In chemistry, phosphorus oxoacid (or phosphorus acid) is a generic name for any acid whose molecule consists of atoms of phosphorus, oxygen, and hydrogen.[1] There is a potentially infinite number of such compounds. Some of them are unstable and have not been isolated, but the derived anions and organic groups are present in stable salts and esters. The most important ones—in biology, geology, industry, and chemical research—are the phosphoric acids, whose esters and salts are the phosphates.

In general, any hydrogen atom bonded to an oxygen atom is acidic, meaning that the –OH group can lose a proton H+
 leaving a negatively charged –O−
 group and thus turning the acid into a phosphorus oxoanion. Each additional proton lost has an associated acid dissociation constant Ka1, Ka2 Ka3, ..., often expressed by its cologarithm (pKa1, pKa2, pKa3, ...). Hydrogen atoms bonded directly to phosphorus are generally not acidic.

Classification

The phosphorus oxoacids can be classified by the oxidation state(s) of the phosphorus atom(s), which may vary from +1 to +5. The oxygen atoms are usually in oxidation state -2, but may be in state -1 if the molecule includes peroxide groups.

Oxidation state +1

Hypophosphorous acid

Oxidation state +3

Phosphorous acid

Oxidation state +4

Hypophosphoric acid
  • Hypophosphoric acid, H
    4    P
    2    O
    6     (or (HO)
    2    P    –P(OH)
    2    ). All four hydrogens are acidic. Its salts and esters are hypophosphates.

Oxidation state +5

The most important members of this group are the phosphoric acids, where each phosphorus atom bonded to four oxygen atoms, one of them through a double bond, arranged as the corners of a tetrahedron. Two or more of these PO
4 tetrahedra may be connected by shared single-bonded oxygens, forming linear or branched chains, cycles, or more complex structures. The single-bonded oxygen atoms that are not shared are completed with acidic hydrogen atoms. Their generic formula is Hn−x+2PnO3n−x+1, where n is the number of phosphorus atoms and x is the number of fundamental cycles in the molecule's structure.

These acids, and their esters and salts ("phosphates") include some of the best-known and most important compounds of phosphorus.

Orthophosphoric acid, H
3PO
4.

The simplest member of this class is:

  • Phosphoric acid proper (also called orthophosphoric acid or monophosphoric acid), H
    3    PO
    4     (or OP(OH)
    3    ), a triprotic acid. It forms orthophosphate salt and esters, commonly called phosphates.

The smallest compounds of this class with two or more phosphorus atoms are called "oligophosphoric acids", and the larger ones, with linear –P–O– backbones, are "polyphosphoric acids"; with no definite separation between the two. Some of the most important members are:

  • Pyrophosphoric acid, H
    4    P
    2    O
    7     (or (HO)
    2    P    –O–P(OH)
    2    ), with four acid hydrogens. Forms pyrophosphates.
  • Triphosphoric acid (or tripolyphosphoric acid), H
    5    P
    3    O
    10     (or (HO)
    2    P    –O–P(OH)–O–P(OH)
    2    ), with five acidic hydrogens. Forms triphosphates or tripolyphosphates.
  • Tetraphosphoric acid, H
    6    P
    4    O
    13     (or (HO)
    2    P    (–O–P(OH))2–O–P(OH)
    2    ), with six acidic hydrogens. Forms tetraphosphates.

The backbone may be branched, as in:

  • Triphosphono phosphoric acid, H
    6    P
    4    O
    13     or P(O)(–OP(O)(OH)
    2    )3, a branched isomer of tetrapolyphosphoric acid.

The PO
4 tetrahedra may be connected to form closed –P–O– chains, as in:

  • Trimetaphosphoric acid (or cyclotriphosphoric acid), H
    3    P
    3    O
    9     (or (HPO
    3    )
    3    , (–P(O)(OH)–O–)3), a cyclic molecule with three acidic hydrogens. Forms the trimetaphosphate salts and esters.

Metaphosphoric acid is a general term for phosphoric acids with a single cycle, (–P(O)(OH)–O–)n, whose elemental formula is HPO
3.

Another compound that may be included in this class is

Mixed oxidation states

Some phosphorus oxoacids have two or more P atoms in different oxidation states. One example is

  • Isohypophosphoric acid, H
    4    P
    2    O
    6     (or H(OH)(O)P−O−P(O)(OH)2), a tetraprotic acid and isomer of hypophosphoric acid, containing P in oxidation state +3 and +5
Phosphoric anhydride
P4O10
Some phosphoric acids

See also

References

  1. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.

Further reading

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