| 词条 | Magnesium carbonate |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 462096540 | Name = Magnesium carbonate | ImageFile=Magnesium carbonate.png | ImageSize=120px | ImageFile2=Uhličitan hořečnatý.PNG | OtherNames = Magnesite Barringtonite (dihydrate) Nesequehonite (trihydrate) Lansfordite (pentahydrate) |Section1={{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 10563 | ChEMBL_Ref = {{ebicite|changed|EBI}} | ChEMBL = 1200736 | InChI = 1/CH2O3.Mg/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2 | InChIKey = ZLNQQNXFFQJAID-NUQVWONBAU | ChEBI_Ref = {{ebicite|correct|EBI}} | ChEBI = 31793 | SMILES = [Mg+2].[O-]C([O-])=O | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/CH2O3.Mg/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = ZLNQQNXFFQJAID-UHFFFAOYSA-L | CASNo = 546-93-0 | CASNo_Comment = (anhydrous) | CASNo_Ref = {{cascite|correct|CAS}} | CASNo2_Ref = {{cascite|changed|??}} | CASNo2 = 13717-00-5 | CASNo2_Comment = (monohydrate) | CASNo3_Ref = {{cascite|changed|??}} | CASNo3 = 5145-48-2 | CASNo3_Comment = (dihydrate) | CASNo4_Ref = {{cascite|changed|??}} | CASNo4 = 14457-83-1 | CASNo4_Comment = (trihydrate) | CASNo5_Ref = {{cascite|changed|??}} | CASNo5 = 61042-72-6 | CASNo5_Comment = (pentahydrate) | PubChem = 11029 | RTECS = OM2470000 |Section2={{Chembox Properties | MolarMass = 84.3139 g/mol (anhydrous) | Formula = MgCO3 | Appearance = white solid hygroscopic | Odor = odorless | Density = 2.958 g/cm3 (anhydrous) 2.825 g/cm3 (dihydrate) 1.837 g/cm3 (trihydrate) 1.73 g/cm3 (pentahydrate) | Solubility = anhydrous: 0.0139 g/100ml (25 °C) 0.00603 g/100ml (100 °C)[1] | SolubilityProduct = 10−7.8[1] | SolubleOther = soluble in acid, aqueous CO2 insoluble in acetone, ammonia | MeltingPtC = 350 | MeltingPt_notes = decomposes (anhydrous) {{convert|165|C|F K}} (trihydrate) | RefractIndex = 1.717 (anhydrous) 1.458 (dihydrate) 1.412 (trihydrate) | MagSus = −32.4·10−6 cm3/mol }} |Section3={{Chembox Structure | Coordination = | CrystalStruct = Trigonal }} |Section5={{Chembox Thermochemistry | DeltaHf = -1113 kJ/mol[2] | Entropy = 65.7 J/mol·K[3][2] | DeltaGf = -1029.3 kJ/mol[3] | HeatCapacity = 75.6 J/mol·K[3] |Section6={{Chembox Pharmacology | ATCCode_prefix = A02 | ATCCode_suffix = AA01 | ATC_Supplemental = {{ATC|A06|AD01}} }} |Section7={{Chembox Hazards | ExternalSDS = ICSC 0969 | EUClass = | NFPA-H = 1 | NFPA-F = 0 | NFPA-R = 0 | NFPA-S = | RPhrases = | SPhrases = | FlashPt = Non-flammable | PEL = TWA 15 mg/m3 (total) TWA 5 mg/m3 (resp)[4] |Section8={{Chembox Related | OtherAnions = Magnesium bicarbonate | OtherCations = Beryllium carbonate Calcium carbonate Strontium carbonate Barium carbonate | OtherCompounds = Artinite Hydromagnesite Dypingite }}{{Expand German|topic=sci|date=December 2018}} Magnesium carbonate, MgCO3 (archaic name magnesia alba), is an inorganic salt that is a white solid. Several hydrated and basic forms of magnesium carbonate also exist as minerals. FormsThe most common magnesium carbonate forms are the anhydrous salt called magnesite (MgCO3) and the di, tri, and pentahydrates known as barringtonite (MgCO3·2 H2O), nesquehonite (MgCO3·3 H2O), and lansfordite (MgCO3·5 H2O), respectively.[9] Some basic forms such as artinite (MgCO3·Mg(OH)2·3 H2O), hydromagnesite (4 MgCO3·Mg(OH)2·4 H2O), and dypingite (4 MgCO3· Mg(OH)2·5 H2O) also occur as minerals. Magnesite consists of white trigonal crystals. The anhydrous salt is practically insoluble in water, acetone, and ammonia. All forms of magnesium carbonate react in acids. Magnesium carbonate crystallizes in the calcite structure where in Mg2+ is surrounded by six oxygen atoms. The dihydrate one has a triclinic structure, while the trihydrate has a monoclinic structure. References to 'light' and 'heavy' magnesium carbonates actually refer to the magnesium hydroxy carbonates hydromagnesite and dypingite (respectively).