Difluoruro di cobalto

Difluoruro di cobalto
Cella unitaria del difluoruro di cobalto
Cella unitaria del difluoruro di cobalto
Nome IUPAC
Difluoruro di cobalto
Nomi alternativi
Fluoruro di cobalto(II)
Caratteristiche generali
Formula bruta o molecolareCoF2
Massa molecolare (u)96,93
Aspettosolido cristallino rosa
Numero CAS10026-17-2
Numero EINECS233-061-9
PubChem24820 e 10219383
SMILES
F[Co]F
Proprietà chimico-fisiche
Densità (g/cm3, in c.s.)4,46 (anidro)
2,22 (tetraidrato)
Solubilità in acqua1,5 g/100 mL (25 °C)
Temperatura di fusione1200 °C (1473 K)
Temperatura di ebollizione1400 °C (1673 K)
Proprietà termochimiche
ΔfH0 (kJ·mol−1)–672[1]
ΔfG0 (kJ·mol−1)–627[1]
S0m(J·K−1mol−1)82,4[1]
C0p,m(J·K−1mol−1)68,9[1]
Indicazioni di sicurezza
Simboli di rischio chimico
tossicità acuta corrosivo
pericolo
Frasi H301 - 314
Consigli P260 - 280 - 301+310+330 - 301+330+331 - 303+361+353 - 305+351+338
Modifica dati su Wikidata · Manuale

Il difluoruro di cobalto o fluoruro di cobalto(II) è il composto inorganico con formula CoF2. È un solido cristallino di colore rosa. Esistono anche le forme idrate CoF2•2H2O , CoF2•3H2O e CoF2•4H2O.

Struttura

CoF2 ha una struttura cristallina tipo rutilo, nel sistema tetragonale con gruppo spaziale P42/mnm e costanti di reticolo a = 469,50(7) pm, c = 318,17(5) pm, V = 70,10 Å3, Z = 2.[2]

Sintesi

Il difluoruro di cobalto anidro si prepara industrialmente trattando carbonato di cobalto(II) con fluoruro di idrogeno a secco o in soluzione:[1]

CoCO3 + 2HF → CoF2 + CO2 + H2O

Se si opera in soluzione si ottengono forme idrate, da cui si può ricavare la forma anidra per disidratazione.

Le forme idrate CoF2•2H2O , CoF2•3H2O e CoF2•4H2O si ottengono anche trattando CoCO3, Co(OH)2 o CoO con soluzioni di HF.[1]

In laboratorio si può preparare CoF2 anche partendo da CoCl2.[3]

Usi

CoF2 è usato principalmente per preparare CoF3, un catalizzatore impiegato nella sintesi di fluorocarburi.[1]

Tossicità / Indicazioni di sicurezza

Il composto è disponibile in commercio. Per ingestione risulta corrosivo e tossico. La tossicità è dovuta principalmente alla liberazione di ioni fluoruro e acido fluoridrico. Per contatto con le mucose e gli occhi è corrosivo. È stato rilevato un effetto cancerogeno su animali di laboratorio, mentre non ci sono evidenze di effetti cancerogeni sull'uomo.[4]

Note

  1. ^ a b c d e f g Meshri 1998
  2. ^ Costa et al. 1993
  3. ^ Brauer 1963, p. 267.
  4. ^ Scheda del composto su Sigma-Aldrich [1]

Bibliografia

  • (EN) G. Brauer, Handbook of preparative inorganic chemistry, vol. 1, 2ª ed., New York, Academic Press, 1963, ISBN 0-323-16127-8.
  • M. M. R. Costa, J. A. Paixão, M. J. M. de Almeida, L. C. R. Andrade, Charge densities of two rutile structures: NiF2 and CoF2, in Acta cryst. B, vol. 49, n. 4, 1993, pp. 591−599, DOI:10.1107/S0108768193001624. URL consultato il 18 ottobre 2013.
  • (EN) Dayal T. Meshri, Fluorine compounds, inorganic - Cobalt, in Kirk-Othmer Encyclopedia of Chemical Technology, 4ª ed., John Wiley & Sons, 1998.

Altri progetti

  Portale Chimica: il portale della scienza della composizione, delle proprietà e delle trasformazioni della materia

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