CHEM101 Study Guide - Midterm Guide: Triple Bond, Bromine, Double Bond
17 Sep 2018
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Chapter 8: chemical bonding i: basic concepts (part 2) 2. Chapter 11: intermolecular forces and liquids and solids 16. Chapter 8: chemical bonding i: basic concepts (part 2) Drawing lewis structures: first step: determine valence, valence- outermost electrons for each atom. 1 = 1 5 = 5 ( ) Second step: determine central atom: h is not central, usually the least electromagnetic. Fourth step: complete octet with remaining electrons. Fifth step: if necessary: use multiple bonds to fill/complete octet. Double check: are all electrons present, each atom has complete octet, all electrons are in pairs. Double bonds- two atoms share two pairs of electrons: 2 pairs = 4 electrons. Triple bonds- two atoms share 3 pairs of electrons. Multiple bonds are shorter and stronger than single bonds. Cases that won"t follow the octet rule: octet= 8 electrons around the atom, can have 4 valence electrons. B- boron, can have 6 valence electrons.
