CHEM 151 1st Edition Lecture 21 Outline of Last Lecture I. ElectronegativityII. BondsOutline of Current Lecture III. Reviewing Ionic BondingIV. Reviewing Covalent BondingV. Lewis StructuresCurrent LectureIonic BondingValence electrons are transferred.Follows the octet rule.Strong net attractive force present between the ions.Covalent BondingElectrons are shared.Both atoms follow the octet rule.Building a Lewis StructureExample: NH3 (ammonia)1. Decide on central atom. (NEVER hydrogen); tends to be atom with lowest electronegativity.In this case, N is the central atom.2. Count valence electrons.H = 1 and N = 5Total: (3)(1) + 5= 8 electrons / 4 pairs3. Form a single bond between the central atom and surrounding atoms.HHHN4. Remaining electrons form lone pairs to complete octet. (start with outside atoms, unless it is
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