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Chemistry: Chapter 7 - Molecular Geometry
Transcript of Chemistry: Chapter 7 - Molecular Geometry
Valence Shell Electron Repulsion Theory (VSEPR) -- Electron dense areas repel each other.
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.
Electron dense areas include: unbonded or lone pairs of electrons, single bonds, double bonds, and triple bonds
By Mrs. Cribb
Molecular Geometry Prezi Questions - All Students (You should be able to copy and paste these into a document if you look at the text for this prezi.)
Answer these questions as you go through the Prezi. Write the questions first. Turn this in for a grade.
1. What are electron dense regions?
2. What are IMFs? Video 1
3. Molecular geometry is what? Video 1
4. What are the 6 basic shapes? Video 1
5. Honors: What are the advanced shapes of the molecules? Video 1
6. What is the electronic shape? Video 1
7. What is the molecular shape? Video 1
8. How many regions of electron density in a linear molecule, and what is the bond angle? Video 2
9. How many regions of electron density in a trigonal planar molecule, and what is the bond angle? Video 2
10. How many regions of electron density in a tetrahedral molecule, and what is the bond angle? Video 2
11. How many regions around expanded octets? Video 2
12. Honors : How many regions of electron density are there in trigonal by-pyramidal molecules? Video 2
13. Honors: What are the bond angles on the octahedral shaped molecules? How many regions of electron density? Video 2
Notice the bond angle! There are 3 bonds all with 120 as the angle. 3*120 = 360. A circle has 360 degrees.
These guys are super helpful!
Lewis Dot exceptions
Additional Practice Problems
Video 3 - Watch only
Video 4 - review only
Video 5 - watch only
Honors videos will be at the end.
Advanced Molecular Geometry Honors Prezi Questions
1. What rule are all of the molecules acting as exceptions too according to video 7?
2. What are axial atoms and equatorial atoms? Video 7
3. What is the bond angle between the axial and the equatorial bond for the trigonal bypyramidal shape ? Video 7
4. What is the bond between the two axial atoms for the trigonal bipyramidal shape? Video 7
5. What is the bond between any of the equatorial bonds for the trigonal bipyramidal shape ? Video 7
6. Why do the bond angles change when you have unshared or unbonded pairs in the molecule? Video7
7. What is the bond angle for the see saw axial atoms? Video 7
8. What is the bond angle for the bond between an axial atom and an equatorial atom on the see saw shape? Video 7
9. What is the bond angle for the bond between the two equatorial atoms on the seesaw shape? Video 7
10. What atoms are replaced with unshared electron pairs first for the trigonal bipyramidal atoms? Axial atoms or equatorial atoms? Video 7
11. What are the molecular shape possibilities when there are 6 things around the central atom? Video 8
12. What is the bond angle between any two bond on the octahedral shape? Video 8
13. What are the bond angles for the square pyramidal bonds? Video 8
14. What are the bond angles for the square planar bonds? Video 8
15. Are there any double or triple bonds in these exceptions to the octet rule? (See Additional Practice Problems Video 9)
16. Draw and label with bond angles 4 of the examples in video 9. One of your drawings MUST be an ion.