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Midterm

CHEM 112 Study Guide - Midterm Guide: Network Covalent Bonding, Thermal Expansion, Gas Constant


Department
Chemistry
Course Code
CHEM 112
Professor
John Carran
Study Guide
Midterm

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Forces
1. Ionic bonding
2. Ion-dipole
3. H-bonding
4. Dipole-dipole
5. London dispersion
As the strength of the intermolecular forces increase, boiling point, melting point, surface tension, and
viscosity increases. Vapour pressure decreases.
1) the size of the molecule has a huge impact on bp. the larger, the higher the bp.
2) branching decreases intermolecular forces by steric hinderance. lower intermolecular forces = lower
bp. ie the higher the branching, the lower the bp....
HAVING AN OH GROUP DECREASES THE VAPOUR PRESSURE
Surface Tension: energy or work that is required to increase the surface area of a liquid
Cohesive: b/w molecules
Adhesive: b/w molecules and surface
Vapour Pressure: pressure exerted when the liquid and vapour are in dynamic equilibrium
- Increases with temperature
- Doesn’t depend on the volume of the liquid or surface area
Viscosity: when a liquid flows, interactions must be broken and reformed
Pentane: nonpolar, so lowest Surface tension, viscosity and intermolecular force, so London dispersion
Pentanal: polar, can’t h-bond (B/C DOUBLE BOND) so dipole-dipole
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