Carbonate rocks are sedimentary rocks consisting of carbonate minerals. The most common carbonates in these rocks are the polymorphs of calcium carbonate CaCO3, calcite and aragonite, and calcium magnesium carbonate CaMg(CO3)2, dolomite. A carbonate rock consisting of calcium carbonate is a limestone, whereas one consisting predominantly of dolomite is a dolostone. Another common carbonate rock, containing a mixture of fine-grained calcite and terrigenous mud, is marl. Carbonate rocks are the second most common sedimentary rocks on Earth after siliciclastic rocks and are produced by the accumulation of fossils, the activity of organisms, and other inorganic processes – all involving dissolved carbonates and water.
Origin of carbonate sediments
Calcium carbonate occurs dissolved in seawater and fresh waters. Calcium derives from the weathering of Ca-bearing minerals in rocks, like plagioclase, and it is present in water as Ca2+ ions. Atmospheric CO2 dissolves in water producing H2CO3 (carbonic acid), a weak acid, following the reaction:
CO2(gas) + H2O(liquid) ⇌ H2CO3
H2CO3 dissociates in water as carbonate [CO32-] and bicarbonate [HCO3–] ions:
H2CO3 ⇌ H+ + HCO3–
HCO3– ⇌ H+ + CO32-
The precipitation of calcium carbonate [CaCO3] from water is, hence, balanced by the reaction:
Ca2+ + 2HCO3– ⇌ CaCO3 + H2CO3
The precipitation of dolomite [CaMg(CO3)2]from a water solution is controlled by a similar reaction. Magnesium is another common ion in water, which, like calcium, derives from the alteration of minerals like olivine:
Ca2+ + Mg2+ + 4HCO3– ⇌ CaMg(CO3)2 + 2H2CO3
The dissolution of calcite and dolomite is, hence, controlled by how acidic water is, or, in other words, how much atmospheric CO2 is dissolved in water: the more carbonic acid, the more aggressive water is to carbonates. CO2 is a gas, so its solubility in water is favored by low temperature (CO2 molecules move slower and are more easily dissolved in water), high pressure (promoting the dissolution of the gas phase to water), or simply because there is more atmospheric CO2 (which is why tropical carbonate reefs are struggling due to CO2 emissions). Consequently, the dissolution of carbonates is favored by low temperature, high pressure, or high amounts of CO2 dissolved in water. On the other hand, high temperatures, low pressures, or any process leading to a decrease of dissolved CO2 favor the precipitation of carbonates from water. In nature, the balance between dissolution and precipitation is controlled both by inorganic and organic processes. In particular, many marine life forms are responsible for the formation of the vast majority of carbonate rocks, since organisms either produce shells and other skeletal parts of carbonates or cause the precipitation of carbonate as a byproduct of their activities.
Organic precipitation of carbonates
Carbonates are common in seawater and marine organisms have learned to use calcium carbonate to produce shells and other skeletal parts. Invertebrates like bivalves, gastropods, cephalopods, brachiopods (“sea shells”), echinids (sea urchins), crinoids (sea lilies), asteroids, ophiurids (starfishes), anellids (segmented worms), and many other taxa produce hard parts of one or both polymorphs of calcium carbonate (calcite or aragonite), but most marine carbonates are produced by microorganisms with carbonate tests (nanoplankton), like foraminifera and coccolithophores. Reefs are constructions of carbonate rocks produced by reef-building organisms like corals, bryozoans, and cyanobacteria (stromatolites). Carbonate precipitation is favored in hot waters and, for this reason, reefs occur in tropical and subtropical seas nowadays. The details of how organisms manage to cause the precipitation of carbonates are not well understood, but they use a wide range of proteins capable of favoring the nucleation of calcite and aragonite crystals in specific orientations.
Carbonate sand with abundant fragments of corals, echinoids, molluscs, and pink foraminifera. Deposits of carbonate sand transform into carbonate rocks during burial and diagenesis. Field of view: 32 mm. Photo © Siim Sepp.
Photosynthetic organisms living in water use sunlight to convert dissolved CO2 to organic compounds, releasing oxygen (O2) in the process. The decrease of dissolved CO2 causes the precipitation of carbonates that end up encrusting photosynthetic organisms like algae, plants, and cyanobacteria. The progressive encrustation of colonies of cyanobacteria (microbial mats) produces layered limestone formations known as stromatolites and also rounded concretions known as oncolites. These organisms also trap carbonate particles coming from the surroundings as they grow.
Inorganic precipitation (and dissolution) of carbonates
The white sands of tropical beaches, like the Bahamas or the Maldives, consists of ooids, spherical concretions of calcium carbonate with a maximum diameter of 2 mm. In tropical areas, waters are commonly saturated with calcium carbonate. Ooids nucleate around a small core, which may consist of any small solid object, like the fragment of a shell or a quartz grain. When the nucleus of the ooid is transported by waves, the instantaneous drop in pressure causes the precipitation of calcium carbonate, typically in the form of aragonite which can hence recrystallize as calcite. The process is repeated by wave action, leading to the formation of several, concentric layers around the original core. When ooids are about 2 mm wide, waves are no longer able to transport them in suspension, and the process halts.
