Answer:
I. Lewis acid-base reaction
II. Arrhenius, Brønsted-Lowry, and Lewis' acid-base reaction
III. Brønsted-Lowry and Lewis'acid-base reaction
IV. Lewis acid-base reaction
Explanation:
According to Arrhenius, an acid is a substance that dissolves in water to produce H+ ions, and a base is a substance that dissolves in water to produce hydroxide (OH−) ions.
In the reaction below, AH is an avid, BOH is a base reacting together to form a salt(A-B+) and water only.
AH + BOH ---> A-B+ + H2O
According to Brønsted-Lowry definition, an acid is any substance that can donate a proton, and a base is any substance that can accept a proton.
In the reaction below, AH is an acid while B is a base, reacting together to form an acid-base conjugate pair.
AH + B <-----> BH+ + A-
According to Lewis' definition, an acid is a species that accepts an electron pair while a base donates an electron pair resulting in a coordinate covalently bonded compound, also known as an adduct. In the reaction below, A+ is an acid, B- is a base, reacting together to form product A-B.
A+ + B- ------> A-B
Considering the above definitions;
I. Cu²+ + 4 Cl− ---> CuCl4²− is a Lewis acid-base reaction because it involves electron sharing only.
II. Al(OH)3 + 3HNO3 ---> Al3+ + 3H2O + 3 NO3− is an Arrhenius, Brønsted-Lowry, and a Lewis acid-base reaction because it involves protons, electrons and hydroxide ions.
III. N2 + 3 H2 ---> 2NH3 is a Lewis acid-base reaction because it involves sharing of electrons only.
IV. CN− + H2O ---> HCN + OH is both a Lewis and Brønsted-Lowry acid-base reaction because both protons and electrons sharing is involved.
In a Bronsted-Lowry acid-base reaction reaction, an acid donates protons which is accepted by the base.
The following are useful definitions of acids and bases;
Based on these, we can now classify the reactions accordingly;
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