マグネシウム、Mg+ 　　

WordNet

a light silver-white ductile bivalent metallic element; in pure form it burns with brilliant white flame; occurs naturally only in combination (as in magnesite and dolomite and carnallite and spinel and olivine) (同)Mg, atomic number 12

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マグネシウム(金属元素;化学記号は『Mg』)
magnesiumの化学記号

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出典(authority):フリー百科事典『ウィキペディア（Wikipedia）』「2015/09/02 20:33:42」(JST)

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マグネシウム（ラテン語: magnesium^[2]）は原子番号 12、原子量 24.305 の金属元素である。元素記号は Mg。マグネシュームと転訛することがある。

周期表第2族元素の一種で、ヒトを含む動物や植物の代表的なミネラル（必須元素）であり、とりわけ植物の光合成に必要なクロロフィルで配位結合の中心として不可欠である。また、有機化学的にはグリニャール試薬の構成元素として重要である。

酸化マグネシウムおよびオキソ酸塩の成分としての酸化マグネシウムを、苦い味に由来して苦土（くど、bitter salts）とも呼称する。

1 性質
- 1.1 同族元素との性質の違い
  - 1.1.1 カルシウム以降との違い
  - 1.1.2 ベリリウムとの違い
- 1.2 異方性
2 歴史
3 用途
- 3.1 金属として
- 3.2 工業
- 3.3 有機合成用試薬
- 3.4 農業、食品、医薬
- 3.5 食品
- 3.6 次世代エネルギー
4 マグネシウムの化合物
- 4.1 無機塩
  - 4.1.1 オキソ酸塩
  - 4.1.2 鉱物
- 4.2 有機塩
5 同位体
6 生化学
- 6.1 薬理作用
  - 6.1.1 糖尿病との関連性
  - 6.1.2 うつ病との関連性
  - 6.1.3 免疫系との関連性
7 関連項目
8 出典
9 外部リンク

性質

マグネシウムリボンの燃焼

酸化数はほぼ常に2価。比重 1.74の柔らかい金属で、融点 650 ℃、沸点 1090-1110 ℃（異なる実験値あり）。結晶構造は六方最密充填構造 (HCP)。

酸素と結合しやすく強い還元作用を持つ。空気中で放置すると、表面が酸化され灰色を帯びる。また、二酸化炭素、水、亜硫酸とも反応するが、いずれも不動態皮膜となるためアルカリ金属やカルシウムと異なり腐食は進行せず、鉱油中で保存する必要はない。

空気中で加熱すると炎と強い光を発して燃焼する（燃焼熱は601.7 kJ/mol）。さらに窒素や二酸化炭素中でも燃焼し、それぞれ窒化マグネシウム (Mg₃N₂)、酸化マグネシウム（生成熱は460.7 kJ/mol）となる。

CO₂ + 2 Mg → 2 MgO + C

熱水や塩水、薄い酸には容易に溶解し水素を発生する。

2 H₂O + Mg → Mg(OH)₂ + H₂

同族元素との性質の違い

マグネシウムとベリリウムは第2族元素だが、アルカリ土類金属ではない。これは第1族元素である水素がアルカリ金属ではないのと同様、化学的性質が異なるためである。ただし全く異なるわけではなく、第2族元素の代名詞として「アルカリ土類金属」の名が使われているため、広義にはアルカリ土類金属に含まれている。

カルシウム以降との違い

アルカリ土類金属とはカルシウム・ストロンチウム・バリウム（およびラジウム）に共通の化学的性質に由来するグループで、周期表に基づく族分類に先立って成立した。マグネシウムはアルカリ土類金属とは違う性質を持つ。

化合物が炎色反応を示さない（アルカリ土類金属は特有の発色を持つ）。
単体（粉末状を除く）が常温の水と反応しない（アルカリ土類金属は激しく反応して水素を発生する）。
常温空気中で表面に酸化不動態を形成する（アルカリ土類金属は内部まで急速に酸化される）。
硫酸塩が易水溶性（アルカリ土類金属は難水溶性）。
水酸化物が難水溶性で弱塩基性を示す（アルカリ土類金属は易水溶性で強塩基性）。
水酸化カルシウムは比較的水に溶けにくいが、それでも水酸化マグネシウムよりは溶けやすい。

ベリリウムとの違い

マグネシウムはベリリウムと共通した化学的性質を持つが、違いもある。

陽性が強い。ベリリウム化合物は共有結合性のものが多いのに対し、マグネシウム化合物は幾分共有結合性を帯びるものの依然イオン結合性のものが多い。
塩基性が強い。ベリリウムは両性元素であるため酸にもアルカリにも溶けるが、マグネシウムは塩基性が強いため酸には溶けるがアルカリには溶けない。

異方性

マグネシウムの異方性

0001：滑り面 0012：双晶面

マグネシウムの結晶構造は室温では2つの面でしか滑りを起こさないため、純マグネシウムや合金を加熱せずに圧延などの加工をすると割れが発生しやすい。加工には加熱が必須となるが燃焼しないよう注意を払う必要がある。

歴史

マグネシウムは安定な酸化物を作るため、ラボアジエはマグネシア（酸化マグネシウム）を元素としてあげている。1755年、スコットランドのジョゼフ・ブラックは炭酸マグネシウムを熱分解し、酸化マグネシウムと二酸化炭素に分離しているが、これをマグネシウムの発見とする事もある。

単離され金属元素であることが証明されたのは、1808年、ハンフリー・デービーによるマグネシアと酸化水銀の溶融電気分解による。マグネシア magnesia またはその語源である産地のギリシャ・マグニシア県にちなんで命名された。

商業生産は1886年、アルミニウムと同時期に開始されたものの、精錬（カルシウムと）が困難で普及が遅れた。第一次大戦を契機に軍事利用が伸び、1936年には軍事目的を陰に五輪の聖火リレーに利用され、1939年には32,850トン、1943年のアメリカで184,000トンが生産されている。日本では第二次大戦前から1994年まで宇部興産により生産されていた。マグネサイト等の鉱石資源は、中国、北朝鮮、ロシアの3国で6割以上を占めている^[3]。

用途

非常に軽い軽合金材料として重要であり、金属マグネシウムとして様々な合金の第一金属（合金の基本となる金属）や、添加剤に利用される。また、反応性の高さから脱酸素剤や脱硫剤、さらに有機合成用試薬として欠かせない。必須元素であり、食品や医薬品のほか、飼料、肥料として広く用いられる。

金属として

詳細は「マグネシウム合金」を参照

合金 - 優れた性質を持ち、需要が伸びている。安価になればプラスチックを代替する可能性もある。

工業的に使用されている最も軽い金属で用途は広く、航空機、自動車、農業機械、工具、精密機械、スポーツ用具、スピーカーの振動板、携帯用機器の筐体、医療機器、宇宙船、兵器などの多種にわたる。かつて問題だった腐食しやすい性質が改善されるにつれ、利用されるようになっていった。

合金添加剤 - 1998年頃には世界需要の半数近くを占めた^[4]。アルミニウム合金などに添加元素として少量付加するだけであっても、その合金としての性質を大きく左右する働きを持つ。この性質から、これまでの合金の硬度、強度、耐食性、耐熱性、その他機械的性質を向上させるための研究が活発に行われている。
鋳鉄 - ダクタイル鋳鉄 (FCD) の黒鉛ノジュラー（球状）化剤
鉄鋼脱硫剤 - 合金用途以外では最も消費量が多く、精錬用フェロアロイ（フェロマグネシウム）

金属還元剤 - ジルコニウム、チタンの製錬
防食 - 防食マグネとして、金属の犠牲電極効果や、酸化物が使用される
カメラのフラッシュ - 酸化剤と混合した発光材（パウダー）が利用され「マグネシウムを焚く」と表現した。光量調節が難しく発光時大量の煙を発生させ、シャッターとの同調も手作業であるため、閃光電球やエレクトロニックフラッシュによって置き換えられた
発火用具（ファイアスタータ）- 水に濡れていても発火できるため、軍事用、キャンプ用など
スピーカーの振動板 - 単体は合金より内部損失が大きく、酸化防止の樹脂コーティングを施して使用される

工業

耐火材 - 炉内耐火材（塩基性耐火煉瓦）として主に電気炉で用いる
吸着材 - 水酸化マグネシウムが多く、酸化、炭酸マグネシウムなども
ゴム、プラスチック配合剤 - 添加剤、充填剤
セラミックス - 原料、焼結助剤
ガラス - 酸化ガラス添加剤
電池 - 空気マグネシウム電池

排煙脱硫剤 - 安価で脱硫効率が高い、水酸化マグネシウム放流法
排水処理 - 石灰と同様、酸性排水の中和（カルシウムが混在したものが使われる）
水質改善 - アオコ対策、赤潮対策、底質改善
重金属処理 - アルカリ剤として不溶化処理、ヘドロなど泥土の固化

有機合成用試薬

マグネシウムはハロゲン化アルキルと反応し、R-MgX（R は有機置換基、X はハロゲン）の一般式で表される有機金属化合物を作る。これはグリニャール試薬と呼ばれ、カルボニル化合物などと反応して炭素-炭素結合を生成する。このため有機合成分野において重要な試薬として用いられる。

