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Chemistry Asked by a SnapAndSolve user · about 3 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) NH3 (N=3.0, I=2.5)
b) NF3 (N=3.0, F=4.0)
c) SeO2
d) SO3
e) SiF4

Answer

  1. NH3 (N=3.0, I=2.5):

    Valence Electrons: 5 (N) + 3(1) (H) = 8
    Electron Geometry: Tetrahedral
    Molecular Shape: Trigonal Pyramidal
    Net Dipole: Yes, directed towards N.

  2. NF3 (N=3.0, F=4.0):

    Valence Electrons: 5 (N) + 3(7) (F) = 26
    Electron Geometry: Tetrahedral
    Molecular Shape: Trigonal Pyramidal
    Net Dipole: Yes, directed towards F.

  3. SeO2:

    Valence Electrons: 6 (Se) + 2(6) (O) = 18
    Electron Geometry: Trigonal Planar
    Molecular Shape: Bent
    Net Dipole: Yes, directed towards O.

  4. SO3:

    Valence Electrons: 6 (S) + 3(6) (O) = 24
    Electron Geometry: Trigonal Planar
    Molecular Shape: Trigonal Planar
    Net Dipole: No, symmetrical.

  5. SiF4:

    Valence Electrons: 4 (Si) + 4(7) (F) = 32
    Electron Geometry: Tetrahedral
    Molecular Shape: Tetrahedral
    Net Dipole: No, symmetrical.

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