Draw the following molecules identify each molecular shape, molecular polarity and bond polarity. 1. NH3 2.beCl2 3.BF3 4.XeF4 5.SF6 6.PCl5?

Molecular shapes.....

You do realize that YA is a text-based forum and not conducive to drawing. In that regard, YA is a bit sketchy --- pun intended.

All of the bonds in all of the compounds you have listed are polar. The electronegativity differences are all non-zero. In addition, all of the molecules are nonpolar with the exception of ammonia, which is polar. Look at the geometry and the corresponding symmetry of the molecules. In general, molecules which are symmetrical are nonpolar, while asymmetrical molecules are polar.

NH3 --- trigonal pyramidal

BeCl2 --- linear

BF3 --- trigonal planar

XeF4 --- square planar

SF6 --- octahedral

PCl5 --- trigonal bipyramidal

VSEPR Theory

#electron pairs ..... e- pair geom..... molecular geom..... bond angle

2 ........................... linear ..................... linear .................... 180

3 (no lone pairs) .. trigonal planar ...... trigonal planar ....... 120

3 (one lone pair) .. trigonal planar ...... bent .........................LT 120

4 (no lone pairs) .. tetrahedral ............ tetrahedral .............. 109.5

4 (one lone pair) .. tetrahedral ............ trigonal pyramidal .. LT 109.5

4 (2 lone pairs) .... tetrahedral ............ bent ...................….. LT. 109.5

5 (no lone pairs) .. trig bipyramidal ....trig bipyramidal ….. 90 and 120

5 (one lone pair) .. trig bipyramidal ... see-saw ................... 90 and 120

5 (2 lone pairs) .... trig bipyramidal ....T-shaped .............,... 90

5 (3 lone pairs) .... trig bipyramidal ....linear ........................180

6 (no lone pairs) .. octahedral ............ octahedral ................ 90

6 (one lone pair) .. octahedral ............ square pyramidal ......90

6 (2 lone pairs) .... octahedral ............ square planar .............90

(LT = "less than")

Sample drawing: