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Which best describes a compound such as magnesium oxide? an impure substance that is made up of two elements a mixture of two uncommon substances a mixture of two common elements a pure substance that is made up of different elementsWhen magnesium (Mg) metal is burned in the presence of oxygen (O2), magnesium oxide (MgO) is produced. The properties of magnesium oxide are different than the individual properties of magnesium and oxygen because magnesium oxide is? A. a solution B. a mixture C. a compound D. an element and when you find the answer please explain why it is that answer so i can understand the topic. thank you.Hate to break it to you, Jacllyn, but Magnesium oxide is only 4% absorbed by the body, and that's why it loosens bowels with lots of water. Some magnesium is absorbed long before it gets to the large intestine, and therefore has no diuretic effect-such as Magnesium Chloride.When the magnesium metal burns it reacts with oxygen found in the air to form Magnesium Oxide. A compound is a material in which atoms of different elements are bonded to one another. Oxygen and magnesium combine in a chemical reaction to form this compound. After it burns, it forms a white powder of the magnesium oxide.Magnesium is an element your body needs to function normally. Magnesium oxide may be used for different reasons. Some people use it as an antacid to relieve heartburn, sour stomach, or acid indigestion. Magnesium oxide also may be used as a laxative for short-term, rapid emptying of the bowel (before surgery, for example).

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Magnesium oxide is a solid at normal temperature and pressure. Don't ask why, it just is. It's a refractory, melting at 2850°C (5166°F) and vaporizing at 3600°C (6510°F). It's one of the most common refractories for high temperature processing like arc furnaces.Magnesium Oxide is the oxide salt of magnesium with antacid, laxative and vascular smooth muscle relaxant activities. Magnesium combines with water to form magnesium hydroxide which reacts chemically to neutralize or buffer existing quantities of stomach acid; stomach-content and intra-esophageal pH rise, resulting in a decrease in pepsin activity. This agent's laxative effect is the resultWhich best describes a compound such as magnesium oxide? A.)an impure substance that is made up of two elements . B.)a mixture of two uncommon substances . C.)a mixture of two common elements . D.)a pure substance that is made up of different elements. Answer Save. 3 Answers. Relevance. mohamad.When magnesium (Mg) metal is burned in the presence of oxygen gas (O 2), magnesium oxide (MgO) is produced. The properties of magnesium oxide are different from the individual properties of magnesium and oxygen because magnesium oxide is

Types of Magnesium: The Best and The Worst

Magnesium is a group 2 metal which exists as a number of isotopes and forms many compounds. In addition to magnesium oxide, magnesium forms another compound when burned in air. Suggest the formula of this compound Which term describes the role of sodium chloride... 13N.1.hl.TZ0.2:What is Magnesium Oxide? Magnesium oxide is a compound that occurs in nature but it can also be made by burning magnesium with oxygen. It has the highest amount of elemental magnesium by weight but it's not absorbed well by the body.Magnesium oxide is a compound that forms an ionic bond between the atoms of magnesium and those of oxygen. Magnesium oxide can be broken down chemically by a process called decomposition. It is largely ceramic in nature that fractures easily and is also a great insulator.magnesium oxide is a compound that is composed of one atom of magnesium and two atoms of oxygen. The compound is a combination of Mg2+ ion and O2-. The ions translate into atoms which reflects on the subscripst of the elements already. magnesium oxide is a basic oxide with the pH level greater than 7.…hydroxide produces the oxygen compound magnesium oxide, commonly called magnesia, MgO. It is a white solid used in the manufacture of high-temperature refractory bricks, electrical and thermal insulators, cements, fertilizer, rubber, and plastics. It is also used medically as a laxative and antacid.

