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Chemical Bonding And Molecular Structure

Question
CBSEENCH11008374
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In which of the following molecules the central atom does not have sp3 hybridisation?

  • CH4

  • SF4

  • BF4-

  • NH4+

Solution

B.

SF4

When the number of hybrid orbitals, H  is 4, the hybridization is sp3 hybridization
straight H space equals space 1 half left square bracket space straight V space plus space straight M space minus space straight C space plus space straight A right square bracket where comma space straight V space equals space number space of space monovalent space atoms straight C space equals space total space positive space charge straight A space equals space negative space charge straight a right parenthesis space For space CH subscript 4 straight H space equals space 1 half left square bracket space 4 space plus space 4 space minus 0 space plus space 0 right square bracket space equals space 4 space sp cubed straight b right parenthesis space space For space SF subscript 4 comma end subscript straight H space equals space 1 half left square bracket space 6 plus 4 minus 0 plus 0 right square bracket space equals space 5 space sp cubed straight d straight c right parenthesis space For space BF subscript 4 superscript minus comma straight H space equals space 1 half left square bracket space 3 plus space 4 minus 0 plus 1 right square bracket space equals space 4 comma space thus space sp cubed straight d right parenthesis space For space NH subscript 4 superscript plus straight H space equals space 1 half left square bracket 5 plus 4 minus 1 plus 0 right square bracket space equals space 4 space thus space sp cubed
Thus, only in SF4 the central atom does not have sp3 hybridisation.

Some More Questions From Chemical Bonding and Molecular Structure Chapter

What are 'Lewis structures'?

Name the conditions for the formation of an ionic bond between two atoms.

What is crystal lattice?

What is electrovalency?

What bond is present in MgCl2 molecules?

Write Lewis dot symbols for atoms of the elements Mg, Na, B, O, N, Br.

Draw the Lewis structure for the ionic compound by aluminium and fluorine.

Two elements A and B have the electronic configuration as:
A = 1s22s22p63s2 and B = 1s22s22p5
Write the empirical formula of the substance containing A and B.

What type of bonding would you expect between:
(i) a metal and a non-metal
(ii) a non-metal and another non-metal?

Give reasons in one or two sentences for the observation that in their compounds non-metals form anions and not cations.

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