Which of the following pairs of species have | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) To determine the shapes,we calculate the hybridization and number of lone pairs for each species using the $VSEPR$ theory: $1$. $NO^{+}_2$: $N$ is

Vedclass · Accepted Answer

$XeF_4$ and $ICl^{-}_4$

Vedclass · Answer

(C) To determine the shapes,we calculate the hybridization and number of lone pairs for each species using the $VSEPR$ theory: $1$. $NO^{+}_2$: $N$ is central,$sp$ hybridized,linear shape. $NO^{-}_2$: $N$ is central,$sp^2$ hybridized,bent shape. $2$. $PCl_5$: $sp^3d$ hybridized,trigonal bipyramidal. $BrF_5$: $sp^3d^2$ hybridized,square pyramidal. $3$. $XeF_4$: $Xe$ has $8$ valence electrons,$4$ bond pairs,$2$ lone pairs,$sp^3d^2$ hybridization,square planar. $ICl^{-}_4$: $I$ has $7+1=8$ valence electrons,$4$ bond pairs,$2$ lone pairs,$sp^3d^2$ hybridization,square planar. $4$. $TeCl_4$: $sp^3d$ hybridized,see-saw shape. $XeO_4$: $sp^3$ hybridized,tetrahedral shape. Thus,$XeF_4$ and $ICl^{-}_4$ both have a square planar geometry.

Which of the following pairs of species have identical shapes?

Similar Questions

Compare $x$ and $y$ bond angles in the following molecule:

Which of the following molecules has a three-fold axis of symmetry?

What is bond angle? Explain.

What is the shape of the $SF_2Cl_2$ molecule?

Which of the following has a square planar structure?

Vedclass Test Series

Exam Paper Generator

Online Exam Module