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Question: What atomic or hybrid orbitals make up the sigma bond between \[I\] and \[Cl\] in iodine pentachlori...

What atomic or hybrid orbitals make up the sigma bond between II and ClCl in iodine pentachloride, ICl5IC{l_5}?

Explanation

Solution

The intermixing of two or more pure atomic orbitals of an atom with almost the same energy to give the same number of identical and degenerate new types of orbitals is known as hybridization. The new orbitals formed are also known as hybrid orbitals.
Formula to find the hybridization of a molecule is given by
Hybridisation=Number of σ bonds+ Number of lone pairsHybridisation = Number{\text{ }}of{\text{ }}\sigma {\text{ }}bonds + {\text{ }}Number{\text{ }}of{\text{ }}lone{\text{ }}pairs

Complete answer:
If the sum is 22 \to hybridization − spsp
If the sum is 33 \to hybridization − sp2s{p^2}
If the sum is 44 \to hybridization − sp3s{p^3}
If the sum is 55 \to hybridization− sp3ds{p^3}d
If the sum is 66 \to hybridization− sp3d2s{p^3}{d^2}
COMPLETE STEP BY STEP ANSWER-
Lewis dot structure of ICl5IC{l_5}:

Considering central metal atom, II
Number{\text{ }}of{\text{ }}lone{\text{ }}pairs = 1 \\\ Number{\text{ }}of{\text{ }}bond{\text{ }}pairs = 5 \\\
Hybridisation=1+5=6Hybridisation = 1 + 5 = 6
Therefore, IClI - Cl bond is sp3d2s{p^3}{d^2} hybridized.
About ICl5IC{l_5},
Hybridisation-sp3d2s{p^3}{d^2}
Geometry- Octahedral
Shape- Square pyramidal

Note:
You can expect bond angles of 90{90^ \circ } and 180{180^ \circ }.
Also note that when forming hybrid orbitals, you use nn atomic orbitals to make nn hybrid orbitals, where nn is the total amount of orbitals. Here, in case of ICl5IC{l_5}, n=6n = 6