そのほかにもたくさんの錯体・塩基性塩などの化合物を合成する。これらは主に化学実験において、合成試料や試薬として使われる。

農業、食品、医薬

肥料 - 水酸苦土肥料、硫酸苦土肥料など
にがり - 主に塩化マグネシウムが、豆腐製造の凝固剤（塩析剤）として
食品添加物 - 膨張剤（炭酸マグネシウム）、栄養強化剤、加工助剤など
医薬品 - クエン酸マグネシウムが大腸検査用下剤など

食品

精製・加工していない食品に広く含まれ、ゴマやアーモンドなどの種実類、ひじきなどの海藻類に多く、加工食品に少ない。

次世代エネルギー

燃焼にて二酸化炭素を発生しない事から、化石燃料に替わる次世代エネルギーとしての利用研究が進められている。

水素に比べて常温・常圧下で固体なので輸送・貯蔵がしやすいというメリットがある。水と反応させて燃えるときの熱を利用する他、同反応により発生する水素を燃料として利用する方法が挙げられる。燃焼後の酸化物のリサイクルのための還元処理が最大の課題であり、レーザーによる高温を利用する方法などが提案されている^[5]。

但し、マグネシウムを燃料として使用する場合、燃焼させて熱エネルギーに変換した場合熱機関を利用する以上カルノー効率を超えることは出来ない。また、水と反応させて水素を取り出しその水素を燃焼させる場合や生成した水素を燃料電池で電気エネルギーに変換するという用途も同様に効率が低い。

マグネシウムの持つ化学エネルギーを効率良く電気エネルギーに変換する方法としては電池の陰極としてマグネシウムを使用する方法が効率が良い。但し、水溶液を電解質として使用する場合は反応性が高い為、マグネシウムが水と反応するので不適である。有機系の電解質の使用が望ましい。電解質に溶融塩を使用する選択肢もある。

詳細は「空気マグネシウム電池」を参照

マグネシウムの化合物

無機塩

酸化マグネシウム MgO - 苦土
過酸化マグネシウム MgO₂
水酸化マグネシウム Mg(OH)₂

フッ化マグネシウム MgF₂
塩化マグネシウム MgCl₂
臭化マグネシウム MgBr₂
ヨウ化マグネシウム MgI₂
水素化マグネシウム MgH₂
二ホウ化マグネシウム MgB₂
窒化マグネシウム Mg₃N₂
硫化マグネシウム MgS

オキソ酸塩

炭酸マグネシウム MgCO₃ - 菱苦土石
炭酸カルシウムマグネシウム CaMg(CO₃)₂ - 苦灰石、ドロマイト
硝酸マグネシウム Mg(NO₃)₂
硫酸マグネシウム MgSO₄
亜硫酸マグネシウム MgSO₃
過塩素酸マグネシウム MgClO₄
リン酸三マグネシウム Mg₃(PO₄)₂•8H₂O
過マンガン酸マグネシウム Mg(MnO₄)₂
リン酸マグネシウム（英語版）

鉱物

三ケイ酸マグネシウム 2MgO•3SiO₂•nH₂O
尖晶石、スピネル MgO•Al₂O₃
滑石 Mg₃Si₄O₁₀(OH)₂
蛇紋石 Mg₃Si₂O₅(OH)₄

有機塩

有機酸との塩である。

酢酸マグネシウム Mg(CH₃COO)₂
クエン酸マグネシウム
リンゴ酸マグネシウム
L-グルタミン酸マグネシウム
安息香酸マグネシウム C₁₄H₁₀MgO₄
ステアリン酸マグネシウム Mg(CH₃(CH₂)₁₆COO)₂

同位体

詳細は「マグネシウムの同位体」を参照

マグネシウムは3つの安定同位体 ²⁴Mg、²⁵Mg、²⁶Mg を持つ。

生化学

マグネシウムは植物の光合成色素であるクロロフィルに含まれて、光を受け止める役割を担っている。このためマグネシウムが欠乏すると、植物は生育が減退し、収穫量の減量につながる。これは砂地で生育する植物に特に現れる。カリウムが豊富に含まれる土壌でも、植物へのマグネシウムの供給が行われにくくなることもわかっている。このため肥料として、マグネシウム化合物を含んだものが使用されることがある。

70 kgのヒトにおいては約35 gのマグネシウムが存在し^[6]^{[要高次出典]}、その60-70%がリン酸塩として骨組織に、残りの30%は血漿、赤血球、筋肉中の各組織に存在する。血清中のマグネシウムは、約75-85%がイオンや塩類の形態の透析型で、残りの15-25%はアルブミンなどと結合した蛋白結合型（非透析型）で存在する。

人体にとってもリボソームの構造維持やタンパク質の合成、その他エネルギー代謝に関する生体機能に必須な元素であるためマグネシウムの欠乏は虚血性心疾患などの原因のひとつと考えられている。生体内でマグネシウムは主に骨の表面近くにマグネシウムイオンとして保存され、代謝が不足した場合にはカルシウムイオンと置き換わり、マグネシウムが体内に補充される。マグネシウムの生体内での栄養素や薬理的な働きについては広範にわたって研究が行われているが、いまだその重要な面に関しては不明な点が多い。最近では、ミネラル成分のひとつとしてサプリメントや清涼飲料水などに添加されることが多くなってきている。

マグネシウムは動植物に対して毒性の強い元素でないため、植物肥料として過剰使用を特に警戒する必要はないが、動物が直接食物から摂取する場合には、他の無機物（リンやカルシウム）とのバランスを適切にしなければ、尿路結石などの原因になりうることがわかっている。これを受けて、猫用の飼料は、組成中のマグネシウムを減らすように改良されるようになった。

薬理作用

マグネシウム欠乏症の治療と予防に用いられるほか、乳酸が溜まった状況下で、足のつり（こむら返り）等の緩和に有効性が示唆されている。

マグネシウムは生体に必要不可欠な成分である反面、マグネシウムが豆乳を豆腐に固化することに見られるように高濃度のマグネシウムイオンはタンパク質を固化する性質を有する。マグネシウムの吸収機構は解明されていないが^[7]^{[要高次出典]}、腸管からのマグネシウムの吸収率は、マグネシウム摂取量が多ければ吸収率が低下し、摂取量が少なければ吸収率は高くなる^[8]。腸管から吸収されなければ、マグネシウムイオン濃度の高まりにより腸管内での浸透圧が高まることになる。このためマグネシウムの過剰摂取で下痢を起こす。この作用を利用し、クエン酸マグネシウムなどは大腸検査のときの下剤として使われる。また、便秘の不快症状を緩和する目的の下剤として酸化マグネシウム（通称カマ）が投与される場合がある。弱い塩基である酸化マグネシウムや水酸化マグネシウムは、胃酸中和のために胃腸薬に配合される。食品では、豆腐や天然塩などに含まれるにがりからマグネシウムが微量に摂取される。

過剰摂取により高マグネシウム血症を引き起こす。重篤な腎不全患者における大量摂取は非常に危険。心ブロック患者には静脈注射が禁忌^[9]。なお、近年のダイエットブームにより、にがりの過剰摂取で死亡した事例もあるので、安易な過剰摂取は厳に慎むべきである。マグネシウムの急性毒性は、塩化マグネシウムとして、マウス経口 LD50は4700 mg/kg、ラット経口 LD50は2800 mg/kgである^[10]^{[要高次出典]}。このラットのデータを70 kgのヒトに当てはめれば約200 gの塩化マグネシウムを一時に摂取すれば50%の確率で死に至ることに相当する。

なお、1999年の「第6次改定日本人の栄養所要量について」によると、マグネシウムの所要量は約200～320 mg/日、マグネシウムの許容上限摂取量は約700 mg/日、である^[11]。

また、マグネシウム摂取量が多いグループの男性の大腸癌リスクが低い^[12]、との報告がある。

糖尿病との関連性

平成22年国民健康・栄養調査によれば、日本人成人（30～49歳男性）の推定摂取量は240～244mg/日とされ、WHO推奨量である420mg/日より不足している^[13]。慢性的な摂取不足は、脂肪細胞から分泌される分泌蛋白アディポネクチンの低下を招き、高感度CRPやIL-6の上昇に関連しており、2型糖尿病発症リスクを上昇させている^[14]。

うつ病との関連性

マグネシウム欠乏下では興奮性グルタミン酸神経のNMDA受容体の抑えが効かなくなり^[15]、その神経毒性によりうつ病が引き起こされているのではないかという仮説がある。NMRを用いた計測では治療抵抗性うつ病で自殺企図あるいは自殺未遂経験のある患者では脳脊髄液中のマグネシウム量が低いこと。抗うつ薬は脳内マグネシウム量を増やす作用があること。2008年の糖尿性うつ病患者へのマグネシウム投与で成果をあげている^[16]ことなどから、治療抵抗性うつ病患者に限らずマグネシウムの処方は有益であるとする報告がある^[17]。また、magnesium glycinate または magnesium taurinate の投与によりおよそ1週間程度の短期での症状改善の報告がある^[18]。

免疫系との関連性

閉経後の女性に関するコホート研究において、さまざまな変数を調整後のマグネシウムの摂取量と炎症に関係するバイオマーカーの数値とが反比例するとの報告がある^[19]。すなわち、マグネシウムの摂取量が多いほど体内の炎症反応が少ないことを示している。