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Magnesium oxide Names IUPAC title Magnesium oxide Other names MagnesiaPericlase Identifiers CAS Number 1309-48-4 ChEMBL ChEMBL1200572 ECHA InfoCard 100.013.793 EC Number 215-171-9 E quantity E530 (acidity regulators, ...) PubChem CID 14792 RTECS number OM3850000 UNII 3A3U0GI71G CompTox Dashboard (EPA) DTXSID9049665 Properties Chemical components MgO Molar mass 40.304 g/mol[1] Appearance White powder Odor Odorless Density 3.6 g/cm3[1]Melting point 2,852 °C (5,166 °F; 3,125 K)[1] Boiling level 3,600 °C (6,510 °F; 3,870 K)[1] Solubility Soluble in acid, ammonia insoluble in alcohol Band hole 7.Eight eV[2]Magnetic susceptibility (χ) −10.2·10−6 cm3/mol[3]Thermal conductivity 45–60 W·m−1·K−1[4]Refractive index (nD) 1.7355 Dipole second 6.2 ± 0.6 D Structure Crystal structure Halite (cubic), cF8 Space team Fm3m, No. 225 Lattice consistent a = 4.212Å Coordination geometry Octahedral (Mg2+); octahedral (O2−) Thermochemistry Heat capability (C) 37.2 J/mol Ok[5]Std molarentropy (So298) 26.95 ± 0.15 J·mol−1·Ok−1[6]Std enthalpy offormation (ΔfH⦵298) −601.6 ± 0.3 kJ·mol−1[6]Gibbs unfastened energy (ΔfG˚) -569.Three kJ/mol[5]Pharmacology ATC code A02AA02 (WHO) A06AD02 (WHO), A12CC10 (WHO) Hazards Main hazards Metal fume fever, Irritant Safety data sheet ICSC 0504 R-phrases (old-fashioned) R36, R37, R38 NFPA 704 (hearth diamond) 1 0 0 Flash level Non-flammable NIOSH (US health publicity limits): PEL (Permissible) TWA 15 mg/m3 (fume)[7]REL (Recommended) None designated[7]IDLH (Immediate danger) 750 mg/m3 (fume)[7]Related compounds Other anions Magnesium sulfide Other cations Beryllium oxideCalcium oxideStrontium oxideBarium oxide Related compounds Magnesium hydroxideMagnesium nitride Except where in a different way noted, information are given for fabrics of their usual state (at 25 °C [77 °F], 100 kPa). examine (what is ?) Infobox references

Magnesium oxide (MgO), or magnesia, is a white hygroscopic forged mineral that occurs naturally as periclase and is a supply of magnesium (see additionally oxide). It has an empirical components of MgO and consists of a lattice of Mg2+ ions and O2− ions held together by means of ionic bonding. Magnesium hydroxide forms in the presence of water (MgO + H2O → Mg(OH)2), however it may be reversed through heating it to remove moisture.

Magnesium oxide used to be historically known as magnesia alba (literally, the white mineral from Magnesia – different assets give magnesia alba as MgCO3), to differentiate it from magnesia negra, a black mineral containing what is referred to now as manganese.

While "magnesium oxide" usually refers to MgO, magnesium peroxide MgO2 is also known as a compound. According to evolutionary crystal structure prediction,[8] MgO2 is thermodynamically stable at pressures above 116 GPa (gigapascals), and a semiconducting suboxide Mg3O2 is thermodynamically strong above 500 GPa. Because of its steadiness, MgO is used as a style system for investigating vibrational houses of crystals.[9]

Production

Magnesium oxide is produced via the calcination of magnesium carbonate or magnesium hydroxide. The latter is acquired via the treatment of magnesium chloride answers, usually seawater, with limewater or milk of lime.[10]

