Acid Base Reaction Acid Base Reaction An acid–base reaction is a chemical reaction that occurs between an acid and a base. Several concepts that provide alternative definitions for the reaction mechanisms involved and their application in solving related problems exist. Despite several differences in definitions, their importance becomes apparent as different methods of analysis when applied to acid–base reactions for gaseous or liquid species, or when acid or base character may be somewhat less apparent. The first of these scientific concepts of acids and bases was provided by the French chemist Antoine Lavoisier, circa 1776. Definitions :- The Lewis definitions of acid and base describe an acid as an "electron pair acceptor" and a base as an "electron pair donor" A Bronstead-Lowry acid is a molecule or ion that donates a proton and a Bronstead base is a molecule or ion that accepts a proton. According to Arrhenius theory acids are molecules that dissociate in water to make the hydronium ion (H3O+). Bases on the other hand are molecules that dissociate to form hydroxide ions (OH-).
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Lewis Acid Base Theory The Lewis concept of acids and bases does not depend on the presence of a particular element as do Bronstead - Lowry and Arrhenius systems. Acidic or basic properties are instead ascribed to the behavior of valence electrons, which all substances possess. Because the Lewis acid-base system incorporates a broader range of reactions as acid-base reactions, there is a greater range of reactivity patterns between Lewis acids and bases. An example is borontrifluoride ammonia ad duct, BF3.NH3. The BF3 molecule has a planar triangular structure with some double bond character in each B-F bond as fluorine is considered to be the most electronegative element. The boron atom in BF3 is quite positive and the boron is frequently described as electrondeficient. The lone pair in the HOMO of the ammonia molecule combines with the empty LUMO of the BF3 which has very large, empty orbital lobes on boron to form the ad duct. Bron stead-Lowery Theory The definition for acid and base given is expanded to the Arrhenius list of acids and bases to include the gases HCl and NH3, along with many other compounds. This definition also introduced the concept of conjugate acids and bases, differing only in the presence or absence of a proton and described all reactions as occurring between a stronger acid and base to form a weaker acid and base.
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Lewis definition :- The hydrogen requirement of Arrhenius and Brønsted–Lowry was removed by the Lewis definition of acid–base reactions, devised by Gilbert N. Lewis in 1923, [13] in the same year as Brønsted–Lowry, but it was not elaborated by him until 1938. Instead of defining acid–base reactions in terms of protons or other bonded substances, the Lewis definition defines a base (referred to as a Lewis base) to be a compound that can donate an electron pair, and an acid (a Lewis acid) to be a compound that can receive this electron pair.
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