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Template:Chemical Element Template:WP1.0 Article changed over to new Misplaced Pages: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 Misplaced Pages: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

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." 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.

Insufficient magnesium

I totally disagree with the statments about insufficient magnesium intake, an healty person will very rarly be affected by severe symptoms, see source: Centre Evian pour l'eau (in French) I'm looking for an English source, but what they say is: "Acute deficiency is rare. It is never due to an insufficiency of food contribution. It is the fact of various specific diseases whose majority are rare." --Astrowob 00:22, 17 Apr 2005 (UTC)

Your quote refers to "acute deficiency". But there is ample evidence that hypomagnesemia is common. See for example this Feb 2005 article in the Journal of Family Practice, including the footnotes referring to several relevant studies/papers.

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." (http://www.eh.doe.gov/techstds/standard/hdbk1081/hbk1081c.html) 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.

Insufficient magnesium I totally disagree with the statments about insufficient magnesium intake, an healty person will very rarly be affected by severe symptoms, see source: Centre Evian pour l'eau (in French) (http://www.centre-evian.com/dossier_presse/index.html?contenu-medias.html?http://www.centre-evian.com/dossier_presse/dos-media/11132.html?http://www.centre-evian.com/dossier_presse/dos-media/11132.html) I'm looking for an English source, but what they say is: "Acute deficiency is rare. It is never due to an insufficiency of food contribution. It is the fact of various specific disease

i love the info. your giving but try to give it more"curb-appeal".

Uses

The extremely high temperature at which magnesium burns makes it a handy tool for starting emergency fires during outdoor recreation. Some camping equipment suppliers sell a small block of magnesium with a flint strip on one side. It is used to make camp and emergency fire. You shave the magnesium with a knife, then strike the flint with the blade to ignite it.

Description from Cabelas: This handy tool consists of a small block of solid magnesium, with a full-length flint sparking insert set into one edge. The soft magnesium is scraped with a pocket knife into a small pile, which is ignited by scraping the edge of the sparking insert with the knife. Ignites to a temperature of 5,400°F, more than enough to light the most stubborn campfire. Works even if wet. PrometheusX303 23:01, 3 March 2006 (UTC)

See also

this should probably state that its 70% of the proven reserves, as 70% of the earth's Iron and Magnesium ore is somewhat presumptuous - NDR

You are correct. The article is wrong. If you look at El Mutún it says theres 40 billion tons of Iron there while it says that total world reserves are 230 billion tons. 40/230 = 17%. I removed this statement as it is clearly wrong. Dr. Morbius 01:42, 14 February 2007 (UTC)

Magnesium and diabetes

Low blood serum levels of magnesium are found in a disproportionaly high number of diabetics. --41.241.193.144 13:09, 12 February 2007 (UTC)

Al-induced magnesium depletion

Aluminium can deplete magnesium (and calcium) --41.241.193.144 13:09, 12 February 2007 (UTC)

El Mutun as a source of Magnesium ore?

I have looked at several sources on this topic and have been unable to find anything to corroborate that El Mutun contains Magnesium ore. El Mutun contains large quantities of Magnetite which is an iron ore. Perhaps this was misread as Magnesite which is a Magnesium mineral. Please provide a source for this statement. If one is not provided I will remove this reference. Dr. Morbius 01:04, 14 February 2007 (UTC)

Ok I'm removing the reference to El Mutun since no one has been able to provide any evidence to it being a source of Magnesium or Magnesium ore. Dr. Morbius 20:23, 26 February 2007 (UTC)

Magnalium redirect

The article magnalium currently redirects to magnesium. Magnalium refers to an alloy of magnesium and aluminum that is commonly used in engineering and pyrotechnics. I am considering creating a separate article for this alloy. What do other users think? --Pyrochem 06:33, 25 February 2007 (UTC)

Go for it. Never ask for permission to ADD to Misplaced Pages. Be BOLD (WP:BOLD). If you know enough to even start a stub which has material which would be too specialized for magnesium, go for it. I'm already thinking the magnesium article has a little too much about mag wheels and so on, in it, and a lot of this material could use offloading to a main article on magnalium or magnesium alloys (with a magnalium section), and leave just a short summary and redirect in the element article. Rather as is done for iron and steel.SBHarris 07:41, 25 February 2007 (UTC)

Solubility of Mg(OH)₂

You state that "So-called "milk of magnesia" is a water suspension of one of the few insoluble magnesium compounds, magnesium hydroxide;" how therefore is it possible for this insoluable compound to form an aqueous soloution "Magnesium (solid) + steam → Magnesium hydroxide (aqueous) + Hydrogen (gas)"? 88.104.61.131 20:20, 1 May 2007 (UTC)

I agree. The magnesium hydroxide formed would be in the solid, not aqueous, phase. Will fix it. Warut 14:58, 10 November 2007 (UTC)

Human health and general biology sections

I just altered the layout of this section a bit. It still needs a lot of work and may need spliting into it own article as it is getting a bit off the central thread of an article on magnesium per seReveldrummond 07:14, 18 July 2007 (UTC)

