CHM 2045C Lecture Notes - Lecture 9: Formal Charge, Electronegativity, Lattice Energy
Document Summary
Bonding theories: explain how atoms bond together to form molecules, explain why some combos of atoms are stable and others are not, and predict the shapes of the molecules which determines the physical and chemical properties of compounds. Lewis bond theory: atoms bond because it results in a more stable electron configuration (more stable=lower potential energy). Atoms bond by either transferring or sharing electrons. Usually, this results in all atoms obtaining an outer shell with eight electrons (octet rule). Radius decreases across, ie and ea decrease down. Chemical bonds form because they lower the potential energy between the charged particles that compose atoms. The force of attraction between oppositely charged particles is directly proportional to the product of the charges. Larger charge means the ions are more strongly attracted, which means there is larger lattice energy. When hlattice or eel is positive, ions are repelled, it requires energy, and is endothermic.
