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Compounds of nickel are chemical compounds containing the element nickel which is a member of the group 10 of the periodic table. Most compounds in the group have an oxidation state of +2. Nickel is classified as a transition metal with nickel(II) having much chemical behaviour in common with iron(II) and cobalt(II). Many salts of nickel(II) are isomorphous with salts of magnesium due to the ionic radii of the cations being almost the same. Nickel forms many coordination complexes. Nickel tetracarbonyl was the first pure metal carbonyl produced, and is unusual in its volatility. Metalloproteins containing nickel are found in biological systems.

Nickel forms simple binary compounds with non metals including halogens, chalcogenides, and pnictides. Nickel ions can act as a cation in salts with many acids, including common oxoacids Salts of the hexaaqua ion (Ni · 6 H₂O²⁺) are especially well known. Many double salts containing nickel with another cation are known. There are organic acid salts. Nickel can be part of a negatively charged ion (anion) making what is called a nickellate. Numerous quaternary compounds (with four elements) of nickel have been studied for super conductivity properties, as nickel is adjacent to copper and iron in the periodic table can can form compounds with the same structure as the high-temperature superconductors that are known.

General

Colour

Most of the common salts of nickel are green due to the presence of hexaaquanickel(II) ion, Ni(H₂O)₆²⁺.

Geometry

Nickel atoms can connect to surrounding atoms or ligands in a variety of ways. Six coordinated nickel is the most common and is octahedral, but this can be distorted if ligands are not equivalent. For four coordinate nickel arrangements can be square planar, or tetrahedral. Five coordinated nickel is rarer.

Magnetism

Some nickel compounds are ferromagnetic at sufficiently low temperatures. In order to show magnetic properties the nickel atoms have to be close enough together in the solid structure.

Binary compounds

A binary compound of nickel contains one other element. Substances that contain only nickel atoms are not actually compounds.

In a noble gas matrix, nickel can form dimers, a molecule with two nickel atoms: Ni₂.^[1] Ni₂ has a bonding energy of 2.07±0.01 eV. For Ni₂⁺ the bond energy is around 3.3 eV. Nickel dimers and other clusters can also be formed in a gas and plasma phase by shooting a powerful laser at a nickel rod in cold helium gas.^[2]

Oxides

Nickel oxides include Nickel(II) oxide and Nickel(III) oxide.

Hydroxides

Nickel hydroxides are used in nickel–cadmium and Nickel–metal hydride batteries. Nickel(II) hydroxide Ni(OH)₂, the main hydroxide of nickel is coloured apple green. It is known as the mineral theophrastite. β-NiO(OH) is a black powder with nickel in the +3 oxidation state. It can be made by oxidising nickel nitrate in a cold alkaline solution with bromine. A mixed oxidation state hydroxide Ni₃O₂(OH)₄ is made if oxidation happens in a hot alkaline solution. A Ni⁴⁺ hydroxide: nickel peroxide hydrate NiO₂ · H₂O, can be made by oxidising with alkaline peroxide. It is black, and unstable and oxidises water.

Halides

Nickel(II) fluoride NiF₂ is yellow, crystallising in the rutile structure and can form a trihydrate, NiF₂·3H₂O.^[3] A tetrahydrate also exists.^[4]

Nickel chloride NiCl₂ is yellow, crystallising in the cadmium chloride structure. It can form a hexahydrate, NiCl₂·6H₂O, a tetrahydrate NiCl₂·4H₂O over 29 °C and a dihydrate, NiCl₂·2H₂O over 64 °C.^[3]

nickel bromide NiBr₂ is yellow, also crystallising in the cadmium chloride structure. It can form a hexahydrate, NiBr₂·6H₂O.^[3] Crystallisation above 29° forms a trihydrate NiBr₂·3H₂O, and a dihydrate NiBr₂·2H₂O.^[5] Nonahydrate, NiBr₂·9H₂O can crstallise from water below 2 °C.^[3] Nickelous hexammine bromide Ni(NH₃)₆Br₂is violet or blue. It is soluble in boiling aqueous ammonia, but is insoluble in cold.^[3] Diammine, monoammine, and dihydrazine nickel bromides also exist.^[3]

With four bromide atoms nickel(II) forms a series of salts called tetrabromonickelates.

Nickel iodide NiI₂ is black, also crystallising in the cadmium chloride structure. It can form a green hexahydrate, NiI₂·6H₂O.^[3] Nickel iodide has a brown diammine NiI₂•2NH₃ and a bluish-violet hexammine NiI₂•6NH₃.^[3]

Nickel(III) fluoride NiF₃

Nickel(IV) fluoride NiF₄

Chalcogenides

By reacting nickel with chalcogens, nickel sulfide, nickel selenide, and nickel telluride are formed. There are numerous sulfides: Ni_1.5S, Ni₁₇S₁₈, Ni₃S₂ (heazlewoodite), Ni₃S₄ (polydymite), Ni₉S₈ (godlevskite), NiS (millerite) and two other NiS forms, NiS₂ (vaesite) in pyrite structure. Black nickel tetrasulfide NiS₄ is formed from ammonium polysulfide and nickel in water solution. Mixed and double sulfides of nickel also exist. Nickel with selenium forms several compounds Ni_1−xSe 0≤x≤0.15, Ni₂Se₃, NiSe₂ also known as a mineral penroseite.

Nickel forms two different polonides by heating nickel and polonium together: NiPo and NiPo₂.^[6]

Pnictides

Non-stoichiometric compounds of nickel with phosphorus, arsenic and antimony exist, and some are found in nature. One interstitial nitride has formula Ni₃N (hexagonal P6322, Z = 2, a = 4.6224 Å and c = 4.3059 Å).^[7] In a solid nitrogen matrix, nickel atoms combine with nitrogen molecules to yield Ni(N₂)₄.^[1]

Nickel phosphide Ni₂P has density 7.33 and melts at 1100 °C.^[4]

The mineral Nickelskutterudite has formula NiAs_2-3, nickeline has formula NiAs and breithauptite has formula NiSb. NiAs melts at 967° and has density 7.77. NiSb melts at 1174°. It has the highest density of a nickel compound at 8.74 g/cm³.^[4]

NiAsS gersdorffite, and NiSbS ullmannite, NiAsSe Jolliffeite are pnictide/chalcogenide compounds that occur as minerals.

Other

Nickel also forms carbides and borides. Nickel boride can take the forms Ni₂B (a green/black solid), NiB, Ni₃B, o-Ni₄B₃ and m-Ni₄B₃.^[8] Nickel hydride NiH is only stable under high pressures of hydrogen.

Diatomic molecules

Hot nickel vapour reacting with other atoms in the gas phase can produce molecules consisting of two atoms. Nickel monofluoride can be observed by its emission spectrum in the gas phase.^[9]

Nickel subchloride NiCl is formed in gaseous form when nickel chloride is vapourised, and is the most common in the gas phase above 1450 K. It is formed when nickel is exposed to hot, low pressure chlorine.^[10]

Nickel monobromide, NiBr can exist in the gas phase when an electric discharge goes through NiBr₂ gas.^[9]^[11]^[12]

Nickelmonoiodide can exist in the gas phase.^[9]

Formula	distance	energy	refs
	pm	kcal/mol
NiH
NiF
NiCl
NiBr
NiI
Ni₂		46	^[2]
NiAu		58	^[13]

Alloys

Compounds of nickel with other metals can be called alloys. The substances with fixed composition include nickel aluminide (NiAl) melting at 1638° with hexagonal structure.^[4] NiY, NiY₃, Ni₃Y, Ni₄Y, NiGd₃,^[14]

BaNi₂Ge₂ changes structure from orthorhombic to tetragonal around 480 °C.^[15] THis is a ternary intermetallic compound. Others include BaNiSn₃ and the superconductors SrNi₂Ge₂, SrNi₂P₂, SrNi₂As₂, BaNi₂P₂, BaNi₂As₂.^[15]

Simple salts

Oxo acid salts

bright green crystals in two clusters on a white and grey rock — Mint green Annabergite, a nickel arsenite

Important nickel oxo acid salts include nickel(II) sulfate can crystallise with six water molecules yielding Retgersite or with seven making Morenosite which is isomorphic to Epsom salts. These contain the hexaquanickel(II) ion.^[16] There is also an anhydrous form, a dihydrate and a tetrahydrate, the last two crystallised from sulfuric acid. The hexahydrate has two forms, a blue tetragonal form, and a green monoclinic form, with a transition temperature around 53 °C.^[17] The heptahydrate crystallises from water below 31.5 above this blue hexhydrate forms, and above 53.3 the green form.^[18] Heating nickel sulfate dehydrates it, and then 700° it loses sulfur trioxide, sulfur dioxide and oxygen.

