Nickel(II) thiocyanate

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Nickel(II) thiocyanate
NiNCS2 powder.png
Sample of nickel(II) thiocyanate
NiSCN2 crystal structure.png
Crystal structure of nickel(II) thiocyanate
3D model (JSmol)
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EC Number
  • 237-205-1
  • InChI=1S/2CHNS.Ni/c2*2-1-3;/h2*3H;/q;;+2/p-2
  • C(#N)[S-].C(#N)[S-].[Ni+2]
Molar mass 174.86 g/mol[1]
Appearance green-brown powder
Density 2.59 g/cm3[1]
Melting point decomposes[1]
0.005 cm3/mol[2]
Hg(SCN)2 structure
GHS labelling:
GHS07: Exclamation markGHS08: Health hazardGHS09: Environmental hazard
H317, H334, H341, H350i, H360D, H372, H410
P201, P202, P260, P261, P264, P270, P272, P273, P280, P281, P285, P302+P352, P304+P341, P308+P313, P314, P321, P333+P313, P342+P311, P363, P391, P405, P501
Related compounds
Other anions
Nickel(II) bromide, Nickel(II) chloride, Nickel(II) iodide
Other cations
Copper(I) thiocyanate, Cobalt(II) thiocyanate, Mercury(II) thiocyanate, Ammonium thiocyanate
Potassium thiocyanate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Nickel(II) thiocyanate is a coordination polymer with formula Ni(SCN)2.[1] It is a green-brown solid and its crystal structure was determined first in 1982.[1]


The structure of Ni(SCN)2 was determined via single-crystal X-ray diffraction and consists of two-dimensional sheets held together through Van der Waals forces. It belongs to mercury thiocyanate structure-type and can be considered a distorted form of the NiBr2 (CdI2) structure. Each nickel is octahedrally coordinated by four sulfurs and two nitrogens. The sulfur end of the SCN- ligand is doubly bridging.[1]


Nickel(II) thiocyanate can be prepared via salt metathesis using the reaction of methanolic solutions of KSCN and nickel(II) perchlorate hexahydrate, filtering off the precipitated KClO4 to yield a solution of Ni(SCN)2. On removal of the methanol, a pure microcrystalline powder of Ni(SCN)2 can be obtained.


Nickel(II) thiocyanate, like nickel(II) iodide, nickel(II) bromide and nickel(II) chloride, is an antiferromagnet at low temperatures.[2]


  1. ^ a b c d e f Dubler, Erich; Relier, Armin; Oswald, H. R. (1982-01-01). "Intermediates in thermal decomposition of nickel(II) complexes: The crystal structures of Ni(SCN)2(NH3)2 and Ni(SCN)2". Zeitschrift für Kristallographie - Crystalline Materials. 161 (1–4). doi:10.1524/zkri.1982.161.14.265. ISSN 2196-7105. S2CID 201671776.
  2. ^ a b DeFotis, G. C.; Dell, K. D.; Krovich, D. J.; Brubaker, W. W. (1993-05-15). "Antiferromagnetism of Ni(SCN)2". Journal of Applied Physics. 73 (10): 5386–5388. doi:10.1063/1.353740. ISSN 0021-8979.