Hydron

Hydron

Names
Systematic IUPAC name Hydron[1] (substitutive) Hydrogen(1+)[1] (additive)
Other names Proton
Identifiers
CAS Number	12408-02-5 Y
3D model (JSmol)	Interactive image
ChEBI	CHEBI:15378
ChemSpider	1010 Y
IUPHAR/BPS	2346
KEGG	C00080 Y
PubChem CID	1038
UNII	5046UKT60S Y
InChI InChI=1S/p+1 Y Key: GPRLSGONYQIRFK-UHFFFAOYSA-N Y
SMILES [H+]
Properties
Chemical formula	H+
Molar mass	1.007 g·mol−1
Thermochemistry
Std molar entropy (So298)	108.95 J K−1 mol−1
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

In chemistry, the hydron, informally called proton,^[2] is the cationic form of atomic hydrogen, represented with the symbol H⁺. The general term "hydron", endorsed by the IUPAC, encompasses cations of hydrogen regardless of their isotopic composition: thus it refers collectively to protons (¹H⁺) for the protium isotope, deuterons (²H⁺ or D⁺) for the deuterium isotope, and tritons (³H⁺ or T⁺) for the tritium isotope.

Unlike most other ions, the hydron consists only of a bare atomic nucleus. The negatively charged counterpart of the hydron is the hydride anion, H⁻.

Properties

Solute properties

Other things being equal, compounds that readily donate hydrons (Brønsted acids, see below) are generally polar, hydrophilic solutes and are often soluble in solvents with high relative static permittivity (dielectric constants). Examples include organic acids like acetic acid (CH₃COOH) or methanesulfonic acid (CH₃SO₃H). However, large nonpolar portions of the molecule may attenuate these properties. Thus, as a result of its alkyl chain, octanoic acid (C₇H₁₅COOH) is considerably less hydrophilic compared to acetic acid.

The unsolvated hydron (a completely free or "naked" hydrogen atomic nucleus) does not exist in the condensed (liquid or solid) phase. Although superacids are sometimes said to owe their extraordinary hydron-donating power to the presence of "free hydrons", such a statement is highly misleading: even for a source of "free hydrons" like H₂F⁺, one of the superacidic cations present in the superacid fluoroantimonic acid (HF:SbF₅), detachment of a free H⁺ still comes at an enormous energetic penalty on the order of several hundred kcal/mol. This effectively rules out the possibility of the free hydron being present in solution, even as a fleeting intermediate. For this reason, in liquid strong acids, hydrons are believed to diffuse by sequential transfer from one molecule to the next along a network of hydrogen bonds through what is known as the Grotthuss mechanism.^[3]

Acidity

The hydron ion can incorporate an electron pair from a Lewis base into the molecule by adduction:

[H]⁺ + :L → [HL]⁺

Because of this capture of the Lewis base (L), the hydron ion has Lewis acidic character. In terms of Hard/Soft Acid Base (HSAB) theory, the bare hydron is an infinitely hard Lewis acid.

The hydron plays a central role in Brønsted–Lowry acid–base theory: a species that behaves as a hydron donor in a reaction is known as the Brønsted acid, while the species accepting the hydron is known as the Brønsted base. In the generic acid–base reaction shown below, HA is the acid, while B (shown with a lone pair) is the base:

HA + :B → [HB]⁺ + :A^–

The hydrated form of the hydrogen cation, the hydronium (hydroxonium) ion H₃O⁺(aq), is a key object of Arrhenius' definition of acid. Other hydrated forms, the Zundel cation H₅O+2, which is formed from a proton and two water molecules, and the Eigen cation H₉O+4, which is formed from a hydronium ion and three water molecules, are theorized to play an important role in the diffusion of protons though an aqueous solution according to the Grotthuss mechanism. Although the ion H₃O⁺(aq) is often shown in introductory textbooks to emphasize that the hydron is never present as an unsolvated species in aqueous solution, it is somewhat misleading, as it oversimplifies infamously complex speciation of the solvated proton in water; the notation H⁺(aq) is often preferred, since it conveys aqueous solvation while remaining noncommittal with respect to the number of water molecules involved.

Isotopes of hydron

1. Proton, having the symbol p or ¹H⁺, is the +1 ion of protium, ¹H.
2. Deuteron, having the symbol ²H⁺ or D⁺, is the +1 ion of deuterium, ²H or D.
3. Triton, having the symbol ³H⁺ or T⁺, is the +1 ion of tritium, ³H or T.

Other isotopes of hydrogen are too unstable to be relevant in chemistry.

History of the term

The term "hydron" is recommended by IUPAC to be used instead of "proton" if no distinction is made between the isotopes proton, deuteron and triton, all found in naturally occurring undifferentiated isotope mixtures. The name "proton" refers to isotopically pure ¹H⁺.^[4] On the other hand, referring to the hydron as simply hydrogen ion is not recommended because hydrogen anions also exist.^[5]

The term "hydron" was defined by IUPAC in 1988.^[6][7] Traditionally, the term "proton" was^[2] and is^{[citation needed]} used in place of "hydron". The latter term is generally only used in the context where comparisons between the various isotopes of hydrogen is important (as in the kinetic isotope effect or hydrogen isotopic labeling). Otherwise, referring to hydrons as protons is still considered acceptable, for example in such terms as protonation, deprotonation, proton pump, or proton channel. The transfer of H⁺ in an acid-base reaction is usually referred to as proton transfer. Acid and bases are referred to as proton donors and acceptors correspondingly.

99.9844% of natural hydrons (hydrogen nuclei) are protons, and the remainder (about 156 per million in sea water) are deuterons (see deuterium), except for some very rare natural tritons (see tritium).

See also

• Deprotonation
• Dihydrogen cation
• Hydrogen ion cluster
• Solvated electron
• Superacid
• Trihydrogen cation

References

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