Chemistry:Nickel organic acid salts

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The nickel organic acid salts are organic acid salts of nickel. In many of these the ionised organic acid acts as a ligand. Nickel acetate has the formula (CH3COO)2Ni·4H2O. It has monodentate acetate and hydrogen bonding. A dihydrate also exists. Nickel acetate is used to seal anodised aluminium.[1]

Nickel formate Ni(HCOO)
2.2H
2O decomposes when heated to yield carbon dioxide, carbon monoxide, hydrogen, water and finely divided porous nickel.[2] All the nickel atoms are six coordinated, but half have four water molecules and two formate oxygens close to the atom, and the other half are coordinated by six oxygens of formate groups.[3]

Aspergillus niger is able to dispose of otherwise toxic levels of nickel in its environment by forming nickel oxalate dihydrate crystals.[4] nickel oxalate can also be formed in to various nanorods and nanofibres by use of surfacants.[5] When heated nickel oxalate dihydrate dehydrates at 258° and decomposes to Ni metal[6] over 316 °C.[7] Double oxalate salts where oxalate is a ligand on the nickel atom may be called oxalatonickelates.

Other organic acid salts of nickel include nickel oleate, nickel propionate, nickel butyrate, nickel caprylate, nickel lactate, nickel benzoate, nickel bis(acetyl acetonate), nickel salicylate, nickel alkyl phenyl salicylate. Nickel stearate forms a green solution, however when precipitated with alcohol a gel is produced, that also contains a mixture of basic salts, and free stearic acid.[8]

Nickel malonate, and nickel hydrogen malonate both crystallise with two molecules of water. They decomposes when heated to yield gaseous water, carbon dioxide, carbon monoxide, ethanol, acetic acid, methyl formate and ethyl formate. Nickel acetate exists as an intermediate and the final result is that solid nickel, nickel oxide, Ni3C and carbon remain.[9] With malonate nickel can form a bis-malonato-nickelate anion, which can form double salts.[10] Nickel maleate can be made from maleic acid and nickel carbonate in boiling water. A dihydrate crystallises from the water solution.[11] Nickel fumarate prepared from fumaric acid and nickel carbonate is pale green as a tetrahydrate, and mustard coloured as an anhydride. It decomposes when heated to 300° to 340° in vacuum. Decomposition mostly produces nickel carbide, carbon dioxide, carbon monoxide and methane. But also produced were butanes, benzene, toluene, and organic acid.[12]

Nickel succinate can form metal organic framework compounds.[13]

Nickel citrate complexes are found in leaves of some nickel accumulating plant species in New Caledonia such as Pycnandra acuminata.[14] Citrate complexes include NiHcit, NiHcit23−, Nicit−, Nicit24−, and Ni2H2cit24−. (ordered from low to high pH). Also there is Ni4H4cit35−. Nickel citrate is important in nickel plating.[15] When precipitation of nickel citrate is attempted a gel forms. This apparently consists of tangled fibres of [(C6H6O7)Ni]n, which can be reduced to nickel metal fibres less than a micron thick, and meters long.[16] Double nickel citrates exist, including tetraanion citrate when pH is over 9.5.[17] An amorphous nickel iron citrate Ni3Fe6O4(C6H6O7)8·6H2O produces carbon monoxide, carbon dioxide and acetone when heated over 200 °C leaving Trevorite, NiFe2O4 a nickel ferrite.[18] A green crystalline nickel citrate with formula Ni3(C6H5O7)2·10H2O melts at 529K and decomposition starts at 333K.[19]

Nickel glutarate in the form called Mil-77, [Ni20{(C5H6O4)20(H2O)8}]⋅40H2O is pale green. It crystallises in a porous structure containing twenty member rings. The 40 water molecules "occluded" in the porous channels come out when it is heated to 150 °C retaining the crystal framework. At 240 °C the crystal form changes and over 255° the remaining water is lost. Between 330° and 360° the organic components burn and it is destroyed.[20]

