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Fluorine

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Fluorine
chemical element (en) Fassara da lithophile element (en) Fassara
Bayanai
Ƙaramin ɓangare na diatomic nonmetal (en) Fassara, nonmetal (en) Fassara da Halogens
Bangare na perfluorinated compound (en) Fassara, period 2 (en) Fassara da Halogens
Suna saboda hydrofluoric acid (en) Fassara
Associated hazard (en) Fassara fluorine exposure (en) Fassara
Ta biyo baya Ne (mul) Fassara
Yana haddasa fluorine exposure (en) Fassara
Mai ganowa ko mai ƙirƙira Henri Moissan (mul) Fassara da André-Marie Ampère (mul) Fassara
Time of discovery or invention (en) Fassara 1810
Location of discovery (en) Fassara Faransa
Element symbol (en) Fassara F
Sinadaran dabara F
Electron configuration (en) Fassara 1s² 2s² 2p⁵ da [He] 2s² 2p⁵
NIOSH Pocket Guide ID (mul) Fassara 0289

Fluorine sinadari ne mai sinadarai ; yana da alamar F da lambar atomic 9. Shi ne halogen mafi sauƙi kuma yana wanzuwa a yanayi na yau da kullun kamar iskar diatomic mai launin rawaya. Fluorine yana da matuƙar amsawa yayin da yake amsawa da duk sauran abubuwa banda iskar gas mai daraja mai haske. Fluorine a cikin sifarsa mai guba sosai.

Daga cikin abubuwan da ke cikin ƙasa, fluorine yana matsayi na 24 a yawan sararin samaniya da kuma na 13 a yawan ɓawon burodi . Fluorite, babban tushen ma'adinai na fluorine, wanda ya ba wa sinadarin suna, an fara bayyana shi a shekarar 1529; yayin da aka ƙara shi a cikin ma'adanai na ƙarfe don rage yawan narkewar su don narkewa, fi'ilin Latin fluo Ma'anar ' ta ba wa ma'adinin suna. An gabatar da shi a matsayin wani sinadari a shekarar 1810, fluorine ya zama da wahala kuma mai haɗari a raba shi da mahaɗansa, kuma masu gwaji da yawa na farko sun mutu ko sun sami raunuka sakamakon yunƙurinsu. Sai a shekarar 1886 ne masanin kimiyyar sinadarai ɗan Faransa Henri Moissan ya ware sinadarin fluorine ta amfani da electrolysis mai ƙarancin zafin jiki, wani tsari da har yanzu ake amfani da shi don samar da zamani. Samar da iskar gas ta fluorine a masana'antu don wadatar da uranium, mafi girman aikace-aikacensa, ya fara ne a lokacin Aikin Manhattan a Yaƙin Duniya na Biyu .

Saboda kuɗin tace sinadarin fluorine mai tsarki, yawancin aikace-aikacen kasuwanci suna amfani da mahaɗan fluorine, tare da kusan rabin fluorite da aka haƙa da ake amfani da shi wajen yin ƙarfe . Sauran fluorite ɗin ana canza shi zuwa hydrogen fluoride a hanyarsa ta zuwa nau'ikan fluoride na halitta, ko kuma zuwa cryolite, wanda ke taka muhimmiyar rawa a cikin tace sinadarin aluminum . Haɗin carbon-fluorine yawanci yana da ƙarfi sosai. Ana amfani da mahaɗan Organofluorine sosai azaman masu sanyaya, rufin lantarki, da PTFE (Teflon). Magunguna kamar atorvastatin da fluoxetine suna ɗauke da haɗin C−F. Ion fluoride daga gishirin fluoride da aka narkar yana hana ramukan haƙori don haka ana amfani da shi a cikin man goge baki da fluoride na ruwa . Tallace-tallacen fluoride na duniya ya wuce dala 15. biliyan a kowace shekara.

