Question

Predict the shape of CIF3 on the basis of VSEPR theory​

Answer 1

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☑️THE STANDARD APPLICATION OF VSEPR THEORY TP THIS MOLECULE IS AS FOLLOWS☑️-------

✍️ Central Atom = Chlorine

✍️Valence electron of central atom = 7

✍️Three Flourine atoms contribute = 1 each

✍️Total:10= Five Electron pairs..

✍️The highest repulsion is between any two 'lone Electron pairs', resulting in these moving apart as far as Possible.

✍️The next Highest is between one lone pair and a bond pair.

✍️The lowest is between two bond pairs...

Answer 2

Chlorine trifluoride has 5 regions of electron density around the central chlorine atom (3 bonds and 2 lone pairs). These are arranged in a trigonal bipyramidal shape with a 175° F(axial)-Cl-F(axial) bond angle. The two lone pairs take equatorial positions because they demand more space than the bonds.