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Chemistry Asked by a SnapAndSolve user · about 2 hours ago

Use VSEPR theory to predict the shape of each of the following. THEN, determine if the molecule has a net...

1. Use VSEPR theory to predict the shape of each of the following. THEN, determine if the molecule has a net dipole. SHOW YOUR WORK. If electronegativity values aren’t shown that means you should be able to predict relative values.
a) NI3 (N=3.0, I=2.5)
b) NF3
c) SeO2
d) SO3

Answer

  1. NI3 (N=3.0, I=2.5):

    The shape of NI3 is trigonal pyramidal due to the presence of a lone pair on the nitrogen atom. The molecule has a net dipole moment because the bond dipoles do not cancel out, as iodine is less electronegative than nitrogen.

  2. NF3:

    NF3 also has a trigonal pyramidal shape due to the lone pair on nitrogen. It has a net dipole moment because the bond dipoles do not cancel out, with nitrogen being more electronegative than fluorine.

  3. SeO2:

    SeO2 has a bent shape due to the lone pairs on the selenium atom. It has a net dipole moment because the bond dipoles do not cancel out.

  4. SO3:

    SO3 has a trigonal planar shape. It does not have a net dipole moment because the bond dipoles cancel out due to the symmetrical shape.

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