Fluoro acid salts

Nickel tetrafluoroborate, Ni(BF₄)₂ · 6 H₂O is very soluble in water, alcohol and acetonitrile. It is prepared by dissolving nickel carbonate in tetrafluoroboric acid.^[19]^[20] Nickel tetrafluoroberyllate NiBeF₄•xH₂O, can be hydrated with six or seven water molecules.^[21] Both nickel hexafluorostannate ${\ce {NiSnF6.6H2O}}$ and nickel fluorosilicate ${\ce {NiSnF6.6H2O}}$ crystallise in the trigonal system.^[22] Nickel hexafluorogermanate NiGeF₆ has a rosy-tan colour and a hexagonal crystal with a = 5.241 Å unit cell volume is 92.9 Å³. It is formed in the reaction with GeF₄ and K₂NiF₆.^[23] Nickel fuorotitanate ${\ce {NiTiF6.6H2O}}$ crystallises in hexagonal green crystals. It can be made by dissolving nickel carbonate, and titanium dioxide in hydrofluoric acid. The crystal dimensions are a = 9.54, c = 9.91 density = 2.09 (measure 2.03).^[24]

Ni(AsF₆)₂, Ni(SbF₆)₂, Ni(BiF₆)₂ are made by reacting the hexafluoro acid with NiF₂ in hydrofluoric acid.^[23] They all have hexagonal crystal structure, resembling the similar salts of the other first row transition metals.^[23] For Ni(AsF₆)₂ a = 4.98, c = 26.59, and V = 571, formula weight Z=3.^[23] Ni(SbF₆)₂ is yellow with a = 5.16Å, c = 27.90Å Z = 3. The structure resembles LiSbF₆, but with every second metal along the c axis missing.^[25]

Others include the green fluorohafnate NiHfF₆ · 6 H₂O, and Ni₂HfF₈ · 12 H₂O,^[26] NiZrF₆ · 6 H₂O^[27]

Chloroacid salts

Nickel tetrachloroiodate Ni(ICl₄)₂ can be made by reacting iodine with nickel chloride. It consists of green needles.^[28]

Nitrogen anion salts

Nickel cyanide tetrahydrate Ni(CN)₂ · 4 H₂O is insoluble in water, but dissolves in aqueous ammonia.^[4] It forms double salts with interesting structures.^[29]

Nickel azide Ni(N₃)₂ is a sensitive explosive. It can be made by treating nickel carbonate with hydrazoic acid. Acetone causes the precipitation of the hydrous solid salt, which is green. At 490K it slowly decomposes to nitrogen and nickel metal powder, losing a half of the nitrogen in four hours.^[30] Nickel azide is complexed by one azo group when dissolved in water, but in other solvents, the nickel atom can have up to four azo groups attached.^[31] Nickel azide forms a dihydrate: Ni(N₃)₂ · 2 H₂O and a basic salt called nickel hydroxy azide Ni(OH)N₃.^[32]

Nickel amide, Ni(NH₂)₂ is a deep red compound that contains Ni₆ clusters surrounded by 12 NH₂ groups.^[33] Nickel amide also forms a series of double salts. Other homoleptic nickel amides derived by substituting the hydrogen atoms are Ni[N(C₆H₅)₂]₂ (diphenyl) and boryl amides Ni[NBMes₂Mes]₂ and Ni[NBMes₂C₆H₅]₂.^[34]

Organic acid salts

Nickel acetate has the formula (CH₃COO)₂Ni·4H₂O. It has monodentate acetate and hydrogen bonding. A dihdrate also exists. Nickel acetate is used to seal anodised aluminium.^[35]

Nickel formate ${\ce {Ni(HCOO)2.2H2O}}$ decomposes when heated to yield carbon dioxide, carbon monoxide, hydrogen, water and finely divided porous nickel.^[36] 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.^[37]

Aspergillus niger is able to dispose of otherwise toxic levels of nickel in its environment by forming nickel oxalate dihydrate crystals.^[38] nickel oxalate can also be formed in to various namorods and nanofibres by use of surfacants.^[39] When heated nickel oxalate dihydrate dehydrates at 258° and decomposes to NiO over 316 °C.^[40] 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.^[41]

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.^[42] With malonate nickel can form a bis-malonato-nickelate anion, which can form double salts.^[43] Nickel maleate can be made from maleic acid and nickel carbonate in boiling water. A dihydrate crystallises from the water solution.^[44] 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.^[45]

Nickel succinate can form metal organic framework compounds.^[46]

Nickel citrate complexes are found in leaves of some nickel accumulating plant species in New Caledonia such as Pycnandra acuminata.^[47] 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.^[48] 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.^[49] Double nickel citrates exist, including tetraanion citrate when pH is over 9.5.^[50] 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.^[51] A green crystalline nickel citrate with formula Ni₃(C₆H₅O₇)₂·10H₂O melts at 529K and decomposition starts at 333K.^[52]

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.^[53]

Cyclopropane carboxylic acid forms two basic salts with nickel, a hydrate ${\ce {Ni9(OH)2(H2O)6(C4H5O2)8.2H2O}}$ with density 1.554 Mg/m³ and an anhydrous form Ni₅(OH)₂(C₄H₅O₂)₈ with density 2.172 mg/m³.^[54]

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.^[55]

Nickel naphthenate is used as a fuel additive to suppress smoke,^[56] 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.^[57] It can crystallise as anhydrous, a trihydrate or a tetrahydrate.^[58]

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.^[59]

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				^[37]
[Ni₂₀{(C₅H₆O₄)₂₀(H₂O)₈}] · 40 H₂O	Nickel glutarate		cubic	16.581				4559			pale green	^[53]
Ni₉(OH)₂(H₂O)₆(C₄H₅O₂)₈·2H₂O	nickel cyclopropane carboxylate hydrate		orthorhombic	14.810	24.246	24.607		8836	4	1.554	bright green	^[54]
Ni₅(OH)₂(C₄H₅O₂)₈	nickel cyclopropane carboxylate		orthorhombic	19.406	18.466	21.579	90	7733	8	2.172	pale green	^[54]
[Ni₃(CF₃COO)₆(CF₃COOH)₆](CF₃COOH)	Nickel acid trifluoroacetate		trigonal	13.307		53.13		8148	6	2.205	emerald green	^[55]
[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	^[55]
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	^[60]
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	^[61]
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	^[60]^[62]
Na₂[Ni(C₆H₄O₇)] · 2 H₂O	disodium nickel citrate										green dec 371	^[50]
(NH₄)₂[Ni(HCit) · 2 H₂O]₂ · 2 H₂O	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	^[63]
(NH₄)₄[Ni(HCit)₂] · 2 H₂O	tetrammonium dicitratonickelate (11) dihydrate	545.10	monoclinic	9.361	13.496	9.424	115.476	1074.9	2	1.684		^[63]
Na₂[Ni(HCit) · 2 H₂O]₂ · 2 H₂O	Dimeric sodium diaquocitratonickelate (II) dihydrate											^[63]
K₂[Ni(HCit) · 2 H₂O]₂ · 2 H₂O	Dimeric potassium diaquocitratonickelate (II) dihydrate											^[63]
(NH₄)₂[Ni(H₂O)₆][Ti(H₂cit)₃]₂·6H₂O		1547.43	hexagonal	15.562		7.690		1605.5	1	1.600	light green	^[64]
[Ni(C₅H₇O₂)₂]₃	Nickel(II) acetylacetonate	256.91	orthorhombic	23.23	9.64	15.65		3505	4	1.46	dark green	^[65]
Ni[C₄O₄] · 2 H₂O	nickel squarate		?cubic	8.068	8.068	8.068	90°	525		1.93	green	^[66]
Ni[C₄O₄] · 8 H₂O	nickel squarate octahydrate	428.93	monoclinic	10.288	6.372	12.852	106.98	805.8	2	1.768	green	^[67]
Ni[C₅O₅] · 3 H₂O	Nickel croconate trihydrate		orthorhombic								green	^[68]
K₂[Ni(C₅O₅)₂(H₂O)₂] · 4 H₂O	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	^[69]
Ni(C₅H₅COO)₂ · 2 H₂O	nickel dibenzoate tetrahydrate	354.98	monoclinic	6.1341	34.180	6.9793	95.331	1457.0	4	1.618	light green	^[58]
Ni(C₅H₅COOCOOH)₂ · 6 H₂O	nickel dihydrogen diphthalate hexahydrate		monoclinic	16.024	5.574	12.500	113.42		2	1.611		^[70]
Ni[C₆H₄(COO)₂] · 4 H₂O	Nickel terephthalate										green	^[59]
Ni(OH)[C₆H₄(COO)(COOH)] · H₂O	basic nickel terephthalate										green	^[59]

Double salts

Nickel is one of the metals that can form Tutton's salts. The singly charged ion can be any of the full range of potassium, rubidium, cesium, ammonium ( ${\ce {NH4}}$ ), or thallium.^[71] As a mineral the ammonium nickel salt, (NH₄)₂Ni(SO₄)₂ · 6 H₂O, can be called nickelboussingaultite.^[72] With sodium, the double sulfate is nickelblödite Na₂Ni(SO₄)₂ · 4 H₂O from the blödite family. Nickel can be substituted by other divalent metals of similar sized to make mixtures that crystallise in the same form.^[73]

Nickel forms double salts with Tutton's salt structure with tetrafluoroberyllate with the range of cations of ammonia,^[74] potassium, rubidium, cesium,^[75] and thallium.^[76]

Anhydrous salts of the formula M₂Ni₂(SO₄)₃, which can be termed metal nickel triusulfates, belong to the family of langbeinites. The known salts include (NH₄)₂Ni₂(SO₄)₃, K₂Ni₂(SO₄)₃ and Rb₂Ni₂(SO₄)₃, and those of Tl and Cs are predicted to exist.

Some minerals are double salts, for example Nickelzippeite Ni₂(UO₂)₆(SO₄)₃(OH)₁₀ · 16H₂O which is isomorphic to cobaltzippeite, magnesiozippeite and zinczippeite, part of the zippeite group.^[77]

Double hydrides of nickel exist, such as Mg₂NiH₄.^[78]

Ternary chalcogenides

Nickel forms a series of double nickel oxides with other elements, which may be termed "nickelates". There are also many well defined double compounds with sulfur, selenium and tellurium.

Polyoxometallates

Nickel can enter into metal oxygen clusters with other high oxidation state elements to form polyoxometalates. These may stabilize higher oxidation states of nickel, or show catalytic properties.

