NSCI 1322 Study Guide - Intermolecular Force, Chemical Polarity, London Dispersion Force

• School: Fordham University
• Department: Natural Science
• Course: NSCI 1322
• Professor: Marie Thomas

Document Summary

Dipole moment: quantitative measurement of the polarity of a bond (also dependent on the shape of the molecule) polar molecules have dipole moments. Co2 is a nonpolar molecule w/ polar bonds (as seen on the right) Stuff for dipoles: (dipole moment) = (charge) x (distance between charges) 1debye (d) = 3. 36 x 10-30 (c)(m) coolumb meters. Boiling point: how much liquid wants to be together. Melting point: how much a solid wants to stay together. The stronger the interaction of a molecule, the more it wants to be hydrated. The smaller the ion, the larger the force. The larger the ion, the smaller the force. Attractive forces that arise as a result of temporary dipoles induced in an atom/molecule. There are london forces in all atoms and molecules. Strength increases with larger molar mass solid. Special dipole-dipole interaction between (h) in atoms (exa: n-h o-h f-h) N, o, f are very electronegative and therefore pull the electron over for themselves.