CHEM261 Lecture Notes - Lecture 4: London Dispersion Force, Intermolecular Force, Lone Pair

• School: University of Alberta
• Department: Chemistry
• Course: CHEM261
• Professor: Christopher Cairo

Document Summary

Donors: h on o, n, or halogen. Acceptors: lone pair on o, n, or halogen. Xe: the larger the atom (expanded electron density), the easier the formation of temporary dipoles temporary association. This is the reason why ch4 associates with ch4, due to london forces. Because its temporary dipoles it is not miscible in water water would rather hydrogen bond to itself like dissolves like. Progress of reaction is also called reaction coordinate. = starting material or reactants (e. g. pentane, oxygen) Nb: e = g: gibbs free energy (total) change for the reaction. The above reaction is an exothermic reaction, heat is released during reaction. G will be negative ( g <0) for an exothermic (heat releasing) reaction, but will be positive ( g >0) for endothermic reaction. Ea= activation energy: minimum amount of energy required to activate molecules or atoms to be able to undergo a chemical reaction.