CHEM 201 - 10.8.07

CHEM 201 - 10.8.07 - o CsBr (Ionic), SiCl 4 (Polar), CaCl 2...

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CHEM 201 – October 8, 2007 Octet Rule o Group 1A – low E i1 – lose ns 1 – becomes like a noble gas o Group 2A – low E i1+2 – lose ns 1 ns 2 o Group 3A – loses np 1 , ns 2 and ns 1 o Group 6A – high E ea – gain np 5 , np 6 o Group 7A – high E ea – gain np 6 o Group 8A – essentially inert Covalent Bonding o Sharing of at least two electrons (one electron pair) o Non-polar covalent bonds Electron clouds are distributed evenly o Polar covalent bonds Electron clouds are unevenly distributed Creates a dipole Percent Ionic Character o General rule for 2 atoms in a bond o ΔElectro-negativity = Electro-negativity(y) – Electro-negativity(x) If 0 ≤ ΔEN ≤ 0.5 non-polar covalent If 0.5 ≤ ΔEN ≤ 2.0 polar covalent If ΔEN > 2.0 ionic
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Unformatted text preview: o CsBr (Ionic), SiCl 4 (Polar), CaCl 2 (Ionic, Polar), CH 4 (non-polar), HCl (Polar), HCl (aq) (Acts Ionic), TiCl 4 (Polar), CCl 4 (Polar, non-polar), NH 3 (Polar), H 2 O (polar) Electron-Dot Structures o Lewis Diagrams o Valence electrons are represented as dots around the elemental symbol o How to Do Count total number of valence electrons Draw the structure with single bonds putting the most electronegative atom in the center Distribute electron pairs around the peripheral atoms Put the remaining pairs on the central atom Share lone pairs between bonded atoms, creating multiple bonds Bond Energy E HH H H H-H...
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This note was uploaded on 04/07/2008 for the course CHEM 201 taught by Professor Harris during the Fall '07 term at Bucknell.

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