First, we need to draw the Lewis structure of IF5.

In short, these are the steps you need to follow for drawing a Lewis structure:

**1. Write the correct skeletal structure for the molecule.**

** * Hydrogen atoms are always terminal (only one bond)**

** * Put more electronegative elements in terminal positions**

**2. Sum the valence electrons from all the atoms.**

**3. Use a pair of electrons to form a bond between each pair of bound atoms.**

**4. Add the remaining electrons to satisfy the octet for a more electronegative atom first.**

**5. If any atoms lack an octet, make a double or triple bond to give them an octet.**

Br is the central atom, so we can draw a preliminary skeletal structure:

There are 5×7 + 7 = 42 electrons, out of which, 10 are used to make 5 covalent bonds. The remaining 30 are divided between the five fluorine atoms, each taking 6 electrons as 3 lone pairs, and Br takes the last pair of electrons:

The hybridization of iodine in IF_{5} is the same as bromine in BrF_{5}, and we have seen in problem 23 that there are 5 atoms and one lone pair on the central atom, therefore, the **electron geometry is octahedral**, while the **molecular geometry is square pyramidal**:

Steric number six indicates *sp*^{3}*d*^{2} hybridization.

Check this 99-question multiple-choice quiz on Geometry and Hybridization:

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