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UNIT VIII Lewis Structure Lesson 5
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Lewis Structure
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Gilbert Newton Lewis Invented “Electron-dot” formulas or “Lewis Structures” I’m so tired of writing all those useless inner electrons, in the Bohring models!
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Valence Electrons – electrons in the outermost occupied energy level. (s and p electrons outside the core) Valence electrons can be represented by “dots” drawn around the atom.
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Remember the rules…
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VIII.3 CHEMICAL BONDING C. Writing Lewis Structures a. Simple Ionic Compounds: Draw the Lewis Structure of: a) MgO
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VIII.3 CHEMICAL BONDING b)KCl c) CaF 2
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VIII.3 CHEMICAL BONDING b. Covalent Compounds: Octet Rule : most atoms, other than hydrogen, tend to attain an octet of electrons as a result of forming covalent bonds
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VIII.3 CHEMICAL BONDING Rules: 1. Count the TOTAL # of valence e- (Subtract 1 e- for every positive charge, and add 1 e- for every negative charge on the molecule.) 2. Determine which atoms are bonded together, put 2 e- into each bond 3. Use the remaining valence e- to complete the octets of the atoms surrounding the central atom 4. If central atom has less than an octet of e-, have a neighbour share e- with the “deficient atom” by putting an extra pair of e- 5. Replace each pair of e- with a dash
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VIII.3 BONDING Ex. 1 CH 4
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VIII.3 BONDING Ex. 2 NH 4 +
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VIII.3 BONDING Ex. 3 O 2
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VIII.3 BONDING Ex. 4 NO +
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VIII.3 CHEMICAL BONDING Ex. 5 CHO 2 -
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O NE LAST TO TRY HPO 2
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H OMEWORK ON L EWIS STRUCTURE Homework p. 183 #85 p. 188 # 86a-u
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