| Revision as of 12:52, 15 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,071 edits Saving copy of the {{chembox}} taken from revid 476791101 of page Boron_trifluoride for the Chem/Drugbox validation project (updated: ''). |
Latest revision as of 04:01, 13 January 2025 edit AnomieBOT (talk | contribs)Bots6,586,904 editsm Dating maintenance tags: {{How?}} |
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{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}} |
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{{Chembox |
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{{Chembox |
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| verifiedrevid = 455199202 |
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| Watchedfields = changed |
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| verifiedrevid |
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| verifiedrevid = 476996956 |
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| Name = Boron trifluoride |
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| ImageFileL1 = Boron-trifluoride-2D-dimensions.png |
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| Name = Boron trifluoride |
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| IUPACName = Boron trifluoride |
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| ImageSizeL1 = 130px |
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| ImageNameL1 = Boron trifluoride in 2D |
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| ImageFileL1 = Boron-trifluoride-2D-dimensions.png |
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| ImageFileR1 = Boron-trifluoride-3D-vdW.png |
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| ImageNameL1 = Boron trifluoride in 2D |
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| ImageFileR1 = Boron-trifluoride-3D-vdW.png |
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| ImageSizeR1 = 120px |
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| ImageNameR1 = Boron trifluoride in 3D |
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| ImageNameR1 = Boron trifluoride in 3D |
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| OtherNames = Boron fluoride, Trifluoroborane |
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| Section1 = {{Chembox Identifiers |
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| SystematicName = Trifluoroborane |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| Section1 = {{Chembox Identifiers |
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| ChemSpiderID = 6116 |
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|ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| InChI = 1/BF3/c2-1(3)4 |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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|ChemSpiderID = 6116 |
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|ChEBI_Ref = {{ebicite|correct|EBI}} |
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| ChEBI = 33093 |
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|ChEBI = 33093 |
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| SMILES = FB(F)F |
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|SMILES = FB(F)F |
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|SMILES2 = =(F)F |
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| InChIKey = WTEOIRVLGSZEPR-UHFFFAOYAW |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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|StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI = 1S/BF3/c2-1(3)4 |
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|StdInChI = 1S/BF3/c2-1(3)4 |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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|StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = WTEOIRVLGSZEPR-UHFFFAOYSA-N |
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|StdInChIKey = WTEOIRVLGSZEPR-UHFFFAOYSA-N |
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| CASNo = 7637-07-2 |
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|CASNo = 7637-07-2 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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|CASNo_Ref = {{cascite|correct|CAS}} |
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|CASNo1_Ref = {{cascite|correct|??}} |
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| CASNo1 = 13319-75-0 |
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| CASNo1_Comment = (dihydrate) |
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|CASNo1 = 13319-75-0 |
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|CASNo1_Comment = (dihydrate) |
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|UNII_Ref = {{fdacite|changed|FDA}} |
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| PubChem = 6356 |
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|UNII = 7JGD48PX8P |
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| EINECS = 231-569-5 |
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|PubChem = 6356 |
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| RTECS = ED2275000 |
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|EINECS = 231-569-5 |
