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Nickel compounds

December 05, 2023

See also: Category:Nickel compounds

Nickel compounds 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 superconductivity properties, as nickel is adjacent to copper and iron in the periodic table can form compounds with the same structure as the high-temperature superconductors that are known.

Colour edit

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

Geometry edit

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 edit

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 edit

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 edit

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

Hydroxides edit

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 edit

 
nickel chloride hexahydrate

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] Ammine complexes like hexaamminenickel chloride also exist.

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 crystallise 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 edit

 
needles of Halls Gap Millerite

By reacting nickel with chalcogens, nickel sulfide, nickel selenide, and nickel telluride are formed. There are numerous sulfides: Ni1.5S, 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 Ni1−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 edit

 
The nickel arsenide nickeline

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 NiAs2-3, 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 edit

Nickel also forms carbides and borides. Nickel borides include 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.

Nickel silicides include Ni3Si,[9] Ni31Si12, Ni2Si, Ni3Si2, NiSi and NiSi2.[10] Nickel silicides are used in microelectronics.

Diatomic molecules edit

Hot nickel vapour reacting with other atoms in the gas phase can produce molecules consisting of two atoms. These can be studied by their emission spectrum. The nickel monohalides are well studied.[11][12][13][14][15]

Alloys edit

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,[16]

BaNi2Ge2 changes structure from orthorhombic to tetragonal around 480 °C.[17] This is a ternary intermetallic compound. Others include BaNiSn3 and the superconductors SrNi2Ge2, SrNi2P2, SrNi2As2, BaNi2P2, BaNi2As2.[17]

Simple salts edit

Oxo acid salts edit

Main article: Nickel oxo acid salts
 
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.[18] 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.[19] The heptahydrate crystallises from water below 31.5 above this blue hexhydrate forms, and above 53.3 the green form.[20] Heating nickel sulfate dehydrates it, and then 700° it loses sulfur trioxide, sulfur dioxide and oxygen. Other important nickel compounds in this class are nickel carbonate, nickel nitrate, and nickel phosphate

Fluoro acid salts edit

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.[21][22] Nickel tetrafluoroberyllate NiBeF4•xH2O, can be hydrated with six or seven water molecules.[23] Both nickel hexafluorostannate   and nickel fluorosilicate   crystallise in the trigonal system.[24] 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.[25] Nickel fuorotitanate   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).[26]

Ni(AsF6)2, Ni(SbF6)2, Ni(BiF6)2 are made by reacting the hexafluoro acid with NiF2 in hydrofluoric acid.[25] They all have hexagonal crystal structure, resembling the similar salts of the other first row transition metals.[25] For Ni(AsF6)2 a = 4.98, c = 26.59, and V = 571, formula weight Z=3.[25] 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.[27]

Others include the green fluorohafnate NiHfF6 · 6 H2O, and Ni2HfF8 · 12 H2O,[28] NiZrF6 · 6 H2O[29]

Chloroacid salts edit

Nickel tetrachloroiodate Ni(ICl4)2 can be made by reacting iodine with nickel chloride and chlorine gas. It consists of green needles.[30]

Nitrogen anion salts edit

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.[31]

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.[32] 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.[33] Nickel azide forms a dihydrate: Ni(N3)2 · 2 H2O and a basic salt called nickel hydroxy azide Ni(OH)N3.[34]

Nickel amide, Ni(NH2)2 is a deep red compound that contains Ni6 clusters surrounded by 12 NH2 groups.[35] 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.[36]

Organic acid salts edit

Main article: Nickel organic acid salts

Nickel forms many known salts with organic acids. In many of these the ionised organic acid acts as a ligand.

Double salts edit

Main article: Nickel 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 ( ), or thallium.[37] As a mineral the ammonium nickel salt, (NH4)2Ni(SO4)2 · 6 H2O, can be called nickelboussingaultite.[38] 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.[39]

Nickel forms double salts with Tutton's salt structure with tetrafluoroberyllate with the range of cations of ammonia,[40] potassium, rubidium, cesium,[41] and thallium.[42]

Anhydrous salts of the formula M2Ni2(SO4)3, which can be termed metal nickel trisulfates, 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.[43]

Double hydrides of nickel exist, such as Mg2NiH4.[44]

Ternary chalcogenides edit

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.