The Human health info has gone to the magnesium in biology page

The magnesium in biology and magnesium in biological systems and the magnesium transporters pages all need quite a lot of work to fit them into the appropriate portal project. I will have a go at this over the next little while. Is there anyone who can write a section on the animal physiology of magnesium? Reveldrummond 21:58, 20 July 2007 (UTC)

Commonality in Earth vs Universe

I'm not a chemist, but how would we know that magnesium is the nth most common element in the UNIVERSE? Changed this to Earth. If someone with more knowledge would like to reply and correct that, please feel free - as I said, I'm not an expert. Aaeamdar (talk) —Preceding comment was added at 01:56, 21 December 2007 (UTC)

That info was probably taken from here. Since it is unsourced, I doubt that too. Warut (talk) 11:07, 21 December 2007 (UTC)

Elemental abundances in the universe are determined spectroscopically by looking at where most of the elemental (non-dark) mass is, which is in stars, where it lights up well. Granted, for VERY far distances you can only say something about abundances in the early universe, but most of these don't change that much until you get right near the beginning, before much nucleosynthesis. But stellar nuclosynthesis came surprisingly early, so that's a long way. In any case, the most common Mg isotope is made from 6 "alphas" (or more properly, helium nuclei), so it's pretty common. Likewise, C, O, Ne, Si, etc. SBHarris 18:19, 21 December 2007 (UTC)

Ummm....

How in the heck did anyone ever figure out that White-Hot Magnesium is toxic even though the lower temperature form isn't? How do you test something like that? I'm suspicious that this is joke content subtly inserted... —Preceding unsigned comment added by 82.46.180.56 (talk) 03:01, 4 October 2007 (UTC)

I agree. Magnesium oxide fume produced may be toxic but that is not the toxicity of magnesium itself. I'll remove that paragraph. Warut 15:18, 10 November 2007 (UTC)

Im doing an science homework on Metals, Gases and bases, and we had 2 weeks to complete this fact file. But Im still looking for more info on like... Normal phase, Nonmeatl etc, Family and facts on Magnesium. If I dont I ll get a detention. —Preceding unsigned comment added by 219.89.231.96 (talk) 06:34, 24 October 2007 (UTC)

kill robots —Preceding unsigned comment added by 71.170.76.182 (talk) 02:30, 30 October 2007 (UTC)

So what's up with the number on the graphic being "14" when the atomic number is 12? —Preceding unsigned comment added by 152.18.36.12 (talk) 15:47, 16 January 2008 (UTC)

Contents reordering

I think the reordering of the contents made by 4.237.53.25 on 10 November 2007 was not vandalism, and, in fact, was very reasonable since it made the order of the contents more in line with other chemical elements. Warut 13:04, 10 November 2007 (UTC)

You may have a valid point and 4.237.53.25 may well have been acting in good faith, in which case I apologise unreservedly for my revert, but the moves messed up the formatting of the page, leaving large gaps. If you think the change was justified, by all means re-do it, but try to keep the formatting tidy. Best wishes, Plantsurfer 13:20, 10 November 2007 (UTC)

OK, I'll reorder the contents the way 4.237.53.25 did and move the magnesium products picture to the left so as to solve the unsightly gap problem. Hopefully, this will make the article look better. Warut 14:42, 10 November 2007 (UTC)

WikiProject Food and drink Tagging

This article talk page was automatically added with {{WikiProject Food and drink}} banner as it falls under Category:Food or one of its subcategories. If you find this addition an error, Kindly undo the changes and update the inappropriate categories if needed. The bot was instructed to tagg these articles upon consenus from WikiProject Food and drink. You can find the related request for tagging here . Maximum and carefull attention was done to avoid any wrongly tagging any categories , but mistakes may happen... If you have concerns , please inform on the project talk page -- TinucherianBot (talk) 17:41, 3 July 2008 (UTC)

length

could someone add a tag to simpilify this page? it has somewhat too much detail for an encyclopedia —Preceding unsigned comment added by 76.19.155.125 (talk) 06:27, 9 August 2008 (UTC)

Would you like elaborate? You might find simple:Magnesium more beneficial. Wizard191 (talk) 19:37, 9 August 2008 (UTC)

extraction from seawater

I find the statement that magnesium is separated as a carbonate from seawater by adding calcium carbonate suspicious. The solubility of calcium carbonate is smaller than that of magnesium carbonate so this reaction probably does not take place. Instead calcium hydroxide is used and the less soluble magnesium hydroxide is precipitated.Dinogep (talk) 18:14, 3 November 2008 (UTC)

Farmer story source?

Can anyone provide a valid source for the story of the farmer and his Espom Salts? Thanks. —Preceding unsigned comment added by 71.127.210.103 (talk) 22:42, 15 January 2009 (UTC)

What about this sentence?

