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Overlaps Taking All Together

Predict the s...

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Predict the shape of XeO3 with bond pair ,lone pair calculation using valence electrons

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Q. The pair of valence electrons which participates in bonding is termed as lone pair.

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. 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}}^{-}

Q. 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.

Q. You might have observed in

C O_{2}

molecule, that there are two pairs of valence electrons on each of the oxygen atoms that are not bonded. Such a pair of electrons is called a lone pair. Now how many lone pairs are present is

S_{8}

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Overlaps Taking All Together

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