Ternary pnictides edit

Ternary pnictides that contain nickel are metallic and include MgNi2Bi4,[45] SrNi2P2, SrNi2As2, BaNi2P2, and BaNi2As2.[17]

Ternary halides edit

Nickel can form anions and salts with halogens including the hexafluoronickelates, and tetrafluoronickelates, tetrachloronickelates, tetrabromonickelates and tetraiodonickelates. The subiodide Bi12Ni4I3 is also known.[45]

Polyoxometallates edit

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.[46]

There is a dark brown heptamolybdonickelate(IV) potassium salt, K2H8NiMo7O28·6H2O.[47]

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.[48] Nickel(IV) heteropolyniobates such as the dark maroon Na12NiNb12O38 · 21 H2O are also known.[49] 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.[50]

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.[51]

Na8Li12[Ni2(P2W15O56)2] · 74 H2O forms a sandwich structure, and Na4Li5[Ni3(OH)3(H2O)3P2W16O59] · 48 H2O is a Wells-Dawson polyoxometalate.[52]

Acidic salts edit

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

Basic salts edit

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 edit

 
Sample of potassium tetracyanonickelate hydrate

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+.[18] Some complexes have fivefold coordination.   (tris(N,N-dimethyl-2-aminoethyl)amine); P(o-C6H4SMe)3; P(CH2CH2CH2AsMe2)3.[18]

Other ligands for octahedral coordination include PPh3, PPh2Me and thiourea.[18]

Nickel tetrahedral complexes are often bright blue and 20 times or more intensely coloured than the octahedral complexes.[18] The ligands can include selections of neutral amines, arsines, arsine oxides, phosphines or phosphine oxides and halogens.[18]

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.[53]

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

Biological molecules edit

 
Active site of Nickel superoxide dismutase

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.[54] Plant ureases contain a bis-μ-hydroxo dimeric nickel cluster.[55] 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.[56]

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.[57]

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.[58]

Organometallics edit

Main article: Organonickel

Well known nickel organometalic (or organonickel) compounds include Nickelocene, bis(cyclooctadiene)nickel(0) and nickel tetracarbonyl.[59]

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.[60] The nickel tetracarbonyl molecule is tetrahedral, with a bond length for nickel to carbon of 1.82 Å.[60] Nickel tetracarbonyl easily starts breaking apart over 36° forming Ni(CO)3, Ni(CO)2, and Ni.[60] Ni(CO) and NiC appear in mass spectroscopy of nickel carbonyl.[60]

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.[61]

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−.[62]

With oxygen or air the explosive Ni(CO)3O2 can be formed from nickel carbonyl.[63]

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.[64] tetrasulfur tetranitride when reduced with nickel carbonyl makes Ni[N2S2H]2 also coloured dark violet.[64]

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.[65]

Alkoxy compounds edit

Nickel tert-butoxide Ni[OC(CH3)3]2 is coloured violet. It is formed in the reaction of di-tert-butylperoxide with nickel carbonyl.[60]

Nickel dimethoxide is coloured green.[66] 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.[67]

Other alkoxy compounds known for nickel include nickel dipropoxide, nickel di-isopropoxide, nickel tert-amyloxide, and nickel di-tert-hexanoxide.[68] These can be formed by crystallising nickel chloride from the corresponding alcohol, which forms an adduct. This is then heated with a base.[69] Nickel(II) alkoxy compounds are polymeric and non-volatile.[70]

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.[71]

Homoletptic bimetallic alkoxides have two different metals, and the same alkoxy group. They include Ni[(μ−OMe)3AlOMe]2, Ni[Al(OBut)4]2 (nickel tetra-tert-butoxyaluminate) and Ni[Al(OPri)4]2. (nickel tetra-isopropoxyaluminate a pink liquid)[72] 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.[73] A trimetallic one exists [Zr2(OPri)9]Ni[Al(OPri)4].[74] NiGe(OBut)8], NiSn(OBut)8] and NiPb(OBut)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−OBut)Al(OBut)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].[75]

Aryloxy compounds edit

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.[76]

μ-bonded molecules edit

Others include cyclododecatriene nickel and t-Ni(cdt).

Sulfur rings edit

Nickel bis-dithiobenzoate can form a violet coloured sodium salt.[60]

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[77]

Nickel chalcogen cluster compound edit

A hexameric compound [Ni(SR)2]6 is produced in the reaction of nickel carbonyl with dialkyl sulfides (RSR).[77]

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−.[78] In the natural world cube shaped metal sulfur clusters can have sulfur atoms that are part of cysteine.

