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Explain why the following compounds beha...

Explain why the following compounds behave as Lewis acids ?
(a) `BCl_(3)`
(b) `AlCl_(3)`

Text Solution

Verified by Experts

Both these compounds behave as Lewis acids because the central atoms in both are `sp^(2)` hybridised and the electron deficient in nature.
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DINESH PUBLICATION-P BLOCK ELEMENTS (GROUP 13 AND 14 )-Short answer type
  1. Explain the nature of boric acid as a Lewis acid in water.

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  2. Draw the structure of boric acid showing hydrogen bonding. Which speci...

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  3. Explain why the following compounds behave as Lewis acids ? (a) BCl(...

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  4. Give reasons for the following (a) C Cl(4) is immiscible in water, w...

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  5. Explain the following (a) CO(2) is a gas whereas SiO(2) is a solid ...

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  6. The +1 oxidation state in group 13 and +2 oxidation state in group 14 ...

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  7. Carbon and silicon both belong to the group 14, but inspite of the sto...

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  8. If a trivalent atom replaces a few silicon atoms in three dimensional ...

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  9. When BCl(3) is treated with water, it hydrolyses and forms [B(OH)(4)]^...

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  10. Aluminium dissovles in mineral acids and aqueous alkalies and thus sho...

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  11. Explain the following : (a) Boron has high melting and boiling point...

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  12. Identify the compound A, X and Z in the following reactions: (i) A+2...

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  13. Complete the following chemical equations: (i) z+3LiAlH(4)rarrX+3Li...

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  14. Describe the general trends in the following properties of the element...

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  15. Account for the following observation: (i) AlCl(3) is Lewis acid (...

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  16. When aqueous solution of borax is acidified with hydrochloric acid, a ...

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  17. Three pairs of compounds are given below, identify that compound in e...

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  18. BCl(3) exists as monomer whereas AlCl(3) is dimerised through halogen ...

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  19. Explain why BF(3) exist but BH(3) does not.

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  20. What are silicones ?

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