[5] PreparationMagnesium carbonate is ordinarily obtained by mining the mineral magnesite. Seventy percent of the world's supply is mined and prepared in China.[6] Magnesium carbonate can be prepared in laboratory by reaction between any soluble magnesium salt and sodium bicarbonate: MgCl2(aq) + 2NaHCO3(aq) → MgCO3(s) + 2NaCl(aq) + H2O(l) + CO2(g) If magnesium chloride (or sulfate) is treated with aqueous sodium carbonate, a precipitate of basic magnesium carbonate—a hydrated complex of magnesium carbonate and magnesium hydroxide—rather than magnesium carbonate itself is formed: 5MgCl2(aq) + 5Na2CO3(aq) + 5H2O(l) → Mg(OH)2·3MgCO3·3H2O(s) + Mg(HCO3)2(aq) + 10NaCl(aq) High purity industrial routes include a path through magnesium bicarbonate, which can be formed by combining a slurry of magnesium hydroxide and carbon dioxide at high pressure and moderate temperature.[7] The bicarbonate is then vacuum dried, causing it to lose carbon dioxide and a molecule of water: Mg(OH)2 + 2 CO2 → Mg(HCO3)2 Mg(HCO3)2 → MgCO3 + CO2 + H2O ReactionsWith acidsLike many common group 2 metal carbonates, magnesium carbonate reacts with aqueous acids to release carbon dioxide and water: MgCO3 + 2 HCl → MgCl2 + CO2 + H2O MgCO3 + H2SO4 → MgSO4 + CO2 + H2O DecompositionAt high temperatures MgCO3 decomposes to magnesium oxide and carbon dioxide. This process is important in the production of magnesium oxide.[7] This process is called calcining: MgCO3 → MgO + CO2 (ΔH = +118 kJ/mol) The decomposition temperature is given as 350 °C (662 °F).[8][9] However, calcination to the oxide is generally not considered complete below 900 °C due to interfering readsorption of liberated carbon dioxide. The hydrates of the salts lose water at different temperatures during decomposition.[10] For example in the trihydrate, which molecular formula may be written as Mg(HCO3)(OH)•2(H2O), the dehydration steps occur at 157 °C and 179 °C as follows:[11] Mg(HCO3)(OH)•2(H2O) → Mg(HCO3)(OH)•(H2O) + H2O at 157 °C Mg(HCO3)(OH)•(H2O) → Mg(HCO3)(OH) + H2O at 179 °C UsesThe primary use of magnesium carbonate is the production of magnesium oxide by calcining. Magnesite and dolomite minerals are used to produce refractory bricks.[7] MgCO3 is also used in flooring, fireproofing, fire extinguishing compositions, cosmetics, dusting powder, and toothpaste. Other applications are as filler material, smoke suppressant in plastics, a reinforcing agent in neoprene rubber, a drying agent, a laxative to loosen the bowels, and colour retention in foods. In addition, high purity magnesium carbonate is used as antacid and as an additive in table salt to keep it free flowing. Magnesium carbonate can do this because it doesn't dissolve in water, only acid, where it will effervesce (bubble).[12] Because of its low solubility in water and hygroscopic properties, MgCO3 was first added to salt in 1911 to make it flow more freely. The Morton Salt company adopted the slogan "When it rains it pours" with reference to the fact that its MgCO3-containing salt would not stick together in humid weather.[13] Magnesium carbonate, most often referred to as 'chalk', is also used as a drying agent on athletes' palms in rock climbing, gymnastics and weight lifting. As a food additive magnesium carbonate is known as E504, for which the only known side effect is that it may work as a laxative in high concentrations.[14] Magnesium carbonate is also used in taxidermy for whitening skulls. It can be mixed with hydrogen peroxide to create a paste, which is then spread on the skull to give it a white finish. As a matte white coating for projection screens.[15] SafetyMagnesium carbonate is non-toxic. Compendial status