[Ni4Se23]4− has a cube with NiIV4Se4 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.[79]

Nitrosyl compounds edit

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.[60]

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.[60]

See also edit

References edit

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Sources edit

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December 05, 2023
nickel, compounds, also, category, chemical, compounds, containing, element, nickel, which, member, group, periodic, table, most, compounds, group, have, oxidation, state, nickel, classified, transition, metal, with, nickel, having, much, chemical, behaviour, . See also Category Nickel compounds Nickel compounds 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 H2O 2 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 superconductivity properties as nickel is adjacent to copper and iron in the periodic table can form compounds with the same structure as the high temperature superconductors that are known Contents 1 Colour 2 Geometry 3 Magnetism 4 Binary compounds 4 1 Oxides 4 2 Hydroxides 4 3 Halides 4 4 Chalcogenides 4 5 Pnictides 4 6 Other 4 7 Diatomic molecules 5 Alloys 6 Simple salts 6 1 Oxo acid salts 6 2 Fluoro acid salts 6 3 Chloroacid salts 6 4 Nitrogen anion salts 6 5 Organic acid salts 7 Double salts 7 1 Ternary chalcogenides 7 2 Ternary pnictides 7 3 Ternary halides 7 4 Polyoxometallates 8 Acidic salts 9 Basic salts 10 Complexes 11 Biological molecules 12 Organometallics 12 1 Alkoxy compounds 12 2 Aryloxy compounds 12 3 m bonded molecules 12 4 Sulfur rings 12 5 Nickel chalcogen cluster compound 12 6 Nitrosyl compounds 13 See also 14 References 15 SourcesColour editMost of the common salts of nickel are green due to the presence of hexaaquanickel II ion Ni H2O 62 Geometry editNickel 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 editSome 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 editA 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 edit Nickel oxides include Nickel II oxide and Nickel III oxide Hydroxides edit 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 b 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 edit nbsp nickel chloride hexahydrateNickel 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 Ammine complexes like hexaamminenickel chloride also exist 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 crystallise 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 NiF3Nickel IV fluoride NiF4 Chalcogenides edit nbsp needles of Halls Gap MilleriteBy reacting nickel with chalcogens nickel sulfide nickel selenide and nickel telluride are formed There are numerous sulfides Ni1 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 Ni1 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 edit nbsp The nickel arsenide nickelineNon 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 A and c 4 3059 A 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 NiAs2 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 edit Nickel also forms carbides and borides Nickel borides include 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 Nickel silicides include Ni3Si 9 Ni31Si12 Ni2Si Ni3Si2 NiSi and NiSi2 10 Nickel silicides are used in microelectronics Diatomic molecules edit Hot nickel vapour reacting with other atoms in the gas phase can produce molecules consisting of two atoms These can be studied by their emission spectrum The nickel monohalides are well studied 11 12 13 14 15 Alloys editCompounds 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 16 BaNi2Ge2 changes structure from orthorhombic to tetragonal around 480 C 17 This is a ternary intermetallic compound Others include BaNiSn3 and the superconductors SrNi2Ge2 SrNi2P2 SrNi2As2 BaNi2P2 BaNi2As2 17 Simple salts editOxo acid salts edit Main article Nickel oxo acid salts nbsp Mint green Annabergite a nickel arseniteImportant 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 18 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 19 The heptahydrate crystallises from water below 31 5 above this blue hexhydrate forms and above 53 3 the green form 20 Heating nickel sulfate dehydrates it and then 700 it loses sulfur trioxide sulfur dioxide and oxygen Other important nickel compounds in this class are nickel carbonate nickel nitrate and nickel phosphate Fluoro acid salts edit 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 21 22 Nickel tetrafluoroberyllate NiBeF4 xH2O can be hydrated with six or seven water molecules 23 Both nickel hexafluorostannate NiSnF 6 6 H 2 O displaystyle ce NiSnF6 6H2O nbsp and nickel fluorosilicate NiSiF 6 6 H 2 O displaystyle ce NiSiF6 6H2O nbsp crystallise in the trigonal system 24 Nickel