Mg2+ + Ca(OH)2 → Mg(OH)2 + Ca2+

Calcining at other temperatures produces magnesium oxide of various reactivity. High temperatures 1500 – 2000 °C diminish the available floor area and produces dead-burned (often called dead burnt) magnesia, an unreactive shape used as a refractory. Calcining temperatures 1000 – 1500 °C produce hard-burned magnesia, which has limited reactivity and calcining at decrease temperature, (700–1000 °C) produces light-burned magnesia, a reactive shape, also recognized as caustic calcined magnesia. Although some decomposition of the carbonate to oxide happens at temperatures under 700 °C, the ensuing fabrics appears to reabsorb carbon dioxide from the air.[11]

Applications

MgO is prized as a refractory material, i.e. a cast that is physically and chemically strong at top temperatures. It has two useful attributes: top thermal conductivity and coffee electric conductivity. Filling the spiral Calrod range most sensible heating components on kitchen electrical stoves is a main use. "By far the largest consumer of magnesia worldwide is the refractory industry, which consumed about 56 % of the magnesia in the United States in 2004, the remaining 44 % being used in agricultural, chemical, construction, environmental, and other industrial applications."[12] MgO is used as a basic refractory material for crucibles.

It is a foremost fireproofing aspect in building fabrics. As a construction material, magnesium oxide wallboards have a number of attractive characteristics: hearth resistance, termite resistance, moisture resistance, mould and mildew resistance, and strength.[13]

Niche uses

MgO is one of the parts in Portland cement in dry process crops.

Magnesium oxide is used broadly within the soil and groundwater remediation, wastewater remedy, consuming water treatment, air emissions treatment, and waste treatment industries for its acid buffering capability and comparable effectiveness in stabilizing dissolved heavy steel species.

Many heavy metals species, such as lead and cadmium are most soluble in water at acidic pH (under 6) as well as high pH (above 11). Solubility of metals impacts bioavailability of the species and mobility soil and groundwater systems. Most metal species are toxic to humans at certain concentrations, therefore it is imperative to reduce steel bioavailability and mobility.

Granular MgO is ceaselessly combined into metals-contaminated soil or waste material, which may be recurrently of a low (acidic) pH, so as to power the pH into the 8–10 vary where maximum metals are at their lowest solubilities. Metal-hydroxide complexes have a tendency to precipitate out of aqueous solution within the pH vary of 8–10. MgO is broadly appeared as the most effective metals stabilization compound when in comparison to Portland cement, lime, kiln mud merchandise, energy era waste products, and quite a lot of proprietary merchandise due to MgO's superior buffering capacity, cost effectiveness, and simplicity/safety of dealing with.

Most, if now not all products which can be marketed as metals stabilization technologies create very prime pH stipulations in aquifers whereas MgO creates an ideal aquifer situation with a pH of 8–10. Additionally, magnesium, an very important part to maximum biological systems, is equipped to soil and groundwater microbial populations all over MgO-assisted metals remediation as an added get advantages.

Medical

Magnesium oxide is used for reduction of heartburn and dyspepsia, as an antacid, magnesium complement, and as a short-term laxative. It could also be used to beef up signs of indigestion. Side effects of magnesium oxide might include nausea and cramping.[14] In quantities sufficient to obtain a laxative impact, side effects of long-term use come with enteroliths resulting in bowel obstruction.[15]

