Most of the reactions in organic chemistry involved proton transfer and so the topic is very useful in our journey through this subject. We discussed the definitions of the following concepts: Arrhenius Concept, Bronsted-Lowry Concept, and Lewis Concept.
Arrhenius Concept is only applicable in an aqueous system. It stated that when in water, acids have hydrogen ions while base have hydronium ions. According to the Bronsted-Lowry Concept, an acid is a proton donor while a base is a proton acceptor. A compound that has both H+ and a pair of electron can act either as an acid or base. It also introduced the concept of conjugate acid-base. It states that an acid is always one unit more positive than its conjugated base while a base is always one unit more negative than conjugate acid. The Lewis Concept states that an acid is an electron pair acceptor while a base is an electron pair donor. All Bronsted-Lowry Base are Lewis Base but not all Lewis Acid are Bronsted-Lowry Acid.
The reaction of an acid with a base is in equilibrium with the conjugate base and conjugate acid products. Atom bonded to acidic hydrogen, hybridization, hydrogen bonding, inductive effect, steric effect, resonance, resonance in aromatic compounds are the factors that affect the acidity and basicity of a compound.
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