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| UNNumber = Compressed: ].<!-- <br />''Complex with acetic acid: ''].<br/>''Complex with propionic acid: ''].<br/>''Boron trifuoride diethyl etherate: ''].<br/>''Boron trifluoride dimethyl etherate: ''].--><br/>Boron trifluoride dihydrate: ]. |
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|RTECS = ED2275000 |
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}} |
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|UNNumber = compressed: ].<!-- <br />''Complex with acetic acid: ''].<br/>''Complex with propionic acid: ''].<br/>''Boron trifuoride diethyl etherate: ''].<br/>''Boron trifluoride dimethyl etherate: ''].--><br/>boron trifluoride dihydrate: ]. |
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| Section2 = {{Chembox Properties |
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| Formula = BF<sub>3</sub> |
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| MolarMass = 67.82 g/mol (anhydrous) <br /> 103.837 g/mol (dihydrate) |
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| Appearance = colorless gas (anhydrous) <br /> colorless liquid (dihydrate) |
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| Density = 0.00276 g/cm<sup>3</sup> (anhydrous gas) <br /> 1.64 g/cm<sup>3</sup> (dihydrate) |
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| SolubleOther = soluble in ], ], ], ] and ] |
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| Solubility = very soluble |
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| MeltingPt = −126.8 °C, 146.4 K |
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| BoilingPt = −100.3 °C, 172.9 K |
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| Crit Temp = −12.3 °C, 260.9 K |
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}} |
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| Section7 = {{Chembox Hazards |
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| ExternalMSDS = |
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| EUClass = Very toxic ('''T+''')<br/>Corrosive ('''C''') |
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| Reference = <ref>{{CLP Regulation|index=005-001-00-X|page=341}}</ref><ref>{{PGCH-ref|id=0062|name=Boron trifluoride}}.</ref> |
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| EUIndex = 005-001-00-X |
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| MSDS = {{ICSC-small|0231}} |
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| GHSPictograms = {{GHS04|Press. Gas}}{{GHS06|Acute Tox. 2}}{{GHS05|Skin Corr. 1A}} |
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| GHSSignalWord = DANGER |
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| HPhrases = {{H-phrases|330|314}} <ref group="note">Within the European Union, the following additional hazard statement (EUH014) must also be displayed on labelling: Reacts violently with water.</ref> |
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| RPhrases = {{R14}}, {{R26}}, {{R35}} |
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| SPhrases = {{S1/2}}, {{S9}}, {{S26}}, {{S28}}, {{S36/37/39}}, {{S45}} |
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| NFPA-H = 4 |
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| NFPA-F = 0 |
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| NFPA-R = 1 |
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| NFPA-O = W |
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| FlashPt = 4 °C |
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}} |
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| Section8 = {{Chembox Related |
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| OtherCpds = ]<br />]<br />]<br/>] |
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}} |
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}} |
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}} |
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| Section2 = {{Chembox Properties |
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|Formula = {{chem2|BF3}} |
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|MolarMass = 67.82 g/mol (anhydrous) <br /> 103.837 g/mol (dihydrate) |
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|Appearance = colorless gas (anhydrous) <br /> colorless liquid (dihydrate) |
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|Odor = Pungent |
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|Density = 0.00276 g/cm<sup>3</sup> (anhydrous gas) <br /> 1.64 g/cm<sup>3</sup> (dihydrate) |
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|SolubleOther = soluble in ], ], ], ] and ] |
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|Solubility = exothermic decomposition <ref>{{cite book|url=http://www.nap.edu/openbook.php?record_id=4911&page=266|title=Prudent Practices in the Laboratory|date=16 August 1995|website=nap.edu|access-date=7 May 2018|doi=10.17226/4911|url-status=live|archive-url=https://web.archive.org/web/20141214075308/http://www.nap.edu/openbook.php?record_id=4911&page=266|archive-date=14 December 2014|isbn=978-0-309-05229-0}}</ref> (anhydrous)<br />very soluble (dihydrate) |
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|MeltingPtC = −126.8 |
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|BoilingPtC = −100.3 |