Cyclopropane carboxylic acid forms two basic salts with nickel, a hydrate Ni
9(OH)
2(H
2O)
6(C
4H
5O
2)
8 • 2H
2O with density 1.554 Mg/m3 and an anhydrous form Ni5(OH)2(C4H5O2)8 with density 2.172 mg/m3.[21]

Nickel trifluoroacetate tetrahydrate exists, as well as two emerald green acid trifluoroacetates, a bridged trinuclear form [Ni3(CF3COO)6(CF3COOH)6](CF3COOH) and a hydrated acid form [Ni3(CF3COO)6(CF3COOH)2(H2O)4](CF3COOH)2 both with triclinic crystal form. The first has density 2.205 and the second 2.124. They are made by dissolving the nickel trifluoroacetate tetrahydrate in trifluoroacetic acid either anhydrous or 1% hydrated.[22]

Nickel naphthenate is used as a fuel additive to suppress smoke,[23] as a rubber catalyst and as an oil additive.

When Nickel benzoate is heated in a vacuum, carbon dioxide, carbon monoxide, benzene, benzoic acid, phenol, biphenyl, nickel, nickel oxide, and nickel carbide are formed.[24] It can crystallise as anhydrous, a trihydrate or a tetrahydrate.[25]

Nickel terephthalate can be made by a double decomposition of sodium terephthalate and nickel nitrate. Nickel terephthalate precipitates. Its solubility is 0.38 g/100g water at 25 °C. In ammonium hydroxide a violet solution forms. Boiling acetic acid converts the nickel to nickel acetate. The terephthalate converts to a basic salt when boiled in water. Understating this compound is important when reducing coloured contaminants in polymers made from terephthalate.[26]

