りん

危険有害性情報のコード(GHS)

• 絵表示(GHS)

  

• 注意喚起語

  Warning

• 危険有害性情報

  H228：可燃性固体

  H412：長期的影響により水生生物に有害

• 注意書き

  P210：熱/火花/裸火/高温のもののような着火源から遠ざ けること。－禁煙。

  P240：容器を接地すること/アースをとること。

  P241：防爆型の電気機器/換気装置/照明機器/．．．機器を使 用すること。

  P273：環境への放出を避けること。

  P280：保護手袋/保護衣/保護眼鏡/保護面を着用するこ と。

  P370+P378：火災の場合：消火に．．．を使用すること。

りん 価格

MSDS Information

• Phosphorus

りん 化学特性,用途語,生産方法

• 外観

  暗赤色の粉末

• 定義

  本品は、自然界に存在する元素(P)である。

• 解説

  リン，原子番号15の元素．電子配置[Ne]3s23p3の周期表15族元素．原子量30.973762(2)．天然には質量数31の核種のみ存在する単核種元素の一つ．質量数24～46の放射性核種が知られる．32Pは半減期14.3 d でトレーサーとして多用される．

  森北出版「化学辞典（第2版）
  

• 溶解性

  水にほとんど溶けない。

• 性質

  リン，融点44.2 ℃，沸点280 ℃，密度1.82(白リン(黄リン))，2.2(赤リン)．2.69(黒リン)g cm－3(20 ℃)．リンの変態には P4 分子からなる非金属性の白リンとグラファイトに似た金属リンとがある．黄リン，赤リン，紅リンはこれらの変態の固溶体，紫リン，黒リンは金属リン変態とされている．導電性，化学反応性，溶解度，毒性などが変態によりいちじるしく差がある．白リンは絶縁体，黒リンは半導体．白リンは水に不溶，二硫化炭素に可溶．空気中で自然発火して十酸化四リンP4O10となる．

• 用途

  マッチ(側薬)、軽金属の脱酸、リン青銅の原料、医薬品、農薬などの原料及び製造

• 用途

  合成原料。

• 发现

  錬金術時代(1669年)にH.Brandにより尿中に黄リンが発見され，りん光を発することから“光を運ぶ”という意味のギリシア語φ ωσφ οροζ"(fosforos)から命名された．宇田川榕菴は天保8年(1837年)出版の「舎密開宗」で，波斯波律斯(ホスホーリュス)燐と記載している．主要鉱物として，りん灰石(アパタイト，Ca5F(PO4)3)，藍(らん)鉄鉱Fe3(PO4)2·8H2O，銀星石Al3(PO4)2(OH)3·5H2Oなど．埋蔵量ではモロッコとサハラ西部42％，中国26％，アメリカ7％．産出量(2007年)では中国24％，アメリカ20％，モロッコとサハラ西部19％．リン酸カルシウム(リン鉱石，骨灰，海鳥ふん)にケイ酸を混合し，炭素(コークスなど)で還元すると，リンが気体の P4 として蒸留される．これを急冷して白リン(黄リン)をつくる．

• 製造

  光(日光)照射または自己の蒸気存在下の加熱により，赤リンにかわる．工業的には，黄リンを水相中で沸点以下でゆっくり加熱転化すると得られる．二硫化炭素に不溶．417 ℃(大気圧)で昇華する．リンは硝酸によりリン酸となり，濃い水酸化ナトリウム溶液ではリン化水素PH3とホスフィン酸ナトリウムNaPH2O2を生じる．酸素，塩素とははげしく反応し，酸化数5のP4O10(五酸化二リンではない)および五塩化リンとなる．

• 主な用途／役割

  エポキシ樹脂系接着剤に使用される。

• 説明

  White or yellow white phosphorus is a yellow waxy or colourless, transparent, volatile crystalline solid, waxy appearance with a garlic-like odour. On exposure to light, it darkens and ignites in air. It is also called yellow phosphorus colour because of impurities. White phosphorus does not occur naturally but is manufactured from phosphate rocks. It is insoluble in water, slightly soluble in benzene, ethanol, and chloroform, and is soluble in carbon disulphide. White phosphorus reacts rapidly with oxygen, easily catching fire at temperatures 10°C–15°C above room temperature. White phosphorus is used by the military in various types of ammunition and to produce smoke for concealing troop movements and identifying targets. It is also used by industry to produce phosphoric acid and other chemicals for use in fertilisers, food additives, and cleaning compounds. Small amounts of white phosphorus were used in the past in pesticides and fireworks.White phosphorus is used mainly for producing phosphoric acid and other chemicals. These chemicals are used to make fertilisers, additives in foods and drinks, cleaning compounds, and other products. In the military, white phosphorus is used in ammunitions such as mortar and artillery shells, and grenades.

