Difference between lewis base and bronsted base
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Acids and Bases: Lewis vs Bronsted.
There are two complementary definitions of acids and bases that are important: the Bronsted (or Bronsted-Lowry) definition: an acid is a proton (H+ ion) donor, and a base is a proton acceptor; the Lewis definition: an acid is an electron acceptor, and a base is an electron donor.
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DIFFERERNCE
According to the Bronsted definition:
Acid: is an #H^+# donor.
Base: is an #H^+# acceptor.
Example:
Bronsted Acid: #HCl->H^++Cl^-#
Bronsted Base: #NH_3+H^(+)->NH_4^+#
According to the Lewis definition:
Acid: is an electron lone pair acceptor.
Base: is an electron lone pair donor.
Example:
Lewis Acid: #AlCl_3#
Lewis Base: #H_2O#
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