the molecular geometry (shape) for ICl3?

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the molecular geometry (shape) for ICl3?

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• T-shaped.

  When the Chlorine bonds with the Iodine, the iodine will have 3 electrons from the chlorine added to the 7 it already has, giving it 10. Electrons pair, giving you 5 pairs (2 unbonded). Now the most stable configuration those pairs can move into is the one where the pairs are as far apart as possible. This electron geometry is trigonal bipyramidal, it allows three pairs to be 120 degrees apart, with the other two at 90 degrees. But unbonded pairs of electrons take up more space, so they would be more stable if they were able to spread out more. This means the two unbonded pairs will be situated so they can be 120 degrees apart, with one bonded pair taking up the third spot. The other 2 bonded pairs will be above and below this plane at 90 degree angles. It’s hard to describe and a picture is infinitely more valuable:

  http://employees.csbsju.edu/hjakubowski/classes/ch…

  See t-shape.

  I know you asked for the molecular geometry, but understanding the electron geometry is crucial to understanding why the molecular is the way it is.

• Icl3 Molecular Geometry

• The I and Cl atoms each have 7 valence electrons for a total of 28 valence electrons for all of the atoms in the ICl3 molecule.

  The I atom will be the central atom. 3 atoms of Cl will be single bonded to the I atom and the bond will be a covalent bond shared between the I and Cl atoms. That will take care of 24 of the 28 electrons. The remaining 4 electrons will be placed around the I atom.

  The ICl3 molecule will have a T-shaped molecular geometry.

  The electron geometry will be trigonal bipyramidal.

• This Site Might Help You.

  RE:

  the molecular geometry (shape) for ICl3?

• Icl3 Lewis Structure