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Article[edit]

Calcite

Original text[edit]

Calcite is transparent to opaque and may occasionally show phosphorescence or fluorescence. A transparent variety called "Iceland spar" is used for optical purposes.

Microbiologically precipitated calcite has a wide range of applications, such as soil remediation, soil stabilization and concrete repair.

Changes[edit]

Three references are added to the above parts. Reference one is a brief introduction to Icelandic spar.[1] The second reference describes how Microbiologically precipitated calcite stabilizes soil.[2] The third one is the influence of Microbiologically precipitated calcite on biological concrete.[3]These sources are reliable and come from the journal.

In addition, some sentences in the article are modified to make the whole sentence look more concise.


Add new content to the article(not published in the article yet)[edit]

Other uses of microbial precipitation calcite (MICP): MICP can be used for tailings management and is designed to promote sustainable development in the mining industry.[4]

Extended content[edit]

Properties

Distribution

Use and application

Climate change

Properties[edit]

Thermoluminescence

Calcite has thermoluminescent properties mainly due to manganese divalent (Mn2+).[5] An experiment was conducted by adding activators such as ions of Mn, Fe, Co, Ni, Cu, Zn, Ag, Pb, and Bi to the calcite samples to observe if they emitted heat or light. The results showed that adding ions (Cu+, Cu2+, Zn2+, Ag+, Bi3+, Fe2+, Fe3+, Co2+, Ni2+) did not react.[5] However, a reaction occurred when both manganese and lead ions were present in calcite.[5] By changing the temperature and observing the glow curve peaks, it was found that Pb2+ and Mn2+ acted as activators in the calcite lattice, but Pb2+ was much less efficient than Mn2+.[5]

Mineral thermoluminescence can form various glow curves of crystals under different conditions, such as temperature changes, because impurity ions or other crystal defects present in minerals supply luminescence centers and trapping levels.[5] Observing these curve changes also can help infer geological correlation and age determination. [5]

Distribution[edit]

Calcite is found all over the world, and its leading global distribution is as follows:

The United States

Calcite Quarry, Michigan.

Calcite is found in many different areas in the United States. One of the best examples is the Calcite Quarry in Michigan.[6] The Calcite Quarry is the largest carbonate mine in the world and has been in use for more than 85 years.[6] Large quantities of calcite can be mined from these sizeable open pit mines.

Canada

Calcite can also be found throughout Canada, such as in Thorold Quarry and Madawaska Mine, Ontario, Canada. [7]

Mexico

Abundant calcite is mined in the Santa Eulalia mining district, Chihuahua, Mexico.[8]

Iceland

Large quantities of calcite in Iceland are concentrated in the Helgustadir mine.[9] The mine was once the primary mining location of "Iceland spar".[10] However, it currently serves as a nature reserve, and calcite mining will not be allowed.[10]

England

Calcite is found in parts of England, such as Alston Moor, Egremont, and Frizington, Cumbria. [9]

Germany

St. Andreasberg, Harz Mountains, and Freiberg, Saxony can find calcite. [9]

Use and application[edit]

Microbiologically precipitated calcite also can be used for tailings management and is designed to promote sustainable development in the mining industry. [11]

Calcite can help synthesize precipitated calcium carbonate (PCC) (mainly used in the paper industry) and increase carbonation.[12] Furthermore, due to its particular crystal habit, such as rhombohedron, hexagonal prism, etc., it promotes the production of PCC with specific shapes and particle sizes.[12]

Calcite can be formed naturally or synthesized. However, artificial calcite is the preferred material to be used as a scaffold in bone tissue engineering due to its controllable and repeatable properties.[13]

Calcite can be used to alleviate water pollution caused by the excessive growth of cyanobacteria. Lakes and rivers can lead to cyanobacteria blooms due to eutrophication, which pollutes water resources.[14] Phosphorus (P) is the leading cause of excessive growth of cyanobacteria.[14] As an active capping material, calcite can help reduce P release from sediments into the water, thus inhibiting cyanobacteria overgrowth.[14]

Climate change[edit]

Ocean acidification reduces pH, which affects calcification in shelled organisms.