Iskar gas ta Fluorocarbon galibi iskar gas ce mai dumama yanayi wadda ke da ƙarfin dumamar yanayi sau 100 zuwa 23,500 fiye da iskar carbon dioxide, kuma yana da mafi girman ƙarfin ɗumamar yanayi fiye da duk wani abu da aka sani. Sinadaran Organofluorine galibi suna ci gaba da kasancewa a cikin muhalli saboda ƙarfin haɗin carbon-fluorine. Fluorine ba shi da wani aiki da aka sani na rayuwa a cikin dabbobi masu shayarwa, amma wasu tsire-tsire da soso na ruwa suna haɗa gubar organofluorine (galibi monofluoroacetates ) waɗanda ke taimakawa wajen hana farauta. [1]

 

Halaye

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Tsarin lantarki

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Kwayoyin fluorine suna da electrons tara, ɗaya ƙasa da neon, da kuma tsarin electrons 1s 2 2s 2 2p 5 : electrons biyu a cikin harsashi na ciki da aka cika da bakwai a cikin harsashi na waje wanda ke buƙatar ƙarin ɗaya don a cika. Elektrons na waje ba su da tasiri a kariyar nukiliya, kuma suna fuskantar babban ƙarfin nukiliya na 9 − 2 = 7; wannan yana shafar halayen zahiri na kwayar halittar. [2]

Makamashin ionization na farko na fluorine shine na uku mafi girma a cikin dukkan abubuwa, bayan helium da neon, [3] wanda ke rikitar da cire electrons daga atoms ɗin fluorine masu tsaka-tsaki. Hakanan yana da babban haɗin lantarki, na biyu kawai bayan chlorine, [4] kuma yana iya kama electron don zama isoelectronic tare da neon gas mai daraja; [2] yana da mafi girman electronegativity na kowane abu mai amsawa. [5] Atoms ɗin fluorine suna da ƙaramin radius na covalent na kusan 60 picometers, kama da na zamaninsa suna maƙwabtaka da iskar oxygen da neon. [6] [7] [8]

Amsawa

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Ƙarfin haɗin difluorine ya yi ƙasa da na ɗayan biyun. ko kuma yayi kama da haɗin peroxide mai sauƙin rabawa; wannan, tare da babban ƙarfin lantarki, yana haifar da sauƙin rabuwar fluorine, babban amsawa, da haɗin gwiwa mai ƙarfi ga ƙwayoyin da ba su da fluorine. [9] [10] Akasin haka, haɗin gwiwa da wasu ƙwayoyin halitta yana da ƙarfi sosai saboda yawan ƙarfin lantarki na fluorine. Abubuwa marasa aiki kamar ƙarfe foda, gutsuttsuran gilashi, da zare asbestos suna amsawa da sauri tare da iskar fluorine mai sanyi; itace da ruwa suna ƙonewa kwatsam a ƙarƙashin jet ɗin fluorine. [2] [11]

Halayen sinadarin fluorine da ƙarfe suna buƙatar yanayi daban-daban. Karafan Alkali suna haifar da fashewa kuma karafan ƙasa na alkaline suna nuna ƙarfi sosai; don hana passivation daga samuwar yadudduka na fluoride na ƙarfe, yawancin sauran karafa kamar aluminum da ƙarfe dole ne a yi musu foda, [1] kuma karafa masu daraja suna buƙatar iskar fluorine mai tsabta a 300–450 °C (572–842 °F) . [1] Wasu sinadarai masu ƙarfi waɗanda ba ƙarfe ba (sulfur, phosphorus) suna amsawa da ƙarfi a cikin fluorine mai ruwa. [1] Hydrogen sulfide [1] da sulfur dioxide [1] suna haɗuwa cikin sauƙi tare da fluorine, na ƙarshen wani lokacin yana fashewa; sulfuric acid yana nuna ƙarancin aiki, yana buƙatar yanayin zafi mai yawa. [1]

Hydrogen, kamar wasu ƙarfe na alkali, yana yin tasiri mai ƙarfi da fluorine. [9] Carbon, kamar yadda fitilar baƙar fata take, yana yin tasiri a zafin ɗaki don samar da tetrafluoromethane . Graphite yana haɗuwa da fluorine sama da 400 °C (752 °F) don samar da carbon monofluoride mara stoichiometric ; yanayin zafi mafi girma yana haifar da fluorocarbons na iskar gas, wani lokacin tare da fashewa. [12] Carbon dioxide da carbon monoxide suna amsawa a ko sama da zafin ɗaki, [13] yayin da paraffins da sauran sinadarai na halitta suna haifar da halayen ƙarfi: [14] har ma da haloalkanes da aka maye gurbinsu gaba ɗaya kamar carbon tetrachloride, wanda yawanci ba ya ƙonewa, na iya fashewa. [15] Kodayake nitrogen trifluoride yana da ƙarfi, nitrogen yana buƙatar fitar da lantarki a yanayin zafi mai yawa don amsawa tare da fluorine ya faru, saboda ƙarfin haɗin gwiwa uku a cikin nitrogen na asali; [16] ammonia na iya amsawa da fashewa. [17] [18] Oxygen baya haɗuwa da fluorine a ƙarƙashin yanayi na yanayi, amma ana iya sa shi ya amsa ta amfani da fitar da lantarki a ƙananan yanayin zafi da matsin lamba; samfuran suna iya wargajewa zuwa abubuwan da ke cikin su lokacin da aka yi zafi. [19] [20] [21] Halogens masu nauyi [2] suna amsawa cikin sauƙi da fluorine kamar yadda radon gas mai daraja yake amsawa; [22] na sauran iskar gas mai daraja, xenon da krypton ne kawai ke amsawa, kuma a ƙarƙashin yanayi na musamman kawai. [23] Argon baya amsawa da iskar fluorine; duk da haka, yana samar da mahaɗi tare da fluorine, argon fluorohydride .

