CHEM 110 Chapter Notes - Chapter 11: Gas Constant, Vapor Pressure, Covalent Radius

• School: McGill University
• Department: Chemistry
• Course: CHEM 110
• Professor: Laura Pavelka

Document Summary

Physical states and phase changes: potential energy: manifested as intermolecular forces (draw molecules together, kinetic energy: random motion of molecules (average speed and temp. , phase change: change in physical state, explained by interactions. Intramolecular forces: within each molecule: chemical behaviour of each state is identical bc each state has same bent polar molecules held together by identical covalent bonding forces. Intermolecular forces: between the molecules: physical behaviour of states is different bc strength of forces differ, as temperature increase, the average kinetic energy increases so particles can overcome attraction forces more easily. Small p compared to k, particles far apart. Particles touching so stronger attraction, enough k to move randomly. Attractions dominate motion, particles fixed/just jiggling in place. Effects on vapour pressure: temperature: changes fraction of molecules moving fast enough to escape liquid/slowly enough to be recaptured, higher temp = higher pressure.