Listing

formula name mol struct cell Å ° V Z density colour refs
wt a b c β Å3 g/cm3
Ni(HCOO)
2 · 2H2O 		Nickel formate hydrate monoclinic 8.60 7.06 9.21 96°50′ 4 [3]
[Ni20{(C5H6O4)20(H2O)8}] • 40H2O Nickel glutarate cubic 16.581 4559 pale green [20]
Ni
9(OH)
2(H
2O)
6(C
4H
5O
2)
8 · 2H2O 		nickel cyclopropane carboxylate hydrate orthorhombic 14.810 24.246 24.607 8836 4 1.554 bright green [21]
Ni5(OH)2(C4H5O2)8 nickel cyclopropane carboxylate orthorhombic 19.406 18.466 21.579 90 7733 8 2.172 pale green [21]
[Ni3(CF3COO)6(CF3COOH)6](CF3COOH) Nickel acid trifluoroacetate trigonal 13.307 53.13 8148 6 2.205 emerald green [22]
[Ni3(CF3COO)6(CF3COOH)2(H2O)4](CF3COOH)2 Nickel acid trifluoroacetate hydrate triclinic 9.12 10.379 12.109 α=84.59° β=72.20° γ=82.80° 1080.9 1 2.124 emerald green [22]
K2[Ni(C6H5O7)(H2O)2]2·4H2O potassium nickel citrate triclinic 6.729 9.100 10.594 α=94.86 β=100.76 γ=103.70 613.5 1 1.942 green [27]
K2[Ni2(C6H5O7)2(H2O)4]·4H2O Dipotassium tetraaquabis(μ-citrato-k4O:O',O'',O''')nickelate(II) tetrahydrate 717.94 monoclinic 10.616 13.006 9.0513 93.09 1247.8 2 1.911 green [28]
N(CH3)4[Ni4(C6H4O7)3(OH)(H2O)]·18H2O tetramethyl ammonium nickel basic citrate triclinic 11.84 14.29 20.93 96.16 β=106.36 γ=94.89 3352 1 bright green extremely weak [27][29]
Na2[Ni(C6H4O7)] • 2H2O disodium nickel citrate green dec 371 [17]
(NH4)2[Ni(HCit) • 2H2O]2 • 2H2O Dimeric ammonium diaquocitratonickelate (II) dihydrate 639.79 triclinic 6.407 9.471 9.6904 α=105.064 β=91.99 γ=89.33 567.5 1 1.872 green [30]
(NH4)4[Ni(HCit)2] • 2H2O tetrammonium dicitratonickelate (11) dihydrate 545.10 monoclinic 9.361 13.496 9.424 115.476 1074.9 2 1.684 [30]
Na2[Ni(HCit) • 2H2O]2 • 2H2O Dimeric sodium diaquocitratonickelate (II) dihydrate [30]
K2[Ni(HCit) • 2H2O]2 • 2H2O Dimeric potassium diaquocitratonickelate (II) dihydrate [30]
(NH4)2[Ni(H2O)6][Ti(H2cit)3]2·6H2O 1547.43 hexagonal 15.562 7.690 1605.5 1 1.600 light green [31]
[Ni(C5H7O2)2]3 Nickel(II) acetylacetonate 256.91 orthorhombic 23.23 9.64 15.65 3505 4 1.46 dark green [32]
Ni[C4O4] • 2H2O nickel squarate ?cubic 8.068 8.068 8.068 90° 525 1.93 green [33]
Ni[C4O4] • 8H2O nickel squarate octahydrate 428.93 monoclinic 10.288 6.372 12.852 106.98 805.8 2 1.768 green [34]
Ni[C5O5] • 3H2O Nickel croconate trihydrate orthorhombic green [35]
K2[Ni(C5O5)2(H2O)2] • 4H2O Poly[[di-μ2-aqua-di-μ5-croconato(2-)-nickel(II)dipotassium(I)] tetrahydrate] 525.11 monoclinic 8.015 6.660 16.489 90.20 880.1 2 1.982 green [36]
Ni(C5H5COO)2 • 2H2O nickel dibenzoate tetrahydrate 354.98 monoclinic 6.1341 34.180 6.9793 95.331 1457.0 4 1.618 light green [25]
Ni(C5H5COOCOOH)2 • 6H2O nickel dihydrogen diphthalate hexahydrate monoclinic 16.024 5.574 12.500 113.42 2 1.611 [37]
Ni[C6H4(COO)2] • 4H2O Nickel terephthalate green [26]
Ni(OH)[C6H4(COO)(COOH)] • H2O basic nickel terephthalate green [26]