Nonamolybdonickelate(IV), [NiMo₉O₃₂]⁶⁻ can oxidize aromatic hydrocarbons to alcohols.^[79]

There is a dark brown heptamolybdonickelate(IV) potassium salt, K₂H₈NiMo₇O₂₈·6H₂O.^[80]

13-Vanadonickelate(IV) compounds such as K₇NiV₁₃O₃₈ · 16 H₂O with black octahedral crystals exist. It can be made from isopolyvanadate, with nickel(II) oxidised by peroxydisulfate at a pH around 4.^[81] Nickel(IV) heteropolyniobates such as the dark maroon Na₁₂NiNb₁₂O₃₈ · 21 H₂O are also known.^[82] An alternate orange red hydrate perhaps with 44 water molecules also exists. With nickel-II (tetramethylammonium)₆[H₃NiNb₉O₂₈ · 17 H₂O forms a green salt that is very soluble in water, but hardly soluble in ethanol.^[83]

H₄₃K₁₄Na₆Nb₃₂ Ni₁₀O₁₈₃ is a nickel-cation-bridged polyoxoniobate which crystallizes in the monoclinic system with cell dimensions a=15.140 b=24.824 c=25.190 Å and β=103.469 and two formulas per unit cell.^[84]

Na₈Li₁₂[Ni₂(P₂W₁₅O₅₆)₂] · 74 H₂O forms a sandwich structure, and Na₄Li₅[Ni₃(OH)₃(H₂O)₃P₂W₁₆O₅₉] · 48 H₂O is a Wells-Dawson polyoxometalate.^[85]

Acid salts

Nickel hydrofluoride, H₅NiF₇·6H₂O is made by using excess hydrofluoric acid solution on nickel carbonate. It is deep green.^[3]

Basic salts

Nickel oxyfluoride Ni₄F₄O(OH)₂ is green.^[3]

Nickelous enneaoxydiiodide 9NiO•Nil₂ · 15 H₂O forms when solutions of nickel iodide are exposed to air and evaporated.^[3]

Complexes

Simple complexes of nickel include hexaquonickel(II), yellow tetracyanonickelate [Ni(CN)₄]²⁻, red pentacyanonickelate [Ni(CN)₅]³⁻ only found in solution, [Ni(SCN)₄]²⁻ and [Ni(SCN)₆]⁴⁻. Halo- complexes include [NiCl₄]²⁻, [NiF₄]²⁻, [NiF₆]⁴⁻, [NiCl₂(H₂O)₄] [Ni(NH₃)₄(H₂O)₂]²⁺, [Ni(NH₃)₆]²⁺, [Ni(en)₃)]²⁺.^[16] Some complexes have fivefold coordination. ${\ce {N[CH2CH2NMe2]3}}$ (tris(N,N-dimethyl-2-aminoethyl)amine); P(o-C₆H₄SMe)₃; P(CH₂CH₂CH₂AsMe₂)₃.^[16]

Other ligands for octahedral coordination include PPh₃, PPh₂Me and thiourea.^[16]

Nickel tetrahedral complexes are often bright blue and 20 times or more intensely coloured than the octahedral complexes.^[16] The ligands can include selections of neutral amines, arsines, arsine oxides, phosphines or phosphine oxides and halogens.^[16]

Several nickel atoms can cluster together in a compound with other elements to produce nickel cluster complexes. One example where nickel atoms form a square pyramid is a nickel hydride cluster complexed by triphenyl phosphine ligands and bonding a hydrogen atom on each edge. Another example has a square planar Ni₄H₄ shape in its core.^[86]

Nickel bis(dimethylglyoximate), an insoluble red solid is important for gravimetric analysis.

Bio molecules

Cofactor F430 contains nickel in a tetrapyrrole derivative, and is used in the production of methane. Some hydrogenase enzymes contain a nickel-iron cluster as an active site in which the nickel atom is held in place by cysteine or selenocysteine.^[87] Plant ureases contain a bis-μ-hydroxo dimeric nickel cluster.^[88] CO-methylating acetyl-CoA synthase contains two active nickel atoms, one is held in a square planar coordination by two cysteine and two amide groups, and the other nickel is held by three sulfur atoms. It is used to catalyse the reduction of carbon monoxide to acetyl-CoA.^[89]

Nickel superoxide dismutase (or Ni-SOD) from Streptomyces contains six nickel atoms. The nickel holding is done by a "nickel binding hook" which as the amino acid pattern H₂N-His-Cys-X-X-Pro-Cys-Gly-X-Tyr-rest of protein, where the bold bits are ligands for the nickel atom.^[90]

Nickel transporter proteins exist to move nickel atoms in the cell. in E. coli these are termed NikA, NikB, NikC, NikD, NikE. In order to come through a cell membrane a nickel permease protein is used. In Alcaligenes eutrophus the gene for this is hoxN.^[91]

Organometallics

Well known nickel organometalic (or organonickel) compounds include Nickelocene, bis(cyclooctadiene)nickel(0) and nickel tetracarbonyl. Nickel^[92]^[93]

Nickel tetracarbonyl was the first discovered organonickel compound. It was discovered that carbon monoxide corroded a nickel reaction chamber valve. And then that the gas coloured a bunsen burner flame green, and then that a nickel mirror condensed from heating the gas. The Mond process was thus inspired to purify nickel.^[94] The Nickel tetracarbonyl molecule is tetrahedral, with a bond length for nickel to carbon of 1.82 Å.^[94] Nickel tetracarbonyl easily starts breaking apart over 36° forming Ni(CO)₃, Ni(CO)₂, and Ni.^[94] Ni(CO) and NiC appear in mass spectroscopy of nickel carbonyl.^[94]

There are several nickel carbonyl cluster anions formed by reduction from nickel carbonyl. These are [Ni₂(CO)₅]²⁻, dark red [Ni₃(CO)₈]²⁻, [Ni₄(CO)₉]²⁻, [Ni₅(CO)₉]²⁻, [Ni₆(CO)₁₂]²⁻. Salts such as Cd[Ni₄(CO)₉] and Li₂[Ni₃(CO)₈]•5acetone can be crystallised.^[95]

Mixed cluster carbonyl anions like [Cr₂Ni₃(CO)₁₆]²⁻, [Mo₂Ni₃(CO)₁₆]²⁻ and [W₂Ni₃(CO)₁₆]²⁻ [Mo<Ni₄(CO)₁₄]²⁻ can form salts with bulky cations like tetraethylammonium. The brown [NiCo₃(CO)₁₁]⁻ changes to red [Ni₂Co₄(CO)₁₄]²⁻.^[96]

With oxygen or air the explosive Ni(CO)₃O₂ can be formed from nickel carbonyl.^[97]

Yet other ligands can substitute for carbon monoxide in nickel carbonyl. These lewis base ligands include triphenylphosphine, triphenoxyphosphine, trimethoxyphosphine, tributylphosphine, triethoxyphosphine, triethylisonitrolphosphine, triphenylarsine, and triphenylstibine.

Nickel forms dark blue planar complexes with 1,2-Diimino-3,5-cyclohexadiene or bisacetylbisaniline [(C₆H₅N-C(CH₃)=)₂]₂Ni. Another planar bis compound of nickel is formed with phenylazothioformamide C₆H₅N=NC(S)NR₂, and dithizone C₆H₅N=NC(S)NHNHC₆H₅.^[98] tetrasulfur tetranitride when reduced with nickel carbonyl makes Ni[N₂S₂H]₂ also coloured dark violet.^[98]

One nickellabenzene is known where nickel substitutes for carbon in benzene. At nickel the plane of the molecule is bent, however the connection to the ring has aromatic character.^[99]

Alkoxy compounds

Nickel tert-butoxide Ni[OC(CH₃)₃]₂ is coloured violet. It is formed in the reaction of di-tert-butylperoxide with nickel carbonyl.^[94]

Nickel dimethoxide is coloured green.^[100] There are also nickel chloride methoxides with formulae: NiClOMe, Ni₃Cl₂(OMe)₄ and Ni₃Cl(OMe)₅ in which Nickel and oxygen appear to form a cubane-type cluster.^[101]

Other alkoxy compounds known for nickel include nickel dipropoxide, nickel di-isopropoxide, nickel tert-amyloxide, and nickel di-tert-hexanoxide.^[102] These can be formed by crystallising nickel chloride from the corresponding alcohol, which forms an adduct. This is then heated with a base.^[103] Nickel(II) alkoxy compounds are polymeric and non-volatile.^[104]

Ziegler catalysis uses nickel as a catalyst. In addition it uses diethylaluminum ethoxide, phenylacetylene and triethylaluminium It converts ethylene into 1-butene. It can dimerise propylene. The catalyst, when combined with optically active phosphines, can produce optically active dimers. An intermediate formed is tris(ethylene)nickel.(CH₂=CH₂)₃Ni in which the ethylene molecules connect to the nickel atom side on.^[105]

Homoletptic bimetallic alkoxides have two different metals, and the same alkoxy group. They include Ni[(μ−OMe)₃AlOMe]₂, Ni[Al(OBu^t)₄]₂ (nickel tetra-tert-butoxyaluminate) and Ni[Al(OPrⁱ)₄]₂. (nickel tetra-isopropoxyaluminate a pink liquid)^[106] Potassium hexaisoproxynoibate and tantalate can react with nickel chloride to make Ni[Nb(OPrⁱ)₆]₂ and Ni[Ta(OPrⁱ)₆]₂. Ni[Zr₂(OPrⁱ)₉]₂ The bimetallic alkoxides are volatile and can dissolve in organic solvents.^[107] A trimetallic one exists [Zr₂(OPrⁱ)₉]Ni[Al(OPrⁱ)₄].^[108] NiGe(OBu^t)₈], NiSn(OBu^t)₈] and NiPb(OBu^t)₈] are tricyclic. [Ni₂(μ3−OEt)₂(μ−OEt)₈Sb₄(OEt)₆]

Heteroleptic bitmetallic ethoxides have more than one variety of alkoxy group, e.g. Ni[(μ−OPrⁱ)(μ−OBu^t)Al(OBu^t)₂]₂ which is a purple solid.

