4. For each of the following molecules: 1) Draw the Lewis Structure in the proper shape 2) Name
the shape and assign bond angles 3) Use electronegativity values determine the polarity of each
bond 4) Assign dipoles, if necessary 5) Determine the polarity of the overall molecule.
a. OF2
b. Bl3
c. NF3
d. CIF3
e. IF4-
f. SBr6

The shape of a molecule is determined by the valence shell electron pair repulsion theory. We know that this theory has to do with the number of electron pairs that are found on the valence shell of the central atom of the molecule.

Let us now talk about each of the molecules;

1) OF2 - This molecule is polar and has a V shape. The direction of the dipole is towards the fluorine atom and the bond angles in the molecule is 103º.

2) BI3 - The compound is nonpolar because it is symmetrical as such the compound is trigonal planar and the dipoles cancel out. The bod angles in the molecule is 120°.

3) NF3 - The molecule NF3 is polar because of the net dipole moment arising from the trigonal pyramidal structure of the molecule. The bond angle of the molecule is 101.9°.

4) CIF3 - The molecule CIF3 is a polar molecule and the structure is a T shape owing to the two lone pairs on the chlorine atom. The bond angle in the molecule is 175o

5) IF4- The molecule IF4- is nonpolar and has a square planar geometry with the two lone pairs lying above and below the plane. The bond angle here is 90 degrees.

6) SBr6 - The molecule is a nonpolar molecule due to the symmetrical nature of the octahedral molecule. The bond angle of the molecule is 90 degrees as all the Br atoms are found at the corners f a regular octahedron.

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