hexafluorogermanate NiGeF6 has a rosy tan colour and a hexagonal crystal with a 5 241 A unit cell volume is 92 9 A3 It is formed in the reaction with GeF4 and K2NiF6 25 Nickel fuorotitanate NiTiF 6 6 H 2 O displaystyle ce NiTiF6 6H2O nbsp 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 26 Ni AsF6 2 Ni SbF6 2 Ni BiF6 2 are made by reacting the hexafluoro acid with NiF2 in hydrofluoric acid 25 They all have hexagonal crystal structure resembling the similar salts of the other first row transition metals 25 For Ni AsF6 2 a 4 98 c 26 59 and V 571 formula weight Z 3 25 Ni SbF6 2 is yellow with a 5 16A c 27 90A Z 3 The structure resembles LiSbF6 but with every second metal along the c axis missing 27 Others include the green fluorohafnate NiHfF6 6 H2O and Ni2HfF8 12 H2O 28 NiZrF6 6 H2O 29 Chloroacid salts edit Nickel tetrachloroiodate Ni ICl4 2 can be made by reacting iodine with nickel chloride and chlorine gas It consists of green needles 30 Nitrogen anion salts edit 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 31 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 32 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 33 Nickel azide forms a dihydrate Ni N3 2 2 H2O and a basic salt called nickel hydroxy azide Ni OH N3 34 Nickel amide Ni NH2 2 is a deep red compound that contains Ni6 clusters surrounded by 12 NH2 groups 35 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 36 Organic acid salts edit Main article Nickel organic acid salts Nickel forms many known salts with organic acids In many of these the ionised organic acid acts as a ligand Double salts editMain article Nickel 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 NH 4 displaystyle ce NH4 nbsp or thallium 37 As a mineral the ammonium nickel salt NH4 2Ni SO4 2 6 H2O can be called nickelboussingaultite 38 With sodium the double sulfate is nickelblodite Na2Ni SO4 2 4 H2O from the blodite family Nickel can be substituted by other divalent metals of similar sized to make mixtures that crystallise in the same form 39 Nickel forms double salts with Tutton s salt structure with tetrafluoroberyllate with the range of cations of ammonia 40 potassium rubidium cesium 41 and thallium 42 Anhydrous salts of the formula M2Ni2 SO4 3 which can be termed metal nickel trisulfates 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 43 Double hydrides of nickel exist such as Mg2NiH4 44 Ternary chalcogenides edit 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 Ternary pnictides edit Ternary pnictides that contain nickel are metallic and include MgNi2Bi4 45 SrNi2P2 SrNi2As2 BaNi2P2 and BaNi2As2 17 Ternary halides edit Nickel can form anions and salts with halogens including the hexafluoronickelates and tetrafluoronickelates tetrachloronickelates tetrabromonickelates and tetraiodonickelates The subiodide Bi12Ni4I3 is also known 45 Polyoxometallates edit 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 46 There is a dark brown heptamolybdonickelate IV potassium salt K2H8NiMo7O28 6H2O 47 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 48 Nickel IV heteropolyniobates such as the dark maroon Na12NiNb12O38 21 H2O are also known 49 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 50 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 A and b 103 469 and two formulas per unit cell 51 Na8Li12 Ni2 P2W15O56 2 74 H2O forms a sandwich structure and Na4Li5 Ni3 OH 3 H2O 3P2W16O59 48 H2O is a Wells Dawson polyoxometalate 52 Acidic salts editNickel hydrofluoride H5NiF7 6H2O is made by using excess hydrofluoric acid solution on nickel carbonate It is deep green 3 Basic salts editNickel 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 edit nbsp Sample of potassium tetracyanonickelate hydrateSimple 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 18 Some complexes have fivefold coordination N CH 2 CH 2 NMe 2 3 displaystyle ce N CH2CH2NMe2 3 nbsp tris N N dimethyl 2 aminoethyl amine P o C6H4SMe 3 P CH2CH2CH2AsMe2 3 18 Other ligands for octahedral coordination include PPh3 PPh2Me and thiourea 18 Nickel tetrahedral complexes are often bright blue and 20 times or more intensely coloured than the octahedral complexes 18 The ligands can include selections of neutral amines arsines arsine oxides phosphines or phosphine oxides and halogens 18 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 53 Nickel bis dimethylglyoximate an insoluble red solid is important for gravimetric analysis Biological molecules edit nbsp Active site of Nickel superoxide dismutaseCofactor 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 54 Plant ureases contain a bis m hydroxo dimeric nickel cluster 55 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 56 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 