出典

^ Bernath, P. F., Black, J. H., & Brault, J. W. (1985). "The spectrum of magnesium hydride". Astrophysical Journal 298: 375.
^ http://www.encyclo.co.uk/webster/M/6
^ 2.7 マグネシウム（Mg） (PDF) 東北経済産業局
^ 日本マグネシウム協会
^ [1]
^ 桜井弘氏講演生体元素と医薬品の開発（第一回）講演録
^ 8.マグネシウムの再吸収異常と生活習慣病との関連性について研究内容の紹介紹介ページのひとつ
^ 専門領域の最新情報　最新栄養学　第8版：建帛社
^ 「健康食品」の安全性・有効性情報国立健康・栄養研究所
^ 製品安全データシート 0.01mol/1(M/100)-塩化マグネシウム溶液キシダ化学株式会社
^ 第６次改定日本人の栄養所要量について
^ マグネシウム摂取と大腸がんとの関連について JPHC Study 多目的コホート研究独立行政法人国立がん研究センター
^ マグネシウム国立健康・栄養研究所
^ マグネシウム摂取不足の解消こそが糖尿病の増加を抑える日経メディカルオンライン 2012年5月22日
^ マグネシウムはNMDA受容体の活性をブロックするモジュレータ(英)として働く。
^ Barragán-Rodríguez, L; Rodríguez-Morán, M; Guerrero-Romero, F (2008). "Efficacy and safety of oral magnesium supplementation in the treatment of depression in the elderly with type 2 diabetes: a randomized, equivalent trial". Magnesium research : official organ of the International Society for the Development of Research on Magnesium 21 (4): 218–23. PMID 19271419.
^ Eby Ga, 3rd; Eby, KL (2010). "Magnesium for treatment-resistant depression: a review and hypothesis". Medical hypotheses 74 (4): 649–660. doi:10.1016/j.mehy.2009.10.051. PMID 19944540.
^ George A. Eby; Karen L. Eby (2006). "Rapid recovery from major depression using magnesium treatment". Medical hypotheses 67 (2): 362–370. doi:10.1016/j.mehy.2006.01.047.
^ Sara A. Chacko, MPH, Yiqing Song, MD, SCD, Lauren Nathan, MD, Lesley Tinker, PHD, Ian H. de Boer, MD, Fran Tylavsky, DRPH, Robert Wallace, MD and Simin Liu, MD, SCD1 (2009). "Relations of Dietary Magnesium Intake to Biomarkers of Inflammation and Endothelial Dysfunction in an Ethnically Diverse Cohort of Postmenopausal Women". Diabetes Care 33 (2): 304–310. doi:10.1016/j.mehy.2006.01.047.

外部リンク

マグネシウム解説 -「健康食品」の安全性・有効性情報（国立健康・栄養研究所）
マグネシウム　理科ねっとわーく（一般公開版） - 科学技術振興機構

wiki en

[Wiki en表示]

Magnesium is a chemical element with symbol Mg and atomic number 12. It is a shiny gray solid which bears a close physical resemblance to the other five elements in the second column (Group 2, or alkaline earth metals) of the periodic table: they each have the same electron configuration in their outer electron shell producing a similar crystal structure.

Magnesium is the ninth most abundant element in the universe.^[4]^[5] It is synthesized in large, aging stars from the sequential addition of three helium nuclei to a carbon nucleus. When such a star explodes as a supernova, much of its magnesium is expelled into the interstellar medium, where it can be recycled into new star systems. Consequently, magnesium is the eighth most abundant element in the Earth's crust^[6] and the fourth most common element in the Earth (below iron, oxygen and silicon), making up 13% of the planet's mass and a large fraction of the planet's mantle. It is the third most abundant element dissolved in seawater, after sodium and chlorine.^[7]

Magnesium only occurs naturally in combination with other elements, where it invariably has a +2 oxidation state. The free element (metal) can be produced artificially, and is highly reactive (though once produced, it is coated in a thin layer of oxide, which partly inhibits this reactivity — see passivation). The free metal burns with a characteristic brilliant-white light, making it a useful ingredient in flares. The metal is now obtained mainly by electrolysis of magnesium salts obtained from brine. In commerce, the chief use for the metal is as an alloying agent to make aluminium-magnesium alloys, sometimes called magnalium or magnelium. Since magnesium is less dense than aluminium, this alloy is prized for its properties of lightness combined with strength.

Magnesium is the eleventh most abundant element by mass in the human body. Its ions are essential to all cells. They interact with polyphosphate compounds such as ATP, DNA, and RNA. Hundreds of enzymes require magnesium ions to function. Magnesium compounds are used medicinally as common laxatives, antacids (e.g., milk of magnesia), and to stabilize abnormal nerve excitation or blood vessel spasm such as in eclampsia. Magnesium ions are sour to the taste, and in low concentrations they help impart a natural tartness to fresh mineral waters. Magnesium is the metallic ion at the center of chlorophyll, and is a common additive to fertilizers.^[8]

1 Characteristics
- 1.1 Physical properties
- 1.2 Chemical properties
  - 1.2.1 Flammability
  - 1.2.2 Source of light
- 1.3 Occurrence
2 Forms
- 2.1 Alloy
  - 2.1.1 Corrosion
  - 2.1.2 High-temperature creep and flammability
- 2.2 Compounds
- 2.3 Isotopes
3 Production
4 History
5 Uses as a metal
- 5.1 Aircraft
- 5.2 Automotive
- 5.3 Electronics
- 5.4 Other
- 5.5 Safety precautions
6 Uses in compounds
7 Biological roles
- 7.1 Mechanism of action
- 7.2 Dietary sources, recommended intake, and supplementation
- 7.3 Metabolism
- 7.4 Detection in serum and plasma
- 7.5 Deficiency
- 7.6 Therapy
- 7.7 Overdose
- 7.8 Function in plants
8 See also
9 Notes
10 References
11 External links

Characteristics

Physical properties

Elemental magnesium is a gray-white lightweight metal, two-thirds the density of aluminium. It tarnishes slightly when exposed to air, although, unlike the other alkali metals, an oxygen-free environment is unnecessary for storage because magnesium is protected by a thin layer of oxide that is fairly impermeable and difficult to remove. Magnesium has both the lowest melting and the lowest boiling points of any of the alkali earth metals, at 923 K (1,202 °F) and 1,363 K (1,994 °F), respectively.^[9]

Magnesium reacts with water at room temperature, though it reacts much more slowly than the similar earth alkali metal calcium. When submerged in water, hydrogen bubbles almost unnoticeably begin to form on the surface of the metal—though, if powdered, it reacts much more rapidly. The reaction occurs faster with higher temperatures (see precautions). Magnesium's ability to react with water can be harnessed to produce energy and run a magnesium-based engine.

Magnesium also reacts exothermically with most acids, such as hydrochloric acid (HCl). This reaction with HCl produces the chloride of the metal and releases hydrogen gas (just as when HCl reacts with aluminium, zinc, and many other metals).

Chemical properties

Flammability

Magnesium is a highly flammable metal, especially when powdered or shaved into thin strips; (it is, however, difficult to ignite in mass or bulk). Flame temperatures of magnesium and magnesium alloys can reach 3,100 °C (3,370 K; 5,610 °F),^[10] although flame height above the burning metal is usually less than 300 mm (12 in).^[11] Once ignited, it is difficult to extinguish, being able to burn in nitrogen (forming magnesium nitride), carbon dioxide (forming magnesium oxide, and carbon) and water (forming magnesium oxide and hydrogen). This property was used in incendiary weapons used in the firebombing of cities in World War II, the only practical civil defense being to smother a burning flare under dry sand to exclude the atmosphere. Magnesium may also be used as an ignition source for thermite, a mixture of aluminium and iron oxide powder that is otherwise difficult to ignite.

Source of light

On burning in air, magnesium produces a brilliant-white light that includes strong ultraviolet. Thus, magnesium powder (flash powder) was used as a source of illumination in the early days of photography. Later, magnesium ribbon was used in electrically ignited flashbulbs. Magnesium powder is used in the manufacture of fireworks and marine flares where a brilliant white light is required.

Occurrence

Magnesium is the eighth-most-abundant element in the Earth's crust by mass and tied in seventh place with iron in terms of molarity.^[6] It is found in large deposits of magnesite, dolomite, and other minerals, and in mineral waters, where magnesium ion is soluble.

Although magnesium is found in over 60 minerals, only dolomite, magnesite, brucite, carnallite, talc, and olivine are of commercial importance.

The Mg2+
cation is the second-most-abundant cation in seawater (occurring at about 12% of the mass of sodium there), which makes seawater and sea-salt an attractive commercial source of Mg. To extract the magnesium, calcium hydroxide is added to seawater to form magnesium hydroxide precipitate.

MgCl
2 + Ca(OH)
2 → Mg(OH)
2 + CaCl
2

Magnesium hydroxide (brucite) is insoluble in water, so it can be filtered out and reacted with hydrochloric acid to obtain concentrated magnesium chloride.

Mg(OH)
2 + 2 HCl → MgCl
2 + 2 H
2O

From magnesium chloride, electrolysis produces magnesium.

