CHMA10H3 Lecture Notes - Lecture 24: Intermolecular Force, Vsepr Theory, Lewis Structure
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CHMA10H3 Full Course Notes
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For a molecule to be polar it must: have polar bonds. There should be an electronegativity difference; predicted by theory. There must be bond dipole moments; measured practically in lab: have an unsymmetrical shape. Use vector addition to add up all the dipole moments. Polarity affects the intermolecular forces of attraction which determine boiling points and solubilities. Non-bonding pairs affect molecular polarity strong pull in its direction. Molecular dipole moment will depend on the dipole moment of its bond and their geometry. Draw a lewis structure and determine molecular geometry from vsepr. Determine whether the polar bonds add together to give a net dipole moment. Draw a dipole vector for each bond and add them up. Intermolecular forces hold molecules together in a liquid or solid. Determine bulk properties such melting/boiling point: dipole-dipole interactions. If a molecular has a net dipole moment, they align so as to maximize electrostatic attractions: london dispersion forces (aka van der waals forces)
