Explain the lewis concept of acids and bases?
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Explanation:
Answer:
Gilbert Lewis (1875–1946) proposed a third theory of acids and bases that is even more general than either the Arrhenius or Brønsted-Lowry theories. A Lewis acid is a substance that accepts a pair of electrons to form a covalent bond. A Lewis base is a substance that donates a pair of electrons to form a covalent bond. So, a Lewis acid-base reaction is represented by the transfer of a pair of electrons from a base to an acid. A hydrogen ion, which lacks any electrons, accepts a pair of electrons. It is an acid under both the Brønsted-Lowry and Lewis definitions. Ammonia consists of a nitrogen atom as the central atom with a lone pair of electrons. The reaction between ammonia and the hydrogen ion can be depicted as shown in the Figure 1.
Ammonia is both a Bronsted base and a Lewis The lone pair on the nitrogen atom is transferred to the hydrogen ion, making the NH3 a Lewis base while the H + is a Lewis acid.
Some reactions that do not qualify as acid-base reactions under the other definitions do so under only the Lewis definition. An example is the reaction of ammonia with boron trifluoride.
Boron trifluoride is a Lewis acid but not a Bronsted acidBoron trifluoride is the Lewis acid, while ammonia is again the Lewis base. As there is no hydrogen ion involved in this reaction, it qualifies as an acid-base reaction only under the Lewis definition. The Table below summarizes the three acid-base theories.
Acid-Base Definitions
Type Acid Base
Arrhenius H + ions in solution OH − ions in solution
Brønsted-Lowry H + donor H + acceptor
Lewis electron-pair acceptor electronbase.