Forms

Alloy

As of 2013, magnesium alloy consumption was less than one million tons per year, compared with 50 million tons of aluminum alloys. Its use has been historically limited by its tendency to corrode, high-temperature creep, and flammability.^[12]

Corrosion

The presence of iron, nickel, copper, and cobalt strongly activates corrosion. This is due to their low solid solubility limits (above a very small percentage, they precipitate out as intermetallic compounds) and because they behave as active cathodic sites that reduce water and cause the loss of magnesium.^[12] Reducing the quantity of these metals improves corrosion resistance. Sufficient manganese overcomes the corrosive effects of iron. This requires precise control over composition, increasing costs.^[12] Adding a cathodic poison captures atomic hydrogen within the structure of a metal. This prevents the formation of free hydrogen gas, which is required for corrosive chemical processes. The addition of about one-third of a percent of arsenic reduces its corrosion rate in a salt solution by a factor of nearly ten.^[12]^[13]

High-temperature creep and flammability

Research and development eliminated magnesium's tendency toward high-temperature creep by inclusion of scandium and gadolinium. Flammability was greatly reduced by introducing a small amount of calcium into the mix.^[12]

Compounds

Magnesium forms a variety of industrially and biologically important compounds, including magnesium carbonate, magnesium chloride, magnesium citrate, magnesium hydroxide (milk of magnesia), magnesium oxide, magnesium sulfate, and magnesium sulfate heptahydrate (Epsom salts).

Isotopes

Magnesium has three stable isotopes: 24
Mg, 25
Mg and 26
Mg. All are present in significant amounts (see table of isotopes above). About 79% of Mg is 24
Mg. The isotope 28
Mg is radioactive and in the 1950s to 1970s was made commercially by several nuclear power plants for use in scientific experiments. This isotope has a relatively short half-life (21 hours) and so its use was limited by shipping times.

26
Mg has found application in isotopic geology, similar to that of aluminium. 26
Mg is a radiogenic daughter product of 26
Al, which has a half-life of 717,000 years. Large enrichments of stable 26
Mg have been observed in the Ca-Al-rich inclusions of some carbonaceous chondrite meteorites. The anomalous abundance of 26
Mg is attributed to the decay of its parent 26
Al in the inclusions. Therefore, the meteorite must have formed in the solar nebula before the 26
Al had decayed. Hence, these fragments are among the oldest objects in the solar system and have preserved information about its early history.

It is conventional to plot 26
Mg/24
Mg against an Al/Mg ratio. In an isochron dating plot, the Al/Mg ratio plotted is27
Al/24
Mg. The slope of the isochron has no age significance, but indicates the initial 26
Al/27
Al ratio in the sample at the time when the systems were separated from a common reservoir.

Production

Country	2011 production (tonnes)^[14]
China	661,000
U.S.^{[note 1]}	63,500
Russia	37,000
Israel	30,000
Kazakhstan	21,000
Brazil	16,000
Ukraine	2,000
Serbia	1,500
Total	832,000

Magnesium sheets and ingots

China is the dominant supplier of magnesium, with approximately 80% of the world market share. China is almost completely reliant on the silicothermic Pidgeon process (the reduction of the oxide at high temperatures with silicon, often provided by a ferrosilicon alloy in which the iron is but a spectator in the reactions) to obtain the metal.^[15] The process can also be carried out with carbon at approx 2300 °C:

2MgO
(s) + Si
(s) + 2CaO
(s) → 2Mg
(g) + Ca
2SiO
4(s)

MgO
(s) + C
(s) → Mg
(g) + CO
(g)

In the United States, magnesium is obtained principally with the Dow process, by electrolysis of fused magnesium chloride from brine and sea water. A saline solution containing Mg2+
ions is first treated with lime (calcium oxide) and the precipitated magnesium hydroxide is collected:

Mg2+
(aq) + CaO
(s) + H
2O → Ca2+
(aq) + Mg(OH)
2(s)

The hydroxide is then converted to a partial hydrate of magnesium chloride by treating the hydroxide with hydrochloric acid and heating of the product:

Mg(OH)
2(s) + 2 HCl → MgCl
2(aq) + 2H
2O
(l)

The salt is then electrolyzed in the molten state. At the cathode, the Mg2+
ion is reduced by two electrons to magnesium metal:

Mg2+
+ 2 e− → Mg

At the anode, each pair of Cl−
ions is oxidized to chlorine gas, releasing two electrons to complete the circuit:

2 Cl−
→ Cl
2 (g) + 2 e−

A new process, solid oxide membrane technology, involves the electrolytic reduction of MgO. At the cathode, Mg2+
ion is reduced by two electrons to magnesium metal. The electrolyte is Yttria-stabilized zirconia (YSZ). The anode is a liquid metal. At the YSZ/liquid metal anode O2−
is oxidized. A layer of graphite borders the liquid metal anode, and at this interface carbon and oxygen react to form carbon monoxide. When silver is used as the liquid metal anode, there is no reductant carbon or hydrogen needed, and only oxygen gas is evolved at the anode.^[16] It has been reported that this method provides a 40% reduction in cost per pound over the electrolytic reduction method.^[17] This method is more environmentally sound than others because there is much less carbon dioxide emitted.

The United States has traditionally been the major world supplier of this metal, supplying 45% of world production even as recently as 1995. Today, the US market share is at 7%, with a single domestic producer left, US Magnesium, a Renco Group company in Utah born from now-defunct Magcorp.^[18]

History

The name magnesium originates from the Greek word for a district in Thessaly called Magnesia.^[19] It is related to magnetite and manganese, which also originated from this area, and required differentiation as separate substances. See manganese for this history.

In 1618, a farmer at Epsom in England attempted to give his cows water from a well there. The cows refused to drink because of the water's bitter taste, but the farmer noticed that the water seemed to heal scratches and rashes. The substance became known as Epsom salts and its fame spread. It was eventually recognized as hydrated magnesium sulfate, MgSO
4·7 H
2O.

The metal itself was first produced by Sir Humphry Davy in England in 1808. He used electrolysis on a mixture of magnesia and mercuric oxide.^[20] Antoine Bussy prepared it in coherent form in 1831. Davy's first suggestion for a name was magnium,^[20] but the name magnesium is now used.

Uses as a metal

An unusual application of magnesium as an illumination source while wakeskating in 1931

Magnesium is the third-most-commonly-used structural metal, following iron and aluminium. It has been called the lightest useful metal by The Periodic Table of Videos.^[21]

The main applications of magnesium are, in order: component of aluminium alloys, in die-casting (alloyed with zinc),^[22] to remove sulfur in the production of iron and steel, and the production of titanium in the Kroll process.^[23]

Historically, magnesium was one of the main aerospace construction metals and was used for German military aircraft as early as World War I and extensively for German aircraft in World War II.

The Germans coined the name "Elektron" for magnesium alloy. The term is still used today. The application of magnesium in the commercial aerospace industry was generally restricted to engine-related components, due either to perceived hazards with magnesium parts in the event of fire or to corrosion. Currently, the use of magnesium alloys in aerospace is increasing, mostly driven by the increasing importance of fuel economy and the need to reduce weight.^[24] The development and testing of new magnesium alloys continues, notably Elektron 21, which has successfully undergone extensive aerospace testing for suitability in engine and internal and airframe components.^[25] The European Community runs three R&D magnesium projects in the Aerospace priority of Six Framework Program.

Aircraft

Wright Aeronautical used a magnesium crankcase in the WWII-era Wright Duplex Cyclone aviation engine. This presented a serious problem for the earliest examples of the Boeing B-29 heavy bomber, as engine fires in flight could ignite the engine crankcases, literally "torching" the wing spar apart.^[26]^[27]

Automotive

Mg alloy motorcycle engine blocks

Mercedes-Benz used the alloy Elektron in the body of an early model Mercedes-Benz 300 SLR; these cars ran (with successes) at Le Mans, the Mille Miglia, and other world-class race events in 1955.
Porsche used magnesium alloy frames in the 917/053 that won Le Mans in 1971, and continues to use magnesium alloys for its engine blocks due to the weight advantage.
Volkswagen Group has used magnesium in its engine components for many years.^{[citation needed]}
Mitsubishi Motors also uses magnesium for its paddle shifters.
BMW used magnesium alloy engine blocks in the 2006 325i and 330i models, including an aluminium alloy insert for the cylinder walls and cooling jackets surrounded by a high-temperature magnesium alloy AJ62A.
Chevrolet used the magnesium alloy AE44 in the 2006 Corvette Z06.

Both AJ62A and AE44 are recent developments in high-temperature low-creep magnesium alloys. The general strategy for such alloys is to form intermetallic precipitates at the grain boundaries, for example by adding mischmetal or calcium.^[28] New alloy development and lower costs that make magnesium competitive with aluminium will increase the number of automotive applications.

Electronics

Because of low weight and good mechanical and electrical properties, magnesium is widely used for manufacturing of mobile phones, laptop and tablet computers, cameras, and other electronic components.

