Carbonate facts for kids
Quick facts for kids Carbonate |
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Preferred IUPAC name
Carbonate
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Trioxidocarbonate
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| Identifiers | |
| CAS number | |
| PubChem | |
| SMILES | C(=O)([O-])[O-] |
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InChI
InChI=1/CH2O3/c2-1(3)4/h(H2,2,3,4)/p-2
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| Properties | |
| Molecular formula | |
| Molar mass | 0 g mol-1 |
| Conjugate acid | Bicarbonate |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
A carbonate is a salt of carbonic acid, (H
2CO
3), characterized by the presence of the carbonate ion, a polyatomic ion with the formula CO2−
3. The word "carbonate" may also refer to a carbonate ester, an organic compound containing the carbonate group O=C(–O–)
2.
The term is also used as a verb, to describe carbonation: the process of raising the concentrations of carbonate and bicarbonate ions in water to produce carbonated water and other carbonated beverages – either by the addition of carbon dioxide gas under pressure or by dissolving carbonate or bicarbonate salts into the water.
In geology and mineralogy, the term "carbonate" can refer both to carbonate minerals and carbonate rock (which is made of chiefly carbonate minerals), and both are dominated by the carbonate ion, CO2−
3. Carbonate minerals are extremely varied and ubiquitous in chemically precipitated sedimentary rock. The most common are calcite or calcium carbonate, CaCO
3, the chief constituent of limestone (as well as the main component of mollusc shells and coral skeletons); dolomite, a calcium-magnesium carbonate CaMg(CO
3)
2; and siderite, or iron(II) carbonate, FeCO
3, an important iron ore. Sodium carbonate ("soda" or "natron"), Na
2CO
3, and potassium carbonate ("potash"), K
2CO
3, have been used since antiquity for cleaning and preservation, as well as for the manufacture of glass. Carbonates are widely used in industry, such as in iron smelting, as a raw material for Portland cement and lime manufacture, in the composition of ceramic glazes, and more. New applications of alkali metal carbonates include: thermal energy storage, catalysis and electrolyte both in fuel cell technology as well as in electrosynthesis of H
2O
2 in aqueous media.
Contents
Structure and bonding
The carbonate ion is the simplest oxocarbon anion. It consists of one carbon atom surrounded by three oxygen atoms, in a trigonal planar arrangement, with D3h molecular symmetry. It has a molecular mass of 60.01 g/mol and carries a total formal charge of −2. It is the conjugate base of the hydrogencarbonate (bicarbonate) ion, HCO−
3, which is the conjugate base of H
2CO
3, carbonic acid.
The Lewis structure of the carbonate ion has two (long) single bonds to negative oxygen atoms, and one short double bond to a neutral oxygen atom.
This structure is incompatible with the observed symmetry of the ion, which implies that the three bonds are the same length and that the three oxygen atoms are equivalent. As in the case of the isoelectronic nitrate ion, the symmetry can be achieved by a resonance among three structures:
This resonance can be summarized by a model with fractional bonds and delocalized charges:
Chemical properties
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Metal carbonates generally decompose on heating, liberating carbon dioxide leaving behind an oxide of the metal. This process is called calcination, after calx, the Latin name of quicklime or calcium oxide, CaO, which is obtained by roasting limestone in a lime kiln:
- CaCO
3 → CaO + CO
2
As illustrated by its affinity for Ca2+, carbonate is a ligand for many metal cations. Transition metal carbonate and bicarbonate complexes feature metal ions covalently bonded to carbonate in a variety of bonding modes.
Lithium, sodium, potassium, rubidium, caesium, and ammonium carbonates are water-soluble salts, but carbonates of 2+ and 3+ ions are often poorly soluble in water. Of the insoluble metal carbonates, CaCO
3 is important because, in the form of scale, it accumulates in and impedes flow through pipes. Hard water is rich in this material, giving rise to the need for infrastructural water softening.
Acidification of carbonates generally liberates carbon dioxide:
- CaCO
3 + 2 HCl → CaCl
2 + CO
2 + H
2O
Thus, scale can be removed with acid.
In solution the equilibrium between carbonate, bicarbonate, carbon dioxide and carbonic acid is sensitive to pH, temperature, and pressure. Although di- and trivalent carbonates have low solubility, bicarbonate salts are far more soluble. This difference is related to the disparate lattice energies of solids composed of mono- vs dianions, as well as mono- vs dications.
In aqueous solution, carbonate, bicarbonate, carbon dioxide, and carbonic acid participate in a dynamic equilibrium. In strongly basic conditions, the carbonate ion predominates, while in weakly basic conditions, the bicarbonate ion is prevalent. In more acid conditions, aqueous carbon dioxide, CO
2(aq), is the main form, which, with water, H
2O, is in equilibrium with carbonic acid – the equilibrium lies strongly towards carbon dioxide. Thus sodium carbonate is basic, sodium bicarbonate is weakly basic, while carbon dioxide itself is a weak acid.
Organic carbonates
In organic chemistry a carbonate can also refer to a functional group within a larger molecule that contains a carbon atom bound to three oxygen atoms, one of which is double bonded. These compounds are also known as organocarbonates or carbonate esters, and have the general formula R–O–C(=O)–O–R′, or RR′CO
3. Important organocarbonates include dimethyl carbonate, the cyclic compounds ethylene carbonate and propylene carbonate, and the phosgene replacement, triphosgene.
Buffer
Three reversible reactions control the pH balance of blood and act as a buffer to stabilise it in the range 7.37–7.43:
- H+
+ HCO−
3 ⇌ H
2CO
3 - H
2CO
3 ⇌ CO
2(aq) + H
2O - CO
2(aq) ⇌ CO
2(g)
Exhaled CO
2(g) depletes CO
2(aq), which in turn consumes H
2CO
3, causing the equilibrium of the first reaction to try to restore the level of carbonic acid by reacting bicarbonate with a hydrogen ion, an example of Le Châtelier's principle. The result is to make the blood more alkaline (raise pH). By the same principle, when the pH is too high, the kidneys excrete bicarbonate (HCO−
3) into urine as urea via the urea cycle (or Krebs–Henseleit ornithine cycle). By removing the bicarbonate, more H+
is generated from carbonic acid (H
2CO
3), which comes from CO
2(g) produced by cellular respiration.
Crucially, a similar buffer operates in the oceans. It is a major factor in climate change and the long-term carbon cycle, due to the large number of marine organisms (especially coral) which are made of calcium carbonate. Increased solubility of carbonate through increased temperatures results in lower production of marine calcite and increased concentration of atmospheric carbon dioxide. This, in turn, increases Earth temperature. The amount of CO2−
3 available is on a geological scale and substantial quantities may eventually be redissolved into the sea and released to the atmosphere, increasing CO
2 levels even more.
Presence outside Earth
It is generally thought that the presence of carbonates in rock is strong evidence for the presence of liquid water. Recent observations of the planetary nebula NGC 6302 show evidence for carbonates in space, where aqueous alteration similar to that on Earth is unlikely. Other minerals have been proposed which would fit the observations.
Small amounts of carbonate deposits have been found on Mars via spectral imaging and Martian meteorites also contain small amounts. Groundwater may have existed at Gusev and Meridiani Planum.
Related pages
- Bicarbonate
- Calcium carbonate
- Polycarbonate
- Sodium carbonate
- Cap carbonates
- Orthocarbonic acid, H
4CO
4, or C(OH)
4, a hypothetic unstable molecule - Oxalate
- Peroxocarbonate
- Sodium percarbonate
See also
In Spanish: Carbonato para niños