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|Dipole = 0 D |
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|VaporPressure = >50 atm (20 °C)<ref name=PGCH/> |
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}} |
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| Section3 = {{Chembox Thermochemistry |
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|DeltaHf = −1137 kJ/mol |
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|DeltaGf = −1120 kJ/mol |
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|Entropy = 254.3 J/(mol·K) |
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|HeatCapacity = 50.46 J/(mol·K) |
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}} |
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| Section4 = {{Chembox Hazards |
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|ExternalSDS = {{ICSC-small|0231}} |
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|Hazards_ref = <ref>{{CLP Regulation|index=005-001-00-X|page=341}}</ref><ref>{{PGCH-ref|id=0062|name=Boron trifluoride}}.</ref> |
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|GHSPictograms = {{GHS06|Acute Tox. 2}} {{GHS05|Skin Corr. 1A}} {{GHS08}} |
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|GHSSignalWord = DANGER |
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|HPhrases = {{H-phrases|330|314|335|373}} |
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|PPhrases = {{P-phrases|260|280|303+361+353|304+340|310|305+351+338|403+233}} |
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|NFPA-H = 3 |
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|NFPA-F = 0 |
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|NFPA-R = 1 |
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|FlashPt = Nonflammable |
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|PEL = C 1 ppm (3 mg/m<sup>3</sup>)<ref name=PGCH>{{PGCH|0062}}</ref> |
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|REL = C 1 ppm (3 mg/m<sup>3</sup>)<ref name=PGCH/> |
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|IDLH = 25 ppm<ref name=PGCH/> |
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|LC50 = 1227 ppm (mouse, 2 hr)<br/>39 ppm (guinea pig, 4 hr)<br/>418 ppm (rat, 4 hr)<ref>{{IDLH|7637072|Boron trifluoride}}</ref> |
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}}<ref>{{cite web|url=http://www.newenv.com/resources/nfpa_chemicals|title=New Environment Inc. - NFPA Chemicals|first=New Environment|last=Inc|website=www.newenv.com|access-date=7 May 2018|url-status=live|archive-url=https://web.archive.org/web/20160827183112/https://www.newenv.com/resources/nfpa_chemicals/|archive-date=27 August 2016}}</ref> |
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| Section5 = {{Chembox Related |
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|OtherAnions = {{ubl|]|]|]}} |
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|OtherCations = {{ubl|]|]|]|]}} |
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|OtherCompounds = ] |
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}} |
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}} |
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'''Boron trifluoride''' is the ] with the ] {{chem2|BF3}}. This pungent, colourless, and ] gas forms white fumes in moist air. It is a useful ] and a versatile building block for other ] compounds. |
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==Structure and bonding== |
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The geometry of a ] of {{chem2|BF3}} is ]. Its D<sub>3h</sub> ] conforms with the prediction of ]. The molecule has no dipole moment by virtue of its high symmetry. The molecule is ] with the carbonate anion, {{chem2|CO3(2-)}}. |
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{{chem2|BF3}} is commonly referred to as "]," a description that is reinforced by its ] reactivity toward ]s. |
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In the ] trihalides, {{chem2|BX3}}, the length of the B–X bonds (1.30 Å) is shorter than would be expected for single bonds,<ref name=greenwood>{{Greenwood&Earnshaw2nd}}</ref> and this shortness may indicate stronger B–X ] in the fluoride. A facile explanation invokes the symmetry-allowed overlap of a p orbital on the boron atom with the in-phase combination of the three similarly oriented p orbitals on fluorine atoms.<ref name = greenwood/> Others point to the ionic nature of the bonds in {{chem2|BF3}}.<ref>{{cite journal | author = Gillespie, Ronald J. | title = Covalent and Ionic Molecules: Why Are BeF<sub>2</sub> and AlF<sub>3</sub> High Melting Point Solids whereas BF<sub>3</sub> and SiF<sub>4</sub> Are Gases? | journal = ] | year = 1998 | volume = 75 | issue = 7 | page = 923 | doi = 10.1021/ed075p923 | bibcode = 1998JChEd..75..923G }}</ref> |
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] |
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==Synthesis and handling== |
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{{chem2|BF3}} is manufactured by the reaction of boron oxides with ]: |
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:{{chem2|B2O3 + 6 HF → 2 BF3 + 3 H2O}} |
