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Question
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 |
Solution
| Column I | Column II |
| (i) Tetrahedral | (c) sp3 |
| (ii) Trigonal | (a) sp2 |
| (iii) Linear | (b) sp |
Explanation:
(i) 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.
(ii) There are two possibilities for the central atom to have sp2 hybridization. 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.
(iii) 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.
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