Niobium(V) fluoride

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Niobium(V) fluoride
Niobium(V) fluoride.png
Names
IUPAC names
Niobium(V) fluoride
Niobium pentafluoride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.109
EC Number 232-020-2
Properties
F5Nb
Molar mass 187.89839 g·mol−1
Appearance colorless hygroscopic solid
Density 3.293 g/cm3
Melting point 72 to 73 °C (162 to 163 °F; 345 to 346 K)
Boiling point 236 °C (457 °F; 509 K)
reacts
Solubility slightly soluble in chloroform, carbon disulfide, sulfuric acid
Hazards
GHS pictograms GHS05: CorrosiveGHS07: Harmful
GHS signal word Warning
H302, H312, H314, H318, H332
P260, P261, P264, P270, P271, P280, P301+312, P301+330+331, P302+352, P303+361+353, P304+312, P304+340, P305+351+338, P310, P312, P321, P322, P330, P363, P405, P501
Flash point Non-flammable
Related compounds
Other anions
Niobium(V) chloride
Niobium(V) bromide
Niobium(V) iodide
Other cations
Vanadium(V) fluoride
Tantalum(V) fluoride
Related niobium fluorides
Niobium(III) fluoride
Niobium(IV) fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Niobium(V) fluoride, also known as niobium pentafluoride, is the inorganic compound]] with the formula NbF5. The solid consists of tetramers [NbF5]4. It is a colorless solid that is rarely used.[1]

Preparation and reactions[edit]

Niobium pentafluoride is obtained by treatment of any niobium compound with fluorine:[2]

2 Nb + 5 F2 → 2 NbF5
2 NbCl5 + 5 F2 → 2 NbF5 + 5 Cl2

It reacts with hydrogen fluoride to give H2NbF7, a superacid.

Related compounds[edit]

In hydrofluoric acid, NbF5 converts to [[NbF7]2- and [[NbF5O]2-. The relative solubility of these potassium salts and related tantalum fluorides are the basis of the Marignac process for separation of Nb and Ta.

NbCl5 forms a dimeric structure (edge-shared bioctahedron) in contrast to the corner-shared tetrameric structure of the fluoride.

External links[edit]

References[edit]

  1. ^ Joachim Eckert, Hermann C. Starck (2005). "Niobium and Niobium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a17_251.CS1 maint: Uses authors parameter (link)
  2. ^ Homer F. Priest (1950). "Anhydrous Metal Fluorides". Inorganic Syntheses. 3: 171. doi:10.1002/9780470132340.ch47.