See also
Notes and references1. ^{{cite journal |first1= Pascale |last1= Bénézeth |first2= Giuseppe D. |last2= Saldi |first3= Jean-Louis |last3= Dandurand |first4= Jacques |last4= Schott |title= Experimental determination of the solubility product of magnesite at 50 to 200 °C |journal= Chemical Geology |volume= 286 |issue=1–2 |year= 2011 |pages= 21–31 |doi= 10.1016/j.chemgeo.2011.04.016 }} 2. ^1 {{cite book| author = Zumdahl, Steven S.|title =Chemical Principles 6th Ed.| publisher = Houghton Mifflin Company| year = 2009| isbn = 0-618-94690-X|page=A22}} 3. ^1 2 3 http://chemister.ru/Database/properties-en.php?dbid=1&id=634 4. ^{{PGCH|0373}} 5. ^{{cite journal|doi=10.1016/S0304-386X(01)00197-9|title=Preparation of a magnesium hydroxy carbonate from magnesium hydroxide | year=2001 | last1=Botha | first1=A. | last2=Strydom | first2=C.A. | journal=Hydrometallurgy | volume=62 | issue=3 | pages=175}} 6. ^{{cite web |title=The Hidden Environmental Cost of Climbing Chalk |url=https://www.climbing.com/gear/the-hidden-environmental-cost-of-climbing-chalk/ |last=Allf |first=Bradley |date=2018-05-21 |website=Climbing Magazine |publisher=Cruz Bay Publishing |access-date=2018-05-22 |quote=In fact, China produces 70 percent of the world’s magnesite. Most of that production—both mining and processing—is concentrated in a small corner of Liaoning, a hilly industrial province in northeast China between Beijing and North Korea.}} 7. ^1 2 3 {{Ullmann | title = Magnesium Compounds | author1 = Margarete Seeger | author2 = Walter Otto | author3 = Wilhelm Flick | author4 = Friedrich Bickelhaupt | author5 = Otto S. Akkerman | doi = 10.1002/14356007.a15_595.pub2}} 8. ^{{cite web|url=http://avogadro.chem.iastate.edu/MSDS/MgCO3_anhydrous.htm|title=IAState MSDS}} 9. ^{{cite book |author= Weast, Robert C.|title=CRC Handbook of Chemistry and Physics |edition=59th |year=1978 |publisher=CRC Press |location=West Palm Beach, FL |id={{Listed Invalid ISBN|0-8493-0549-8}}|page=B-133 |display-authors=etal}} 10. ^{{cite web|url=http://core.kmi.open.ac.uk/download/pdf/10883918.pdf|title=Conventional and Controlled Rate Thermal analysis of nesquehonite Mg(HCO3)(OH)·2(H2O)}} 11. ^{{cite web|url=http://core.kmi.open.ac.uk/download/pdf/10883918.pdf|title=Conventional and Controlled Rate Thermal analysis of nesquehonite Mg(HCO3)(OH)•2(H2O)}} 12. ^{{Cite web|url=https://sciencing.com/magnesium-carbonate-5626269.html|title=What Is Magnesium Carbonate?|website=Sciencing|language=en|access-date=2018-04-15}} 13. ^{{cite web |title=Her Debut - Morton Salt |url=http://www.mortonsalt.com/heritage-era/her-first-appearance/ |accessdate = 2017-12-27 }} 14. ^{{cite web|title=Food-Info.net : E-numbers : E504: Magnesium carbonates|url=http://www.food-info.net/uk/e/e504.htm}} 080419 food-info.net 15. ^{{Cite book|title = Certified Technology Specialist-Installation|last = Noronha|first = Shonan|publisher = McGraw Hill Education|year = 2015|isbn = 978-0071835657|location = |pages = 256}} 16. ^{{cite web |last=British Pharmacopoeia Commission Secretariat |title=Index, BP 2009 |year=2009 |url=http://www.pharmacopoeia.co.uk/pdf/2009_index.pdf |accessdate=31 January 2010 |deadurl=yes |archiveurl=https://web.archive.org/web/20090411071437/http://www.pharmacopoeia.co.uk/pdf/2009_index.pdf |archivedate=11 April 2009 |df= }} 17. ^{{cite web |title=Japanese Pharmacopoeia, Fifteenth Edition |year=2006 |url=http://jpdb.nihs.go.jp/jp15e/JP15.pdf |accessdate=31 January 2010 |deadurl=yes |archiveurl=https://web.archive.org/web/20110722105441/http://jpdb.nihs.go.jp/jp15e/JP15.pdf |archivedate=22 July 2011 |df= }} External links{{commons category|Magnesium carbonate}}
3 : Magnesium compounds|Carbonates|Antacids |
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