8.2 Lewis Dot Structures | High School Chemistry

Chad provides a comprehensive lesson on how to draw Lewis dot structures which involve the valence electrons of an atom/molecule. He begins with the octet rule and shows how electrons can be transferred (ionic bonding) or shared (covalent bonding) in order to achieve a 'filled octet.' Chad then covers the 3 major exceptions to the octet rule:
1) H, Be, B, and Al go under the octet rule,
2) elements in the 3rd period and lower on the periodic table can exceed the octet rule, and
3) molecules with an odd number of electrons will have an atom that does not satisfy the octet rule.

Chad then shows how to draw the Lewis structures of a multitude of examples including CCl4, NF3, HCN, CO2, N2O, SF4, ICl3, XeF4, and NO3- (the nitrate ion). He introduces the concept of formal charge along the way, shows how to determine it from a Lewis structure, and how it can be used to distinguish between multiple Lewis structures in certain examples. He also covers examples involving resonance and explains how resonance implies delocalized pi electrons and how resonance structures are a useful tool for determining what the actual structure of a molecule exhibiting resonance is (the resonance hybrid).

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00:00 Lesson Introduction
00:44 The Octet Rule
06:13 Octet Rule Exceptions
10:46 CCl4 Lewis Structure
14:26 NF3 Lewis Structure
16:31 HCN Lewis Structure
18:56 CO2 Lewis Structure
21:34 Formal Charge
26:39 N2O Lewis Structure
31:42 SF4 Lewis Structure
33:44 ICl3 Lewis Structure
35:14 XeF4 Lewis Structure
37:00 NO3- Lewis Structure

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