Pisoids are similar to ooids but are much bigger: they are concentric carbonate concretions that can reach several centimeters in diameter. Their formation is caused by periodic changes in the surface of groundwater saturated in calcium carbonate within a sediment. Each time the water table changes, it deposits a thin layer of calcium carbonate over the grains of a sediment. The process is seasonal and can continue forever, until the porosity of the sediment is eventually sutured by the growth of pisoids. Another ambient where pisoids form are caves, where concretion of carbonates can deposit on grains transported by water or on karst breccias.
Karst and caves
Karstic environments occur anywhere there are outcrops of carbonate rocks exposed on the surface and are a great example of how subtle the equilibrium between dissolution and precipitation of carbonates is at ambient conditions. Rainwater that falls on carbonates contains atmospheric CO2 that progressively attacks carbonate rocks. The dissolution of carbonates is a selective process which runs faster where water is stagnant, as in small pools, or where it can infiltrate rocks, as along fractures. The infiltration of aggressive water in fractured carbonates progressively enlarges the fractures, enhancing the infiltration of acidic waters at depth, ultimately leading to the formation of cave systems. Once water reaches caves, carbonate precipitation can occur, producing cave formations like stalactites and stalagmites. Stalactites and stalagmites form from water droplets dripping in the cave that release CO2 when they fall and when they hit the ground, due to the instantaneous drop in pressure, causing the precipitation of carbonate from water, droplet after droplet.
Travertines are carbonate rocks produced by the inorganic precipitation of carbonate from hot springs and fresh waters. Hot springs derive from deep waters that are released by geothermal systems (or from other sources) and may contain large amounts of dissolved CO2 (which may be released for example by cooling igneous intrusions). When these waters reach the atmosphere, they rapidly release most of the dissolved CO2 ,causing the rapid precipitation of carbonates from water. Travertine deposits encrust the surrounding rocks, soil, and can trap organisms and produce molds of fossils, commonly leaves.
Identification of carbonate rocks
Limestone is easily recognizable because it fizzes in contact with HCl (hydrochloric acid), due to the reaction:
CaCO3 + 2HCl ⇌ CO2 + H2O + CaCl2
Dolostone does not fizz on a 10% diluted HCl solution, but can fizz if the solution is put in contact with a dolomite powder or if a less diluted solution (around 30%) is used. Both dolostone and limestone can show karst features in the field, are weaker than metal on scratch, and produce conchoidal fractures. Alteration of dolostone can produce yellow to orange dust, since dolomite may contain some iron that alters as oxides and hydroxides (rust). Marl produces a reaction on HCl, whose intensity decreases at increasing amount of silicate mud mixed with calcite. Marls are easily recognizable because phyllosilicates (mud) remain as an insoluble residuum after reaction with HCl. Marls show the characteristic fissility of clay-bearing mudrocks.
- Limestone – Limestone is a carbonate sedimentary rock that consists predominantly of calcite [CaCO3]. Limestones are the commonest rocks that contain non-silicate minerals as primary components and, even if they represent only a fraction of all sedimentary rocks (about 20 – 25%), their study is fundamental to understand past environments, climate, and the evolution of life. Limestones also represent the primary reservoir… Read More »Limestone
- Dolostone – Dolostone, also known as dolomite (not to be confused with the mineral dolomite), is a type of carbonate sedimentary rock consisting predominantly of dolomite [CaMg(CO3)2] and to a lesser extent of other carbonates, like calcite and aragonite. Like the mineral, the name derives from the French mineralogist Déodat Gratet de Dolomieu, after whom also the Dolomites of Italy, where the… Read More »Dolostone
- Marl – Marls are sedimentary rocks with mixed composition, consisting in part of carbonate sediment (carbonate ooze) and in part of fine-grained siliciclastic sediment (clay and silt). The most abundant carbonate mineral in marls is calcite, even though dolomite and aragonite can also be present, whereas the silicate fraction consists of clay minerals and other detrital components, like quartz, feldspar, micas, etc.… Read More »Marl
Adams, A.E., & McKenzie, W.S. (1998). A color atlas of carbonate sediments and rocks under the microscope. Wiley, 1st edition.
Dunham, R. J. (1962). Classification of carbonate Rocks according to depositional texture. In: Ham, W. E. (ed.), Classification of carbonate Rocks: American Association of Petroleum Geologists Memoir, p. 108-121.
Flugel, E., & Flügel, E. (2004). Microfacies of carbonate rocks: analysis, interpretation and application. Springer Science & Business Media.
Folk, R.L. (1959). Practical petrographic classification of limestones: American Association of Petroleum Geologists Bulletin, v. 43, p. 1-38.
Folk, R.L. (1962). Spectral subdivision of limestone types, in Ham, W.E., ed., Classification of carbonate Rocks-A Symposium: American Association of Petroleum Geologists Memoir 1, p. 62-84.
James, N. P., & Jones, B. (2015). Origin of carbonate sedimentary rocks. John Wiley & Sons.
Murray, R. C. (1960). Origin of porosity in carbonate rocks. Journal of Sedimentary Research, 30(1), 59-84.
Scholle, P. A. & Ulmer-Scholle, D. S. (2003). A Color Guide to the Petrography of carbonate Rocks: AAPG Memoir 77, 474 p.
Scholle, P. A., Bebout, D. G., & Moore, C. H. (Eds.). (1983). Carbonate depositional environments: AAPG Memoir 33 (No. 33). AAPG.
Limestone – Sandatlas.org
Dolomite rock – Sandatlas.org
Tulane – Carbonate Rocks
Limestone Cycle – School Movie on Chemistry