:Oxocarbon anion

File:Carbonate-3D-vdW.png

The carbonate ion has a trigonal planar structure, point group D_3h. The three C-O bonds have the same length of 136 pm and the 3 O-C-O angles are 120°. The carbon atom has 4 pairs of valence electrons, which shows that the molecule obeys the octet rule. This is one factor that contributes to the high stability of the ion, which occurs in rocks such as limestone. The electronic structure is described by two main theories which are used to show how the 4 electron pairs are distributed in a molecule that only has 3 C-O bonds.

With valence bond theory the electronic structure of the carbonate ion is a resonance hybrid of 3 canonical forms.

:400pxFile:Carbonate-ion-delocalised-partial-charges-2D.png

In each canonical form there are two single bonds one double bond. The three canonical forms contribute equally to the resonance hybrid, so the three bond C-O bonds have the same length.

File:Pi-Bond.svg

With molecular orbital theory the 3-fold axis is designated as the z axis of the molecule. Three σ bonds are formed overlap of the s, p_x and p_y orbitals on the carbon atom with a p orbital on each oxygen atom. In addition, a delocalized π bond is made by overlap of the p_z orbital on the carbon atom with the p_z orbital on each oxygen atom which is perpendicular to the plane of the molecule.

Note that the same bonding schemes may be applied the nitrate ion, NO₃⁻, which is isoelectronic with the carbonate ion.

Similarly, the two-fold symmetrical structure of a carboxylate group,{{chem|CO|2|–}}, may be described as a resonance hybrid of two canonical forms in valence bond theory, or with 2 σ bonds and a delocalized π bond in molecular orbital theory.

An oxocarbon anion {{chem|C|x|O|y|n−}} can be seen as the result of removing all protons from a corresponding acid C_xH_nO_y. Carbonate {{chem|CO|3|2−}}, for example, can be seen as the anion of carbonic acid H₂CO₃. Sometimes the "acid" is actually an alcohol or other species; this is the case, for example, of acetylenediolate {{chem|C|2|O|2|2−}} that would yield acetylenediol C₂H₂O₂. However, the anion is often more stable than the acid (as is the case for carbonate);[http://adsabs.harvard.edu/abs/1991AcS....47..255M "Infrared and mass spectral studies of proton irradiated H₂O + CO₂ ice: evidence for carbonic acid"], by Moore, M. H.; Khanna, R. K. and sometimes the acid is unknown or is expected to be extremely unstable (as is the case of methanetetracarboxylate C(COO⁻)₄).

Every oxocarbon anion {{chem|C|x|O|y|n−}} can be matched in principle to the electrically neutral (or oxidized) variant C_xO_y, an oxocarbon (oxide of carbon) with the same composition and structure except for the negative charge. As a rule, however, these neutral oxocarbons are less stable than the corresponding anions. Thus, for example, the stable carbonate anion corresponds to the extremely unstable neutral carbon trioxide CO₃;

{{cite journal

| title = Formation of carbon trioxide in the photolysis of ozone in liquid carbon dioxide

|author1=DeMore W. B. |author2=Jacobsen C. W. | pages = 2935–2938

| doi = 10.1021/j100843a026

| year = 1969

| volume =73

| issue =9

| journal =Journal of Physical Chemistry}}

oxalate {{chem|C|2|O|4|2−}} correspond to the even less stable 1,2-dioxetanedione C₂O₄;

{{cite journal |author1=Herman F. Cordes |author2=Herbert P. Richter |author3=Carl A. Heller | year = 1969 | title = Mass spectrometric evidence for the existence of 1,2-dioxetanedione (carbon dioxide dimer). Chemiluminescent intermediate | journal = J. Am. Chem. Soc. | volume = 91 | issue = 25 | pages = 7209 | doi = 10.1021/ja01053a065}}

and the stable croconate anion {{chem|C|5|O|5|2−}} corresponds to the neutral cyclopentanepentone C₅O₅, which has been detected only in trace amounts.