Other As a food additive, it's used as an anticaking agent. It is known to america Food and Drug Administration for cacao products; canned peas; and frozen dessert.[16] It has an E selection of E530. It used to be traditionally used as a reference white colour in colorimetry, owing to its just right diffusing and reflectivity houses.[17] It could also be smoked onto the surface of an opaque subject matter to form an integrating sphere. It is used widely as an electrical insulator in tubular development heating components. There are several mesh sizes available and maximum often used ones are 40 and 80 mesh in line with the American Foundry Society. The in depth use is because of its prime dielectric power and average thermal conductivity. MgO is generally overwhelmed and compacted with minimal airgaps or voids. The electrical heating trade additionally experimented with aluminium oxide, however it's not used anymore. As a reagent within the set up of the carboxybenzyl (Cbz) workforce the use of benzyl chloroformate in EtOAc for the N-protection of amines and amides.[18] It may be used as an insulator in heat-resistant electric cable. MgO doping has been shown to effectively inhibit grain expansion in ceramics and make stronger their fracture toughness via transforming the mechanism of crack expansion at nanoscale.[19] Unpolished MgO crystal Pressed MgO is used as an optical material. It is transparent from 0.Three to 7 µm. The refractive index is 1.Seventy two at 1 µm and the Abbe number is 53.58. It is every now and then identified via the Eastman Kodak trademarked name Irtran-5, even supposing this designation is obsolete. Crystalline pure MgO is available commercially and has a small use in infrared optics.[20] MgO is packed round transuranic waste at the Waste Isolation Pilot Plant, to regulate the solubility of radionuclides.[21] MgO has an important position as a business plant fertilizer [22] and as animal feed.[23] An aerosolized solution of MgO is utilized in library science and collections management for the deacidification of at-risk paper items. In this process, the alkalinity of MgO (and an identical compounds) neutralizes the slightly prime acidity function of low-quality paper, thus slowing the velocity of deterioration.[24] MgO may be used as a protective coating in plasma displays. Magnesium oxide is used as an oxide barrier in spin-tunneling gadgets. Owing to the crystalline structure of its skinny motion pictures, which will also be deposited by magnetron sputtering, for example, it presentations traits awesome to these of the repeatedly used amorphous Al2O3. In explicit, spin polarization of about 85% has been accomplished with MgO[25] versus 40–60 % with aluminium oxide.[26] The price of tunnel magnetoresistance could also be significantly higher for MgO (600% at room temperature and 1,100 % at 4.2 Ok[27]) than Al2O3 (ca. 70% at room temperature[28]). MgO is thermally strong up to about 700 Okay, vs. 600 Ok for Al2O3.

Precautions

Inhalation of magnesium oxide fumes may cause metal fume fever.[29]