57 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 58 Organometallics editMain article Organonickel Well known nickel organometalic or organonickel compounds include Nickelocene bis cyclooctadiene nickel 0 and nickel tetracarbonyl 59 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 60 The nickel tetracarbonyl molecule is tetrahedral with a bond length for nickel to carbon of 1 82 A 60 Nickel tetracarbonyl easily starts breaking apart over 36 forming Ni CO 3 Ni CO 2 and Ni 60 Ni CO and NiC appear in mass spectroscopy of nickel carbonyl 60 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 61 Mixed cluster carbonyl anions like Cr2Ni3 CO 16 2 Mo2Ni3 CO 16 2 and W2Ni3 CO 16 2 Mo lt Ni4 CO 14 2 can form salts with bulky cations like tetraethylammonium The brown NiCo3 CO 11 changes to red Ni2Co4 CO 14 2 62 With oxygen or air the explosive Ni CO 3O2 can be formed from nickel carbonyl 63 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 64 tetrasulfur tetranitride when reduced with nickel carbonyl makes Ni N2S2H 2 also coloured dark violet 64 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 65 Alkoxy compounds edit Nickel tert butoxide Ni OC CH3 3 2 is coloured violet It is formed in the reaction of di tert butylperoxide with nickel carbonyl 60 Nickel dimethoxide is coloured green 66 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 67 Other alkoxy compounds known for nickel include nickel dipropoxide nickel di isopropoxide nickel tert amyloxide and nickel di tert hexanoxide 68 These can be formed by crystallising nickel chloride from the corresponding alcohol which forms an adduct This is then heated with a base 69 Nickel II alkoxy compounds are polymeric and non volatile 70 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 71 Homoletptic bimetallic alkoxides have two different metals and the same alkoxy group They include Ni m OMe 3AlOMe 2 Ni Al OBut 4 2 nickel tetra tert butoxyaluminate and Ni Al OPri 4 2 nickel tetra isopropoxyaluminate a pink liquid 72 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 73 A trimetallic one exists Zr2 OPri 9 Ni Al OPri 4 74 NiGe OBut 8 NiSn OBut 8 and NiPb OBut 8 are tricyclic Ni2 m3 OEt 2 m OEt 8Sb4 OEt 6 Heteroleptic bitmetallic ethoxides have more than one variety of alkoxy group e g Ni m OPri m OBut Al OBut 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 m4 O 2 m3 OEt 3 OEt 9 OEt 3 EtOH 4 75 Aryloxy compounds edit 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 76 m bonded molecules edit Others include cyclododecatriene nickel and t Ni cdt Sulfur rings edit Nickel bis dithiobenzoate can form a violet coloured sodium salt 60 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 77 Nickel chalcogen cluster compound edit A hexameric compound Ni SR 2 6 is produced in the reaction of nickel carbonyl with dialkyl sulfides RSR 77 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 78 In the natural world cube shaped metal sulfur clusters can have sulfur atoms that are part of cysteine Ni4Se23 4 has a cube with NiIV4Se4 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 79 Nitrosyl compounds edit 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 60 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 p C5H5NiNO is produced 60 See also editNickel IV organometallic complexReferences edit 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 Lian Li Su C X Armentrout P B May 1991 The bond energy of Ni 2 displaystyle ce Ni 2 nbsp 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 CRC Press 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 Ni 3 N displaystyle ce Ni3N nbsp Determined by Neutron Diffraction Inorganic Chemistry 40 23 5818 5822 doi 10 1021 ic0104860 PMID 11681891 Robert A Scott 2011 Boron Inorganic Chemistry Encyclopedia of Inorganic Chemistry Wiley p 401 ISBN 9780470862100 Itahara Hiroshi Simanullang Wiyanti F Takahashi Naoko Kosaka Satoru Furukawa Shinya 15 April 2019 Na Melt Synthesis of Fine Ni3Si Powders as a Hydrogenation Catalyst Inorganic Chemistry 58 9 5406 5409 doi 10 1021 acs inorgchem 9b00521 ISSN 0020 1669 PMID 30983337 S2CID 115204460 Dahal Ashutosh Gunasekera Jagath Harringer Leland Singh Deepak K Singh David J July 2016 Metallic nickel silicides Experiments and theory for NiSi and first principles calculations for other phases Journal of Alloys and Compounds 672 110 116 arXiv 1602 05840 doi 10 1016 j jallcom 2016 02 133 S2CID 55434466 Hauffe1 Karl Puschmann Herbert 2008 A26 nickel Corrosion Handbook Wiley pp NA doi 10 1002 9783527610433 chb203030 ISBN 978 3527610433 a href Template Cite book html title Template Cite book cite book a CS1 maint numeric names authors list link 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 