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CSU - CHEM 111 - Class Notes - Week 8

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CSU - CHEM 111 - Class Notes - Week 8

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background image 4.4 Exceptions to octet rule continued Example problems Draw the Lewis structure for SF₆ 1) S has 6, F has 7 and we have 6 Fs (7x6=42). Total we have 48
2) S is the least electronegative so it is the inner atom.
3) We have used 12 electrons so far. So, we have 36 left. S can have an  expanded octet so it can have more than 4 bonds. 4) Now we have used all the electrons. Draw the Lewis structure for SO₂²⁻ 1) S has 6, O has 6 and we have 2 Os (6x2=12), and there is a -2 charge so  we gain 2 electrons. Total we have 20. 2) S is the least electronegative so it is the inner atom. 3) We have used 4 electrons. So, we have 16 left. 4) Now all electrons have been used. 4.5 Resonance Resonance- when double or triple bonds can exist in multiple spaces
background image The actual observed structure of ozone (O₃) is a hybrid of the above  structure. Where both bonds are the same length and strength. The bonds end up 
being 1.5 bond.
The electrons are delocalized leading to resonance stabilization. Bond order= number of bonds/ number of bonding positions Example problems Draw the resonance forms of NO₃⁻ and determine the bond order 1) First let’s draw the Lewis structure.  This structure needs one more bond between the N and an O. Which mean
the bond could be placed in three different spots.
2) Let’s draw all the resonance structures 3) For the bond order there are 4 bonds and 3 bonding positions. So the bond order is 4/3 Determine the Lewis structure(s) for phosphate (PO₄³⁻) and determine the 
bond order
1) First lets draw the Lewis structure.
background image 2) In this structure there are a lot of formal charges. To minimize this we can  add another bond between the P and one of the 4 Os. This creates 
resonance structures.
3) There are 5  bonds and 4 bonding positions. The bond order is 5/4 or 1.25 Some resonance structure don’t contribute equally The best structure contributes the most to the actual structure 4.6 Molecular Structure/shape Ball and stick model shows the bond angles in 3D For 2D we use Valence Shell Electron Pair Repulsion Theory (VSEPR) Predicts that electron pairs will be as far apart as possible surrounding the  central atom Terminology Electron domain- lone pair of electrons or a bond in the valence shell around 
an atom
Includes bonds and nonbounded electron pairs

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School: Colorado State University
Department: Chemistry
Course: General Chemistry I
Professor: Ruth Tucker
Term: Summer 2016
Name: Chem 111 week 8
Description: - Resonance structures - Bond order - Molecular structure - Valence shell electron pair repulsion theory - Electron domain - Steric number - Electronic geometry - Determining shape with ligands - Polarity
Uploaded: 03/19/2018
7 Pages 48 Views 38 Unlocks
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