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Acid:Electron pair;Base:Proton
Depending on the type of acid/base (Arrhenius, Bronsted, Lewis), the acid donates protons and a base doesn't but accepts protons, or the base donates OH- and the acid doesn't, or the acid accepts a pair of electrons and the base donates a pair of electrons. They are just different, that's why.
There are three definitions for acids and bases. Arrhenius definition: An acid is a substance that produces hydrogen (H+) ions in water while a base produces hydroxide (OH-) ions. Bronsted-Lowry definition: An acid gives up or donates a proton (H+) to another molecule while a base accepts a proton. Lewis definition: An acid accepts an electron pair in bonding to another molecule/ion while a base donates and electron pair. Note that if a substance meets one of the first two definitions it probably meets the others as well.
A Lewis acid.
A Bronsted-Lowry Acid Donates H+ ions
Acid:Electron pair;Base:Proton
Acid:Electron pair;Base:Proton
Acid:Electron pair;Base:Proton
Acid:Electron pair;Base:Proton
Acid:Electron pair;Base:Proton
Acid:Electron pair;Base:Proton
It would be beat to include the chart soba person will know which is theist common range of elements. Including this would make it easier for someone to know the right answer.
The Lewis Theory describes a base as a compound that donates an electron pair. By donating the electron pair there is a covalent bond.
A substance that can donate a lone pair of electrons is called a Lewis base. The definition of a Lewis base is a compound or ionic species that can donate an electron pair to an acceptor compound.
Each atom only donates ONE atom, so they form a pair together.
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Depending on the type of acid/base (Arrhenius, Bronsted, Lewis), the acid donates protons and a base doesn't but accepts protons, or the base donates OH- and the acid doesn't, or the acid accepts a pair of electrons and the base donates a pair of electrons. They are just different, that's why.