Oxoalkoxides contain extra oxygen in addition to the alcohol. With only nickel, none are known, but with antimony an octanuclear molecule exists [Ni₅Sb₃(μ4−O)₂(μ3−OEt)₃(−OEt)₉(OEt)₃(EtOH)₄].^[109]

Aryloxy compounds

There are many nickel compounds with the formula template Ni(OAr)XL₂ and Ni(OAr)₂L₂. L is a ligand with phosphorus or nitrogen atoms. OAr is a phenol group or O- attached to an aromatic ring. Often an extra molecule of the phenol is hydrogen bonded to the oxygen attached to nickel.^[110]

μ-bonded molecules

Others include cyclododecatriene nickel.

Sulfur rings

Nickel bis-dithiobenzoate can form a violet coloured sodium salt.^[94]

Two bisperfluoromethyl-l,2-dithietene molecules react with nickel carbonyl to make a double ring compound with nickel linked to four sulfur atoms. This contains four trifluoromethyl groups and is dark purple. Instead of this methyl or phenyl can substitute. These can be made by substituted acetylenes with sulfur on nickel carbonyl, or on nickel sulfide. Bis-diphenyldithiene nickel has a planar structure^[111]

Nickel chalcogen cluster compound

A hexameric compound [Ni(SR)₂]₆ is produced in the reaction of nickel carbonyl with dialkyl sulfides (RSR).^[111]

Nickel can be part of a cubane-type cluster with iron and chalcogens. The metal atoms are arranged in a tetrahedron shape, with the sulfur or selenium making up another tetrahedron that combines to make a cube. For example, the [NiFe₃S₄(PPh₃)(SEt)₃]²⁻ is a dianion that has a tetraethyl ammonium salt. Similar ion clusters are [NiFe₃Se₄(PPh₃)(SEt)₃]²⁻ and [NiFe₃Se₄(SEt)₄]³⁻.^[112] In the natural world cube shaped metal sulfur clusters can have sulfur atoms that are part of cysteine.

[Ni₄Se₂₃]⁴⁻ has a cube with Ni^IV₄Se₄ at its core, and then the nickel atoms are bridge across the cube faces by five Se₃ chains and one Se⁴ chain. It is formed as a tetraethylammonium salt, from Li₂Se, Se, NEt₄Cl and nickel dixanthate in dimethylformamide as a solvent. This reaction also produces (NEt₄)₂Ni(Se₄)₂.^[113]

Nitrosyl compounds

When liquid nickel carbonyl is dissolved in liquid hydrogen chloride, it can react with nitrosyl chloride to form a dimer Ni(NOCl)₂. This then decomposes to Ni(NO)Cl₂, which is polymeric.^[94]

Nickel carbonyl reacting with nitric oxide yields blue coloured mononitrosyl nickel NiNO. With cyclohexane as well, pale blue Ni(NO₂)NO is produced with nitrous oxide as a side product. With cyclopentadiene as well, π-C₅H₅NiNO is produced.^[94]