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 5146 Bibcode 1968JChPh 49 5144K doi 10 1063 1 1670012 Krishnamurty V G 16 April 1952 The Complex Band Spectrum of Nickel Bromide NiBr Indian Journal of Physics Indian Association for the Cultivation of Science 26 429 hdl 10821 1696 ISSN 0973 1458 Kristallicheskie struktury soedinenij Ni www kipt kharkov ua a b c Hlukhyy Viktor Trots Dmytro Fassler Thomas F 13 January 2017 First Order Phase Transition in BaNi2Ge2 and the Influence of the Valence Electron Count on Distortion of the ThCr 2 Si 2 displaystyle ce ThCr2 Si2 nbsp Structure Type Inorganic Chemistry 56 3 1173 1185 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 amp 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 S2CID 96193596 Ray Nirmalendu Nath 20 April 1932 Fluoberyllate und ihre Analogie mit den Sulfaten II Fluoberyllate einiger zweiwertiger Metalle Zeitschrift fur anorganische und allgemeine Chemie 205 3 257 267 doi 10 1002 zaac 19322050307 Karnezos M Friedberg S A August 1978 FERROMAGNETISM IN NiSnF 6 6 H 2 O displaystyle ce NiSnF6 6H2O nbsp AND NiSiF 6 6 H 2 O displaystyle ce NiSiF6 6H2O nbsp 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 S2CID 95953256 Christe Karl O Wilson William W Bougon Roland A Charpin Pierrette January 1987 Preparation and characterization of Ni SbF 6 2 displaystyle ce Ni SbF6 2 nbsp 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 doi 10 1007 BF00911649 Karnezos M Meier D Friedberg S A 9 12 December 1975 Magnetic ordering in NiZrF 6 6 H 2 O displaystyle ce NiZrF6 6H2O nbsp AIP Conference Proceedings 29 505 Bibcode 1976AIPC 29 505K doi 10 1063 1 30416 Weinland R F Schlegelmilch Fr 7 March 1902 Uber Doppelsalze des Jodtrichlorids mit Chloriden zweiwertiger Metalle Zeitschrift fur 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 PMID 17683027 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 S2CID 95478362 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 Ni 6 NH 2 12 displaystyle ce Ni6 NH2 12 nbsp 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 Wang Xia Xinxin Zhuang Genbo Su Youping He 2008 A new ultraviolet filter Rb 2 Ni SO 4 2 6 H 2 O displaystyle ce Rb2Ni SO4 2 6H2O nbsp 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 Nickelblodite Nickelblodite 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 Ray Nirmalendunath 18 April 1936 Fluoberyllate und ihre Analogie mit Sulfaten IV Doppelsalze mit Rubidium und Casiumfluoberyllaten Zeitschrift fur 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 S2CID 98423115 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 Mg 2 NiH 4 displaystyle ce Mg2NiH4 nbsp Inorganic Chemistry 7 11 2254 2256 doi 10 1021 ic50069a016 a b Hertz Mary B Baumbach Ryan E Latturner Susan E 15 January 2020 Flux Synthesis of MgNi2Bi4 and Its Structural Relationship to NiBi3 Inorganic Chemistry 59 6 3452 3458 doi 10 1021 acs inorgchem 9b03196 PMID 31939654 S2CID 210814692 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 Vol 15 pp 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 Andre Casey William H 2013 Highly soluble iron and nickel substituted decaniobates with tetramethylammonium countercations Dalton Transactions 42 21 7529 33 doi 10 1039 C3DT50887K PMID 23588819 Liang Zhijie Zhang Dongdi Wang Haiying Ma Pengtao Yang Zongfei Niu Jingyang Wang Jingping 2016 The Ni 10 Nb 32 displaystyle ce Ni10Nb32 nbsp 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 PMID 26479899 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 m4 NR O and BH Ligands Inorganic Chemistry 57 5 2438 2446 doi 10 1021 acs inorgchem 7b02546 PMID 29140692 Greening C Berney M Hards K Cook G M Conrad R 3 March 2014 A soil actinobacterium scavenges atmospheric H 2 displaystyle ce H2 nbsp 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 PMC 3964045 PMID 24591586 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 PMC 423235 PMID 15173586 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 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 amp 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 NiFe 3 Q 4 displaystyle ce NiFe3Q4 nbsp 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 Ni 4 Se 4 Se 3 5 Se 4 4 displaystyle ce Ni4Se4 Se3 5 Se4 4 nbsp anion a Ni IV cubane species Journal of the American Chemical Society 113 18 7078 7079 doi 10 1021 ja00018a079 Sources editMellor 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 pages accessible by changing number on url Nichols David 1975 The chemistry of iron cobalt and nickel Oxford Pergamon Press ISBN 0080188737 Retrieved from https en wikipedia org w index php title Nickel compounds amp oldid 1176760198, wikipedia, wiki, book, books, library,

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