CHM 113 Lecture Notes - Lewis Structure, Formal Charge, Double Bond
Document Summary
Covalent bonding: sharing of one or more ve pairs: occurs between atoms with a zero or small different in en, example: cl2. Shares one pair of ve"s making each cl have 8 ve"s and full shell (stable) Lewis structure: ve"s represented as dots around element"s symbol. Octet rule: elements will share ve"s (bond) in order to fill their valence shells with. 8 electrons: noble gases don"t like to share ve"s because valence shells are already full, exceptions to the octet rule: Free radicals: compounds with odd number of electrons. Compounds that have less than 8 electrons on one or more of the atoms. H only wants 2 ve to fill shell (like he) Elements of 3rd group of periodic table (b, al, etc) typically want 6 electrons. Expanded octets: atoms that have more than an octet around them. Central atom must be in the 3rd row of periodic table or beyond: relatively large, can accommodate.