References

^ ^a ^b Barrett, Paul H.; Montano, P. A. (1977). "Proposed iron–nitrogen molecule produced in a solid nitrogen matrix". Journal of the Chemical Society, Faraday Transactions 2. 73 (3): 378–383. doi:10.1039/F29777300378.
^ ^a ^b Lian, Li; Su, C.-X.; Armentrout, P.B. (May 1991). "The bond energy of ${\ce {Ni^{+2}}}$ ". Chemical Physics Letters. 180 (3): 168–172. Bibcode:1991CPL...180..168L. doi:10.1016/0009-2614(91)87135-X.
^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k Mellor, J. W. (1946). "Nickel". A COMPREHENSIVE TREATISE ON INORGANIC AND THEORETICAL CHEMISTRY VOLUME XV Ni Ru, Rh Pd, Os, Ir. Retrieved 17 January 2019.
^ ^a ^b ^c ^d ^e Haynes, W. M., ed. (2014). CRC Handbook of Chemistry and Physics (95 ed.). pp. 4–77–4–78. ISBN 9781482208672.
^ Nicholls p1126-1127
^ Meyer, R. J. (1974). "Nickel und Polonium". Gmelins Handbuch Der Anorganischen Chemie - Nickel: Teil B — Lieferung 2. Verbindungen bis Nickel-Polonium (in German). Berlin: Springer-Verlag. p. 764. ISBN 9783662133026.
^ Leineweber, Andreas; Jacobs, Herbert; Hull, Steve (November 2001). "Ordering of Nitrogen in Nickel Nitride ${\ce {Ni3N}}$ Determined by Neutron Diffraction". Inorganic Chemistry. 40 (23): 5818–5822. doi:10.1021/ic0104860.
^ Robert A. Scott (2011). "Boron: Inorganic Chemistry". Encyclopedia of Inorganic Chemistry. Wiley. p. 401. ISBN 9780470862100.
^ ^a ^b ^c Muzangwa, L.G.; Ayles, V.L.; Nyambo, S.; Reid, S.A. (September 2011). "Probing the electronic structure of the nickel monohalides: Spectroscopy of the low-lying electronic states of NiBr and NiCl". Journal of Molecular Spectroscopy. 269 (1): 36–40. Bibcode:2011JMoSp.269...36M. doi:10.1016/j.jms.2011.04.012.
^ Hauffe1, Karl; Puschmann, Herbert (2008). "A26 nickel". Corrosion Handbook. Wiley. doi:10.1002/9783527610433.chb203030.{{cite book}}: CS1 maint: numeric names: authors list (link)
^ Krishnamurty, V. G. (16 April 1952). "The band spectrum of the diatomic molecule NiBr extending from 3930 to 5000 Å has been obtained in emission using a heavy current discharge". Indian Journal of Physics and Proceedings of the Indian Association for the Cultivation of Science. 26: 429.
^ Reddy, S Paddi; Rao, P Tiruvenganna (1 February 1960). "The Band Spectra of NiCl and NiBr in the Visible". Proceedings of the Physical Society. 75 (2): 275–279. Bibcode:1960PPS....75..275R. doi:10.1088/0370-1328/75/2/314.
^ Kant, Arthur (1968). "Mass-Spectrometric Studies of the Gaseous Systems Au-Ni, Au-Co, and Au-Fe, and Dissociation Energies of AuNi, AuCo, and AuFe". Journal of Chemical Physics. 49 (11): 5144. Bibcode:1968JChPh..49.5144K. doi:10.1063/1.1670012.
^ "Кристаллические структуры соединений Ni". www.kipt.kharkov.ua.
^ ^a ^b Hlukhyy, Viktor; Trots, Dmytro; Fässler, Thomas F. (13 January 2017). "First-Order Phase Transition in BaNi2Ge2 and the Influence of the Valence Electron Count on Distortion of the ${\ce {ThCr2 Si2}}$ Structure Type". Inorganic Chemistry. 56 (3): 1173. doi:10.1021/acs.inorgchem.6b02190. PMID 28085271.
^ ^a ^b ^c ^d ^e ^f Cotton and Wilkinson (1966). Advanced Inorganic Chemistry: A Comprehensive Treatise. John Wiley & Sons. pp. 878–893.
^ Mellor pp462-465
^ Mellor p 466-467
^ O'Brien, James F.; Reynolds, Warren Lind (November 1967). "Nuclear magnetic resonance study of cobalt and nickel tetrafluoroborates". Inorganic Chemistry. 6 (11): 2110–2111. doi:10.1021/ic50057a041.
^ Ryss, A. I.; Radchenko, I. V. (1966). "X-ray study of aqueous solutions of nickel tetrafluoroborate". Journal of Structural Chemistry. 6 (4): 489–492. doi:10.1007/BF00744813.
^ Rây, Nirmalendu Nath (20 April 1932). "Fluoberyllate und ihre Analogie mit den Sulfaten. II. Fluoberyllate einiger zweiwertiger Metalle". Zeitschrift für anorganische und allgemeine Chemie. 205 (3): 257–267. doi:10.1002/zaac.19322050307.
^ Karnezos, M.; Friedberg, S. A. (August 1978). "FERROMAGNETISM IN ${\ce {NiSnF6.6H2O}}$ AND ${\ce {NiSiF6.6H2O}}$ ". Le Journal de Physique Colloques. 39 (C6): C6–814–C6–815. doi:10.1051/jphyscol:19786362. Retrieved 14 May 2016.
^ ^a ^b ^c ^d Chacon, Lisa Carine (December 1997). "The Synthesis, Characterization and Reactivity of High Oxidation State Nickel Fluorides" (PDF). Berkeley California: University of California. Retrieved 27 April 2016.
^ Davidovich, R. L.; Kaidalova, T. A.; Levchishina, T. F. (1971). "X-ray diffraction data for some divalent metal fluorotitanates". Journal of Structural Chemistry. 12 (1): 166–168. doi:10.1007/BF00744565.
^ Christe, Karl O.; Wilson, William W.; Bougon, Roland A.; Charpin, Pierrette (January 1987). "Preparation and characterization of ${\ce {Ni(SbF6)2}}$ ". Journal of Fluorine Chemistry. 34 (3–4): 287–298. doi:10.1016/S0022-1139(00)85173-8.
^ Davidovich, R. L.; Buslaev, Yu. A.; Levchishina, T. F. (March 1968). "Synthesis of some new fluorohafnate complexes". Bulletin of the Academy of Sciences of the USSR Division of Chemical Science. 17 (3): 676–676. doi:10.1007/BF00911649.
^ Karnezos, M.; Meier, D.; Friedberg, S. A. (9–12 December 1975). "Magnetic ordering in ${\ce {NiZrF6.6H2O}}$ ". AIP Conference Proceedings. 29: 505. Bibcode:1976AIPC...29..505K. doi:10.1063/1.30416.
^ Weinland, R. F.; Schlegelmilch, Fr. (7 March 1902). "Über Doppelsalze des Jodtrichlorids mit Chloriden zweiwertiger Metalle". Zeitschrift für anorganische Chemie. 30 (1): 134–143. doi:10.1002/zaac.19020300109.
^ Hibble, Simon J.; Chippindale, Ann M.; Pohl, Alexander H.; Hannon, Alex C. (17 September 2007). "Surprises from a Simple Material—The Structure and Properties of Nickel Cyanide". Angewandte Chemie International Edition. 46 (37): 7116–7118. doi:10.1002/anie.200701246.
^ Sood, R. K.; Nya, A. E.; Etim, E. S. (December 1981). "Thermal decomposition of nickel azide". Journal of Thermal Analysis. 22 (2): 231–237. doi:10.1007/BF01915269.
^ Abu-Eittah, R.; Elmakabaty, S. (1973). "Spectra of Nickel(II)-Azide Complexes in Organic Solvents". Bulletin of the Chemical Society of Japan. 46 (11): 3427–3431. doi:10.1246/bcsj.46.3427.
^ IROM, I I (1 January 2001). "Photolysis of nickel hydroxy azide". Global Journal of Pure and Applied Sciences. 7 (1): 73–80. doi:10.4314/gjpas.v7i1.16208.
^ Tenten, A.; Jacobs, H. (June 1991). "Isolierte ${\ce {Ni6(NH2)12}}$ -Einheiten in Nickel(II)-Amid". Journal of the Less Common Metals. 170 (1): 145–159. doi:10.1016/0022-5088(91)90060-H.
^ Lappert, Michael (2009). Metal amide chemistry. Chichester, U.K.: Wiley. pp. 172–173. ISBN 9780470721841.
^ 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.
^ 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.
^ ^a ^b Krogmann, Klaus; Mattes, Rainer (January 1963). "Die Kristallstruktur von Nickelformiat, ${\ce {Ni(HCOO)2.2H2O}}$ ". Zeitschrift für Kristallographie - Crystalline Materials (in German). 118 (1–6). doi:10.1524/zkri.1963.118.16.291.
^ 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.
^ Vaidya, Sonalika; Rastogi, Pankaj; Agarwal, Suman; Gupta, Santosh K.; Ahmad, Tokeer; Antonelli, Anthony M.; Ramanujachary, K. V.; Lofland, S. E.; Ganguli, Ashok K. (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.
^ 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.
^ 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.
^ 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.
^ 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.
^ 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.
^ 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.
^ 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.
^ 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.
^ 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.
^ 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.
^ ^a ^b 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.
^ 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.
^ 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.
^ ^a ^b 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.
^ ^a ^b ^c 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. Bibcode:2003SSSci...5..635F. doi:10.1016/S1293-2558(03)00055-4.
^ ^a ^b ^c 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.
^ SALOOJA, K. C. (March 1972). "Burner Fuel Additives*". Combustion Science and Technology. 5 (1): 243–249. doi:10.1080/00102207208952528.
^ 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.
^ ^a ^b 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.
^ ^a ^b ^c Sherif, Fawzy G. (1 September 1970). "Heavy Metal Terephthalates". Industrial & Engineering Chemistry Product Research and Development. 9 (3): 408–412. doi:10.1021/i360035a026.
^ ^a ^b 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, ${\ce {K2[Ni(C6H5O7)(H2O)2]2.4H2O}}$ ". Inorganica Chimica Acta. 78: 281–285. doi:10.1016/S0020-1693(00)86530-5.
^ 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. PMC 3884440.
^ 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.
^ ^a ^b ^c ^d 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, ${\ce {(NH4)2[Ni(Hcit)(H2O)2]2-2H2O}}$ AND ${\ce {(NH4)4[Ni(Hcit)2]-2H2O}}$ ". Journal of Coordination Chemistry. 42 (1–2): 131–141. doi:10.1080/00958979708045286.
^ 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. Bibcode:2007JSSCh.180.3152D. doi:10.1016/j.jssc.2007.08.033.
^ 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.
^ Habenschuss, Michael (1974). "An x-ray, spectroscopic, and magnetic study of the structure of nickel squarate dihydrate, ${\ce {NiC4O4.2H2O}}$ ". Journal of Chemical Physics. 61 (3): 852. Bibcode:1974JChPh..61..852H. doi:10.1063/1.1682025.
^ Brach, I.; Rozière, J.; Anselment, B.; Peters, K. (15 March 1987). "An X-ray structure determination of cobalt and nickel squarate octahydrate, ${\ce {[M(H2O)6](C4HO4)2.2H2O}}$ (M=Ni,Co)". Acta Crystallographica Section C. 43 (3): 458–460. doi:10.1107/S0108270187095386.
^ 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.
^ 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.
^ Adiwidjaja, G.; Küppers, H. (15 May 1976). "Nickel dihydrogen diphthalate hexahydrate". Acta Crystallographica Section B. 32 (5): 1571–1574. doi:10.1107/S0567740876005840.
^ Wang, Xia; Xinxin Zhuang; Genbo Su; Youping He (2008). "A new ultraviolet filter: ${\ce {Rb2Ni(SO4)2.6H2O}}$ (RNSH) single crystal" (PDF). Optical Materials. 31 (2): 233–236. Bibcode:2008OptMa..31..233W. doi:10.1016/j.optmat.2008.03.020. ISSN 0925-3467.
^ "Nickelboussingaultite: Nickelboussingaultite mineral information and data". www.mindat.org. Retrieved 3 May 2016.
^ "Nickelblödite: Nickelblödite mineral information and data". www.mindat.org. Retrieved 4 May 2016.
^ Montgomery, H. (15 September 1980). "Diammonium nickel bis(tetrafluoroberyllate)hexahydrate". Acta Crystallographica Section B. 36 (9): 2121–2123. doi:10.1107/S0567740880008060.
^ Rây, Nirmalendunath (18 April 1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten". Zeitschrift für anorganische und allgemeine Chemie (in German). 227 (1): 32–36. doi:10.1002/zaac.19362270105.
^ Bose, A.; Mitra, S. C.; Datta, S. K. (11 November 1958). "The Behaviour of the Paramagnetic Ions in the Single Crystals of Some Similarly Constituted Salts of the Iron Group of Elements. II. Hydrated NiFormula Salts". Proceedings of the Royal Society A. 248 (1253): 153–168. Bibcode:1958RSPSA.248..153B. doi:10.1098/rspa.1958.0236.
^ "Nickelzippeite: Nickelzippeite mineral information and data". www.mindat.org. Retrieved 10 May 2016.
^ Reilly, James J.; Wiswall, Richard H. (November 1968). "Reaction of hydrogen with alloys of magnesium and nickel and the formation of ${\ce {Mg2NiH4}}$ ". Inorganic Chemistry. 7 (11): 2254–2256. doi:10.1021/ic50069a016.
^ Bhattacharya, Santanu; Saha, Basudeb; Dutta, Amitava; Banerjee, Pradyot (March 1998). "Electron transfer reactions of nickel(III) and nickel(IV) complexes". Coordination Chemistry Reviews. 170 (1): 47–74. doi:10.1016/S0010-8545(98)00065-4.
^ Roy, Ajoy; Chaudhury, Muktimoy (September 1983). "A New Series of Heptamolybdonickelate(IV) and Manganate(IV). Investigation of the Unusual Magnetic and Electronic Spectral Behavior of the Nickel(IV) Compound". Bulletin of the Chemical Society of Japan. 56 (9): 2827–2830. doi:10.1246/bcsj.56.2827.
^ George B. Kauffman; Russell Fuller; James Felser; Charles M. Flynn, Jr.; Michael T. Pope (1974). Parshall, George W. (ed.). "13‐Vanadomanganate(IV) and Nickelate(IV)". Inorganic Syntheses. 15: 103–110. doi:10.1002/9780470132463.ch24. ISBN 0070485216.
^ Flynn, Charles M.; Stucky, Galen D. (February 1969). "Heteropolyniobate complexes of manganese(IV) and nickel(IV)". Inorganic Chemistry. 8 (2): 332–334. doi:10.1021/ic50072a029.
^ Son, Jung-Ho; Ohlin, C. André; Casey, William H. (2013). "Highly soluble iron- and nickel-substituted decaniobates with tetramethylammonium countercations". Dalton Transactions. 42 (21): 7529. doi:10.1039/C3DT50887K. PMID 23588819.
^ Liang, Zhijie; Zhang, Dongdi; Wang, Haiying; Ma, Pengtao; Yang, Zongfei; Niu, Jingyang; Wang, Jingping (2016). "The ${\ce {{Ni10Nb32}}}$ aggregate: a perspective on isopolyniobates as ligands". Dalton Trans. 45 (41): 16173–16176. doi:10.1039/C6DT02575G. PMID 27711767.
^ Guo, Weiwei; Lv, Hongjin; Bacsa, John; Gao, Yuanzhe; Lee, Je Seong; Hill, Craig L. (19 January 2016). "Syntheses, Structural Characterization, and Catalytic Properties of Di- and Trinickel Polyoxometalates". Inorganic Chemistry. 55 (2): 461–466. doi:10.1021/acs.inorgchem.5b01935.
^ Shoshani, Manar M.; Beck, Robert; Wang, Xiaoping; McLaughlin, Matthew J.; Johnson, Samuel A. (15 November 2017). "Synthesis of Surface-Analogue Square-Planar Tetranuclear Nickel Hydride Clusters and Bonding to μ4-NR, -O and -BH Ligands". Inorganic Chemistry. 57 (5): 2438–2446. doi:10.1021/acs.inorgchem.7b02546.
^ Greening, C.; Berney, M.; Hards, K.; Cook, G. M.; Conrad, R. (3 March 2014). "A soil actinobacterium scavenges atmospheric ${\ce {H2}}$ using two membrane-associated, oxygen-dependent [NiFe] hydrogenases". Proceedings of the National Academy of Sciences. 111 (11): 4257–4261. Bibcode:2014PNAS..111.4257G. doi:10.1073/pnas.1320586111.
^ Karplus PA, Pearson MA, Hausinger RP (1997). "70 years of crystalline urease: What have we learned?". Accounts of Chemical Research. 30 (8): 330–337. doi:10.1021/ar960022j.
^ EVANS, D (August 2005). "Chemistry relating to the nickel enzymes CODH and ACS". Coordination Chemistry Reviews. 249 (15–16): 1582–1595. doi:10.1016/j.ccr.2004.09.012.
^ Wuerges, J.; Lee, J.-W.; Yim, Y.-I.; Yim, H.-S.; Kang, S.-O.; Carugo, K. D. (1 June 2004). "Crystal structure of nickel-containing superoxide dismutase reveals another type of active site". Proceedings of the National Academy of Sciences. 101 (23): 8569–8574. Bibcode:2004PNAS..101.8569W. doi:10.1073/pnas.0308514101.
^ Cammack, Richard; Vliet, Pieter (1999). "Catalysis by Nickel in Biological Systems". In Reedijk, Jan; Bouwman, Elisabeth (eds.). Bioinorganic Catalysis (2 ed.). New York: Marcel Dekker. p. 233. ISBN 0-8247-0241-7.
^ Cite error: The named reference Jolly was invoked but never defined (see the help page).
^ Jolly, P. W.; Wilke, G. (1975). The organic chemistry of nickel. Vol. 2. New York: Academic Press. ISBN 0-12-388402-0.
^ ^a ^b ^c ^d ^e ^f ^g ^h Jolly, P. W.; Wilke, G. (1974). The organic chemistry of nickel. Vol. 1. New York: Academic Press. pp. 1–9. ISBN 0-12-388401-2.
^ Jolly, P. W.; Wilke, G. (1974). The organic chemistry of nickel. Vol. 1. New York: Academic Press. pp. 20–22. ISBN 0-12-388401-2.
^ Jolly, P. W.; Wilke, G. (1974). The organic chemistry of nickel. Vol. 1. New York: Academic Press. pp. 23–24. ISBN 0-12-388401-2.
^ Jolly, P. W.; Wilke, G. (1974). The organic chemistry of nickel. Vol. 1. New York: Academic Press. p. 16. ISBN 0-12-388401-2.
^ ^a ^b Jolly, P. W.; Wilke, G. (1974). The organic chemistry of nickel. Vol. 1. New York: Academic Press. p. 19. ISBN 0-12-388401-2.
^ Wright, L. James (2017). Metallabenzenes: An Expert View. John Wiley & Sons. p. 97. ISBN 9781119068099.
^ Bradley], D.C. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. p. 97. ISBN 0-12-124140-8.
^ Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. p. 100. ISBN 978-0-12-124140-7.
^ Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. p. 11. ISBN 978-0-12-124140-7.
^ Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. p. 19. ISBN 978-0-12-124140-7.
^ Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. p. 68. ISBN 978-0-12-124140-7.
^ Jolly, P. W.; Wilke, G. (1975). The organic chemistry of nickel. Vol. 2. New York: Academic Press. p. 3. ISBN 0-12-388402-0.
^ Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. p. 208. ISBN 978-0-12-124140-7.
^ Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. pp. 185–192. ISBN 978-0-12-124140-7.
^ Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. pp. 215–216. ISBN 978-0-12-124140-7.
^ Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. pp. 432–433. ISBN 978-0-12-124140-7.
^ Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. pp. 619–621. ISBN 978-0-12-124140-7.
^ ^a ^b Jolly, P. W.; Wilke, G. (1974). The organic chemistry of nickel. Vol. 1. New York: Academic Press. pp. 18–19. ISBN 0-12-388401-2.
^ Ciurli, Stefano; Ross, Paul K.; Scott, Michael J.; Yu, Shi Bao; Holm, R. H. (June 1992). "Synthetic nickel-containing heterometal cubane-type clusters with ${\ce {NiFe3Q4}}$ cores (Q=sulfur, selenium)". Journal of the American Chemical Society. 114 (13): 5415–5423. doi:10.1021/ja00039a063.
^ McConnachie, Jonathan M.; Ansari, Mohammad A.; Ibers, James A. (August 1991). "Synthesis and characterization of nickel chalcogenide ${\ce {[Ni4Se4(Se3)5(Se4)]4}}$ - anion, a Ni(IV) cubane species". Journal of the American Chemical Society. 113 (18): 7078–7079. doi:10.1021/ja00018a079.

