The hybridisation of the central iodine atom | vedclass

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Question

(A) The correct option is $A$.Explanation:$1$. For $IF_5$: Iodine has $7$ valence electrons. It forms $5$ sigma bonds with $F$ atoms and has $1$ lone

Vedclass · Accepted Answer

$sp^3d^2, sp^3d, sp^3$

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(A) The correct option is $A$.Explanation:$1$. For $IF_5$: Iodine has $7$ valence electrons. It forms $5$ sigma bonds with $F$ atoms and has $1$ lone pair. Total electron pairs = $5 + 1 = 6$,which corresponds to $sp^3d^2$ hybridisation.$2$. For $I_3^-$: The central iodine atom has $7$ valence electrons,plus $1$ electron from the negative charge,totaling $8$. It forms $2$ sigma bonds with other $I$ atoms and has $3$ lone pairs. Total electron pairs = $2 + 3 = 5$,which corresponds to $sp^3d$ hybridisation.$3$. For $I_3^+$: The central iodine atom has $7$ valence electrons,minus $1$ electron from the positive charge,totaling $6$. It forms $2$ sigma bonds with other $I$ atoms and has $2$ lone pairs. Total electron pairs = $2 + 2 = 4$,which corresponds to $sp^3$ hybridisation.

Molecule	Hybridisation of central atom	Shape
$(a)$ $PCl_5$	$dsp^3$	square pyramidal
$(b)$ $[Ni(CN)_4]^{2-}$	$sp^3$	tetrahedral
$(c)$ $SF_6$	$sp^3d^2$	octahedral
$(d)$ $IF_3$	$dsp^3$	pyramidal

The hybridisation of the central iodine atom in $IF_5$,$I_3^-$,and $I_3^+$ are respectively:

Similar Questions

Hybridization is due to the overlapping of

Identify the correct set from the following table:
Molecule Hybridisation of central atom Shape
$(a)$ $PCl_5$ $dsp^3$ square pyramidal
$(b)$ $[Ni(CN)_4]^{2-}$ $sp^3$ tetrahedral
$(c)$ $SF_6$ $sp^3d^2$ octahedral
$(d)$ $IF_3$ $dsp^3$ pyramidal

The state of hybridisation of $B$ in $BCl_3$ is

Explain $sp^3d^2$ hybridization with a suitable example.

In which of the following molecules/ions is the central atom $sp^2$ hybridized?

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