CHEM 11200 Lecture Notes - Lecture 16: London Dispersion Force, Metal, Intermolecular Force
19 Jul 2020
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Document Summary
A molecule is polar if there is an uneven distribution of electron density over the entire molecule. Van der waals: dispersion forces, hydrogen bonding, london forces. Hydrogen bonding: connects f,o,n lone pairs to hydrogen. London forces: temporary interactions between polar and nonpolar molecules. Ionic solid: held together by electrostatic attraction between cations and anions. The bonds that hold the ions together are the same ones that bind the pairs of ions. Network solids: atoms are connected in a lattice structure of covalent bonds. Metallic solids: covalent bond lattice of nuclei in a sea/cloud of electrons, known as conduction electrons = makes metals excellent conductor. Molecular solid: molecular forces held together by intermolecular forces. Making these solids weaker, and therefore, not even solids at room temp. Phases: states in which matter can remain in == solid, liquid, gas. Physical changes such as phase changes has an effect on the intermolecular forces between molecules in a phase.