References

^ a b c d .mw-parser-output cite.quotationfont-style:inherit.mw-parser-output .quotation qquotes:"\"""\"""'""'".mw-parser-output .id-lock-free a,.mw-parser-output .citation .cs1-lock-free abackground:linear-gradient(transparent,transparent),url("//upload.wikimedia.org/wikipedia/commons/6/65/Lock-green.svg")right 0.1em middle/9px no-repeat.mw-parser-output .id-lock-limited a,.mw-parser-output .id-lock-registration a,.mw-parser-output .citation .cs1-lock-limited a,.mw-parser-output .citation .cs1-lock-registration abackground:linear-gradient(transparent,clear),url("//upload.wikimedia.org/wikipedia/commons/d/d6/Lock-gray-alt-2.svg")right 0.1em heart/9px no-repeat.mw-parser-output .id-lock-subscription a,.mw-parser-output .citation .cs1-lock-subscription abackground:linear-gradient(transparent,transparent),url("//upload.wikimedia.org/wikipedia/commons/a/aa/Lock-red-alt-2.svg")correct 0.1em heart/9px no-repeat.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registrationcolor:#555.mw-parser-output .cs1-subscription span,.mw-parser-output .cs1-registration spanborder-bottom:1px dotted;cursor:lend a hand.mw-parser-output .cs1-ws-icon abackground:linear-gradient(clear,clear),url("//upload.wikimedia.org/wikipedia/commons/4/4c/Wikisource-logo.svg")correct 0.1em middle/12px no-repeat.mw-parser-output code.cs1-codecolour:inherit;background:inherit;border:none;padding:inherit.mw-parser-output .cs1-hidden-errordisplay:none;font-size:100%.mw-parser-output .cs1-visible-errorfont-size:100%.mw-parser-output .cs1-maintshow:none;color:#33aa33;margin-left:0.3em.mw-parser-output .cs1-formatfont-size:95%.mw-parser-output .cs1-kern-left,.mw-parser-output .cs1-kern-wl-leftpadding-left:0.2em.mw-parser-output .cs1-kern-right,.mw-parser-output .cs1-kern-wl-rightpadding-right:0.2em.mw-parser-output .quotation .mw-selflinkfont-weight:inheritHaynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.74. ISBN 1439855110. ^ Taurian, O.E.; Springborg, M.; Christensen, N.E. (1985). "Self-consistent electronic structures of MgO and SrO" (PDF). Solid State Communications. 55 (4): 351–5. Bibcode:1985SSCom..55..351T. doi:10.1016/0038-1098(85)90622-2. ^ Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.133. ISBN 1439855110. ^ Application of magnesium compounds to insulating heat-conductive fillers Archived 2013-12-30 at the Wayback Machine. konoshima.co.jp ^ a b Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 5.15. ISBN 1439855110. ^ a b Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 5.2. ISBN 1439855110. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0374". National Institute for Occupational Safety and Health (NIOSH). ^ Zhu, Qiang; Oganov A.R.; Lyakhov A.O. (2013). "Novel stable compounds in the Mg-O system under high pressure" (PDF). Phys. Chem. Chem. Phys. 15 (20): 7696–7700. Bibcode:2013PCCP...15.7696Z. doi:10.1039/c3cp50678a. PMID 23595296. ^ Mei, AB; O. Hellman; C. M. Schlepütz; A. Rockett; T.-C. Chiang; L. Hultman; I. Petrov; J. E. Greene (2015). "Reflection Thermal Diffuse X-Ray Scattering for Quantitative Determination of Phonon Dispersion Relations". Physical Review B. 92 (17): 174301. Bibcode:2015PhRvB..92q4301M. doi:10.1103/physrevb.92.174301. ^ Margarete Seeger; Walter Otto; Wilhelm Flick; Friedrich Bickelhaupt; Otto S. Akkerman. "Magnesium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a15_595.pub2. ^ Ropp, R C (2013-03-06). Encyclopedia of the alkaline earth compounds. Elsevier. p. 109. ISBN 9780444595508. ^ Mark A. Shand (2006). The chemistry and era of magnesia. John Wiley and Sons. ISBN 978-0-471-65603-6. Retrieved 10 September 2011. ^ Mármol, Gonzalo; Savastano, Holmer (July 2017). "Study of the degradation of non-conventional MgO-SiO 2 cement reinforced with lignocellulosic fibers". Cement and Concrete Composites. 