Products made of magnesium: firestarter and shavings, sharpener, magnesium ribbon

Other

Magnesium, being readily available and relatively nontoxic, has a variety of uses:

Magnesium is flammable, burning at a temperature of approximately 3,100 °C (3,370 K; 5,610 °F),^[10] and the autoignition temperature of magnesium ribbon is approximately 473 °C (746 K; 883 °F).^[29] It produces intense, bright, white light when it burns. Magnesium's high combustion temperature makes it a useful tool for starting emergency fires. Other uses include flash photography, flares, pyrotechnics, and fireworks sparklers. Magnesium is also often used to ignite thermite or other materials that require a high ignition temperature.

Magnesium firestarter (in left hand), used with a pocket knife and flint to create sparks that ignite the shavings
In the form of turnings or ribbons, to prepare Grignard reagents, which are useful in organic synthesis.
As an additive agent in conventional propellants and the production of nodular graphite in cast iron.
As a reducing agent to separate uranium and other metals from their salts.
As a sacrificial (galvanic) anode to protect boats, underground tanks, pipelines, buried structures, and water heaters.
Alloyed with zinc to produce the zinc sheet used in photoengraving plates in the printing industry, dry-cell battery walls, and roofing.^[22]
As a metal, this element's principal use is as an alloying additive to aluminium with these aluminium-magnesium alloys being used mainly for beverage cans, sports equipment such as golf clubs, fishing reels, and archery bows and arrows.
Specialty, high-grade car wheels of magnesium alloy are called "mag wheels", although the term is often more broadly misapplied to include aluminium wheels. Many car and aircraft manufacturers have made engine and body parts from magnesium.

Safety precautions

The combusting magnesium-bodied Honda RA302 at the 1968 French Grand Prix, after the crash that killed driver Jo Schlesser.

Magnesium metal and its alloys are explosive hazards; they are highly flammable in their pure form when molten or in powder or ribbon form. Burning or molten magnesium metal reacts violently with water. When working with powdered magnesium, safety glasses with welding eye protection are employed, because the bright-white light produced by burning magnesium contains ultraviolet light that can permanently damage the retinas of the eyes.^[30]

Magnesium is capable of reducing water to highly flammable hydrogen gas:^[31]

Mg (s) + 2 H
2O (l) → Mg(OH)
2 (s) + H
2 (g)

As a result, water cannot extinguish magnesium fires. The hydrogen gas produced only intensifies the fire. Dry sand is an effective smothering agent, but only on relatively level and flat surfaces.

Magnesium also reacts with carbon dioxide to form magnesium oxide and carbon:

2 Mg + CO
2 → 2 MgO + C (s)

hence, carbon dioxide fire extinguishers are also ineffective for extinguishing magnesium fires.^[32]

Burning magnesium is usually quenched by using a Class D dry chemical fire extinguisher, or by covering the fire with sand or magnesium foundry flux to remove its air source.

Uses in compounds

Magnesium compounds, primarily magnesium oxide (MgO), are used as a refractory material in furnace linings for producing iron, steel, nonferrous metals, glass, and cement. Magnesium oxide and other magnesium compounds are also used in the agricultural, chemical, and construction industries. Magnesium oxide from calcination is used as an electrical insulator in fire-resistant cables.^[33]

Magnesium reacted with an alkyl halide gives a Grignard reagent, which is a very useful tool for preparing alcohols.

Magnesium salts are frequently included in various foods, fertilizers (magnesium is a component of chlorophyll), and culture media.

Magnesium sulfite is used in the manufacture of paper (sulfite process).

Magnesium phosphate is used to fireproof wood used in construction.

Magnesium hexafluorosilicate is used in mothproofing of textiles.

In the form of turnings or ribbons, Mg is useful in purification of solvents, for example the preparation of super-dry ethanol.

Biological roles

Mechanism of action

Because of the important interaction between phosphate and magnesium ions, magnesium ions are essential to the basic nucleic acid chemistry of life, and thus are essential to all cells of all known living organisms. Over 300 enzymes require the presence of magnesium ions for their catalytic action, including all enzymes utilizing or synthesizing ATP, or those that use other nucleotides to synthesize DNA and RNA. ATP exists in cells normally as a chelate of ATP and a magnesium ion.^[34]

Dietary sources, recommended intake, and supplementation

Examples of food sources of magnesium

Spices, nuts, cereals, cocoa and vegetables are rich sources of magnesium.^[35] Green leafy vegetables such as spinach are also rich in magnesium since they contain chlorophyll.

The UK recommended daily values for magnesium is 300 mg for men and 270 mg for women.^[36] Observations of reduced dietary magnesium intake in modern Western countries compared to earlier generations may be related to food refining and modern fertilizers that contain no magnesium.^[37]

Numerous pharmaceutical preparations of magnesium, as well as magnesium dietary supplements are available. Magnesium oxide, one of the most common forms in magnesium dietary supplements because it has high magnesium content per weight, is the least bioavailable.^[38]^[39]

Metabolism

An adult has 22–26 grams of magnesium,^[40] with 60% in the skeleton, 39% intracellular (20% in skeletal muscle), and 1% extracellular.^[41] Serum levels are typically 0.7–1.0 mmol/L or 1.8–2.4 mEq/L. Serum magnesium levels may be normal even when intracellular magnesium is deficient. The mechanisms for maintaining the magnesium level in the serum are varying gastrointestinal absorption and renal excretion. Intracellular magnesium is correlated with intracellular potassium. Increased magnesium lowers calcium^[42] and can either prevent hypercalcemia or cause hypocalcemia depending on the initial level.^[42] Low and high protein intake inhibit magnesium absorption, as does the amount of phosphate, phytate, and fat in the gut. Excess dietary magnesium is excreted in feces, urine, and sweat.^[37] Magnesium status may be assessed via serum and erythrocyte magnesium concentrations coupled with urinary and fecal magnesium content, but intravenous magnesium loading tests are more accurate and practical.^[43] A retention of 20% or more of the injected amount indicates deficiency.^[44] No biomarker has been established for magnesium.^[45]

Detection in serum and plasma

Magnesium concentrations in plasma or serum may be measured to monitor for efficacy and safety in those receiving the drug therapeutically, to confirm the diagnosis in potential poisoning victims or to assist in the forensic investigation in a case of fatal overdosage. The newborn children of mothers having received parenteral magnesium sulfate during labor may exhibit toxicity with normal serum magnesium levels.^[46]

Deficiency

Magnesium deficiency (hypomagnesemia) is common: it is found in 2.5–15% of the general population.^[47] The primary cause of deficiency is decreased dietary intake: only 32% of people in the United States meet the recommended daily allowance.^[48] Other causes are increased renal or gastrointestinal loss, an increased intracellular shift, and proton-pump inhibitor antacid therapy. Most are asymptomatic, but symptoms referable to neuromuscular, cardiovascular, and metabolic dysfunction may occur.^[47] Alcoholism is often associated with magnesium deficiency. Chronically low serum magnesium levels are associated with metabolic syndrome, diabetes mellitus type 2, fasciculation, and hypertension.^[49]

Therapy

Intravenous magnesium is recommended by the ACC/AHA/ESC 2006 Guidelines for Management of Patients With Ventricular Arrhythmias and the Prevention of Sudden Cardiac Death for patients with ventricular arrhythmia associated with torsades de pointes who present with long QT syndrome; and for the treatment of patients with digoxin induced arrhythmias.^[50]
Magnesium is the drug of choice in the management of pre-eclampsia and eclampsia.^[51]^[52]
Hypomagnesemia, including that caused by alcoholism, is reversible by oral or parenteral magnesium administration depending on the degree of deficiency.^[53]
There is limited evidence that magnesium supplementation may play a role in the prevention and treatment of migraine.^[54]
Oral magnesium may be therapeutic for restless leg syndrome.^[55]

Sorted by type of magnesium salt, other therapeutic applications include:

Magnesium sulfate, as the heptahydrate called Epsom salts, is used as bath salts, as a laxative, and as a highly soluble fertilizer.^[56]
Magnesium hydroxide, suspended in water, is used in milk of magnesia antacids and laxatives.
Magnesium chloride, oxide, gluconate, malate, orotate, glycinate and citrate are all used as oral magnesium supplements.
Magnesium borate, magnesium salicylate, and magnesium sulfate are used as antiseptics.
Magnesium bromide is used as a mild sedative (this action is due to the bromide, not the magnesium).
Magnesium stearate is a slightly flammable white powder with lubricating properties. In pharmaceutical technology, it is used in the manufacturing of numerous kinds of tablets to prevent the tablets from sticking to the equipment during the tablet compression process (i.e., when the tablet's substance is pressed into tablet form).
Magnesium carbonate powder is used by athletes such as gymnasts, weightlifters, and climbers to eliminate moisture and improving the grip on a gymnastic apparatus, lifting bar, and climbing rocks.
Magnesium L-threonate is used as a dietary magnesium supplement

Overdose

Overdose from dietary sources alone is unlikely because excess magnesium in the blood is promptly filtered by the kidneys.^[47] Overdose with magnesium tablets is possible in the presence of impaired renal function. There is a single case report of hypermagnesemia in a woman with normal renal function using high doses of magnesium salts for catharsis.^[57] The most common symptoms of overdose are nausea, vomiting and diarrhea; other symptoms include hypotension, confusion, slowed heart and respiratory rate, deficiencies of other minerals, coma, cardiac arrhythmia, and death from cardiac arrest.^[42]

Function in plants

Plants require magnesium to synthesize chlorophyll, essential for photosynthesis. Magnesium in the center of the porphyrin ring in chlorophyll functions in a manner similar to the iron in the center of the porphyrin ring in heme. Magnesium deficiency in plants causes late-season yellowing between leaf veins, especially in older leaves, and can be corrected by applying to the soil either Epsom salts (which is rapidly leached), or crushed dolomitic limestone.

