Protonation

Protonation is the addition of a proton (H⁺) to an atom, molecule, or ion, increasing its charge by one unit. It is the reverse of deprotonation.

Brønsted–Lowry acid–base theory: An acid–base model in which acids donate protons and bases accept them. Protonation is the proton-accepting half of this model’s acid–base reactions.
Proton: A positively charged subatomic particle found in atomic nuclei; in solution, H⁺ commonly associates with solvent molecules. Protonation names the addition of this particle, often transferred in solvated form.
Protonation state: The pattern of proton attachment and charge on a molecule under specified conditions. A molecule’s protonation state links solution conditions to its charge and reactivity.
Deprotonation: The removal of a proton from an atom, molecule, or ion. It is the direct reverse of protonation, rather than an addition of H⁺.
Conjugate acid: The species formed when a base accepts a proton. A protonated base is the conjugate acid of its unprotonated form.
Brønsted–Lowry base: A chemical species that accepts a proton in Brønsted–Lowry acid–base theory. A protonatable atom or molecule acts as a base when it accepts H⁺.
Acid catalysis: An increase in reaction rate caused by proton donation from an acid. Catalysts often protonate a reactant, making a bond or functional group more reactive.
Electron attachment: The gain of an electron by an atom or molecule. It can change charge, but adds an electron rather than a proton.
Acid dissociation constant: A measure of an acid’s tendency to donate a proton in solution. Its value helps determine the equilibrium between protonated and deprotonated forms.
pH: A logarithmic measure related to hydrogen-ion activity in a solution. Solution pH influences the equilibrium between protonated and unprotonated species.

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