80: 258–267. doi:10.1016/j.cemconcomp.2017.03.015. ^ Magnesium Oxide. MedlinePlus. Last reviewed 02/01/2009 ^ Tatekawa Y, Nakatani K, Ishii H, et al. (1996). "Small bowel obstruction caused by a medication bezoar: report of a case". Surgery Today. 26 (1): 68–70. doi:10.1007/BF00311997. PMID 8680127. S2CID 24976010. ^ "Compound Summary for CID 14792 – Magnesium Oxide". PubChem. ^ Tellex, Peter A.; Waldron, Jack R. (1955). "Reflectance of Magnesium Oxide". JOSA. 45 (1): 19. doi:10.1364/JOSA.45.000019. ^ Dymicky, M. (1989-02-01). "Preparation of Carbobenzoxy-L-Tyrosine Methyl and Ethyl Esters and of the Corresponding Carbobenzoxy Hydrazides". Organic Preparations and Procedures International. 21 (1): 83–90. doi:10.1080/00304948909356350. ISSN 0030-4948. ^ Tan, C.Y.; Yaghoubi, A.; Ramesh, S.; Adzila, S.; Purbolaksono, J.; Hassan, M.A.; Kutty, M.G. (December 2013). "Sintering and mechanical properties of MgO-doped nanocrystalline hydroxyapatite" (PDF). Ceramics International. 39 (8): 8979–8983. doi:10.1016/j.ceramint.2013.04.098. ^ Stephens, Robert E. & Malitson, Irving H. (1952). "Index of Refraction of Magnesium Oxide" (PDF). Journal of Research of the National Bureau of Standards. 49 (4): 249–252. doi:10.6028/jres.049.025. ^ wipp.energy.gov Step-By-Step Guide for Waste Handling at WIPP. Waste Isolation Pilot Plant. wipp.energy.gov ^ Nutrient Science. fertilizer101.org. Retrieved on 2017-04-26. ^ Magnesium oxide for the Animal Feed Industry. lehvoss.de ^ "Mass Deacidification: Saving the Written Word". Library of Congress. Retrieved 26 September 2011. ^ Parkin, S. S. P.; Kaiser, C.; Panchula, A.; Rice, P. M.; Hughes, B.; Samant, M.; Yang, S. H. (2004). "Giant tunnelling magnetoresistance at room temperature with MgO (100) tunnel barriers". Nature Materials. 3 (12): 862–867. Bibcode:2004NatMa...3..862P. doi:10.1038/nmat1256. PMID 15516928. S2CID 33709206. ^ Monsma, D. J.; Parkin, S. S. P. (2000). "Spin polarization of tunneling current from ferromagnet/Al2O3 interfaces using copper-doped aluminum superconducting films". Applied Physics Letters. 77 (5): 720. Bibcode:2000ApPhL..77..720M. doi:10.1063/1.127097. ^ Ikeda, S.; Hayakawa, J.; Ashizawa, Y.; Lee, Y. M.; Miura, Ok.; Hasegawa, H.; Tsunoda, M.; Matsukura, F.; Ohno, H. (2008). "Tunnel magnetoresistance of 604% at 300 K by suppression of Ta diffusion in CoFeB∕MgO∕CoFeB pseudo-spin-valves annealed at high temperature". Applied Physics Letters. 93 (8): 082508. Bibcode:2008ApPhL..93h2508I. doi:10.1063/1.2976435. ^ Wang, D.; Nordman, C.; Daughton, J. M.; Qian, Z.; Fink, J.; Wang, D.; Nordman, C.; Daughton, J. M.; Qian, Z.; Fink, J. (2004). "70% TMR at Room Temperature for SDT Sandwich Junctions with CoFeB as Free and Reference Layers". IEEE Transactions on Magnetics. 40 (4): 2269. Bibcode:2004ITM....40.2269W. CiteSeerX 10.1.1.476.8544. doi:10.1109/TMAG.2004.830219. S2CID 20439632. ^ Magnesium Oxide. National Pollutant Inventory, Government of Australia.