• 化学的特性

  Yellow or white phosphorus ignites spontaneously in air at 34 °C. It should be stored under water. Under this condition, however, it may form phosphoric acid. Stainless steel containers should be used to hold the corrosive material. White phosphorus fires can be controlled by using water or sand or by excluding air.

• 同位体

  There are a 23 isotopes of phosphorus, ranging from P-24 to P-46, with halflivesthat range from a few nanoseconds to about two and half minutes. The one stableisotope is phosphorus-31, which accounts for 100% of the natural phosphorus on Earth.

• 名前の由来

  Its name is derived from the Greek word phosphoros, which means “bringer of light” or “light bearing.”

• 天然物の起源

  Phosphorus is the 12th most abundant element. It makes up about 0.1% of the Earth’s crust.Phosphorous occurs in nature in several forms, mostly as phosphates. The most commonsource is phosphate rock [Ca₃(PO₄)₂] and a mineral called “apatite.” Phosphorus is found inall animal bones and teeth and in most living tissue. Phosphorous nodules are found on theocean floor along with manganese nodules.Most commercial phosphorus is produced in electric furnaces where the phosphate-richminerals are heated to drive off the phosphorus as a gas, which is then condensed under water.Another process uses sulfuric acid to remove the phosphorus.

• 特性

  White phosphorus occurs in nature in phosphate rock. It is insoluble in water and alcoholand will ignite spontaneously in air. It exhibits what is known as phosphorescence; that is, itglows in the dark at room temperature. White phosphorus is poisonous and must be storedunder water.
  Red phosphorus is less reactive than the white variety. It is not poisonous, but largeamounts can explode. It is used in fireworks and matches.
  Black phosphorus is the only one of the three that will conduct electricity; white and redare poor conductors. Black phosphorus has no significant commercial uses.

• 使用

  It is used to make safety matches, incendiary shells,andsmokebombs;inpyrotechnics;and in the manufacture of fertilizers, pesticides, phosphoric acid, and phosphorus halides.

• 定義

  phosphorus: Symbol P. A nonmetallicelement belonging togroup 15 (formerly VB) of the periodictable; a.n. 15; r.a.m. 30.9738; r.d.1.82 (white), 2.34 (red); m.p. 44.1°C(α-white); b.p. 280°C (α-white). It occursin various phosphate rocks,from which it is extracted by heatingwith carbon (coke) and silicon(IV)oxide in an electric furnace (1500°C).Calcium silicate and carbon monoxideare also produced. Phosphorushas a number of allotropic forms.The α-white form consists of P4 tetrahedra(there is also a β-white formstable below –77°C). If α-white phosphorusis dissolved in lead andheated at 500°C a violet form is obtained.Red phosphorus, which is acombination of violet and whitephosphorus, is obtained by heatingα-white phosphorus at 250°C with airexcluded. There is also a black allotrope,which has a graphite-likestructure, made by heating whitephosphorus at 300°C with a mercurycatalyst. The element is highly reactive.It forms metal phosphides andcovalently bonded phosphorus(III)and phosphorus(V) compounds. Phosphorusis an essential element forliving organisms. It is an importantconstituent of tissues (especiallybones and teeth) and of cells, beingrequired for the formation of nucleic acids and energy-carrying molecules(e.g. ATP) and also involved in variousmetabolic reactions. The elementwas discovered by Hennig Brand(c. 1630–92) in 1669.

• 一般的な説明

  A white or yellow colored semi-liquid. Transported at high temperatures. Insoluble in water and denser than water. Contact may cause burns to skin, eyes, and mucous membranes. May be toxic by ingestion, inhalation and skin absorption. May ignite upon exposure to air. Used to make other chemicals.

• 空気と水の反応

  When exposed to air emits a green light and gives off white fumes. Ignites at 30°C in moist air, higher temperatures are required for ignition in dry air [Merck 11th ed. 1989]. The reactivity of phosphorus with oxygen or air depends on the allotrope of phosphorus involved and the conditions of contact, white (yellow) phosphorus being by far more reactive. White phosphorus readily ignites in air if warmed, finely divided, or under conditions where the slow oxidative isotherm cannot be dissipated. Contact with finely divided charcoal or lampblack promotes ignition, probably by the absorbed oxygen. Contact with amalgamated aluminum also promotes ignition [Mellor 1940 and 1971].