References

  1. ↑ Downie, T. C.; Harrison, W.; Raper, E. S.; Hepworth, M. A. (15 March 1971). "A three-dimensional study of the crystal structure of nickel acetate tetrahydrate". Acta Crystallographica Section B 27 (3): 706–712. doi:10.1107/S0567740871002802. 
  2. ↑ FOX, P (January 1971). "The development of internal structure during thermal decomposition: Nickel formate dihydrate". Journal of Catalysis 20 (1): 67–73. doi:10.1016/0021-9517(71)90007-8. 
  3. ↑ 3.0 3.1 Krogmann, Klaus; Mattes, Rainer (January 1963). "Die Kristallstruktur von Nickelformiat, [math]\displaystyle{ \ce{Ni(HCOO)2.2H2O} }[/math]" (in de). Zeitschrift für Kristallographie - Crystalline Materials 118 (1–6). doi:10.1524/zkri.1963.118.16.291. 
  4. ↑ Magyarosy, A.; Laidlaw, R.; Kilaas, R.; Echer, C.; Clark, D.; Keasling, J. (1 July 2002). "Nickel accumulation and nickel oxalate precipitation by Aspergillus niger". Applied Microbiology and Biotechnology 59 (2–3): 382–388. doi:10.1007/s00253-002-1020-x. PMID 12111174. 
  5. ↑ Vaidya, Sonalika; Rastogi, Pankaj; Agarwal, Suman; Gupta, Santosh K.; Ahmad, Tokeer; Antonelli, Anthony M.; Ramanujachary, K. V.; Lofland, S. E. et al. (August 2008). "Nanospheres, Nanocubes, and Nanorods of Nickel Oxalate: Control of Shape and Size by Surfactant and Solvent". Journal of Physical Chemistry C 112 (33): 12610–12615. doi:10.1021/jp803575h. 
  6. ↑ "Pyrophoric Nickel Hydrogenation Catalyst / Nickel Oxalate Preparation". https://m.youtube.com/watch?v=4gO92eqQcB4&t=407s. 
  7. ↑ Zhan, Dan; Cong, Changjie; Diakite, Kahirou; Tao, Youtian; Zhang, Keli (June 2005). "Kinetics of thermal decomposition of nickel oxalate dihydrate in air". Thermochimica Acta 430 (1–2): 101–105. doi:10.1016/j.tca.2005.01.029. 
  8. ↑ Soyenkoff, Basil (January 1929). "Benzene Dispersions of Basic Soaps of Nickel and Iron". Journal of Physical Chemistry 34 (11): 2519–2538. doi:10.1021/j150317a006. 
  9. ↑ Mohamed, Mohamed A; Galwey, Andrew K; Halawy, Samih A (December 1998). "Kinetic and thermodynamic studies of the non-isothermal decompositions of nickel malonate dihydrate and nickel hydrogen malonate dihydrate". Thermochimica Acta 323 (1–2): 27–36. doi:10.1016/S0040-6031(98)00492-4. 
  10. ↑ Xiao, Xunwen; Xu, Wei; Li, Yan; Zhang, Bin; Zhu, Daoben (12 December 2003). "Dipotassium diaquabis(malonato-κ2O,O')nickelate(II) dihydrate". Acta Crystallographica Section E 60 (1): m48–m49. doi:10.1107/S1600536803027508. 
  11. ↑ McGinn, M. J.; Wheeler, B. R.; Galwey, A. K. (1971). "Thermal decomposition of nickel maleate". Transactions of the Faraday Society 67: 1480. doi:10.1039/TF9716701480. 
  12. ↑ McGinn, M. J.; Wheeler, B. R.; Galwey, A. K. (1970). "Thermal decomposition of nickel fumarate". Transactions of the Faraday Society 66: 1809. doi:10.1039/TF9706601809. 
  13. ↑ Guillou, Nathalie; Livage, Carine; Férey, Gérard (December 2006). "Cobalt and Nickel Oxide Architectures in Metal Carboxylate Frameworks: From Coordination Polymers to 3D Inorganic Skeletons". European Journal of Inorganic Chemistry 2006 (24): 4963–4978. doi:10.1002/ejic.200600663. 
