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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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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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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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