Matakai

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Cube with spinning molecules on its corners and its faces
Zane-zanen da ke nuna tsarin lu'ulu'u na β-fluorine. Kwayoyin halittar F 2 da ke fuskokin ƙwayar naúrar suna da juyawa da aka takaita zuwa wani jirgin sama, yayin da waɗanda ke cikin kusurwoyi za su iya juyawa cikin 'yanci.

A zafin ɗaki, fluorine iskar gas ce ta ƙwayoyin diatomic, [2] mai launin rawaya mai haske idan aka yi tsarki (wani lokacin ana kwatanta shi da rawaya-kore). [24] Yana da wari mai kama da halogen mai zafi da cizo wanda za a iya gano shi a digiri 20 ppb . [4] Fluorine yana taruwa zuwa ruwa mai haske rawaya a −188 °C (−306.4 °F), yanayin zafi mai kama da na iskar oxygen da nitrogen. [3]

Fluorine yana da siffofi biyu masu ƙarfi, α- da β-fluorine. Na ƙarshen yana yin lu'ulu'u a −220 °C (−364.0 °F) kuma yana da haske da laushi, tare da tsarin cubic iri ɗaya na iskar oxygen mai ƙarfi da aka sabunta, [3] [26] ba kamar tsarin orthorhombic na sauran halogens masu ƙarfi ba. [27] [28] Ƙarin sanyaya zuwa −228 °C (−378.4 °F) yana haifar da sauyawar lokaci zuwa α-fluorine mai tauri da ba a iya gani, wanda ke da tsarin monoclinic tare da yadudduka masu yawa da kusurwa na ƙwayoyin halitta. Sauyewar daga β- zuwa α-fluorine ya fi exothermic fiye da danshi na fluorine, kuma yana iya zama mai ƙarfi. [27] [28]

Manazarta

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  1. ↑ Lee et al. 2014.
  2. 1 2 3 4 5 Jaccaud et al. 2000.
  3. 1 2 3 Dean 1999.
  4. 1 2 Lide 2004.
  5. ↑ Moore, Stanitski & Jurs 2010.
  6. ↑ Cordero et al. 2008.
  7. ↑ Pyykkö & Atsumi 2009.
  8. ↑ Sources disagree on the radii of oxygen, fluorine, and neon atoms. Precise comparison is thus impossible.
  9. 1 2 Greenwood & Earnshaw 1998.
  10. ↑ Macomber 1996
  11. ↑ Nelson 1947.
  12. ↑ Kuriakose & Margrave 1965.
  13. ↑ Hasegawa et al. 2007.
  14. ↑ Lagow 1970.
  15. ↑ Navarrini et al. 2012.
  16. ↑ Lidin, Molochko & Andreeva 2000.
  17. ↑ Tanner Industries 2011.
  18. ↑ Morrow, Perry & Cohen 1959.
  19. ↑ Emeléus & Sharpe 1974.
  20. ↑ Wiberg, Wiberg & Holleman 2001.
  21. ↑ Brantley 1949.
  22. ↑ Pitzer 1975.
  23. ↑ Khriachtchev et al. 2000.
  24. ↑ Burdon, Emson & Edwards 1987.
  25. ↑ Pauling, Keaveny & Robinson 1970.
  26. ↑ α-Fluorine has a regular pattern of molecules and is a crystalline solid, but its molecules do not have a specific orientation. β-Fluorine's molecules have fixed locations and minimal rotational uncertainty.[25]
  27. 1 2 Young 1975.
  28. 1 2 Barrett, Meyer & Wasserman 1967.
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