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The geometry of electron paris around I ...

The geometry of electron paris around I in `IF_(5)` is

A

Octahedral

B

Trigonal bipyramidal

C

square pyramidal

D

pentagonal planar

Text Solution

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The correct Answer is:
To determine the geometry of electron pairs around iodine in IF₅, we can follow these steps: ### Step 1: Determine the Valence Electrons Iodine (I) is in group 17 of the periodic table, which means it has 7 valence electrons. ### Step 2: Count the Electrons from Fluorine Fluorine (F) is in group 17 as well and has 7 valence electrons. In IF₅, there are 5 fluorine atoms, contributing a total of 5 x 7 = 35 valence electrons. ### Step 3: Calculate Total Valence Electrons The total number of valence electrons in IF₅ can be calculated as follows: - Valence electrons from iodine: 7 - Valence electrons from 5 fluorine atoms: 35 - Total = 7 + 35 = 42 valence electrons. ### Step 4: Determine Bonding and Lone Pairs Iodine forms 5 bonds with the 5 fluorine atoms. Each bond uses 2 electrons, so: - Electrons used in bonding = 5 bonds x 2 = 10 electrons. - Remaining electrons = Total valence electrons - Electrons used in bonding = 42 - 10 = 32 electrons. ### Step 5: Identify Lone Pairs Since iodine is bonded to 5 fluorine atoms, it will have 1 lone pair of electrons left (7 valence electrons - 5 used in bonding = 2 electrons, which form 1 lone pair). ### Step 6: Determine the Steric Number The steric number is calculated as the number of bond pairs plus the number of lone pairs: - Bond pairs = 5 (from the 5 F-I bonds) - Lone pairs = 1 - Steric number = 5 + 1 = 6. ### Step 7: Determine Hybridization The hybridization corresponding to a steric number of 6 is sp³d². ### Step 8: Determine the Molecular Geometry For a molecule with a steric number of 6 and one lone pair, the geometry is square pyramidal. ### Conclusion The geometry of electron pairs around iodine in IF₅ is square pyramidal. ---
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