Acid-Base Question?

Question

Hello, I'd like some feedback for a question I'm on.

1(a) Write a balanced reaction equation for a Lewis Acid with a Bronsted Acid of your choice. Indicate which of the species in your reaction is the Lewis Acid and which is the Bronsted Acid

NH3 + BF3 --> NH3BF3
Bronsted Acid + Lewis Acid
 
1(b) Write a balanced reaction equation for a Lewis Acid with a Bronsted Base of your choice. Indicate which of the species in your reaction is the Lewis Acid and which is the Bronsted Base

(CH3)3CCl + AlCl3 --> (CH3)3CClAlCl3
Bronsted Base + Lewis Acid

Note: Lewis Acid = Accepts e-
          Bronsted Acid = H+ Donor
          Bronsted Base = Acceptes H+

Did I do it correctly?
Any help is greatly appreciated. Thank you!

pisgahchemist · Accepted Answer

Acid/base theories.....

Either explain a reaction using the Lewis theory or the Bronsted-Lowry (BL) theory.  You don't mix the theories. BL theory acids and bases can be explained with the Lewis theory, but Lewis theory acid/base reactions may not be explained by the BL theory.

BL theory has an acid and a base which are the reactants and a conjugate acid and conjugate base which are the products.  Lewis theory reactions frequently have a single product, which is the adduct.  The Lewis acid and the Lewis base combine to form a single product and are identified by the species that donated an electron pair (the base) and the species that accepted the electron pair (the acid).

H3N: + BF3 --> H3N−BF3
Lewis...Lewis....adduct
base....acid

NH3 is a BL base because it can accept a proton to make NH4^+.

================

(CH3)3CCl + AlCl3 --> (CH3)3CClAlCl3 
Lewis base ..Lewis acid .... adduct
The base is a Lewis base because it is an electron pair donor, and aluminum is an electron pair acceptor.
R−C−Cl: + AlCl3 --> R−C−Cl−AlCl3 ...... (assuming such a thing happens)

(CH3)3CCl is not a Bronsted Lowry base.  It is not a "proton acceptor".

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Acid-Base Question?

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