VSEPR Means Valence Shell Electron Pair Repulsion Theory

VSEPR Theory:

VSEPR means Valence Shell Electron Pair Repulsion Theory

This theory is used to predict shapes of molecules.

The basic idea is that the shape of the molecule depends on the number of electron pair that surround the central atom in the molecule.

The rule that is applied is that the electron pairs around the central atom in the molecule will repel each other and go as far apart as possible.

Multiple bonds (double or triple) count as one bonding pair for VSEPR predictions.

Your knowledge of geometry will be used to determine how far apart the electron pairs about the central atom are when they are as far apart as possible.

VSEPR Theory:

VSEPR means Valence Shell Electron Pair Repulsion Theory. This theory is used to predict shapes of molecules. The basic idea is that the shape of the molecule depends on the number of electron pair that surround the central atom in the molecule. The rule that is applied is that the electron pairs around the central atom in the molecule will repel each other and go as far apart as possible. Multiple bonds (double or triple) count as one bonding pair for VSEPR predictions.

Fill out the attached chart from the class Powerpoint to understand how VSEPR theory determines shape, and consequently the polarity of covalent molecules.

Instructions:

1)Draw the molecule or compound in 3-D according to VSPER theory. (Use Lewis dot structures to determine how many bonding and nonbonding pairs are in the molecule or compound to determine the shape if needed.)

2)Name the shape.

3)Look up each atom’s electronegativity and calculate the ΔEN.

4)State if the bond type(s)as ionic, covalent polar, or covalent non-polar. Write in charges or dipoles (partial charges)as necessary. The atom with the higher EN will be negative (or partially negative) and the atom with lower EN will be positive (or partially positive).

5)State if the molecule/compound is ionic, polar or nonpolar overall.

6)Build the molecule/compound

Examples:

1)CCl4

2)Na2O

3)H2O

4)BF3

5)NH3

Practice

1)Draw the molecule or compound in 3-D according to VSPER theory. (Use Lewis dot structures to determine how many bonding and nonbonding pairs are in the molecule or compound to determine the shape if needed.)

2)Name the shape.

3)Look up each atom’s electronegativity and calculate the ΔEN.

4)State if the bond type(s) as ionic, covalent polar, or covalent non-polar. Write in charges or dipoles (partial charges) as necessary. The atom with the higher EN will be negative (or partially negative) and the atom with lower EN will be positive (or partially positive).

5)State if the molecule/compound is ionic, polar or nonpolar overall.

Click on the molecule's name to see the answer, but first try to do it yourself!

(Note: Trigonal pyramidal is listed as tetrahedral. This is because it really is just a variation on the tetrahedral shape, and so is sometimes referred to as such. I expect you to differential between trigonal pyramidal and tetrahedral.)

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