Lecture_21_Covalent - LECTURE NOTES LECTURE 21 Covalent...

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L E C T U R E N O T E S LECTURE 21 Covalent Bonds (Supplement) GENERAL CHEMISTRY Fall 2009 Updated: 11/22/2011
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The Nature of Covalent Bonding The Octet Rule in Covalent Bonding A. Covalent compounds tend to form so that each atom, by sharing electrons, has an octet of electrons in its highest occupied energy level B. Single Covalent Bonds 1. One shared pair of electrons between two atoms a. Example – Diatomic fluorine b. Example - Hydrogen Chloride Lewis Structures A. Unshared Pairs (Lone Pairs) 1. A pair of electrons that is not involved in bonding and that belongs exclusively to one atom B. Lewis Structures 1. Formulas in which atomic symbols represent nuclei and inner-shell electrons, dot pairs or dashes between two atomic symbols represent electron pairs in covalent bonds, and dots adjacent to only one atomic symbol represent unshared electrons C. Structural Formula 1. Formulas indicating the kind, number, arrangement, and bonds but not unshared pairs of the atoms in a molecule Updated: 11/22/2011
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D. Drawing Lewis Structures (trichloromethane, CHCl
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This note was uploaded on 11/22/2011 for the course CHEMISTRY CHM1025 taught by Professor Laurachoudry during the Fall '10 term at Broward College.

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Lecture_21_Covalent - LECTURE NOTES LECTURE 21 Covalent...

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