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what theories out of the major two ( Bronsted-Lowry Theory of acids and bases and The Lewis Theory of acids and bases) should we use in common problems, and which one is more reliable ?
Acut said:Do you have any other suggestions for books on the subject?
The main difference between Bronsted-Lowry and Lewis acid-base theories is their definition of acids and bases. Bronsted-Lowry theory defines an acid as a proton donor and a base as a proton acceptor, while Lewis theory defines an acid as an electron pair acceptor and a base as an electron pair donor. Additionally, Bronsted-Lowry theory only applies to reactions involving the transfer of protons, while Lewis theory can explain a wider range of reactions.
Bronsted-Lowry theory explains acid-base reactions as the transfer of a proton from an acid to a base, while Lewis theory explains them as the formation of a covalent bond between an electron pair donor (base) and an electron pair acceptor (acid). Both theories can be used to predict the direction of an acid-base reaction and the resulting products.
The main strength of Bronsted-Lowry theory is its simplicity and ability to explain a wide range of acid-base reactions. However, it does not account for reactions that do not involve proton transfer. On the other hand, Lewis theory is more comprehensive and can explain a wider range of reactions, but it can be more complex and difficult to apply in some cases.
Bronsted-Lowry and Lewis theories are complementary to each other. Bronsted-Lowry theory can be seen as a subset of Lewis theory, as it only applies to reactions involving the transfer of protons. Lewis theory expands upon Bronsted-Lowry theory by including reactions that do not involve proton transfer.
Both Bronsted-Lowry and Lewis theories are widely accepted in the scientific community and are used to explain and predict acid-base reactions. However, Lewis theory is generally considered to be more comprehensive and is commonly used in modern chemistry.