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Typically the HF is produced '']'' from sulfuric acid and ] ({{chem2|CaF2}}).<ref>{{cite book |author1=Holleman, A. F. |author2=Wiberg, E. | title = Inorganic Chemistry | publisher = Academic Press | location = San Diego | year = 2001 | isbn = 0-12-352651-5 }}</ref> Approximately 2300-4500 tonnes of boron trifluoride are produced every year.<ref name=Ullmann>{{Ullmann | title = Boron Compounds | doi = 10.1002/14356007.a04_309 | author = Brotherton, R. J. | author2 = Weber, C. J. | author3 = Guibert, C. R. | author4 = Little, J. L. }}</ref> |
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===Laboratory scale=== |
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For laboratory scale reactions, {{chem2|BF3}} is usually produced in situ using ], which is a commercially available liquid.{{how?|date=January 2025}} |
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Laboratory routes to the solvent-free materials are numerous. A well documented route involves the thermal decomposition of ]s of {{chem2|-}}:<ref>{{ OrgSynth | author = Flood, D. T. | title = Fluorobenzene | year = 1933 | volume = 13 | pages = 46 | collvol = 2 | collvolpages = 295 | prep = CV2P0295 }}</ref> |
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:{{chem2|+− → ] + BF3 + ]}} |
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It forms by treatment of a mixture ] and ] with sulfuric acid:<ref name="Georg">{{cite book|last=Brauer|first=Georg|title=Handbook of Preparative Inorganic Chemistry|volume=1|edition=2nd|date=1963|publisher=Academic Press|location=New York|isbn=978-0121266011|page=220 & 773|url=https://books.google.com/books?id=TLYatwAACAAJ&q=Handbook+of+Preparative+Inorganic+Chemistry}}</ref> |
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:{{chem2|6 Na + B2O3 + 6 H2SO4 → 8 BF3 + 6 ] + 3 H2O}} |
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Alternatively, ] converts various ] to ]s, evolving the trifluoride gas:<ref>{{cite blog|url=https://labphoto.tumblr.com/post/181931503047/performing-a-halogen-exchange-a-halex-reaction-on|title=Performing a halogen exchange, a HalEx reaction on....|date=11 Jan 2019|first=Kristof|last=Hegedüs|publisher=]|access-date=12 January 2025|archive-url=https://web.archive.org/web/20190119032227/https://labphoto.tumblr.com/post/181931503047/performing-a-halogen-exchange-a-halex-reaction-on|archive-date=19 Jan 2019|website=Pictures from an Organic Chemistry Laboratory|url-status=live}}</ref> |
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:3 R–F + BBr<sub>3</sub> → 3 R–Br + BF<sub>3</sub> |
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==Properties== |
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Anhydrous boron trifluoride has a ] of −100.3 °C and a ] of −12.3 °C, so that it can be stored as a refrigerated liquid only between those temperatures. Storage or transport vessels should be designed to withstand internal pressure, since a refrigeration system failure could cause pressures to rise to the ] of 49.85 bar (4.985 MPa).<ref>{{cite book | editor = Yaws, C. L. | title = Chemical Properties Handbook | publisher = McGraw-Hill | year = 1999 | page = 25 }}</ref> |
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Boron trifluoride is corrosive. Suitable metals for equipment handling boron trifluoride include ], ], and ]. In presence of moisture it corrodes steel, including stainless steel. It reacts with ]s. ], ], ], and ] show satisfactory resistance. The ] used in the equipment should be ] based, as boron trifluoride reacts with the hydrocarbon-based ones.<ref>{{cite encyclopedia | publisher = ] | url = http://encyclopedia.airliquide.com/encyclopedia.asp?GasID=68 | encyclopedia = Gas Encyclopedia | title = Boron trifluoride | url-status = live | archive-url = https://web.archive.org/web/20061206053305/http://encyclopedia.airliquide.com/Encyclopedia.asp?GasID=68 | archive-date = 2006-12-06 |date = 2016-12-15}}</ref> |
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==Reactions== |
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Unlike the aluminium and gallium trihalides, the boron trihalides are all ]ic. They undergo rapid halide exchange reactions: |
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:{{chem2|BF3 + ] → BF2Cl + BCl2F}} |
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Because of the facility of this exchange process, the mixed halides cannot be obtained in pure form. |
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Boron trifluoride is a versatile ] that forms ]s with such ]s as ] and ]s: |
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:{{chem2|] + BF3 → Cs}} |
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:{{chem2|] + BF3 → BF3*O(CH2CH3)2}} |
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] salts are commonly employed as ]s. The adduct with ], boron trifluoride diethyl etherate, or just ], ({{chem2|BF3*O(CH2CH3)2}}) is a conveniently handled ] and consequently is widely encountered as a laboratory source of {{chem2|BF3}}.<ref>{{cite book |doi=10.1002/9780470842898.rb249.pub2|chapter=Boron Trifluoride Etherate|title=Encyclopedia of Reagents for Organic Synthesis|year=2007|last1=Cornel|first1=Veronica|last2=Lovely|first2=Carl J.|isbn=978-0471936237|s2cid=100921225 }}</ref> Another common adduct is the adduct with ] ({{chem2|BF3*S(CH3)2}}), which can be handled as a neat liquid.<ref>{{cite book |doi=10.1002/047084289X.rb247|chapter=Boron Trifluoride-Dimethyl Sulfide|title=Encyclopedia of Reagents for Organic Synthesis|year=2001|last1=Heaney|first1=Harry|isbn=0471936235}}</ref> |