External links

Data web page at UCL Ceramic knowledge page at NIST NIOSH Pocket Guide to Chemical Hazards at CDCvteMagnesium compounds MgB2 MgBr2 MgCO3 MgC2O4 MgC6H6O7 MgC14H10O4 MgCl2 Mg(ClO4)2 MgF2 MgH2 Mg(HCO3)2 MgI2 Mg(NO3)2 MgO MgO2 Mg(OH)2 MgPo MgS MgSO3 MgSO4 MgU2O7 Mg2Al3 Mg2Si Mg2SiO4 Mg2Si3O8 Mg3N2 Mg3(PO4)2 Mg2(CrO4)2 vteDrugs for acid comparable issues: Antacids (A02A)Magnesium (increases motility) Magnesium carbonate Magnesium oxide Magnesium peroxide Magnesium hydroxide Magnesium silicateAluminium (decreases motility) Aceglutamide aluminum Algeldrate Aluminium phosphate Aluminium acetoacetate Aloglutamol Aluminium glycinate CarbaldrateCalcium Calcium carbonate Calcium silicateSodium Sodium bicarbonateCombinations and complexesof aluminium, calcium and magnesium Almagate Almasilate Hydrotalcite Magaldrate vteOxidesCombined oxidation states Antimony tetroxide (Sb2O4) Cobalt(II,III) oxide (Co3O4) Lead(II,IV) oxide (Pb3O4) Manganese(II,III) oxide (Mn3O4) Iron(II,III) oxide (Fe3O4) Silver(I,III) oxide (Ag2O2) Triuranium octoxide (U3O8) Carbon suboxide (C3O2) Mellitic anhydride (C12O9) Praseodymium(III,IV) oxide (Pr6O11) Terbium(III,IV) oxide (Tb4O7) Dichlorine pentoxide (Cl2O5)+1 oxidation state Copper(I) oxide (Cu2O) Caesium oxide (Cs2O) Dicarbon monoxide (C2O) Dichlorine monoxide (Cl2O) Gallium(I) oxide (Ga2O) Lithium oxide (Li2O) Potassium oxide (K2O) Rubidium oxide (Rb2O) Silver oxide (Ag2O) Thallium(I) oxide (Tl2O) Sodium oxide (Na2O) Water (hydrogen oxide) (H2O)+2 oxidation state Aluminium(II) oxide (AlO) Barium oxide (BaO) Beryllium oxide (BeO) Cadmium oxide (CdO) Calcium oxide (CaO) Carbon monoxide (CO) Chromium(II) oxide (CrO) Cobalt(II) oxide (CoO) Copper(II) oxide (CuO) Dinitrogen dioxide (N2O2) Germanium monoxide (GeO)) Iron(II) oxide (FeO) Lead(II) oxide (PbO) Magnesium oxide (MgO) Manganese(II) oxide (MnO) Mercury(II) oxide (HgO) Nickel(II) oxide (NiO) Nitric oxide (NO) Palladium(II) oxide (PdO) Silicon monoxide (SiO) Strontium oxide (SrO) Sulfur monoxide (SO) Disulfur dioxide (S2O2) Thorium monoxide (ThO) Tin(II) oxide (SnO) Titanium(II) oxide (TiO) Vanadium(II) oxide (VO) Zinc oxide (ZnO)+Three oxidation state Actinium(III) oxide (Ac2O3) Aluminium oxide (Al2O3) Antimony trioxide (Sb2O3) Arsenic trioxide (As2O3) Bismuth(III) oxide (Bi2O3) Boron trioxide (B2O3) Cerium(III) oxide (Ce2O3) Chromium(III) oxide (Cr2O3) Cobalt(III) oxide (Co2O3) Dinitrogen trioxide (N2O3) Dysprosium(III) oxide (Dy2O3) Erbium(III) oxide (Er2O3) Europium(III) oxide (Eu2O3) Gadolinium(III) oxide (Gd2O3) Gallium(III) oxide (Ga2O3) Holmium(III) oxide (Ho2O3) Indium(III) oxide (In2O3) Iron(III) oxide (Fe2O3) Lanthanum oxide (La2O3) Lutetium(III) oxide (Lu2O3) Manganese(III) oxide (Mn2O3) Neodymium(III) oxide (Nd2O3) Nickel(III) oxide (Ni2O3) Phosphorus monoxide (PO) Phosphorus trioxide (P4O6) Praseodymium(III) oxide (Pr2O3) Promethium(III) oxide (Pm2O3) Rhodium(III) oxide (Rh2O3) Samarium(III) oxide (Sm2O3) Scandium oxide (Sc2O3) Terbium(III) oxide (Tb2O3) Thallium(III) oxide (Tl2O3) Thulium(III) oxide (Tm2O3) Titanium(III) oxide (Ti2O3) Tungsten(III) oxide (W2O3) Vanadium(III) oxide (V2O3) Ytterbium(III) oxide (Yb2O3) Yttrium(III) oxide (Y2O3)+Four oxidation state Americium dioxide (AmO2) Carbon dioxide (CO2) Carbon trioxide (CO3) Cerium(IV) oxide (CeO2) Chlorine dioxide (ClO2) Chromium(IV) oxide (CrO2) Dinitrogen tetroxide (N2O4) Germanium dioxide (GeO2) Hafnium(IV) oxide (HfO2) Lead dioxide (PbO2) Manganese dioxide (MnO2) Neptunium(IV) oxide (NpO2) Nitrogen dioxide (NO2) Osmium dioxide (OsO2) Plutonium(IV) oxide (PuO2) Praseodymium(IV) oxide (PrO2) Protactinium(IV) oxide (PaO2) Rhodium(IV) oxide (RhO2) Ruthenium(IV) oxide (RuO2) Selenium dioxide (SeO2) Silicon dioxide (SiO2) Sulfur dioxide (SO2) Tellurium dioxide (TeO2) Terbium(IV) oxide (TbO2) Thorium dioxide (ThO2) Tin dioxide (SnO2) Titanium dioxide (TiO2) Tungsten(IV) oxide (WO2) Uranium dioxide (UO2) Vanadium(IV) oxide (VO2) Zirconium dioxide (ZrO2)+5 oxidation state Antimony pentoxide (Sb2O5) Arsenic pentoxide (As2O5) Dinitrogen pentoxide (N2O5) Niobium pentoxide (Nb2O5) Phosphorus pentoxide (P2O5) Protactinium(V) oxide (Pa2O5) Tantalum pentoxide (Ta2O5) Vanadium(V) oxide (V2O5)+6 oxidation state Chromium trioxide (CrO3) Molybdenum trioxide (MoO3) Rhenium trioxide (ReO3) Selenium trioxide (SeO3) Sulfur trioxide (SO3) Tellurium trioxide (TeO3) Tungsten trioxide (WO3) Uranium trioxide (UO3) Xenon trioxide (XeO3)+7 oxidation state Dichlorine heptoxide (Cl2O7) Manganese heptoxide (Mn2O7) Rhenium(VII) oxide (Re2O7) Technetium(VII) oxide (Tc2O7)+8 oxidation state Osmium tetroxide (OsO4) Ruthenium tetroxide (RuO4) Xenon tetroxide (XeO4) Iridium tetroxide (IrO4)Related Oxocarbon Suboxide Oxyanion Ozonide Peroxide Superoxide OxypnictideOxides are sorted by way of oxidation state. Category:Oxides vteOxygen compounds AgO Al2O3 AmO2 Am2O3 As2O3 As2O5 Au2O3 B2O3 BaO BeO Bi2O3 BiO2 Bi2O5 BrO2 Br2O3 Br2O5 CO CO2 C2O3 CaO CaO2 CdO CeO2 Ce3O4 Ce2O3 ClO2 Cl2O Cl2O2 Cl2O3 Cl2O4 Cl2O6 Cl2O7 CoO Co2O3 Co3O4 CrO3 Cr2O3 Cr2O5 Cr5O12 CsO2 Cs2O3 CuO D2O Dy2O3 Er2O3 Eu2O3 FeO Fe2O3 Fe3O4 Ga2O Ga2O3 GeO GeO2 H2O 2H2O 3H2O H218O H2O2 HfO2 HgO Hg2O Ho2O3 I2O4 I2O5 I2O6 I4O9 In2O3 IrO2 KO2 K2O2 La2O3 Li2O Li2O2 Lu2O3 MgO Mg2O3 MnO MnO2 Mn2O3 Mn2O7 MoO2 MoO3 Mo2O3 NO NO2 N2O N2O3 N2O4 N2O5 NaO2 Na2O Na2O2 NbO NbO2 Nd2O3 OF2 O2F2 O3F2 O4F2 O2PtF6 more...Chemical formulas Authority keep an eye on GND: 4168538-6 LCCN: sh85079646 NDL: 00567384 Retrieved from "https://en.wikipedia.org/w/index.php?title=Magnesium_oxide&oldid=1004898312"