Notes

^ Capacity. Production figures withheld to avoid disclosing company proprietary data.

References

^ Conventional Atomic Weights 2013. Commission on Isotopic Abundances and Atomic Weights
^ Standard Atomic Weights 2013. Commission on Isotopic Abundances and Atomic Weights
^ Bernath, P. F., Black, J. H., & Brault, J. W. (1985). "The spectrum of magnesium hydride" (PDF). Astrophysical Journal 298: 375. Bibcode:1985ApJ...298..375B. doi:10.1086/163620.
^ Housecroft, C. E.; Sharpe, A. G. (2008). Inorganic Chemistry (3rd ed.). Prentice Hall. pp. 305–306. ISBN 978-0131755536.
^ Ash, Russell (2005). The Top 10 of Everything 2006: The Ultimate Book of Lists. Dk Pub. ISBN 0-7566-1321-3.
^ ^a ^b "Abundance and form of the most abundant elements in Earth's continental crust" (PDF). Retrieved 15 February 2008.
^ Anthoni, J Floor (2006). "The chemical composition of seawater". seafriends.org.nz.
^ "Magnesium in health". magnesium.com. Retrieved 10 October 2013.
^ http://www.ptable.com/#Property/State
^ ^a ^b Dreizin, Edward L.; Berman, Charles H. & Vicenzi, Edward P. (2000). "Condensed-phase modifications in magnesium particle combustion in air". Scripta Materialia 122: 30–42. doi:10.1016/S0010-2180(00)00101-2.
^ DOE Handbook – Primer on Spontaneous Heating and Pyrophoricity. U.S. Department of Energy. December 1994. p. 20. DOE-HDBK-1081-94. Retrieved 21 December 2011.
^ ^a ^b ^c ^d ^e Dodson, Brian (29 August 2013). "Stainless magnesium breakthrough bodes well for manufacturing industries". Gizmag.com. Retrieved 29 August 2013.
^ Birbilis, N.; Williams, G.; Gusieva, K.; Samaniego, A.; Gibson, M. A.; McMurray, H. N. (2013). "Poisoning the corrosion of magnesium". Electrochemistry Communications 34: 295. doi:10.1016/j.elecom.2013.07.021. edit
^ "2011 Minerals Yearbook, Magnesium" (PDF). USGS. Retrieved 26 April 2013.
^ "Magnesium Overview". China magnesium Corporation. Retrieved 8 May 2013.
^ Pal, Uday B.; Powell, Adam C. (2007). "The Use of Solid-Oxide-Membrane Technology for Electrometallurgy". JOM 59 (5): 44–49. Bibcode:2007JOM....59e..44P. doi:10.1007/s11837-007-0064-x.
^ Derezinski, Steve (12 May 2011). "Solid Oxide Membrane (SOM) Electrolysis of Magnesium: Scale-Up Research and Engineering for Light-Weight Vehicles" (PDF). MOxST. Retrieved 27 May 2013.
^ Vardi, Nathan (22 February 2007). "Man With Many Enemies". Forbes.com. Retrieved 26 June 2006.
^ "Magnesium: historical information". webelements.com. Retrieved 9 October 2014.
^ ^a ^b Davy, H. (1808). "Electro-chemical researches on the decomposition of the earths; with observations on the metals obtained from the alkaline earths, and on the amalgam procured from ammonia". Philosophical Transactions of the Royal Society of London 98: 333–370. Bibcode:1808RSPT...98..333D. doi:10.1098/rstl.1808.0023. JSTOR 107302.
^ "Magnesium Video – The Periodic Table of Videos – University of Nottingham". Retrieved 23 February 2011.
^ ^a ^b Baker, Hugh D. R.; Avedesian, Michael (1999). Magnesium and magnesium alloys. Materials Park, OH: Materials Information Society. p. 4. ISBN 0-87170-657-1.
^ Ketil Amundsen; Terje Kr. Aune; Per Bakke; Hans R. Eklund; Johanna Ö. Haagensen; Carlos Nicolas et al. (2002). "Magnesium". Ullmann's Encyclopedia of Industrial Chemistry. Wiley-VCH. doi:10.1002/14356007.a15_559. ISBN 3527306730.
^ Aghion, E.; Bronfin, B. (2000). "Magnesium Alloys Development towards the 21st Century". Materials Science Forum. 350–351: 19–30. doi:10.4028/www.scientific.net/MSF.350-351.19.
^ Bronfin, B et al. (2007). "Elektron 21 specification". In Kainer, Karl. Magnesium: Proceedings of the 7th International Conference on Magnesium Alloys and Their Applications. Weinheim, Germany: Wiley. p. 23. ISBN 978-3-527-31764-6.
^ Dorr, Robert F (15 September 2012). Mission to Tokyo: The American Airmen Who Took the War to the Heart of Japan. pp. 40–41. ISBN 9781610586634.
^ AAHS Journal. 44–45. American Aviation Historical Society. 1999.
^ Luo, Alan A. & Powell, Bob R. (2001). "Tensile and Compressive Creep of Magnesium-Aluminum-Calcium Based Alloys" (PDF). Materials & Processes Laboratory, General Motors Research & Development Center. Archived from the original (PDF) on 28 September 2007. Retrieved 21 August 2007.
^ "Magnesium (Powder)". International Programme on Chemical Safety (IPCS). IPCS INCHEM. April 2000. Retrieved 21 December 2011.
^ "Science Safety: Chapter 8". Government of Manitoba. Retrieved 21 August 2007.
^ "Chemistry : Periodic Table : magnesium : chemical reaction data". webelements.com. Retrieved 26 June 2006.
^ "Demo Lab: Reaction Of Magnesium Metal With Carbon Dioxide". Retrieved 26 June 2006.
^ Linsley, Trevor (2011). "Properties of conductors and insulators". Basic Electrical Installation Work. p. 362. ISBN 978-0-08-096628-1.
^ Romani, Andrea, M.P. (2013). "Chapter 3. Magnesium in Health and Disease". In Astrid Sigel; Helmut Sigel; Roland K. O. Sigel. Interrelations between Essential Metal Ions and Human Diseases. Metal Ions in Life Sciences 13. Springer. pp. 49–79. doi:10.1007/978-94-007-7500-8_3.
^ "Dietary Supplement Fact Sheet: Magnesium". Office of Dietary Supplements.
^ "Vitamins and minerals – Others – NHS Choices". Nhs.uk. 26 November 2012. Retrieved 19 September 2013.
^ ^a ^b Wester PO (1987). "Magnesium". Am. J. Clin. Nutr. 45 (5 Suppl): 1305–12. PMID 3578120.
^ Firoz M; Graber M (2001). "Bioavailability of US commercial magnesium preparations". Magnes Res 14 (4): 257–62. PMID 11794633.
^ Lindberg JS; Zobitz MM; Poindexter JR; Pak CY (1990). "Magnesium bioavailability from magnesium citrate and magnesium oxide". J Am Coll Nutr 9 (1): 48–55. doi:10.1080/07315724.1990.10720349. PMID 2407766.
^ Saris NE, Mervaala E, Karppanen H, Khawaja JA, Lewenstam A (April 2000). "Magnesium. An update on physiological, clinical and analytical aspects.". Clin Chim Acta 294 (1-2): 1–26. PMID 10727669.
^ "Dietary Supplement Fact Sheet:Magnesium". US National Institute of Health.
^ ^a ^b ^c "Magnesium | University of Maryland Medical Center". Umm.edu. 7 May 2013. Retrieved 19 September 2013.
^ Arnaud MJ (2008). "Update on the assessment of magnesium status". Br. J. Nutr. 99 Suppl 3: S24–36. doi:10.1017/S000711450800682X. PMID 18598586.
^ Rob PM; Dick K; Bley N; Seyfert T; Brinckmann C; Höllriegel V et al. (1999). "Can one really measure magnesium deficiency using the short-term magnesium loading test?". J. Intern. Med. 246 (4): 373–378. doi:10.1046/j.1365-2796.1999.00580.x. PMID 10583708.
^ Franz KB (2004). "A functional biological marker is needed for diagnosing magnesium deficiency". J Am Coll Nutr 23 (6): 738S–41S. doi:10.1080/07315724.2004.10719418. PMID 15637224.
^ Baselt, R. (2008). Disposition of Toxic Drugs and Chemicals in Man (8th ed.). Biomedical Publications. pp. 875–7. ISBN 0-9626523-7-7.
^ ^a ^b ^c Ayuk J., Gittoes N.J. (Mar 2014). "Contemporary view of the clinical relevance of magnesium homeostasis". Annals of Clinical Biochemistry 51 (2): 179–88. doi:10.1177/0004563213517628.
^ "Lack Energy? Maybe It's Your Magnesium Level". United States Department of Agriculture. Retrieved 18 September 2008. Last paragraph
^ Geiger H; Wanner C (2012). "Magnesium in disease" (PDF). Clin Kidney J 5 (Suppl 1): i25–i38. doi:10.1093/ndtplus/sfr165.
^ Zipes DP; Camm AJ; Borggrefe M et al. (2012). "ACC/AHA/ESC 2006 Guidelines for Management of Patients With Ventricular Arrhythmias and the Prevention of Sudden Cardiac Death: a report of the American College of Cardiology/American Heart Association Task Force and the European Society of Cardiology Committee for Practice Guidelines (writing committee to develop Guidelines for Management of Patients With Ventricular Arrhythmias and the Prevention of Sudden Cardiac Death): developed in collaboration with the European Heart Rhythm Association and the Heart Rhythm Society" (PDF). Circulation 114 (10): e385–e484. doi:10.1161/CIRCULATIONAHA.106.178233. PMID 16935995.
^ James MF (2010). "Magnesium in obstetrics". Best Pract Res Clin Obstet Gynaecol 24 (3): 327–337. doi:10.1016/j.bpobgyn.2009.11.004. PMID 20005782.
^ Euser, A. G.; Cipolla, M. J. (2009). "Magnesium Sulfate for the Treatment of Eclampsia: A Brief Review". Stroke 40 (4): 1169–1175. doi:10.1161/STROKEAHA.108.527788. PMC 2663594. PMID 19211496.
^ Giannini, A. J. (1997). Drugs of Abuse (Second ed.). Los Angeles: Physicians Management Information Co. ISBN 0-87489-499-9.
^ Teigen L, Boes CJ (2014). "An evidence-based review of oral magnesium supplementation in the preventive treatment of migraine". Cephalalgia (Review). doi:10.1177/0333102414564891. PMID 25533715. There is a strong body of evidence demonstrating a relationship between magnesium status and migraine. Magnesium likely plays a role in migraine development at a biochemical level, but the role of oral magnesium supplementation in migraine prophylaxis and treatment remains to be fully elucidated. The strength of evidence supporting oral magnesium supplementation is limited at this time.
^ Trenkwalder C, Hening WA, Montagna P, Oertel WH, Allen RP, Walters AS, Costa J, Stiasny-Kolster K, Sampaio C (2008). "Treatment of restless legs syndrome: an evidence-based review and implications for clinical practice". Mov. Disord. 23 (16): 2267–302. doi:10.1002/mds.22254. PMID 18925578.
^ Gowariker, Vasant; Krishnamurthy, V.P.; Gowariker, Sudha; Dhanorkar, Manik; Paranjape, Kalyani (8 April 2009). The Fertilizer Encyclopedia. p. 224. ISBN 9780470431764.
^ Kontani M; Hara A; Ohta S; Ikeda T (2005). "Hypermagnesemia induced by massive cathartic ingestion in an elderly woman without pre-existing renal dysfunction". Intern. Med. 44 (5): 448–452. doi:10.2169/internalmedicine.44.448. PMID 15942092.

