Match the shape of molecules in Column I with the type of hybridisation in Column II.

Column I	Column II
(i) Tetrahedral	(a) sp2
(ii) Trigonal	(b) sp
(iii) Linear	(c) sp3

<p>This is a Matching Type Questions as classified in NCERT Exemplar</p><p><strong>Ans:</strong></p><p><strong> (i)</strong> Tetrahedral&nbsp; &nbsp;<strong> (c)</strong> sp³</p><p><strong> (ii)</strong> Trigonal&nbsp; &nbsp;<strong> (a)</strong> sp²</p><p><strong> (iii)</strong> Linear&nbsp; &nbsp;<strong> (b)</strong>sp</p><p><strong>&nbsp;</strong></p><p><strong>Explanation :-</strong></p><p><strong> (i)</strong> A tetrahedral molecule has four electron pairs and these make sigma bonds with each other. The s and p orbitals overlap with each other thus forming a sp³ hybridized molecule.</p><p><strong> (ii)</strong> There are two possibilities for the central atom to have sp² Either all the bonds are in place i.e, the bond pairs are all sigma bonds or pi bonds or there are only two bonds and one lone pair of electrons.</p><p><strong> (iii)</strong> The sp hybridization involves the mixing of the valence electrons in s orbital with another valence electron in the p orbital which yields two sp orbitals which are oriented in a linear geometry.</p>

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