Potassium heptafluorotantalate

Potassium heptafluorotantalate

Names
IUPAC name Dipotassium heptafluorotantalate
Systematic IUPAC name Dipotassium heptafluorotantalum(2-)
Other names Potassium heptafluorotantalate(V) Potassium fluorotantalate
Identifiers
CAS Registry Number	16924-00-8 Y
ChemSpider	28541740 N
EC-number	240-986-1
InChI InChI=1S/7FH.2K.Ta/h7*1H;;;/q;;;;;;;2*+1;+5/p-7
Jmol-3D images	Image
SMILES F[Ta-2](F)(F)(F)(F)(F)F.[K+].[K+]
Properties
Chemical formula	K2TaF7
Molar mass	392.13 g/mol
Appearance	white solid
Density	4.56 g/mL at 25 °C
Melting point	630 to 820 °C (1,166 to 1,508 °F; 903 to 1,093 K)
Solubility in water	0.5 g/100 mL (15 °C)[1]
Hazards
LD50 (Median lethal dose)	110 mg/kg (Oral: rat)
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Potassium heptafluorotantalate is an inorganic compound with the formula K₂TaF₇. It is the potassium salt of the heptafluorotantalate anion [TaF₇]²⁻. This white, water-soluble solid is an intermediate in the purification of tantalum from its ores and is the precursor to the metal.^[2]

Preparation

Industrial

Potassium heptafluorotantalate is an intermediate in the industrial production of metallic tantalum. Its production involves leaching tantalum ores, such as columbite and tantalite, with hydrofluoric acid and sulfuric acid to produce the water soluble hydrogen pentafluorotantalate.^[2]

Ta₂O₅ + 14 HF → 2 H₂[TaF₇] + 5 H₂O

This solution is subjected to a number of liquid-liquid extraction steps to remove metallic impurities (most importantly niobium) before being treated with potassium fluoride to produce K₂[TaF₇]

H₂[TaF₇] + 2 KF → K₂[TaF₇] + 2 HF

Lab-scale

Hydrofluoric acid is both corrosive and toxic, making it unappealing to work with; as such a number of alternative processes have been developed for small-scale syntheses. Potassium heptafulorotantalate can be produced by both anhydrous and wet methods. The anhydrous method involves the reaction of tantalum oxide with potassium bifluoride or ammonium bifluoride according to the following equation:^[1][3]

Ta₂O₅ + 4 KHF₂ + 6 HF → 2 K₂[TaF₇] + 5 H₂O

The method was originally reported by Berzelius.^[4]

K₂[TaF₇] can also be precipitated from solutions in hydrofluoric acid provided that the concentration of HF is below about 42%. Solutions having higher concentrations of HF yield potassium hexafluorotantalate [KTaF₆]. The K-salt can be also precipitated from a solution in hydrofluoric acid of tantalum pentachloride:

5 HF + 2 KF + TaCl₅ → K₂[TaF₇] + 5 HCl

Structure

Potassium heptafluorotantalate exists in at least two polymorphs. α-K₂[TaF₇] is the most common form and crystallises in the monoclinic P2₁/c space group.^[5] The structure is composed of [TaF₇]²⁻ units interconnected by potassium ions. [TaF₇]²⁻ polyhedra may be described as monocapped trigonal prisms with the capping atom located on one of the rectangular faces. Potassium atoms are 9-coordinated and may be viewed as distorted monocapped square prisms.

At temperatures above 230 °C this converts to β-K₂[TaF₇], which is orthorhombic (space group: Pnma). This structure also consists of potassium ions and the complex anion [TaF₇]²⁻. The structure of the 7-coordinate [TaF₇]²⁻ units is essentially unchanged. However the potassium atoms now exist in 2 environments where they coordinate to either 11 or 8 fluorine atoms.^[6][7]

Reactions

K₂[TaF₇] is primarily used to produce metallic tantalum by reduction with sodium. This takes place at approximately 800 °C in molten salt and proceeds via a number of potential pathways.^[8]

K₂[TaF₇] + 5 Na → Ta + 5 NaF + 2 KF

K₂[TaF₇] is susceptible to hydrolysis. For example, a boiling aqueous solution of K₂TaF₇ yields potassium oxyfluorotantalate (K₂Ta₂O₃F₆), known as “Marignac’s salt”. In order to prevent hydrolysis and co-precipitation of potassium oxyfluorotantalate, a small excess of HF is added to the solution.

References