Under 5 Biological role this sentence sounds a bit funny to me:

"Refining of food can reduce magnesium substantially, however, and use of synthetic fertilizers which do not contain the necessary amount of magnesium may produce which contain less magnesium than produce fertilized organically."

The first part is true: there's magnesium in bran. The second needs a cite and I don't believe it. SBHarris 23:17, 29 January 2009 (UTC)

"use of synthetic fertilizers ...may produce which contain less magnesium than produce fertilized organically." The bold part seems to be grammatically incorrect. Noun Verb Noun. If produce is used as the verb, the noun is missing, "use of synthetic fertilizers ... may produce what"? If produce is used as a noun, the verb is missing, "use of synthetic fertilizers may do what to produce"? IsmAvatar (talk) 19:18, 3 February 2009 (UTC)

On further inspection, the grammar error appeared when you refined upon poor phrasing of a previous statement, adding "produce produce", which a later editor regarded as redundant and removed one of the "produce", even though the first was being used as a verb and the second as a noun. As to the original statement: "Refining of food can reduce magnesium substantially, however, and fertilizers use less magnesium. This has led to observations of reduced dietary magnesium intake as compared to earlier generations." was paraphrased from the cited paper "There are observations that the Mg intake of humans has declined very sharply during the past few decades (68). This may be due to the refining and preparing of food but also to the use of fertilizers with no Mg (53)"

53: Marier JR, Neri LC, Anderson TW. Water hardness, human health and the importance of magnesium. National Research Council of Canada. Report 17581, 1979.

68: Seeling MS. Magnesium deficiency with phosphate and vitamin D excesses--role in pediatric cardiovascular disease? Cardiovasc Med 1978;3n(6):637-50.

The ref was added in originally here: http://en.wikipedia.org/search/?title=Magnesium&diff=prev&oldid=254182698

IsmAvatar (talk) 20:04, 3 February 2009 (UTC)

Semi-protect requested

Vandalism by IP users is getting out of hand on this article and so I've requested semi-protection. --Marc Kupper|talk 07:33, 7 March 2009 (UTC)

It's only averaged about 2 a day and as far as I can see enough folk are reverting. I'll continue to monitor, and feel free to ask again if it gets any worse. --John (talk) 07:58, 7 March 2009 (UTC)

Only two a day is too many! Science editors have better things to do than revert articles which IP schoolkids vandalize daily. Chemical element articles are a good example of articles which should generally be semi-protected. Take a look at hydrogen, helium, and oxygen for examples of nice, clear, evolving sprotected articles. Contrast with the neverending stupidities added every day to carbon, magnesium, and aluminium. As is the usual pattern for non-sprotected US presidents, about half the total edits to the article are IP vandalisms which must be removed. That's also true of the last HISTORY page of THIS article, and I see not a single IP valid contribution there. The whole thing is a waste of time, and a waste of wikipedia resources. In fact, I'm going to repost this section on the Wikiproject element as an RfC. Personally, I'm really tired of it. SBHarris 23:55, 7 March 2009 (UTC)

John, while I agree that the average of two different IP vandals per day is low but this article happens to the most vandalized, by far, of the 202 I'm watching at the moment. In the three years I've been editing on WP this is the second article that I felt merited WP:RPP. The last 50 page edits are 100% vandalism and reverting. I agree with you that a templated warning often stops the IP vandals in their tracks. Presumably the 19 separate vandals involved in those 50 edits now lead saintly lives as a result of getting burned while attempting to set the Magnesium article on fire.

BTW, there seems to be a pattern in that this article is only vandalized on weekdays. The implication is that it's by students bored with their chemistry class.

However, I have also seen that when an off the beaten path article such as this one gets semi-protected for a month that the vandals seem to forget about it and do not return once the article is unprotected. That was my intent in asking for semi-protection. --Marc Kupper|talk 02:05, 8 March 2009 (UTC)

Very well, I've semi-protected for one month. I hope that is to your liking. To put it in perspective, there are articles on my watchlist which attract much more vandalism than this, but I am also aware that as an admin I am entrusted with these tools to make life easier for folks like you. --John (talk) 03:26, 8 March 2009 (UTC)

Thank you John. We'll probably hear from those we deprived of their favorite hobby, reverting vandalism. --Marc Kupper|talk 04:36, 8 March 2009 (UTC)

Yes, thanks. I'm sure the other vandal-reverting Twinklers can find other stuff that needs their attention. SBHarris 04:37, 8 March 2009 (UTC)

Chart suggestion for vitamins and minerals.

Chart suggestion for vitamins and minerals.

Having been in business with a herbal department, there appears to be a need for a standardized presentation of vitamins and minerals to provide handy information to the general public.

Suggestion the following graph, if someone with this ability can present it as so.

Recommend a stardaized chart. Top lines, recommended daily allowance.

Then prioritized items that provide the element, together with amount of item in each serving and a percentage of the recommended daily allowance.

Why?

Well say vitamin C. One glass of orange juice. 100%

Vitamin D. One egg, 20. 3%

At the bottom of the chart important co ingredients required, and or negative factors to absorption.

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