Final Lab Report

Final Lab Report - Zach Lashaway 12-5-07 Chem-134 Dr....

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Unformatted text preview: Zach Lashaway 12-5-07 Chem-134 Dr. Walker Final Lab Report Introduction: In the Molecular Bonding experiment: Lewis structures were drawn, the prediction of geometric structures of molecules were made, constructed geometric models of the molecules or ions, then checked the predictions using a molecular modeling program Spartan 02. A covalent bond is a form of chemical bonding that is characterized by the sharing of pairs of electrons between atoms , or between atoms and other covalent bonds. In short, attraction-to-repulsion stability that forms between atoms when they share electrons. Lewis structures are a two dimensional representation of a molecule or ion, that can show the general placement of bonds and electrons. Lines represent the bonds and dots around an atom represent the attached electrons of a molecule or ion. Rules for Writing Lewis Structures : 1. Put the atoms in the molecule in their correct position General Rules: a) The less electronegative element is usually in the center. b) The much larger atoms prefers the center. c) C prefers 4 bonds and prefers the center. d) H and F are never on the center, they have one bond. e) Cl, Br, I prefer single bonds unless they are central. f) O prefers 2 bonds, but can have 1, 2, or 3 bonds. 2. Calculate the total number of valence electrons a) Neutral molecule: add valance electrons of all atoms. b) Cations: subtract number of e- s equal to the charge c) Anions: add number of e- s equal to the charge. 3. Use octet rule: put 8 e- about each atom (in pairs) except H, B, Be. a) A single bond between two atoms is a shared e- pair. b) Double bonds are 2 shared pairs and triple bonds are 3 shared pairs....
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Final Lab Report - Zach Lashaway 12-5-07 Chem-134 Dr....

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