Answer:
Arrhenius, H⁺, H⁺ and an anion, OH⁻, OH⁻ and a cation, Bronsted-Lowry, donates, accepts, Lewis, accepts, donates.
Explanation:
The earliest and simplest definition of acids and bases was suggested by Arrhenius. He defined an acid as a substance with H⁺ in its formula that dissociates water to yield H⁺ and an anion and a base as a substance with OH⁻ in its formula that dissociates in water to yield OH⁻ and a cation.
Examples:
Acid: [tex]HCl_{(aq)} \rightleftharpoons Cl^-_{(aq)} + H^+_{(aq)}[/tex]
Base: [tex]NaOH \; (aq) \rightarrow Na^+ \; (aq) + OH^- \; (aq)[/tex]
Bronsted-Lowry defined an acid as any species that donates an H⁺ ion, an proton , and a base as any species that accepts an H+ ion, a proton.
Examples:
Acid: [tex]HCl_{(aq)} + H_{2}O_{(l)} \rightleftharpoons Cl^-_{(aq)} + H_{3}O^+_{(aq)}[/tex]
Base: [tex]F^-_{(aq)} + H_2O_{(l)} \rightleftharpoons HF_{(aq)} + OH^-_{(aq)}[/tex]
Lewis defined an acid as any species that an accepts an electron pair to form a bond and a base as any species that donates an electron pair to form a bond.
Arrhenius H⁺ and OH⁻. Bronsted-Lowry, donates, accepts proton and Lewis, accepts, donates electron pair.
Arrhenius proposed that acids are substances that dissociate in water to yield a hydrogen ion (H+), and that bases ionize in water to produce hydroxide ions (OH−).
While on the other hand, Bronsted-Lowry says that any compound that can give a proton to other compound is considered as an acid, and the compound that accepts a proton is considered as base.
According to Lewis, an acid is an electron pair acceptor and a base is an electron pair donor.
Learn more about acid here: https://brainly.com/question/25148363