External links

Magnesium at The Periodic Table of Videos (University of Nottingham)
Chemistry in its element podcast (MP3) from the Royal Society of Chemistry's Chemistry World: Magnesium
"Magnesium – a versatile and often overlooked element: new perspectives with a focus on chronic kidney disease". Clin Kidney J 5 (Suppl 1). February 2012. ]

UpToDate Contents

全文を閲覧するには購読必要です。 To read the full text you will need to subscribe.

1. 低マグネシウム血症の評価および治療 evaluation and treatment of hypomagnesemia
2. マグネシウムバランスの調節 regulation of magnesium balance
3. マグネシウム欠乏の臨床症状 clinical manifestations of magnesium depletion
4. 高マグネシウム血症の原因および治療 causes and treatment of hypermagnesemia
5. 低マグネシウム血症の原因 causes of hypomagnesemia

English Journal

Some physicochemical characteristics of pinus (Pinus halepensis Mill., Pinus pinea L., Pinus pinaster and Pinus canariensis) seeds from North Algeria, their lipid profiles and volatile contents.

Kadri N1, Khettal B2, Aid Y2, Kherfellah S3, Sobhi W2, Barragan-Montero V4.
Food chemistry.Food Chem.2015 Dec 1;188:184-92. doi: 10.1016/j.foodchem.2015.04.138. Epub 2015 May 1.
Physicochemical characteristics of seeds of some pinus species (Pinus halepensis Mill., Pinus pinea L., Pinus pinaster and Pinus canariensis) grown in North Algeria were determined. The results showed that the seeds consist of 19.8-36.7% oil, 14.25-26.62% protein, 7.8-8.6% moisture. Phosphorus, pota
PMID 26041181

Improvement of migraine symptoms with a proprietary supplement containing riboflavin, magnesium and Q10: a randomized, placebo-controlled, double-blind, multicenter trial.

Gaul C1, Diener HC, Danesch U; Migravent® Study Group.
The journal of headache and pain.J Headache Pain.2015 Dec;16(1):516. doi: 10.1186/s10194-015-0516-6. Epub 2015 Apr 3.
BACKGROUND: Non-medical, non-pharmacological and pharmacological treatments are recommended for the prevention of migraine. The purpose of this randomized double-blind placebo controlled, multicenter trial was to evaluate the efficacy of a proprietary nutritional supplement containing a fixed combin
PMID 25916335

Effect of germination on the physicochemical and antioxidant characteristics of rice flour from three rice varieties from Nigeria.

Chinma CE1, Anuonye JC1, Simon OC1, Ohiare RO1, Danbaba N2.
Food chemistry.Food Chem.2015 Oct 15;185:454-8. doi: 10.1016/j.foodchem.2015.04.010. Epub 2015 Apr 9.
This study determined the effect of germination (48h) on the physicochemical and antioxidant characteristics of rice flour from three rice varieties from Nigeria. Local rice varieties (Jamila, Jeep and Kwandala) were evaluated and compared to an improved variety (MR 219). Physicochemical and antioxi
PMID 25952893

Chlorination decomposition of struvite and recycling of its product for the removal of ammonium-nitrogen from landfill leachate.

Huang H1, Huang L2, Zhang Q3, Jiang Y2, Ding L2.
Chemosphere.Chemosphere.2015 Oct;136:289-96. doi: 10.1016/j.chemosphere.2014.10.078. Epub 2014 Nov 20.
Struvite (MgNH4PO4⋅6H2O) precipitation is a promising method for ammonium (NH4(+)) removal from the wastewater. However, the high cost incurred with the use of magnesium and phosphate sources hinders the successful application of this method. This paper presents a novel recycling technology of str
PMID 25465950

Japanese Journal

Goshajinkigan, a Traditional Japanese Medicine, Prevents Oxaliplatin-Induced Acute Peripheral Neuropath by Suppressing Functional Alteration of TRP Channels in Rat

Mizuno Keita,Kono Toru,Suzuki Yasuyuki [他]
Journal of pharmacological sciences 125(1), 91-98, 2014-05
NAID 40020066510

Thermal Stability and Transition Behavior of Nanoclusters during Two-Step Aging at 250°C in Al-Mg-Si(-Cu) Alloys

Kim JaeHwang,Kim SeongNyeong,Kobayashi Equo [他]
Materials transactions 55(5), 768-773, 2014-05
NAID 40020051271

マグネシウム合金 : 車体軽量化に貢献する金属系マテリアル (特集 2020年代に求められるマテリアル高速省エネ鉄道,リニア中央新幹線,大規模補修など鉄道産業のこれから,求められるマテリアル)

河村能人
Material stage 14(1), 15-18, 2014-04
NAID 40020064186

マグネシウム合金製円管の衝撃エネルギー吸収特性

上田哲也,長尾昌樹,池尾直子 [他]
日本金属学会誌 = Journal of the Japan Institute of Metals and Materials 78(4), 142-148, 2014-04
NAID 40020058009

Related Pictures

★リンクテーブル★

リンク元	「マグネシウム」「Mg」
拡張検索	「magnesium pidolate」「serum magnesium level」「magnesium chloride」

「マグネシウム」

Magnesium, ₁₂Mg
	Spectral lines of magnesium
General properties
Name, symbol	magnesium, Mg
Appearance	shiny grey solid
Pronunciation	/mæɡˈniːziəm/; mag-NEE-zee-əm
Magnesium in the periodic table
	sodium ← magnesium → aluminium
Atomic number	12
Standard atomic weight (Ar)	24.305 (24.304–24.307)
Element category	alkaline earth metal
Group, block	group 2 (alkaline earth metals), s-block
Period	period 3
Electron configuration	[Ne] 3s2
per shell	2, 8, 2
Physical properties
Phase	solid
Melting point	923 K (650 °C, 1202 °F)
Boiling point	1363 K (1091 °C, 1994 °F)
Density near r.t.	1.738 g/cm3
when liquid, at m.p.	1.584 g/cm3
Heat of fusion	8.48 kJ/mol
Heat of vaporization	128 kJ/mol
Molar heat capacity	24.869 J/(mol·K)
Atomic properties
Oxidation states	+2, +1 (a strongly basic oxide)
Electronegativity	Pauling scale: 1.31
Ionization energies	1st: 737.7 kJ/mol; 2nd: 1450.7 kJ/mol; 3rd: 7732.7 kJ/mol; (more)
Atomic radius	empirical: 160 pm
Covalent radius	141±7 pm
Van der Waals radius	173 pm
Miscellanea
Crystal structure	hexagonal close-packed (hcp)
Speed of sound thin rod	4940 m/s (at r.t.) (annealed)
Thermal expansion	24.8 µm/(m·K) (at 25 °C)
Thermal conductivity	156 W/(m·K)
Electrical resistivity	43.9 nΩ·m (at 20 °C)
Magnetic ordering	paramagnetic
Young's modulus	45 GPa
Shear modulus	17 GPa
Bulk modulus	45 GPa
Poisson ratio	0.290
Mohs hardness	1–2.5
Brinell hardness	44–260 MPa
CAS Registry Number	7439-95-4
History
Naming	after Magnesia, Greece
Discovery	Joseph Black (1755)
First isolation	Humphry Davy (1808)
Most stable isotopes
	Main article: Isotopes of magnesium
	view; talk; edit; · references

