CHEM 1031 Study Guide - Quiz Guide: Lattice Energy, Octet Rule, Lewis Structure

• School: Temple University
• Department: Chemistry
• Course: CHEM 1031
• Professor: Graham Dobereiner

Document Summary

Requires some form of electron interaction (valence electrons) Size- bigger ions have smaller lattice energies. Magnitude of ionic charge- increasing charges= higher lattice energy. Ex- when al (3+) forms a solid lattice with cl (-), it will release more energy than one of. Most atoms want to have a full valence shell (except h, he- only want 2) Free radicals- odd # of valence electrons. Leave central atom deficient (b, al, be) Use electronegativity to predict polarity of bonds. 0. 4-2 difference = polar covalent (one atom is more selfish but still sharing) For a given bond, draw dipole moment as an arrow pointing toward the most electronegative atom (cid:862)add up(cid:863) the arro(cid:449)s. If they all go in the same direction, the molecule is polar. If they go in different directions, the molecule is nonpolar. Rearrange to satisfy octet rules if needed. Fc is the charge of an atom if all bonds were cut in half.