Nickel(II) chloride

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Nickel(II) chloride
Nickel(II) chloride hexahydrate
IUPAC name Nickel(II) chloride
Other names Nickelous chloride
Identifiers
CAS number 7718-54-9 (anhydr.)
7791-20-0 (hexahydrate)
EINECS number 231-743-0
RTECS number QR6480000
Properties
Molecular formula NiCl2
Density 3.55 g/cm3, anhyd.
Melting point

1001 °C
hydrate loses water

Solubility in water 254 g/100 mL (20 °C)
Solubility in ethanol Soluble (hexahydrate)
Structure
Crystal structure Monoclinic
Coordination
geometry
octahedral at Ni
Thermochemistry
Std enthalpy of
formation
ΔfHo298
-304.93 kJ/mol
(anhyd form)
Standard molar
entropy
So298
98.11 J.K−1.mol−1
for the hexahydrate?
Hazards
MSDS ScienceLab.com
NFPA 704
 
3
 
 
Related compounds
Other anions Nickel(II) bromide
Nickel(II) iodide
Other cations Cadmium(II) chloride
Palladium(II) chloride
Platinum(II) chloride
Related compounds Cobalt(II) chloride
Copper(II) chloride
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)

Infobox disclaimer and references

Nickel(II) chloride (or just nickel chloride), is the chemical compound NiCl2. The anhydrous salt is yellow, but the more familiar hydrate NiCl2·6H2O is green. A dihydrate is also known. In general nickel(II) chloride, in various forms, is the most important source of nickel for chemical synthesis. Nickel salts are carcinogenic.

Contents

[edit] Production and syntheses

Probably the largest scale production of nickel chloride involves the extraction with hydrochloric acid of nickel matte and residues obtained from roasting refining nickel-containing ores.

NiCl2·6H2O is rarely prepared in the laboratory because it is inexpensive and has a long shelf-life. The hydrate can be converted to the anhydrous form upon heating in thionyl chloride or by heating under a stream of HCl gas. Simply heating the hydrates does not afford the anhydrous dichloride.

NiCl2·6H2O + 6 SOCl2 → NiCl2 + 6 SO2 + 12 HCl

The dehydration is accompanied by a color change from green to yellow.[1]

[edit] Structure and properties

NiCl2 adopts the CdCl2 structure.[2] In this motif, each Ni2+ center is coordinated to six Cl- centers, and each chloride is bonded to three Ni(II) centers. In NiCl2 the Ni-Cl bonds have “ionic character”. Yellow NiBr2 and black NiI2 adopt similar structures, but with a different packing of the halides, adopting the CdI2 motif.

In contrast, NiCl2·6H2O consists of separated trans-[NiCl2(H2O)4] molecules linked more weakly to adjacent water molecules. Note that only four of the six water molecules in the formula are bound to the nickel, and the remaining two are water of crystallisation.[2] Cobalt(II) chloride hexahydrate has a similar structure.

Many nickel(II) compounds are paramagnetic, due to the presence of two unpaired electrons on each metal center. Square planar nickel complexes are, however, diamagnetic.

[edit] Coordination chemistry

Most of the reactions ascribed to “nickel chloride” involve the hexahydrate, although specialized reactions require the anhydrous form.

Reactions starting from NiCl2·6H2O can be used to form a variety of nickel coordination complexes because the H2O ligands are rapidly displaced by ammonia, amines, thioethers, thiolates, and organophosphines. In some derivative, the chloride remains within the coordination sphere, whereas chloride is displaced with highly basic ligands. Illustrative complexes include:

Complex Color Magnetism Geometry
[Ni(NH3)6]Cl2 violet paramagnetic octahedral
NiCl2(dppe) orange diamagnetic square planar
[Ni(CN)4]2- colorless diamagnetic square planar
[NiCl4]2-[3][4] blue paramagnetic tetrahedral

Some nickel chloride complexes exist as an equilibrium mixture of two geometries; these examples are some of the most dramatic illustrations of structural isomerism for a given coordination number. For example, NiCl2(PPh3)2, containing four-coordinate Ni(II), exists in solution as a mixture of both the diamagnetic square planar and the paramagnetic tetrahedral isomers. Square planar complexes of nickel can often form five-coordinate adducts.

NiCl2 is the precursor to acetylacetonate complexes Ni(acac)2(H2O)2 and the benzene-soluble (Ni(acac)2)3, which is a precursor to Ni(1,5-cyclooctadiene)2, an important reagent in organonickel chemistry.

In the presence of water scavengers, hydrated nickel(II) chloride reacts with dimethoxyethane (dme) to form the molecular complex NiCl2(dme)2. The dme ligands in this complex are labile. For example, this complex reacts with sodium cyclopentadienide to give the sandwich compound nickelocene.

[edit] Applications in organic synthesis

NiCl2 and its hydrate are occasionally useful in organic synthesis.[5]

  • As a mild Lewis acid, e.g. for the regioselective isomerization of dienols:
General reaction scheme for the isomerisation of dienols
  • In combination with CrCl2 for the coupling of an aldehyde and a vinylic iodide to give allylic alcohols.
  • For selective reductions in the presence of LiAlH4, e.g. for the conversion of alkenes to alkanes.
  • As a precursor to “nickel boride”, prepared in situ from NiCl2 and NaBH4. This reagent behaves like Raney Nickel, comprising an efficient system for hydrogenation of unsaturated carbonyl compounds.
  • As a precursor to finely divided Ni by reduction with Zn, for the reduction of aldehydes, alkenes, and nitro aromatic compounds. This reagent also promotes homo-coupling reactions, that is 2RX → R-R where R = aryl, vinyl.
  • As a catalyst for making dialkyl arylphosphonates from phosphites and aryl iodide, ArI:
ArI + P(OEt)3 → ArP(O)(OEt)2 + EtI

[edit] Other uses

Nickel chloride solutions are used for electroplating.

[edit] References

  1. ^ Pray, A. P. (1990). "Anhydrous Metal Chlorides". Inorganic Syntheses 28: 321-2. doi:10.1002/9780470132401.ch36. 
  2. ^ a b , Wells, A. F. Structural Inorganic Chemistry, Oxford Press, Oxford, United Kingdom, 1984.
  3. ^ Gill, N. S. and Taylor, F. B. (1967). "Tetrahalo Complexes of Dipositive Metals in the First Transition Series". Inorganic Syntheses 9: 136-142. doi:10.1002/9780470132401.ch37. 
  4. ^ G. D. Stucky, J. B. (1967). "The Crystal and Molecular Structure of Tetraethylammonium Tetrachloronickelate(II)". Acta Crystallographica 23: 1064-1070. doi:10.1107/S0365110X67004268. 
  5. ^ Tien-Yau Luh, Yu-Tsai Hsieh Nickel(II) Chloride" in Encyclopedia of Reagents for Organic Synthesis (L. A. Paquette, Ed.) 2001 J. Wiley & Sons, New York. DOI: 10.1002/047084289X.rn012. Article Online Posting Date: April 15, 2001.

[edit] External links