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===Comparative Lewis acidity=== |
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All three lighter boron trihalides, {{chem2|BX3}} (X = F, Cl, Br) form stable adducts with common Lewis bases. Their relative Lewis acidities can be evaluated in terms of the relative exothermicities of the adduct-forming reaction. Such measurements have revealed the following sequence for the Lewis acidity: |
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:{{chem2|BF3}} < {{chem2|BCl3}} < {{chem2|BBr3}} < {{chem2|BI3}} (strongest Lewis acid) |
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This trend is commonly attributed to the degree of ] in the planar boron trihalide that would be lost upon ] of the {{chem2|BX3}} molecule.<ref>{{Cotton&Wilkinson6th }}</ref> which follows this trend: |
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:{{chem2|BF3}} > {{chem2|BCl3}} > {{chem2|BBr3}} < {{chem2|BI3}} (most easily pyramidalized) |
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The criteria for evaluating the relative strength of ] are not clear, however.<ref name = greenwood/> One suggestion is that the F atom is small compared to the larger Cl and Br atoms. As a consequence, the bond length between boron and the halogen increases while going from fluorine to iodine hence spatial overlap between the orbitals becomes more difficult. The lone pair electron in p<sub>''z''</sub> of F is readily and easily donated and overlapped to empty p<sub>z</sub> orbital of boron. As a result, the pi donation of F is greater than that of Cl or Br. |
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In an alternative explanation, the low Lewis acidity for {{chem2|BF3}} is attributed to the relative weakness of the bond in the adducts {{chem2|F3B\sL}}.<ref>{{cite journal |author1=Boorman, P. M. |author2=Potts, D. | title = Group V Chalcogenide Complexes of Boron Trihalides | journal = ] | year = 1974 | volume = 52 | issue = 11 | pages = 2016–2020 | doi = 10.1139/v74-291 }}</ref><ref>{{cite journal |author1=Brinck, T. |author2=Murray, J. S. |author3=Politzer, P. | title = A Computational Analysis of the Bonding in Boron Trifluoride and Boron Trichloride and their Complexes with Ammonia |journal = ] | year = 1993 | volume = 32 | issue = 12 | pages = 2622–2625 | doi = 10.1021/ic00064a008 }}</ref> |
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Yet another explanation might be found in the fact that the p<sub>''z''</sub> orbitals in each higher period have an extra nodal plane and opposite signs of the wave function on each side of that plane. This results in bonding and antibonding regions within the same bond, diminishing the effective overlap and so lowering the π-donating blockage of the acidity.<ref>] an easy to understand table is found, which shows drawings of the several higher p orbitals.</ref> |
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===Hydrolysis=== |
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Boron trifluoride reacts with water to give ] and ]. The reaction commences with the formation of the aquo adduct, {{chem2|H2O\sBF3}}, which then loses HF that gives fluoroboric acid with boron trifluoride.<ref>{{cite journal | author = Wamser, C. A. | title = Equilibria in the System Boron Trifluoride–Water at 25° | journal = ] | year = 1951 | volume = 73 | issue = 1 | pages = 409–416 | doi = 10.1021/ja01145a134 }}</ref> |
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:{{chem2|4 BF3 + 3 H2O → 3 H + B(OH)3}} |
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The heavier trihalides do not undergo analogous reactions, possibly due to the lower stability of the tetrahedral ions {{chem2|-}} and {{chem2|-}}. Because of the high acidity of fluoroboric acid, the fluoroborate ion can be used to isolate particularly electrophilic cations, such as ] ions, that are otherwise difficult to isolate as solids. |
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==Uses== |
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===Organic chemistry=== |
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Boron trifluoride is most importantly used as a reagent in ], typically as a ].<ref name=Ullmann/><ref>{{cite encyclopedia | author = Heaney, H. | chapter = Boron Trifluoride | encyclopedia = ] | year = 2001 | doi = 10.1002/047084289X.rb250 | isbn = 0-471-93623-5 }}</ref> Examples include: |
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* initiates ] reactions of ]s, such as ]s |
