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Question

Which of the following species (molecule or ion) can behave both as a Lewis Base as well as a Bronsted base? 
 
  1. Cl
     
  2. CO
     
  3. BF3
  4. None of the above 


Solution

The correct option is A Cl
 
According to Bronsted-Lowry  and Lewis Concept of acid and bases:
Species (molecule or ion) which has a tendency to accept a proton can act as a Bronsted Lowry base.

Species which has a lone pair of electrons available for donation can act as a Lewis base.

BF3 has a empty p orbital, and can accept a lone pair of elecron to act as a lewis acid, not a lewis base.
CO cannot accept a proton and hence cannot act as a Bronsted base.  It can act as a Lewis base, as the lone pair on carbon can donates it's electrons, (for example forming transition metal coordination complexes).

While Cl accepts a proton to form HCl. It also has a lone pair of electrons available for donation. So, it can act both as a Bronsted Lowry base as well as Lewis base.

 

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