Among the following, which one is a wrong statement?

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$pπ - dπ bonds are present in {SO}_{2}$

$I_{3}^{+} has bent geometry.$

${PH}_{5} and {BiCl}_{5} do not exist.$

${SeF}_{4} and {CH}_{4} have same shape.$

answer is C.

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Detailed Solution

SeF₄ contains 4 bpe- and 1 lpe- on Seatom.
Shape of molecule is see-saw. CH4 contains 4 bpe- arrow C- atom shape of molecule is tetrahedral.
(1) PH₅ does not exists. When “P“ reacts with H, highest oxidation state of P cannot be achieved due to following reasons.
(i) High atomization of H₂
(ii) High electron gain enthalpy of H₂
(ii) low electronegativity of H.
d-orbital could not be hybridised with s and p-orbitals.
(2) BiCl₅ does not exists
Due to large size of Bi and Cl, effective overlapping of hybrid orbital of Bi and p-atomic orbital of Cl. As a result of bond strength, Bi-Cl bond is very weak.
SO2 contains
1 pπ pπ bond
1 pπ dπ bond
(4) I₃⁺ central atom (I) is containing 2 bpeand 2 lpe-s
Hybridization = sp³
Shape = Angular or bent