• 反応プロフィール

  WHITE PHOSPHORUS reacts with air (fire, acidic solution); sulfur and oxidants (fire, explosion). Bromine trifluoride reacts similarly with arsenic, boron, bromine, iodine, phosphorus, and sulfur [Mellor 2:113. 1946-47]. Bromoazide explodes on contact with antimony, arsenic, phosphorus, silver foil, or sodium. Red phosphorus reacts in the cold with selenium oxychloride evolving light and heat; white phosphorus reacts explosively [Mellor 10:906. 1946-47]. When thorium is heated with phosphorus, they unite with incandescence [Svenska Akad. 1829. p. 1].

• 危険性

  Many of the compounds of phosphorus are extremely dangerous, both as fire hazardsand as deadly poisons to the nervous system of humans and animals. Some of the poisonouscompounds (PCl_x) can be absorbed by the skin as well as inhaled or ingested. Flushing withwater is the only way to stop the burning of white phosphorus on the skin, but water doesnot affect the combustion of some phosphorus compounds. Although red phosphorus is notas dangerous or poisonous as white phosphorus, merely applying some frictional heating willinduce the red allotrope to change back to the explosive white allotrope (the striking of a safetymatch is an example).
  Some of the main types of poisonous gases used in warfare have a phosphorus base. Manycountries stockpile these gases, but, by agreement, the supplies are being reduced.

• 健康ハザード

  White phosphorus is a highly toxic substance by all routes of exposure. Contact of the solid with the skin produces deep painful burns, and eye contact can cause severe damage. Ingestion of phosphorus leads (after a delay of a few hours) to symptoms including nausea, vomiting, belching, and severe abdominal pain. Apparent recovery may be followed by a recurrence of symptoms. Death may occur after ingestion of 50 to 100 mg due to circulatory, liver, and kidney effects. Phosphorus ignites and burns spontaneously when exposed to air, and the resulting vapors are highly irritating to the eyes and respiratory tract.
  Red phosphorus is much less toxic than the white allotrope; however, samples of red phosphorus may contain the white form as an impurity. Early signs of chronic systemic poisoning by phosphorus are reported to include anemia, loss of appetite, gastrointestinal distress, chronic cough, a garlic-like odor to the breath, and pallor. A common response to severe chronic poisoning is damage of the jaw (''phossy jaw") and other bones. Phosphorus has not been reported to show carcinogenic effects in humans.

• 火災危険

  White phosphorus ignites spontaneously upon contact with air, producing an irritating, dense white smoke of phosphorus oxides. Use water to extinguish phosphorus fires.

• 燃焼性と爆発性

  White phosphorus ignites spontaneously upon contact with air, producing an irritating, dense white smoke of phosphorus oxides. Use water to extinguish phosphorus fires.
  Red phosphorus is a flammable solid but does not ignite spontaneously on exposure to air. At high temperatures (-300 °C), red phosphorus is converted to the white form.

• 化学性质

  融点589.5℃，空気中で安定。水，二硫化炭素，エーテルに不溶。反応性が乏しいため毒性は低い。空気中約260℃で発火する。

• 貯蔵

  Work with white phosphorus should be conducted in a fume hood to prevent exposure by inhalation, and splash goggles and impermeable gloves should be worn at all times to prevent eye and skin contact. Phosphorus should be stored under water in secondary containers in areas separate from oxidizing agents and other incompatible substances.

• 合成方法

  液状黄リンを還流冷却器付の鉄製転化釜に入れ，黄リン表面を水相で空気と遮断し，沸点以下の温度でゆっくりと加熱することで製造される。

• 純化方法

  Purify white phosphorus by melting it under dilute H2SO4—dichromate (possible carcinogen) mixture and allow to stand for several days in the dark at room temperature. It remains liquid, and the initial milky appearance due to insoluble, oxidisable material gradually disappears. The phosphorus can then be distilled under vacuum in the dark [Holmes Trans Faraday Soc 58 1916 1962]. It sublimes in vacuo. Other methods of purification include extraction with dry CS2 followed by evaporation of the solvent, or washing with 6M HNO3, then H2O, and drying under vacuum. It ignites in air at ~50o, or by friction if dry. Store and cut it under H2O . POISONOUS.

• 不和合性

  White phosphorus reacts with a number of substances to form explosive mixtures. For example, dangerous explosion hazards are produced upon reaction of phosphorus with many oxidizing agents, including chlorates, bromates, and many nitrates, with chlorine, bromine, peracids, organic peroxides, chromium trioxide, and potassium permanganate, with alkaline metal hydroxides (phosphine gas is liberated), and with sulfur, sulfuric acid, and many metals, including the alkali metals, copper, and iron.
  Red phosphorus is much less reactive than the white allotrope but may ignite or react explosively with strong oxidizing agents.

• 廃棄物の処理

  Excess phosphorus and waste material containing this substance should be placed in an appropriate container, clearly labeled, and handled according to your institution's waste disposal guidelines.

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