Question

Among the following, the number of planar, polar species are:
\[N{{H}_{3}},\\text{Cl}{{\text{F}}_{\text{3}}}\text{,B}{{\text{F}}_{\text{3}}}\text{, HN}{{\text{O}}_{\text{3}}}\text{,S}{{\text{F}}_{\text{4}}}\text{,S}{{\text{O}}_{\text{2}}}\text{,Xe}{{\text{F}}_{\text{4}}}\text{, IC}{{\text{l}}_{\text{3}}}\]
A. 3
B. 4
C. 5
D. 6

Answer 1

Hint:The geometry or number of species of any orbital can be concluded by the concept of hybridization. Where hybridization can be defined as the concept of mixing two atomic orbitals with same energy levels and giving a new degenerated type of orbitals.

Complete step-by-step answer:Geometry of any particular substance depends upon the hybridization occurring or also how many bond pairs and lone pairs are present in that orbital. The planar and polar molecules can be described by taking all the examples:
$N{{H}_{3}}$ is $s{{p}^{3}}$ hybridized and of polar nature but non-planar in shape due to one pair present.
$\text{Cl}{{\text{F}}_{\text{3}}}$ and $\text{IC}{{\text{l}}_{\text{3}}}$ are $s{{p}^{3}}d$ hybridized and planar in nature due to the presence of 2 lone pairs have T-shaped like structure and also polar in nature.
$\text{HN}{{\text{O}}_{\text{3}}}$ and $\text{S}{{\text{O}}_{\text{2}}}$ are $s{{p}^{2}}$ hybridized are planar in nature and also show polar behavior due to difference in electronegativity.
$\text{S}{{\text{F}}_{\text{4}}}$ shows $s{{p}^{3}}d$ hybridization polar in nature but it is non-planar.
\[\text{Xe}{{\text{F}}_{\text{4}}}\] have \[s{{p}^{3}}{{d}^{2}}\] hybridization also shows polarity but non-planar in shape.
Thus option B is the correct answer which defines that four species are there which are both planar and polar.

Note:The intermixing of atomic orbitals in case of hybridization based on quantum mechanics which describe that only those atomic orbitals which have same energy level can take part in hybridization and both full filled and half-filled orbitals can also take part in this process if they have equal energy.