CHEM H90 Lecture Notes - Lecture 10: Ionic Bonding, Lewis Structure, Covalent Bond

• School: UC-Irvine
• Department: Chemistry
• Course: CHEM H90
• Professor: Burke

Document Summary

Outline: how to predict the shapes of molecules, topics, lewis dots of atoms, octet rule, multiple bonds, electronegativity, formal charges. In a covalent bond, electrons are shared by nuclei: when you have a pair of identical atoms, things are perfectly symmetric, perfectly covalent (no transfer from one side to another) (e. g. ) Lewis dot symbols of atoms: the number of dots is the number of valence electrons. Octet rule for water (h2o: add up the valence electrons of all the atoms, total valence electrons: 1 + 1+ 6 = 8, use a pair of electrons to form a pair between each pair of bound atoms. 8 4 = 4: arrange remaining electrons to satisfy the duet rule for h and the octet rule for c, n, o and f. 16 4 = 12: arrange remaining electrons to satisfy the duet rule for h and the octet rule for c, n, o, and f.