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* as a catalyst in some ], ],<ref>{{cite journal|last1=Mani|first1=Rama I.|last2=Erbert|first2=Larry H.|last3=Manise|first3=Daniel|title=Boron Trifluoride in the Synthesis of Plant Phenolics: Synthesis of Phenolic Ketones and Phenyl Stryl Ketones|journal=Journal of Tennessee Academy of Science|date=1991|volume=66|issue=1|pages=1–8|url=http://www.tennacadofsci.org/journal/articles/JTAS66-1-1.pdf|access-date=27 October 2016|url-status=dead|archive-url=https://web.archive.org/web/20161027124626/http://www.tennacadofsci.org/journal/articles/JTAS66-1-1.pdf|archive-date=27 October 2016}}</ref> ], ], ],<ref>{{cite journal|last1=Sowa|first1=F. J.|last2=Hennion|first2=G. F.|last3=Nieuwland|first3=J. A.|title=Organic Reactions with Boron Fluoride. IX. The Alkylation of Phenol with Alcohols|journal=Journal of the American Chemical Society|date=1935|volume=57|issue=4|pages=709–711|doi=10.1021/ja01307a034}}</ref> ], ], and other reactions<ref name=Honeywell>{{cite web | publisher = ] | url = http://www51.honeywell.com/sm/bf3/applications.html | title = Boron Trifluoride (BF<sub>3</sub>) Applications | url-status = dead | archive-url = https://web.archive.org/web/20120129231149/http://www51.honeywell.com/sm/bf3/applications.html | archive-date = 2012-01-29 }}</ref>{{Citation needed|reason=Honeywell citation unverifiable|date=March 2015}} |
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===Niche uses=== |
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Other, less common uses for boron trifluoride include: |
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* applied as ] in ] |
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* ] dopant for ]ly grown ] |
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* used in sensitive ] in ]s and devices to monitor radiation levels in the ] |
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* in ] |
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* as a ] for ] magnesium |
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* to prepare ]<ref name="Georg" /> |
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==Discovery== |
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Boron trifluoride was discovered in 1808 by ] and ], who were trying to isolate "fluoric acid" (i.e., ]) by combining ] with vitrified ]. The resulting vapours failed to etch glass, so they named it ''fluoboric gas''.<ref>{{cite journal |author1=Gay-Lussac, J. L. |author2=Thénard, L. J. | title = Sur l'acide fluorique | journal = Annales de Chimie | volume = 69 | year = 1809 | pages = 204–220}}</ref><ref>{{cite journal |author1=Gay-Lussac, J. L. |author2=Thénard, L. J. | title = Des propriétés de l'acide fluorique et sur-tout de son action sur le métal de la potasse | journal = Mémoires de Physique et de Chimie de la Société d'Arcueil | volume = 2 | year = 1809 | pages = 317–331 | url = https://books.google.com/books?id=Nl87AAAAcAAJ&pg=PA317}}</ref> |
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==See also== |
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*] |
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==References== |
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{{Reflist}} |
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==External links== |
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* {{cite web | url = http://www.osha.gov/dts/chemicalsampling/data/CH_221700.html | title = Safety and Health Topics: Boron Trifluoride | publisher = OSHA }} |
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* {{cite web | url = https://www.cdc.gov/niosh/ipcsneng/neng0231.html | title = BORON TRIFLUORIDE ICSC: 0231 | work = International Chemical Safety Cards | publisher = CDC | access-date = 2017-09-08 | archive-url = https://web.archive.org/web/20171123090449/https://www.cdc.gov/niosh/ipcsneng/neng0231.html | archive-date = 2017-11-23 | url-status = dead }} |
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* {{cite web | url = http://www.npi.gov.au/substances/boron/index.html | work = National Pollutant Inventory | title = Boron & Compounds: Overview | publisher = Australian Government }} |
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* {{cite web | url = http://www.npi.gov.au/substances/fluoride-compounds/index.html | work = National Pollutant Inventory | title = Fluoride Compounds: Overview | publisher = Australian Government }} |
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* {{cite web | url = http://webbook.nist.gov/cgi/cbook.cgi?ID=C7637072 | title = Boron trifluoride | work = WebBook | publisher = NIST }} |
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* {{cite web | url = http://www51.honeywell.com/sm/bf3/applications.html | title = Boron Trifluoride (BF<sub>3</sub>) Applications | publisher = Honeywell | access-date = 2012-02-14 | archive-url = https://web.archive.org/web/20120129231149/http://www51.honeywell.com/sm/bf3/applications.html | archive-date = 2012-01-29 | url-status = dead }} |
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{{Boron compounds}} |
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{{fluorine compounds}} |
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{{Authority control}} |
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] |
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] |
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] |
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] |
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] |