Talk:Magnesium

Template:WP1.0 Article changed over to new Wikipedia:WikiProject Elements format by maveric149. Elementbox converted 10:08, 23 Jun 2005 by Femto (previous revision was that of 08:01, 11 Jun 2005).

Production

Anyone know how to isolate Mg?

Electrolysis- obtain a soluble Mg compound, dissolve in water, place 2 leads into water conected to power supply, Mg will form at negative electrode

Information Sources

Some of the text in this entry was rewritten from Los Alamos National Laboratory - Magnesium. Additional text was taken directly from USGS Magnesium Statistics and Information, USGS Periodic Table - Magnesium, from the Elements database 20001107 (via dict.org), Webster's Revised Unabridged Dictionary (1913) (via dict.org) and WordNet (r) 1.7 (via dict.org). Data for the table were obtained from the sources listed on the subject page and Wikipedia:WikiProject Elements but were reformatted and converted into SI units.

Compounds

I am interested in what compounds Magnesium might form with Silicon and Yttrium. If anyone has lab equipment suitable for experiments of this nature, would you mind trying these and posting your findings here?

Other things you might try:

• Mg + Co
• Mg + Cr
• And the Radioactive Elements

According to the ASM Hand Book

Mg-Si crystallographic data Phase Composition, wt% Si Pearson symbol Space group (Mg) 0 hP2 P63/mmc Mg2Si 36.61 cF12 Fmm (Si) 100 cF8 Fdm High-pressure phases Mg2Si(a) 36.61 . . . . . . SiII 100 . . . . . .

(a) Above 2.5 GPa and 900 °C, it forms a hexagonal structure.

Mg-Si (Magnesium - Silicon) A.A. Nayeb-Hashemi and J.B. Clark, 1988

A.A. Nayeb-Hashemi and J.B. Clark, 1988, Phase Diagramsof Binary Magnesium Alloys, ASM International, MetalsPark, OH, USA

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The powder used in athletics is not the metal User:JCWF

Althetic chalk is made of magnesium carbonate. Please fix the article is it states that the metal form of magnesium is used. --mav

The article says that "Once ignited, it is difficult to extinguish, being able to burn in both nitrogen (forming magnesium nitride), and carbon dioxide."

The titanium article on this website says that only titanium can burn in nitrogen. Can magnesium not burn in a pure nitrogen atmosphere, but can still burn nitrogen when its in the air? If so, then this should be made more clear.

Google found a number of "elements" pages that repeat the claim that only titanium burns in nitrogen. But there is a US Dept of Energy handbook on spontaneous heating and pyrophoricity that claims "Magnesium may also burn in an atmosphere of nitrogen to form magnesium nitride." [1] The same page mentions titanium as also having this property. Both metals burn in a CO₂ atmosphere as well. Anyway, I tend to believe this reference. It looks like the titanium article needs updating if the DoE handbook is correct. If people have lingering doubts, maybe someone with access to CRC or some other source could find a corroborating authoritative reference.

The autoignition temperature for magnesium is nowhere close to 4000 F. It is a mere 1205 F, which corresponds to 652 C or 925 K.

Also, magnesium is the 6th most abundant metal according to Dr. Doron Aurbach of the Bar-Ilan University in Israel. Dr. Doron Aurbach is currently working on rechargeable magnesium batteries and has previously discovered several improvements to the Lithium-Ion battery used in most cell phones and other mobile devices this very moment.

I have also done my research on magnesium since I wrote an entire essay (4000 words), and its ability to combust in an atmosphere of carbon dioxide, or even within solid carbon dioxide, more commonly known as dry ice. This essay was checked for accuracy by two experts at the University of Helsinki. To the point, my sources also indicate that magnesium can burn in an atmosphere of nitrogen, as can titanium.

Refs for history

• Bergman, Torbern; Beddoes, Thomas (1784). Physical and chemical essays.
• Black, Joseph (1777). Experiments upon magnesia alba, quick-lime, and other alcaline substances.
• Partington, Charles Frederick (1836). The British cyclopædia of literature, history, geography, law, and politics.
• Henry Pownall (Of Epsom, Eng.) (1825). Some particulars relating to the history of Epsom: Compiled from the best authorities; containing a ... Description of the origin of horse racing, and of Epsom races, with an account of the mineral waters, and the two celebrated palaces of Durdans and Nonsuch, &c., &c. To which is added, an appendix, containing a botanical survey of the neighbourhood.
• Multhauf, R. P. (1976). "Geology, Chemistry, and the Production of Common Salt". Technology and Culture. 17 (4): 634–645. doi:10.2307/3103671. JSTOR 3103671.
• . doi:10.1098/rstl.1722.0071. {{cite book}}: Missing or empty |title= (help)
• Brown, J. (1722). "Observations and Experiments on the Sal Catharticum Amarum, Commonly Called the Epsom Salt. By Mr. John Brown, Chymist, F. R. S". Philosophical Transactions. 32 (370–380): 348–354. doi:10.1098/rstl.1722.0069. JSTOR 103635.

Atomic radius size?

Other places (atomic radius page, ptable, webelements)say the empirical radius of Magnesium is 150 pm, the article says 160.

Semi-protected edit request on 17 June 2016

The first paragraph under "Physical Properties" ends with "alkali earth metals", this should be "alkaline earth metals".

Zair~enwiki (talk) 14:52, 17 June 2016 (UTC)

Done. Thank you! Double sharp (talk) 15:11, 17 June 2016 (UTC)

Bulk modulus edit request

Hey there,

the bulk modulus for Mg is rougly 35 GPa and NOT 45 GPa.

Source: Charles P. Poole Jr (2004): Encyclopedic Dictionary of Condensed Matter Physics, Vol A, Page 749. (https://books.google.de/books?id=CXwrqM2hU0EC&pg=PA749#v=onepage&q&f=false) — Preceding unsigned comment added by 2A02:908:F325:F580:3DC5:577E:1408:CDB6 (talk) 08:46, 24 June 2016 (UTC)

Spamspamspam

That whole paragraph under "threonate" is written in an inappropriately promotional tone. Per WP:MEDRS, the whole bit should be removed until the findings can be replicated. 2600:8807:C104:BE00:4882:4295:B2F0:7FEF (talk) 23:17, 31 July 2016 (UTC)

Done I removed all non-neutral statements but kept the references. Mooseandbruce1 (talk) 05:41, 1 August 2016 (UTC)

bioavailability in food

In the area of nutrition supplements, Magnesium oxide is infamous for being very cheap and common but having extremely low bioavailability, and thus nearly useless for human nutrient purposes. Most other Magn supplement chemical forms are supposed to be much more bioavailable, at about 30%. What form is Magnesium in, in common foods, and what is the bioavailability in various foods -- is there significant variation in this?-71.174.180.38 (talk) 18:51, 6 September 2016 (UTC)

small intestines primary site for Magnesium absorption

This source: www.ancient-minerals.com/magnesium-sources/absorption/
says that in the human body most magnesium absorption occurs in the small intestines. It seems to include some respectable sources. If this is a true fact it would be worth mentioning in the article.-71.174.180.38 (talk) 19:23, 6 September 2016 (UTC)