Iodure de magnésium

Iodure de magnésium
Image illustrative de l’article Iodure de magnésium
__ Mg2+     __ I
Structure cristalline de l'iodure de magnésium
Identification
No CAS 10377-58-9
75535-11-4 (hexahydrtae)
7790-31-0 (octahydrate)
No ECHA 100.030.738
No CE 233-825-1
PubChem 66322
SMILES
InChI
Apparence poudre blanche[1]
Propriétés chimiques
Formule I2Mg
Masse molaire[2] 278,113 9 ± 0,000 7 g/mol
I 91,26 %, Mg 8,74 %,
Propriétés physiques
fusion 637 °C[1]
Solubilité 1 480 g·L-1[1]
Précautions
NFPA 704[1]

Symbole NFPA 704.

 

Unités du SI et CNTP, sauf indication contraire.

L'iodure de magnésium est un composé chimique de formule MgI2. Il se présente sous la forme d'une poudre blanche très hygroscopique et cristallise dans le système trigonal avec le groupe d'espace P3m1 (no 164) et a = 414 pm, c = 688 pm. C'est un halogénure ionique très soluble dans l'eau. Il est stable thermiquement sous une atmosphère d'hydrogène mais se décompose progressivement à l'air libre en donnant de l'iode I2, de l'hydroxyde de magnésium Mg(OH)2 et de l'eau H2O tandis que sa couleur vire au brun. Il se décompose entièrement en oxyde de magnésium lorsqu'il est chauffé à l'air libre. Pour conserver ses propriétés, il doit être stocké sous atmosphère inerte sèche, généralement d'argon. En présence d'humidité, il forme différents hydrates : MgI2·6H2O, MgI2·8H2O, MgI2·9H2O.

L'iodure de magnésium peut être préparé par traitement d'oxyde de magnésium MgO, d'hydroxyde de magnésium Mg(OH)2 ou de carbonate de magnésium MgCO3 avec de l'acide iodhydrique HI[3] :

MgO + 2 HI ⟶ MgI2 + H2O ;
Mg(OH)2 + 2 HI ⟶ MgI2 + 2 H2O ;
MgCO3 + 2 HI ⟶ MgI2 + CO2 + H2O.

Il est également possible d'obtenir de l'iodure de magnésium en mélangeant des poudres d'iode et de magnésium élémentaires sous atmosphère strictement anhydre, par exemple dans l'éther diéthylique comme solvant. Une autre méthode consiste à faire réagir du magnésium avec de l'iodure de mercure(II) (en) HgI2[4] :

Mg + HgI2 (en) ⟶ MgI2 + Hg.

L'utilisation d'iodure de magnésium dans une réaction de Baylis-Hillman tend à donner des composés (Z)-vinyliques[5].

Notes et références

  1. a b c et d « Fiche du composé Magnesium iodide, ultra dry, 99.996% (metals basis)  », sur Alfa Aesar (consulté le ).
  2. Masse molaire calculée d’après « Atomic weights of the elements 2007 », sur www.chem.qmul.ac.uk.
  3. (en) Pradyot Patnaik, Handbook of Inorganic Chemicals, McGraw-Hill Professional, 2003, p. 527–528. (ISBN 0-07-049439-8)
  4. (de) Georg Brauer, en collaboration avec Marianne Baudler, Handbuch der Präparativen Anorganischen Chemie, 3e éd. révisée, vol. II, Ferdinand Enke, Stuttgart 1978, p. 906. (ISBN 3-432-87813-3)
  5. (en) Lutz F. Tietze, « Domino Reactions in Organic Synthesis », Chemical Reviews, vol. 96, no 1,‎ , p. 115-136 (PMID 11848746, DOI 10.1021/cr950027e, lire en ligne)

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