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Shape and Geometry Using VSEPR

Although the ...

Question

Although the number of bond pair of electrons in the valence shell of phosphorus in a $P C l_{3}$ molecule is 3, its shape is not trigonal planar. due to Presence of lone pair of electrons on phosphorous.

A

True

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B

False

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Solution

The correct option is A True
It is true because, the trigonal planar is not formed due to lone pair-bond pair repulsion of the lone pair electrons and bond pair electrons and thus forms tetrahedral structure.

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Similar questions

X Y_{2}

contains two sigma bonds, two pi bonds and one lone pair of electrons in the valence shell of

X

. The shape of molecule is:

Q. Which response contains all of the characteristics listed that should apply to phosphorus trichloride,

P C l_{3},

and no other characteristics?
(1) trigonal planar
(2) one unshared pair of electrons on P
(3)

s p^{2}

hybridized at P
(4) polar molecule
(5) polar bonds

Q. You might have observed in

C O_{2}

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Explain the non-linear shape of $H_{2} S$ and non-planar shape of $P C l_{3}$ using valence shell electron pair repulsion theory.

Q. By the following method you can predict the geometrical shape of species with only one central atom, without first drawing the Lewis structure :
Total number of electron pairs = (number of valence electrons

\pm

electrons (for ionic) charge)/2
Number of bond electron pairs = number of atoms - 1
Number of electron pairs around central atom = total number of electron pairs - 3 [number terminal atoms (except H)]
Number lone pair = (number of central electron pairs - number of bond pairs)

How many of the following have trigonal bipyramidal shape based on this method?

(a) P C l_{5} (b) N H_{3} (c) H_{2} O

(d) {C l O_{3}}^{-} (e) {I C l_{4}}^{-}

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