  14. ↑ Lee, Julian; Reeves, Roger D.; Brooks, Robert R.; Jaffré, Tanguy (January 1978). "The relation between nickel and citric acid in some nickel-accumulating plants". Phytochemistry 17 (6): 1033–1035. doi:10.1016/S0031-9422(00)94274-2. Bibcode: 1978PChem..17.1033L. 
  15. ↑ Rode, Sabine; Henninot, Christophe; Matlosz, Michael (2005). "Complexation Chemistry in Nickel and Copper-Nickel Alloy Plating from Citrate Baths". Journal of the Electrochemical Society 152 (4): C248. doi:10.1149/1.1869980. Bibcode: 2005JElS..152C.248R. 
  16. ↑ Shen, Xiangqian; Jing, Maoxiang; Wang, Taoping; Cao, Kai (June 2006). "Preparation of Superfine Ni and Fe Fibers by the Organic Gel-Thermal Reduction Method". Rare Metal Materials and Engineering. http://en.cnki.com.cn/Article_en/CJFDTOTAL-COSE200606023.htm. 
  17. ↑ 17.0 17.1 Wang, Lian-Ying; Wu, Guo-Qing; Evans, David G. (July 2007). "Synthesis and characterization of a layered double hydroxide containing an intercalated nickel(II) citrate complex". Materials Chemistry and Physics 104 (1): 133–140. doi:10.1016/j.matchemphys.2007.02.098. 
  18. ↑ Gajbhiye, N.S.; Prasad, Seema (August 1996). "Thermal decomposition of hexahydrated nickel iron citrate". Thermochimica Acta 285 (2): 325–336. doi:10.1016/0040-6031(96)02906-1. 
  19. ↑ Masłowska, J. (September 1984). "Thermal decomposition and thermofracto-chromatographic studies of metal citrates". Journal of Thermal Analysis 29 (5): 895–904. doi:10.1007/BF02188835. 
  20. ↑ 20.0 20.1 Guillou, Nathalie; Livage, Carine; Drillon, Marc; Férey, Gérard (10 November 2003). "The Chirality, Porosity, and Ferromagnetism of a 3D Nickel Glutarate with Intersecting 20-Membered Ring Channels". Angewandte Chemie International Edition 42 (43): 5314–5317. doi:10.1002/anie.200352520. PMID 14613163. 
  21. ↑ 21.0 21.1 21.2 Forster, Paul M; Yang, Zuag; Cheetham, Anthony K (April 2003). "Open framework metal monocarboxylates: nickel cyclopropionates containing 16- and 18-membered rings". Solid State Sciences 5 (4): 635–642. doi:10.1016/S1293-2558(03)00055-4. Bibcode: 2003SSSci...5..635F. 
  22. ↑ 22.0 22.1 22.2 Tokareva, A. O.; Tereshchenko, D. S.; Boltalin, A. I.; Troyanov, S. I. (September 2006). "Acid Co(II) and Ni(II) trifluoroacetate complexes: Synthesis and crystal structure". Russian Journal of Coordination Chemistry 32 (9): 663–668. doi:10.1134/S1070328406090077. 
  23. ↑ SALOOJA, K. C. (March 1972). "Burner Fuel Additives*". Combustion Science and Technology 5 (1): 243–249. doi:10.1080/00102207208952528. 
  24. ↑ Galwey, A. K. (1965). "1152. The thermal decomposition of nickel benzoate and of the nickel salt of cyclohexanecarboxylic acid". Journal of the Chemical Society: 6188. doi:10.1039/JR9650006188. 
  25. ↑ 25.0 25.1 Vráblová, Anna; Falvello, Larry R.; Campo, Javier; Miklovič, Jozef; Boča, Roman; Černák, Juraj; Tomás, Milagros (February 2016). "Preparation, First Structure Analysis, and Magnetism of the Long-Known Nickel Benzoate Trihydrate - A Linear Ni···Ni···Ni Polymer and Its Parallels with the Active Site of Urease". European Journal of Inorganic Chemistry 2016 (6): 928–934. doi:10.1002/ejic.201501255. 
  26. ↑ 26.0 26.1 26.2 Sherif, Fawzy G. (1 September 1970). "Heavy Metal Terephthalates". Industrial & Engineering Chemistry Product Research and Development 9 (3): 408–412. doi:10.1021/i360035a026. 
