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Chemistry: Chapter 7 - Molecular Geometry

Chemistry Chapter 7 BJU
by

Kimberly Cribb

on 26 October 2015

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Transcript of Chemistry: Chapter 7 - Molecular Geometry

Molecular Geometry
Valence Shell Electron Repulsion Theory (VSEPR) -- Electron dense areas repel each other.
Basic Shapes
Orbital Hybridization
When the s and p oribitals morph into new orbitals with identical bonds with equal energies.
Sp3 = 1 s orbital and 3 p orbitals morphed
Sp2 = 1 s orbital and 2 p orbitals morphed
Sp = 1 s and and 1 p orbital morphed
Process: How to figure out the shape
Step 1: Draw the Lewis Dot Structure of the molecule
Step 2: Count the regions of electron density around the central atom
Step 3: Make the basic shape based on the regions around the central atom
4 regions = sp3
3 regions = sp2
2 regions = sp
Step 4: attach the bonded atoms and leave the unbonded pairs
Step 5: Determine the molecular shape based on the bonded atoms not the unbonded pair.
Examples
Electron dense areas include: unbonded or lone pairs of electrons, single bonds, double bonds, and triple bonds
Tetrahedral
Trigonal Planar
Carbon (C)
Hydrogen (H)
Nitrogen (N)
Hydrogen (H)
Oxygen (O)
Hydrogen (H)
Hydrogen (H)
Fluorine (F)
By Mrs. Cribb
Answer these questions as you go through the Prezi. Write the questions first. Turn this in for a grade.

1. What are the possible shapes for a molecule? Give an example of a molecule or ion that forms each of the basic shapes. (Example: tetrahedral - CHCl3)
2. What are electron dense regions?
3. What determines the molecular shape?
4. What do like charges do? How does that affect the shape of molecules?
5. What are the shapes called with 5 or 6 regions around the central atom?
Notice the bond angle! There are 3 bonds all with 120 as the angle. 3*120 = 360. A circle has 360 degrees.
Honors Videos
These guys are super helpful!
Lewis Dot exceptions
VSEPR - 5 electron dense regions
VSEPR - 6 electron dense regions
Additional Practice Problems
Honors Questions:
1. What are the molecular shape possibilities when there are 5 things around the central atom? (Hint: Seesaw is the first one.)
2. What are the bond angles around in the trigonal bipyramidal molecular shape?
3. Why do the bond angles change when you have unshared or unbonded pairs in the molecule?
4. What are the molecular shape possibilities when there are 6 things around the central atom?
5. Are there any double or triple bonds in these exceptions to the octet rule? (See Additional Practice Problems Video.)
6. Which atoms get replaced by lone electron pairs first?
7. What are the bond angles in the trigonal bypyramidal and octahedral shapes? Draw one of each and label it.
http://people.southwestern.edu/~footezm/GenChemTutorials/vseprquiz/vsepr_quiz2.html
http://www.glencoe.com/qe/scienceOLC.php?qi=6345
Tetrahedral
Trigonal Planar
Linear
Full transcript