Climate change is exacerbating ocean acidification, which may lead to lower natural calcite production. The oceans absorb large amounts of CO2 from fossil fuels emission into the air.[15] The total amount of artificial CO2 absorbed by the oceans is calculated to be 118 ± 19 Gt C.[16] If a large amount of CO2 dissolves in the sea, it will cause the acidity of the seawater to increase, thereby affecting the pH value of the ocean.[15] Calcifying organisms in the sea, such as molluscs foraminifera, crustaceans, echinoderms and corals, are susceptible to pH changes.[15] Meanwhile, these calcifying organisms are also an essential source of calcite. As ocean acidification causes pH to drop, carbonate ion concentrations will decline, potentially reducing natural calcite production.[15]

Reference[edit]

  1. ^ Harstad, A. O.; Stipp, S. L. S. (2007). "Calcite dissolution; effects of trace cations naturally present in Iceland spar calcites". Geochimica et Cosmochimica Acta. 71(1): 56–70.
  2. ^ Mujah, D.; Shahin, M. A.; Cheng, L. (2017). "State-of-the-Art Review of Biocementation by Microbially Induced Calcite Precipitation (MICP) for Soil Stabilization". Geomicrobiology Journal. 34(6): 524–537.
  3. ^ Castro-Alonso, M. J.; Montañez-Hernandez, L. E.; Sanchez-Muñoz, M. A.; Macias Franco, M. R.; Narayanasamy, R.; Balagurusamy, N. (2019). "Microbially induced calcium carbonate precipitation (MICP) and its potential in bioconcrete: microbiological and molecular concepts". Frontiers in Materials. 6: 126.
  4. ^ Zúñiga-Barra, H.; Toledo-Alarcón, J.; Torres-Aravena, Á.; Jorquera, L.; Rivas, M.; Gutiérrez, L.; Jeison, D. (2022). "Improving the sustainable management of mining tailings through microbially induced calcite precipitation: A review". Minerals Engineering. 189: 107855–.
  5. ^ a b c d e f Medlin, W. L. (1959). "Thermoluminescent properties of calcite". he Journal of Chemical Physics. 30(2): 451–458.
  6. ^ a b NASA. "Calcite Quarry, Michigan". Earth observatory. Retrieved 17 February 2023.
  7. ^ Hudson Institute of Mineralogy. "Calcite from Canada". mindat.org. Retrieved 17 February 2023.
  8. ^ Hudson Institute of Mineralogy. "Santa Eulalia Mining District, Aquiles Serdán Municipality, Chihuahua, Mexico". mindat.org. Retrieved 17 February 2023.
  9. ^ a b c AZoMining. "Calcite – occurrence, properties, and distribution". EDITORIAL FEATURE. Retrieved 17 February 2023.
  10. ^ a b Kristjansson, L. (2002). "Iceland Spar: The Helgustadir Calcite Locality and its Influence on the Development of Science". Journal of Geoscience Education. 50(4): 419-427.
  11. ^ Zúñiga-Barra, H.; Toledo-Alarcón, J.; Torres-Aravena, Á.; Jorquera, L.; Rivas, M.; Gutiérrez, L.; Jeison, D. (2022). "Improving the sustainable management of mining tailings through microbially induced calcite precipitation: A review". Minerals Engineering. 189: 107855–.
  12. ^ a b Jimoh, O. A.; Ariffin, K. S.; Hussin, H. B.; Temitope, A. E. (2018). "Synthesis of precipitated calcium carbonate: a review". Carbonates and Evaporites. 33(2): 331–346.
  13. ^ Chróścicka, A.; Jaegermann, Z.; Wychowański, P.; Ratajska, A.; Sadło, J.; Hoser, G.; Michałowski, S.; Lewandowska-Szumiel, M. (2016). "Synthetic Calcite as a Scaffold for Osteoinductive Bone Substitutes". Annals of Biomedical Engineering. 44(7): 2145–2157.
  14. ^ a b c Han, M.; Wang, Y.; Zhan, Y.; Lin, J.; Bai, X.; Zhang,, Z. (2022). "Efficiency and mechanism for the control of phosphorus release from sediment by the combined use of hydrous ferric oxide, calcite and zeolite as a geo-engineering tool". Chemical Engineering Journal (Lausanne, Switzerland : 1996). 428: 131360–.{{cite journal}}: CS1 maint: extra punctuation (link)
  15. ^ a b c d Tyrrell, T. (2008). "Calcium carbonate cycling in future oceans and its influence on future climates". Journal of Plankton Research. 30(2): 141–156.
  16. ^ Sabine, C. L.; Feely, R. A; Gruber, N.; Key, R. M.; Lee, K.; Bullister, J. L; ...; Rios,, A. F. (2004). "The oceanic sink for anthropogenic CO2". science. 305(5682): 367-371. {{cite journal}}: |last7= has numeric name (help)CS1 maint: extra punctuation (link)
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