  27. ↑ 27.0 27.1 Baker, Edward N.; Baker, Heather M.; Anderson, Bryan F.; Reeves, Roger D. (January 1983). "Chelation of nickel(II) by citrate. The crystal structure of a nickel–citrate complex, [math]\displaystyle{ \ce{K2[Ni(C6H5O7)(H2O)2]2.4H2O} }[/math]". Inorganica Chimica Acta 78: 281–285. doi:10.1016/S0020-1693(00)86530-5. 
  28. ↑ Yao, Hua-Gang; Huang, Jia-Na; Deng, Run-Kang; Yao, Zhi-Bang (17 August 2013). "Dipotassium tetraaquabis(μ-citrato-κ : ′, ′′, ′′′)nickelate(II) tetrahydrate". Acta Crystallographica Section E 69 (9): m502–m503. doi:10.1107/S1600536813022630. PMID 24426997. 
  29. ↑ Strouse, Jane; Layten, Steven W.; Strouse, Charles E. (January 1977). "Structural studies of transition metal complexes of triionized and tetraionized citrate. Models for the coordination of the citrate ion to transition metal ions in solution and at the active site of aconitase". Journal of the American Chemical Society 99 (2): 562–572. doi:10.1021/ja00444a041. PMID 830693. 
  30. ↑ 30.0 30.1 30.2 30.3 Zhou, Zhao-Hui; Lin, Yi-Ji; Zhang, Hong-Bin; Lin, Guo-Dong; Tsai, Khi-Rui (5 October 2006). "SYNTHESES, STRUCTURES AND SPECTROSCOPIC PROPERTIES OF NICKEL(II) CITRATO COMPLEXES, [math]\displaystyle{ \ce{(NH4)2[Ni(Hcit)(H2O)2]2-2H2O} }[/math] AND [math]\displaystyle{ \ce{(NH4)4[Ni(Hcit)2]-2H2O} }[/math]". Journal of Coordination Chemistry 42 (1–2): 131–141. doi:10.1080/00958979708045286. 
  31. ↑ Deng, Yuan-Fu; Zhang, Hua-Lin; Hong, Qi-Ming; Weng, Wei-Zheng; Wan, Hui-Lin; Zhou, Zhao-Hui (November 2007). "Titanium-based mixed oxides from a series of titanium(IV) citrate complexes". Journal of Solid State Chemistry 180 (11): 3152–3159. doi:10.1016/j.jssc.2007.08.033. Bibcode: 2007JSSCh.180.3152D. 
  32. ↑ Bullen, G. J.; Mason, R.; Pauling, Peter (April 1965). "The Crystal and Molecular Structure of Bis(acetylacetonato)nickel (II)". Inorganic Chemistry 4 (4): 456–462. doi:10.1021/ic50026a005. 
  33. ↑ Habenschuss, Michael (1974). "An x-ray, spectroscopic, and magnetic study of the structure of nickel squarate dihydrate, [math]\displaystyle{ \ce{NiC4O4.2H2O} }[/math]". Journal of Chemical Physics 61 (3): 852. doi:10.1063/1.1682025. Bibcode: 1974JChPh..61..852H. 
  34. ↑ Brach, I.; Rozière, J.; Anselment, B.; Peters, K. (15 March 1987). "An X-ray structure determination of cobalt and nickel squarate octahydrate, [math]\displaystyle{ \ce{[M(H2O)6](C4HO4)2.2H2O} }[/math] (M=Ni,Co)". Acta Crystallographica Section C 43 (3): 458–460. doi:10.1107/S0108270187095386. 
  35. ↑ West, Robert.; Niu, Hsien Ying. (September 1963). "New Aromatic Anions. VI. Complexes of Croconate Ion with Some Divalent and Trivalent Metals". Journal of the American Chemical Society 85 (17): 2586–2588. doi:10.1021/ja00900a013. 
  36. ↑ Chen, Hong-Yu; Fang, Qi; Xue, Gang; Yu, Wen-Tao (19 November 2005). "Polydi-μ2-aqua-di-μ5-croconato(2–)-nickel(II)dipotassium(I) tetrahydrate". Acta Crystallographica Section C 61 (12): m535–m537. doi:10.1107/S0108270105036322. PMID 16330841. 
  37. ↑ Adiwidjaja, G.; Küppers, H. (15 May 1976). "Nickel dihydrogen diphthalate hexahydrate". Acta Crystallographica Section B 32 (5): 1571–1574. doi:10.1107/S0567740876005840. 



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