Sources

Mellor, J. W. (May 1936). "Nickel". A COMPREHENSIVE TREATISE ON INORGANIC AND THEORETICAL CHEMISTRY VOLUME XV Ni Ru, Rh Pd, Os, Ir. Archived from the original on 2017-02-07. Retrieved 31 May 2016. {{cite book}}: Unknown parameter |dead-url= ignored (|url-status= suggested) (help) (pages accessible by changing number on url)
Nichols, David (1975). The chemistry of iron, cobalt and nickel. Oxford: Pergamon Press. ISBN 0080188737.

[barrett-1] Barrett, Paul H.; Montano, P. A. (1977). "Proposed iron–nitrogen molecule produced in a solid nitrogen matrix". Journal of the Chemical Society, Faraday Transactions 2. 73 (3): 378–383. doi:10.1039/F29777300378.

[lian91-2] Lian, Li; Su, C.-X.; Armentrout, P.B. (May 1991). "The bond energy of ${\ce {Ni^{+2}}}$ ". Chemical Physics Letters. 180 (3): 168–172. Bibcode:1991CPL...180..168L. doi:10.1016/0009-2614(91)87135-X.

[mellor-3] ^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k Mellor, J. W. (1946). "Nickel". A COMPREHENSIVE TREATISE ON INORGANIC AND THEORETICAL CHEMISTRY VOLUME XV Ni Ru, Rh Pd, Os, Ir. Retrieved 17 January 2019.

[CRC-4] Haynes, W. M., ed. (2014). CRC Handbook of Chemistry and Physics (95 ed.). pp. 4–77–4–78. ISBN 9781482208672.

[nicholls-5] Nicholls p1126-1127

[6] Meyer, R. J. (1974). "Nickel und Polonium". Gmelins Handbuch Der Anorganischen Chemie - Nickel: Teil B — Lieferung 2. Verbindungen bis Nickel-Polonium (in German). Berlin: Springer-Verlag. p. 764. ISBN 9783662133026.

[7] Leineweber, Andreas; Jacobs, Herbert; Hull, Steve (November 2001). "Ordering of Nitrogen in Nickel Nitride ${\ce {Ni3N}}$ Determined by Neutron Diffraction". Inorganic Chemistry. 40 (23): 5818–5822. doi:10.1021/ic0104860.

[Encyclopedia-8] Robert A. Scott (2011). "Boron: Inorganic Chemistry". Encyclopedia of Inorganic Chemistry. Wiley. p. 401. ISBN 9780470862100.

[muzangwa-9] Muzangwa, L.G.; Ayles, V.L.; Nyambo, S.; Reid, S.A. (September 2011). "Probing the electronic structure of the nickel monohalides: Spectroscopy of the low-lying electronic states of NiBr and NiCl". Journal of Molecular Spectroscopy. 269 (1): 36–40. Bibcode:2011JMoSp.269...36M. doi:10.1016/j.jms.2011.04.012.

[10] Hauffe1, Karl; Puschmann, Herbert (2008). "A26 nickel". Corrosion Handbook. Wiley. doi:10.1002/9783527610433.chb203030.{{cite book}}: CS1 maint: numeric names: authors list (link)

[11] Krishnamurty, V. G. (16 April 1952). "The band spectrum of the diatomic molecule NiBr extending from 3930 to 5000 Å has been obtained in emission using a heavy current discharge". Indian Journal of Physics and Proceedings of the Indian Association for the Cultivation of Science. 26: 429.

[12] Reddy, S Paddi; Rao, P Tiruvenganna (1 February 1960). "The Band Spectra of NiCl and NiBr in the Visible". Proceedings of the Physical Society. 75 (2): 275–279. Bibcode:1960PPS....75..275R. doi:10.1088/0370-1328/75/2/314.

[13] Kant, Arthur (1968). "Mass-Spectrometric Studies of the Gaseous Systems Au-Ni, Au-Co, and Au-Fe, and Dissociation Energies of AuNi, AuCo, and AuFe". Journal of Chemical Physics. 49 (11): 5144. Bibcode:1968JChPh..49.5144K. doi:10.1063/1.1670012.

[14] "Кристаллические структуры соединений Ni". www.kipt.kharkov.ua.

[banige-15] Hlukhyy, Viktor; Trots, Dmytro; Fässler, Thomas F. (13 January 2017). "First-Order Phase Transition in BaNi2Ge2 and the Influence of the Valence Electron Count on Distortion of the ${\ce {ThCr2 Si2}}$ Structure Type". Inorganic Chemistry. 56 (3): 1173. doi:10.1021/acs.inorgchem.6b02190. PMID 28085271.

