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Determine the shape, ideal bond angle(s), and the direction of any deviation from those angles for each of the following:
(c) SeF₄

Respuesta :

The shape of SeF₄ is trigonal bipyramidal, ideal bond angle is 120.

What is the explanation?

  • 1 Se + 4 F = 6 + 4×7 = 34 valence electrons. Se must expand its octet. This gives Se four bond pairs and one lone pair. The Lewis structure is like that of SeF₄.
  • The electron arrangement for five electron pairs is trigonal bipyramidal.
  • The bulky lone pair occupies an equatorial position.
  • The molecular shape considers only the Se-Br bonds. As with SF₄, the shape is a see-saw.
  • The hybridization that corresponds to five electron pairs is sp³d.
  • The VSEPR notation is AX₄E.
  • The bond angles are:

                 axial-axial = > 180°;

                 equatorial-equatorial = < 120°;

                 axial-equatorial = < 90°.

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