{{cite journal

| title = Mass spectrometric studies of the oxocarbons C_nO_n (n = 3–6)

| last1=Schröder|first1=Detlef|last2=Schwarz|first2=Helmut|last3=Dua|first3=Suresh|last4=Blanksby|first4=Stephen J.|last5=Bowie|first5=John H.

| doi = 10.1016/S1387-3806(98)14208-2

| journal = International Journal of Mass Spectrometry

| volume = 188

| issue = 1–2

|date=May 1999

| pages = 17–25

|bibcode=1999IJMSp.188...17S}}

Conversely, some oxocarbon anions can be reduced to yield other anions with the same structural formula but greater negative charge. Thus rhodizonate {{chem|C|6|O|6|2−}} can be reduced to the tetrahydroxybenzoquinone (THBQ) anion {{chem|C|6|O|6|4−}} and then to benzenehexolate {{chem|C|6|O|6|6−}}.

Haiyan Chen, Michel Armand, Matthieu Courty, Meng Jiang, Clare P. Grey, Franck Dolhem, Jean-Marie Tarascon, and Philippe Poizot (2009), "Lithium Salt of Tetrahydroxybenzoquinone: Toward the Development of a Sustainable Li-Ion Battery" J. Am. Chem. Soc., 131(25), pp. 8984–8988 {{doi|10.1021/ja9024897}}

An oxocarbon anion {{chem|C|x|O|y|n−}} can also be associated with the anhydride of the corresponding acid. The latter would be another oxocarbon with formula C_xO_{y−{{frac|n|2}}}; namely, the acid minus {{frac|n|2}} water molecules H₂O. The standard example is the connection between carbonate {{chem|CO|3|2−}} and carbon dioxide CO₂. The correspondence is not always well-defined since there may be several ways of performing this formal dehydration, including joining two or more anions to make an oligomer or polymer. Unlike neutralization, this formal dehydration sometimes yields fairly stable oxocarbons, such as mellitic anhydride C₁₂O₉ from mellitate {{chem|C|12|O|12|6−}} via mellitic acid C₁₂H₆O₁₂

J. Liebig, F. Wöhler (1830), "Ueber die Zusammensetzung der Honigsteinsäure" Poggendorfs Annalen der Physik und Chemie, vol. 94, Issue 2, pp.161–164. [https://books.google.com/books?id=ZyUAAAAAMAAJ&pg=PA161 Online version] accessed on 2009-07-08.

{{cite journal

|vauthors=Meyer H, Steiner K | year = 1913

| title = Über ein neues Kohlenoxyd C₁₂O₉ (A new carbon oxide C₁₂O₉)

| journal = Berichte der Deutschen Chemischen Gesellschaft

| volume = 46

| pages = 813–815

| doi=10.1002/cber.191304601105

| url = https://zenodo.org/record/1426491

}}

{{cite journal

| doi = 10.1002/cber.191304601105

|author1=Hans Meyer |author2=Karl Steiner | year = 1913

| title = Über ein neues Kohlenoxyd C₁₂O₉

| journal = Berichte der Deutschen Chemischen Gesellschaft

| volume = 46

| pages = 813–815

|url=https://zenodo.org/record/1426491 }}

For each oxocarbon anion {{chem|C|x|O|y|n−}} there are in principle n−1 partially hydrogenated anions with formulas {{chem|H|k|C|x|O|y|(n−k)−}}, where k ranges from 1 to n−1. These anions are generally indicated by the prefixes "hydrogen"-, "dihydrogen"-, "trihydrogen"-, etc. Some of them, however, have special names: hydrogencarbonate {{chem|HCO|3|-}} is commonly called bicarbonate, and hydrogenoxalate {{chem|HC|2|O|4|-}} is known as binoxalate.

The hydrogenated anions may be stable even if the fully protonated acid is not (as is the case of bicarbonate).

Here is an incomplete list of the known or conjectured oxocarbon anions

Several other oxocarbon anions have been detected in trace amounts, such as {{chem|C|6|O|6|-}}, a singly ionized version of rhodizonate.

Richard B. Wyrwas and Caroline Chick Jarrold (2006), "Production of {{chem|C|6|O|6|-}} from Oligomerization of CO on Molybdenum Anions". J. Am. Chem. Soc. volume 128 issue 42, pages 13688–13689. {{doi|10.1021/ja0643927}}

• Oxocarbon
• Silicate
• Sodium percarbonate (actually a carbonate perhydrate)

{{reflist}}

Category:Carbon oxyanions

Category:Oxocarbons