Cl2 O6 - Cl2 O6 Chlorine (V; VII) Oxide Orbital Box...

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Cl 2 O 6 Chlorine (V; VII) Oxide Orbital Box Diagrams Cl [Ne] ↑↓ ↑↓ ↑↓ _ 3s 3p O [He] ↑↓ ↑↓ _ _ 2s 2p Electron Configuration Cl 1s 2 2s 2 2p 6 3s 2 3p 5 OR [Ne] 3s 2 3p 5 O 1s 2 2s 2 2p 4 OR [He] 2s 2 2p 4 Formal Charges Formal charges help you determine if you have the proper structure for a molecule and make sure you have the correct number of electrons. In this case, the formal the total formal charge is 0. This means that the numbers of bonded and nonbonded pairs are more that correct. Formal Charges for Cl = 7 – ½ (14) – 0 = 0 Formal Charges for O = 6 – ½ (4) – 4 = 0 Hybridizations Cl 2 O 6 has an expanded valence electron configuration. This means that there are more than the usual 8 electrons surrounding an atom. This can be illustrated with a hybrid box diagram: Cl [Ne] _ _ _ _ _ _ _ __ __ There are 7 unbonded 3s 3p 3d electrons in this model. Therefore, chlorine can form 7 bonds. Both Cl atoms have sp 3 hybrid orbitals because there are four electron domains
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This note was uploaded on 05/07/2008 for the course CHEM 119 taught by Professor Blackwell during the Fall '08 term at Lawrence.

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Cl2 O6 - Cl2 O6 Chlorine (V; VII) Oxide Orbital Box...

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