[caw-16] ^ ^a ^b ^c ^d ^e ^f Cotton and Wilkinson (1966). Advanced Inorganic Chemistry: A Comprehensive Treatise. John Wiley & Sons. pp. 878–893.

[17] Mellor pp462-465

[18] Mellor p 466-467

[19] O'Brien, James F.; Reynolds, Warren Lind (November 1967). "Nuclear magnetic resonance study of cobalt and nickel tetrafluoroborates". Inorganic Chemistry. 6 (11): 2110–2111. doi:10.1021/ic50057a041.

[20] Ryss, A. I.; Radchenko, I. V. (1966). "X-ray study of aqueous solutions of nickel tetrafluoroborate". Journal of Structural Chemistry. 6 (4): 489–492. doi:10.1007/BF00744813.

[21] Rây, Nirmalendu Nath (20 April 1932). "Fluoberyllate und ihre Analogie mit den Sulfaten. II. Fluoberyllate einiger zweiwertiger Metalle". Zeitschrift für anorganische und allgemeine Chemie. 205 (3): 257–267. doi:10.1002/zaac.19322050307.

[22] Karnezos, M.; Friedberg, S. A. (August 1978). "FERROMAGNETISM IN ${\ce {NiSnF6.6H2O}}$ AND ${\ce {NiSiF6.6H2O}}$ ". Le Journal de Physique Colloques. 39 (C6): C6–814–C6–815. doi:10.1051/jphyscol:19786362. Retrieved 14 May 2016.

[Chacon-23] Chacon, Lisa Carine (December 1997). "The Synthesis, Characterization and Reactivity of High Oxidation State Nickel Fluorides" (PDF). Berkeley California: University of California. Retrieved 27 April 2016.

[24] Davidovich, R. L.; Kaidalova, T. A.; Levchishina, T. F. (1971). "X-ray diffraction data for some divalent metal fluorotitanates". Journal of Structural Chemistry. 12 (1): 166–168. doi:10.1007/BF00744565.

[25] Christe, Karl O.; Wilson, William W.; Bougon, Roland A.; Charpin, Pierrette (January 1987). "Preparation and characterization of ${\ce {Ni(SbF6)2}}$ ". Journal of Fluorine Chemistry. 34 (3–4): 287–298. doi:10.1016/S0022-1139(00)85173-8.

[26] Davidovich, R. L.; Buslaev, Yu. A.; Levchishina, T. F. (March 1968). "Synthesis of some new fluorohafnate complexes". Bulletin of the Academy of Sciences of the USSR Division of Chemical Science. 17 (3): 676–676. doi:10.1007/BF00911649.

[27] Karnezos, M.; Meier, D.; Friedberg, S. A. (9–12 December 1975). "Magnetic ordering in ${\ce {NiZrF6.6H2O}}$ ". AIP Conference Proceedings. 29: 505. Bibcode:1976AIPC...29..505K. doi:10.1063/1.30416.

[28] Weinland, R. F.; Schlegelmilch, Fr. (7 March 1902). "Über Doppelsalze des Jodtrichlorids mit Chloriden zweiwertiger Metalle". Zeitschrift für anorganische Chemie. 30 (1): 134–143. doi:10.1002/zaac.19020300109.

[hibble-29] Hibble, Simon J.; Chippindale, Ann M.; Pohl, Alexander H.; Hannon, Alex C. (17 September 2007). "Surprises from a Simple Material—The Structure and Properties of Nickel Cyanide". Angewandte Chemie International Edition. 46 (37): 7116–7118. doi:10.1002/anie.200701246.

[30] Sood, R. K.; Nya, A. E.; Etim, E. S. (December 1981). "Thermal decomposition of nickel azide". Journal of Thermal Analysis. 22 (2): 231–237. doi:10.1007/BF01915269.

[31] Abu-Eittah, R.; Elmakabaty, S. (1973). "Spectra of Nickel(II)-Azide Complexes in Organic Solvents". Bulletin of the Chemical Society of Japan. 46 (11): 3427–3431. doi:10.1246/bcsj.46.3427.

[32] IROM, I I (1 January 2001). "Photolysis of nickel hydroxy azide". Global Journal of Pure and Applied Sciences. 7 (1): 73–80. doi:10.4314/gjpas.v7i1.16208.

[33] Tenten, A.; Jacobs, H. (June 1991). "Isolierte ${\ce {Ni6(NH2)12}}$ -Einheiten in Nickel(II)-Amid". Journal of the Less Common Metals. 170 (1): 145–159. doi:10.1016/0022-5088(91)90060-H.

[34] Lappert, Michael (2009). Metal amide chemistry. Chichester, U.K.: Wiley. pp. 172–173. ISBN 9780470721841.

[Downie-35] 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.

[36] 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.

[Krogmann-37] Krogmann, Klaus; Mattes, Rainer (January 1963). "Die Kristallstruktur von Nickelformiat, ${\ce {Ni(HCOO)2.2H2O}}$ ". Zeitschrift für Kristallographie - Crystalline Materials (in German). 118 (1–6). doi:10.1524/zkri.1963.118.16.291.

[38] 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.

[39] Vaidya, Sonalika; Rastogi, Pankaj; Agarwal, Suman; Gupta, Santosh K.; Ahmad, Tokeer; Antonelli, Anthony M.; Ramanujachary, K. V.; Lofland, S. E.; Ganguli, Ashok K. (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.

[40] 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.

[41] 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.

[42] 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.

[43] 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.

[44] 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.

[45] 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.

[46] 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.

[47] 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.

[48] 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.

[49] 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.

[wang7-50] 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.

[51] 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.

[52] 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.

[Guillou003-53] 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.

[forster03-54] 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. Bibcode:2003SSSci...5..635F. doi:10.1016/S1293-2558(03)00055-4.

[Tokareva-55] 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.

[56] SALOOJA, K. C. (March 1972). "Burner Fuel Additives*". Combustion Science and Technology. 5 (1): 243–249. doi:10.1080/00102207208952528.

[57] 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.

[vrab-58] 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.

[sherif-59] Sherif, Fawzy G. (1 September 1970). "Heavy Metal Terephthalates". Industrial & Engineering Chemistry Product Research and Development. 9 (3): 408–412. doi:10.1021/i360035a026.

[baker-60] 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, ${\ce {K2[Ni(C6H5O7)(H2O)2]2.4H2O}}$ ". Inorganica Chimica Acta. 78: 281–285. doi:10.1016/S0020-1693(00)86530-5.

[61] 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. PMC 3884440.

[62] 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.

[zhou6-63] 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, ${\ce {(NH4)2[Ni(Hcit)(H2O)2]2-2H2O}}$ AND ${\ce {(NH4)4[Ni(Hcit)2]-2H2O}}$ ". Journal of Coordination Chemistry. 42 (1–2): 131–141. doi:10.1080/00958979708045286.

[64] 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. Bibcode:2007JSSCh.180.3152D. doi:10.1016/j.jssc.2007.08.033.

[65] 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.

[66] Habenschuss, Michael (1974). "An x-ray, spectroscopic, and magnetic study of the structure of nickel squarate dihydrate, ${\ce {NiC4O4.2H2O}}$ ". Journal of Chemical Physics. 61 (3): 852. Bibcode:1974JChPh..61..852H. doi:10.1063/1.1682025.

[67] Brach, I.; Rozière, J.; Anselment, B.; Peters, K. (15 March 1987). "An X-ray structure determination of cobalt and nickel squarate octahydrate, ${\ce {[M(H2O)6](C4HO4)2.2H2O}}$ (M=Ni,Co)". Acta Crystallographica Section C. 43 (3): 458–460. doi:10.1107/S0108270187095386.

[68] 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.

[69] 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.

[70] Adiwidjaja, G.; Küppers, H. (15 May 1976). "Nickel dihydrogen diphthalate hexahydrate". Acta Crystallographica Section B. 32 (5): 1571–1574. doi:10.1107/S0567740876005840.

[Wang2008-71] Wang, Xia; Xinxin Zhuang; Genbo Su; Youping He (2008). "A new ultraviolet filter: ${\ce {Rb2Ni(SO4)2.6H2O}}$ (RNSH) single crystal" (PDF). Optical Materials. 31 (2): 233–236. Bibcode:2008OptMa..31..233W. doi:10.1016/j.optmat.2008.03.020. ISSN 0925-3467.

[72] "Nickelboussingaultite: Nickelboussingaultite mineral information and data". www.mindat.org. Retrieved 3 May 2016.

[73] "Nickelblödite: Nickelblödite mineral information and data". www.mindat.org. Retrieved 4 May 2016.

[74] Montgomery, H. (15 September 1980). "Diammonium nickel bis(tetrafluoroberyllate)hexahydrate". Acta Crystallographica Section B. 36 (9): 2121–2123. doi:10.1107/S0567740880008060.

[75] Rây, Nirmalendunath (18 April 1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten". Zeitschrift für anorganische und allgemeine Chemie (in German). 227 (1): 32–36. doi:10.1002/zaac.19362270105.

[76] Bose, A.; Mitra, S. C.; Datta, S. K. (11 November 1958). "The Behaviour of the Paramagnetic Ions in the Single Crystals of Some Similarly Constituted Salts of the Iron Group of Elements. II. Hydrated NiFormula Salts". Proceedings of the Royal Society A. 248 (1253): 153–168. Bibcode:1958RSPSA.248..153B. doi:10.1098/rspa.1958.0236.

[77] "Nickelzippeite: Nickelzippeite mineral information and data". www.mindat.org. Retrieved 10 May 2016.