外見
	銀白色; ; ; マグネシウムのスペクトル線
一般特性
名称, 記号, 番号	マグネシウム, Mg, 12
分類	卑金属
族, 周期, ブロック	2, 3, s
原子量	24.3050(6)
電子配置	[Ne] 3s2
電子殻	2, 8, 2（画像）
物理特性
相	固体
密度（室温付近）	1.738 g/cm3
融点での液体密度	1.584 g/cm3
融点	923 K, 650 °C, 1202 °F
沸点	1363 K, 1091 °C, 1994 °F
融解熱	8.48 kJ/mol
蒸発熱	128 kJ/mol
熱容量	(25 °C) 24.869 J/(mol·K)
蒸気圧
原子特性
酸化数	2, 1; (強塩基性酸化物)
電気陰性度	1.31（ポーリングの値）
イオン化エネルギー; （詳細）	第1： 737.7 kJ/mol
	第2： 1450.7 kJ/mol
	第3： 7732.7 kJ/mol
原子半径	160 pm
共有結合半径	141 ± 7 pm
ファンデルワールス半径	173 pm
その他
結晶構造	六方晶系
磁性	常磁性
電気抵抗率	(20 °C) 43.9 nΩ·m
熱伝導率	(300 K) 156 W/(m·K)
熱膨張率	(25 °C) 24.8 µm/(m·K)
音の伝わる速さ; （微細ロッド）	(r.t.) (annealed); 4940 m/s
ヤング率	45 GPa
剛性率	17 GPa
体積弾性率	45 GPa
ポアソン比	0.290
モース硬度	2.5
ブリネル硬度	260 MPa
CAS登録番号	7439-95-4
最安定同位体
	詳細はマグネシウムの同位体を参照
	表示

　　[★]

英: magnesium Mg
関: 硫酸マグネシウム magnesium sulfate。電解質異常。; クエン酸マグネシウム緩下剤

基準値

血漿/血清：1.5-2mEq/L 1.8-2.4mg/dl, 1.5-2.0mEq/L 1.7-2.4mg/dl(HIM.2372), 1.7-2.6mg/dL(臨床検査データブック2017-2018.194)

単位の変換

1mg/dL = 0.4114mEq/L

https://www.zm.emb-japan.go.jp/ja/health/111100Clinical%20Chemistory%20Conversion.pdf

臨床関連

低マグネシウム血症：頻脈、不整脈、振戦、テタニー、筋力低下、虚血性心疾患などの心臓血管障害の誘発。
高マグネシウム血症：悪心、嘔吐、食欲不振、徐脈、起立性低血圧、傾眠、心停止。

参考

1. [charged] Regulation of magnesium balance - uptodate [1]

腎臓におけるマグネシウムの再吸収メカニズムがよく分かる

「Mg」

　　[★] マグネシウム magnesium 　

「magnesium pidolate」

　　[★]

ピドロ酸マグネシウム

関: pyroglutamate、pyroglutamic acid、pyrrolidonecarboxylic acid

「serum magnesium level」

　　[★]

血清マグネシウム値、血清マグネシウムレベル

関: magnesium

「magnesium chloride」

　　[★] 塩化マグネシウム

関: MgCl2

[1] Bernath, P. F., Black, J. H., & Brault, J. W. (1985). "The spectrum of magnesium hydride". Astrophysical Journal 298: 375.

[2] ttp://www.encyclo.co.uk/webster/M/6

[3] 2.7 マグネシウム（Mg） (PDF) 東北経済産業局

[4] 日本マグネシウム協会

[5] [1]

[6] 桜井弘氏講演生体元素と医薬品の開発（第一回）講演録

[7] 8.マグネシウムの再吸収異常と生活習慣病との関連性について研究内容の紹介紹介ページのひとつ

[8] 専門領域の最新情報　最新栄養学　第8版：建帛社

[9] 「健康食品」の安全性・有効性情報国立健康・栄養研究所

[10] 製品安全データシート 0.01mol/1(M/100)-塩化マグネシウム溶液キシダ化学株式会社

[11] 第６次改定日本人の栄養所要量について

[12] マグネシウム摂取と大腸がんとの関連について JPHC Study 多目的コホート研究独立行政法人国立がん研究センター

[13] マグネシウム国立健康・栄養研究所

[14] マグネシウム摂取不足の解消こそが糖尿病の増加を抑える日経メディカルオンライン 2012年5月22日

[15] マグネシウムはNMDA受容体の活性をブロックするモジュレータ(英)として働く。

[16] Barragán-Rodríguez, L; Rodríguez-Morán, M; Guerrero-Romero, F (2008). "Efficacy and safety of oral magnesium supplementation in the treatment of depression in the elderly with type 2 diabetes: a randomized, equivalent trial". Magnesium research : official organ of the International Society for the Development of Research on Magnesium 21 (4): 218–23. PMID 19271419.

[17] Eby Ga, 3rd; Eby, KL (2010). "Magnesium for treatment-resistant depression: a review and hypothesis". Medical hypotheses 74 (4): 649–660. doi:10.1016/j.mehy.2009.10.051. PMID 19944540.

[18] George A. Eby; Karen L. Eby (2006). "Rapid recovery from major depression using magnesium treatment". Medical hypotheses 67 (2): 362–370. doi:10.1016/j.mehy.2006.01.047.

[19] Sara A. Chacko, MPH, Yiqing Song, MD, SCD, Lauren Nathan, MD, Lesley Tinker, PHD, Ian H. de Boer, MD, Fran Tylavsky, DRPH, Robert Wallace, MD and Simin Liu, MD, SCD1 (2009). "Relations of Dietary Magnesium Intake to Biomarkers of Inflammation and Endothelial Dysfunction in an Ethnically Diverse Cohort of Postmenopausal Women". Diabetes Care 33 (2): 304–310. doi:10.1016/j.mehy.2006.01.047.

[15] Capacity. Production figures withheld to avoid disclosing company proprietary data.

[CIAAW-1] Conventional Atomic Weights 2013. Commission on Isotopic Abundances and Atomic Weights

[IUPAC-2] Standard Atomic Weights 2013. Commission on Isotopic Abundances and Atomic Weights

[3] Bernath, P. F., Black, J. H., & Brault, J. W. (1985). "The spectrum of magnesium hydride" (PDF). Astrophysical Journal 298: 375. Bibcode:1985ApJ...298..375B. doi:10.1086/163620.

[4] Housecroft, C. E.; Sharpe, A. G. (2008). Inorganic Chemistry (3rd ed.). Prentice Hall. pp. 305–306. ISBN 978-0131755536.

[5] Ash, Russell (2005). The Top 10 of Everything 2006: The Ultimate Book of Lists. Dk Pub. ISBN 0-7566-1321-3.

[Abundance-6] "Abundance and form of the most abundant elements in Earth's continental crust" (PDF). Retrieved 15 February 2008.

[7] Anthoni, J Floor (2006). "The chemical composition of seawater". seafriends.org.nz.

[8] "Magnesium in health". magnesium.com. Retrieved 10 October 2013.

[9] ttp://www.ptable.com/#Property/State

[Dreizin.2C_Edward_L..3B_Berman.2C_Charles_H._and_Vicenzi.2C_Edward_P._2000_30-10] Dreizin, Edward L.; Berman, Charles H. & Vicenzi, Edward P. (2000). "Condensed-phase modifications in magnesium particle combustion in air". Scripta Materialia 122: 30–42. doi:10.1016/S0010-2180(00)00101-2.

[DOE-11] DOE Handbook – Primer on Spontaneous Heating and Pyrophoricity. U.S. Department of Energy. December 1994. p. 20. DOE-HDBK-1081-94. Retrieved 21 December 2011.

[giz-12] Dodson, Brian (29 August 2013). "Stainless magnesium breakthrough bodes well for manufacturing industries". Gizmag.com. Retrieved 29 August 2013.

[13] Birbilis, N.; Williams, G.; Gusieva, K.; Samaniego, A.; Gibson, M. A.; McMurray, H. N. (2013). "Poisoning the corrosion of magnesium". Electrochemistry Communications 34: 295. doi:10.1016/j.elecom.2013.07.021. edit

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