doesn't explain the relationship between the geometry and shared electrons

• ​Hybridization: the mixing of two or more atomic orbitals of similar energies on the same atom to produce new hybrid atomic orbitals of equal energies

• ​Hybrid Orbitals: Orbitals of equal energy produced by the combination of two or more orbitals in the same atom

​What does this even mean?

• ​Let's look at the molecule BeF_2, Specifically, its electron configuration

  • ​Fluorine is in good shape, its notation is 1s²2s²2p⁵

    • ​Has unpaired electrons

  • ​Beryllium has a configuration of 1s¹2s²

    • ​no unpaired electrons, but still wants to bond to try and get 8

    • ​To bond, Beryllium will move one of its electrons to the p-orbital

      • ​One Fluorine bonds with the s-orbital electron, one bonds with the p-orbital, making a new shape

• ​The Geometry of some molecules are only possible to do hybridization

​Intermolecular Forces

• ​Intermolecular Forces: The forces of attraction between molecules

  • ​Vary in strength, but a generally weaker than bonds

    • ​A good way to measure is to look at boiling points

      • ​Higher boiling point=stronger bond of attraction

​Molecular Polarity and Dipole-Dipole Forces

• ​The strongest intermolecular forces exist between polar molecules, which create dipoles

  • ​Dipole: a force created by equal but opposite charges that are separated by a short distance

    • ​direction moves from positive end to negative end

    • ​Negative end of one attracts positive end of another, creating dipole-dipole force

    • ​How they act depends on molecule shape

      • ​See figure 26 on page 205

​Hydrogen Bonding

• ​Hydrogen bonds tend to have a large electronegativity difference, making them more polar

  • ​Hydrogen has a high positive charge and is small enough to get close to electrons of adjacent molecules

• ​Hydrogen Bonding: the intermolecular force in which a hydrogen atom is that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom

​London Dispersion Forces

• ​In any atom, molecules are in constant motion

  • ​at any instant, charge may be uneven, creating a temporary dipole that can attract other atoms

• ​London Dispersion Forces: the intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles

  • ​Act between all atoms and molecules

  • ​the only forces that act on the Noble Gases

  • ​Increase with the number of electrons/ increasing atomic number