[78] Reilly, James J.; Wiswall, Richard H. (November 1968). "Reaction of hydrogen with alloys of magnesium and nickel and the formation of ${\ce {Mg2NiH4}}$ ". Inorganic Chemistry. 7 (11): 2254–2256. doi:10.1021/ic50069a016.

[79] Bhattacharya, Santanu; Saha, Basudeb; Dutta, Amitava; Banerjee, Pradyot (March 1998). "Electron transfer reactions of nickel(III) and nickel(IV) complexes". Coordination Chemistry Reviews. 170 (1): 47–74. doi:10.1016/S0010-8545(98)00065-4.

[80] Roy, Ajoy; Chaudhury, Muktimoy (September 1983). "A New Series of Heptamolybdonickelate(IV) and Manganate(IV). Investigation of the Unusual Magnetic and Electronic Spectral Behavior of the Nickel(IV) Compound". Bulletin of the Chemical Society of Japan. 56 (9): 2827–2830. doi:10.1246/bcsj.56.2827.

[81] George B. Kauffman; Russell Fuller; James Felser; Charles M. Flynn, Jr.; Michael T. Pope (1974). Parshall, George W. (ed.). "13‐Vanadomanganate(IV) and Nickelate(IV)". Inorganic Syntheses. 15: 103–110. doi:10.1002/9780470132463.ch24. ISBN 0070485216.

[82] Flynn, Charles M.; Stucky, Galen D. (February 1969). "Heteropolyniobate complexes of manganese(IV) and nickel(IV)". Inorganic Chemistry. 8 (2): 332–334. doi:10.1021/ic50072a029.

[83] Son, Jung-Ho; Ohlin, C. André; Casey, William H. (2013). "Highly soluble iron- and nickel-substituted decaniobates with tetramethylammonium countercations". Dalton Transactions. 42 (21): 7529. doi:10.1039/C3DT50887K. PMID 23588819.

[84] Liang, Zhijie; Zhang, Dongdi; Wang, Haiying; Ma, Pengtao; Yang, Zongfei; Niu, Jingyang; Wang, Jingping (2016). "The ${\ce {{Ni10Nb32}}}$ aggregate: a perspective on isopolyniobates as ligands". Dalton Trans. 45 (41): 16173–16176. doi:10.1039/C6DT02575G. PMID 27711767.

[85] Guo, Weiwei; Lv, Hongjin; Bacsa, John; Gao, Yuanzhe; Lee, Je Seong; Hill, Craig L. (19 January 2016). "Syntheses, Structural Characterization, and Catalytic Properties of Di- and Trinickel Polyoxometalates". Inorganic Chemistry. 55 (2): 461–466. doi:10.1021/acs.inorgchem.5b01935.

[86] Shoshani, Manar M.; Beck, Robert; Wang, Xiaoping; McLaughlin, Matthew J.; Johnson, Samuel A. (15 November 2017). "Synthesis of Surface-Analogue Square-Planar Tetranuclear Nickel Hydride Clusters and Bonding to μ4-NR, -O and -BH Ligands". Inorganic Chemistry. 57 (5): 2438–2446. doi:10.1021/acs.inorgchem.7b02546.

[87] Greening, C.; Berney, M.; Hards, K.; Cook, G. M.; Conrad, R. (3 March 2014). "A soil actinobacterium scavenges atmospheric ${\ce {H2}}$ using two membrane-associated, oxygen-dependent [NiFe] hydrogenases". Proceedings of the National Academy of Sciences. 111 (11): 4257–4261. Bibcode:2014PNAS..111.4257G. doi:10.1073/pnas.1320586111.

[karplus-88] Karplus PA, Pearson MA, Hausinger RP (1997). "70 years of crystalline urease: What have we learned?". Accounts of Chemical Research. 30 (8): 330–337. doi:10.1021/ar960022j.

[89] EVANS, D (August 2005). "Chemistry relating to the nickel enzymes CODH and ACS". Coordination Chemistry Reviews. 249 (15–16): 1582–1595. doi:10.1016/j.ccr.2004.09.012.

[90] Wuerges, J.; Lee, J.-W.; Yim, Y.-I.; Yim, H.-S.; Kang, S.-O.; Carugo, K. D. (1 June 2004). "Crystal structure of nickel-containing superoxide dismutase reveals another type of active site". Proceedings of the National Academy of Sciences. 101 (23): 8569–8574. Bibcode:2004PNAS..101.8569W. doi:10.1073/pnas.0308514101.

[91] Cammack, Richard; Vliet, Pieter (1999). "Catalysis by Nickel in Biological Systems". In Reedijk, Jan; Bouwman, Elisabeth (eds.). Bioinorganic Catalysis (2 ed.). New York: Marcel Dekker. p. 233. ISBN 0-8247-0241-7.

[Jolly-92] Cite error: The named reference Jolly was invoked but never defined (see the help page).

[Jolly2-93] Jolly, P. W.; Wilke, G. (1975). The organic chemistry of nickel. Vol. 2. New York: Academic Press. ISBN 0-12-388402-0.

[jolly1-1-94] ^ ^a ^b ^c ^d ^e ^f ^g ^h Jolly, P. W.; Wilke, G. (1974). The organic chemistry of nickel. Vol. 1. New York: Academic Press. pp. 1–9. ISBN 0-12-388401-2.

[jolly1-20-95] Jolly, P. W.; Wilke, G. (1974). The organic chemistry of nickel. Vol. 1. New York: Academic Press. pp. 20–22. ISBN 0-12-388401-2.

[jolly1-23-96] Jolly, P. W.; Wilke, G. (1974). The organic chemistry of nickel. Vol. 1. New York: Academic Press. pp. 23–24. ISBN 0-12-388401-2.

[jolly1-16-97] Jolly, P. W.; Wilke, G. (1974). The organic chemistry of nickel. Vol. 1. New York: Academic Press. p. 16. ISBN 0-12-388401-2.

[jolly1-19-98] Jolly, P. W.; Wilke, G. (1974). The organic chemistry of nickel. Vol. 1. New York: Academic Press. p. 19. ISBN 0-12-388401-2.

[99] Wright, L. James (2017). Metallabenzenes: An Expert View. John Wiley & Sons. p. 97. ISBN 9781119068099.

[100] Bradley], D.C. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. p. 97. ISBN 0-12-124140-8.

[101] Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. p. 100. ISBN 978-0-12-124140-7.

[102] Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. p. 11. ISBN 978-0-12-124140-7.

[103] Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. p. 19. ISBN 978-0-12-124140-7.

[104] Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. p. 68. ISBN 978-0-12-124140-7.

[Jolly2-3-105] Jolly, P. W.; Wilke, G. (1975). The organic chemistry of nickel. Vol. 2. New York: Academic Press. p. 3. ISBN 0-12-388402-0.

[106] Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. p. 208. ISBN 978-0-12-124140-7.

[107] Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. pp. 185–192. ISBN 978-0-12-124140-7.

[108] Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. pp. 215–216. ISBN 978-0-12-124140-7.

[109] Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. pp. 432–433. ISBN 978-0-12-124140-7.

[110] Bradley, Don C.; Mehrotra, R. C.; Rothwell, Ian; Sin, A. (2001). Alkoxo and aryloxo derivatives of metals. San Diego: Academic Press. pp. 619–621. ISBN 978-0-12-124140-7.

[jolly1-18-111] Jolly, P. W.; Wilke, G. (1974). The organic chemistry of nickel. Vol. 1. New York: Academic Press. pp. 18–19. ISBN 0-12-388401-2.

[112] Ciurli, Stefano; Ross, Paul K.; Scott, Michael J.; Yu, Shi Bao; Holm, R. H. (June 1992). "Synthetic nickel-containing heterometal cubane-type clusters with ${\ce {NiFe3Q4}}$ cores (Q=sulfur, selenium)". Journal of the American Chemical Society. 114 (13): 5415–5423. doi:10.1021/ja00039a063.

[113] McConnachie, Jonathan M.; Ansari, Mohammad A.; Ibers, James A. (August 1991). "Synthesis and characterization of nickel chalcogenide ${\ce {[Ni4Se4(Se3)5(Se4)]4}}$ - anion, a Ni(IV) cubane species". Journal of the American Chemical Society. 113 (18): 7078–7079. doi:10.1021/ja00018a079.

[1]

[2]

[3]

[4]

[5]

[6]

[7]

[8]

[9]

[10]

[11]

[12]

[13]

[14]

[15]

[16]

[17]

[18]

[19]

[20]

[21]

[22]

[23]

[24]

[25]

[26]

[27]

[28]

[29]

[30]

[31]

[32]

[33]

[34]

[35]

[36]

[37]

[38]

[39]

[40]

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[43]

[44]

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[67]

[68]

[69]

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[78]

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v t e Nickel compounds
Nickel(0)	Ni(CO)₄ Ni(COD)₂
Nickel(II)	NiF₂ K₂NiF₄ NiF²⁻ ₄ NiCl₂ NiCl²⁻ ₄ NiBr₂ NiBr²⁻ ₄ NiI₂ NiI²⁻ ₄ Ni(CN)₂ K₂Ni(CN)₄ Ni(SCN)₂ NiO Ni(OH)₂ NiCO₃ NiSO₄ Ni₃(PO₄)₂ NiCrO₄ NiTiO₃ NiSeO₄ NiS NiSe Ni(ClO₄)₂ Ni(NO₃)₂ Ni(NO₂)₂ Ni(NO₂)³⁻ ₅ / Ni(NO₂)⁴⁻ ₆ Ni(CO₂H)₂ C ₂₄H ₄₆NiO ₄ C ₃₆H ₇₀NiO ₄ Ni(acac)₂
Nickel(III)	NiF₃ Ni₂O₃ NiOOH
Nickel(IV)	NiF₄ K₂NiF₆ MNiO_$x$