7440-02-0

Basic information

• Product Name: Nickel
• Synonyms: Nickel foil1000mm;Nickel wire, 0.25mm dia., 99.99% trace metals basis;Nickel flake, -325 mesh, 0.37 micron thick, 99.5% trace metals basis;Nickel powder, APS 5-15 micron, 99.8% trace metals basis;Nickel slug, 3.175mm dia. x 6.35mm length, 99.95% trace metals basis;Nickel plate1000mm;Nickel foil50x250mm;Nickel, beads
• CAS NO: 7440-02-0
• Molecular Formula: Ni
• Molecular Weight: 58.69
• EINECS: 231-853-9
• Product Categories: Metals;Inorganics;Catalysts for Organic Synthesis;Classes of Metal Compounds;Heterogeneous Catalysts;Ni (Nickel) Compounds;Synthetic Organic Chemistry;Transition Metal Compounds;NickelMetal and Ceramic Science;Catalysis and Inorganic Chemistry;Chemical Synthesis;Alternative Energy;Electrode MaterialsMetal and Ceramic Science;Materials Science;Metal and Ceramic Science;Industrial Raw Materials;Industrial Raw MaterialsApplication CRMs;Industrial Raw MaterialsCertified Reference Materials (CRMs);IRMM/BCR Certified Reference Materials;Matrix CRMs;Metals&AlloysAlphabetic;N;NA - NICertified Reference Materials (CRMs);Physical Properties;Reference/Calibration Standards;NA - NIReference/Calibration Standards;Application CRMs;Certified Reference Materials (CRMs);Industrial Raw MaterialsAlphabetic;Reactor DosimetryCertified Reference Materials (CRMs);Reactor Neutron Dosimetry;Reactor Neutron DosimetryCertified Reference Materials (CRMs);28: Ni;Nanomaterials;Nano
• Mol File: 7440-02-0.mol
• Article Data: 713

Chemical Properties

• Melting Point: 212 °C (dec.)(lit.)
• Boiling Point: 2732 °C(lit.)
• Appearance: White to gray-white/wire
• Density: 8.9
• Vapor Density: 5.8 (vs air)
• Storage Temp.: Flammables area
• Water Solubility: It is insoluble in water.
• Sensitive: air sensitive
• Stability: Stable in massive form. Powder is pyrophoric - can ignite spontaneously. May react violently with titanium, ammonium nitrate, po
• Merck: 14,8107
• CAS DataBase Reference: Nickel(CAS DataBase Reference)
• NIST Chemistry Reference: Nickel(7440-02-0)
• EPA Substance Registry System: Nickel(7440-02-0)

Safety Data

• Hazard Codes: C,Xi,Xn,F,T
• Statements: 34-50/53-43-40-10-17-52/53-48/23
• Safety Statements: 26-45-60-61-36-22-36/37-16-15-5-36/37/39-43-28
• RIDADR: UN 1493 5.1/PG 2
• WGK Germany: 3
• RTECS: VW4725000
• F: 8
• TSCA: Yes
• HazardClass: 4.1
• PackingGroup: II
• Hazardous Substances Data: 7440-02-0(Hazardous Substances Data)

Usage

History

Different sources of media describe the History of 7440-02-0 differently. You can refer to the following data:
1. Nickel was isolated first and recognized as an element by Cronstedt in 1751. The metal was derived in pure form by Richter in 1804. The metal takes its name from two German words ‘Nickel’ and ‘kupfernickel’, which mean Old Nick’s (or Satan) and Old Nick’s copper, respectively. The abundance of nickel in the earth’s crust is only 84 mg/kg, the 24th most abundant element. It is found in most meteorites, particularly in the iron meteorites or siderites, alloyed with iron. Its average concentration in seawater is 0.56 μg/mL. Nickel is one of the major components of the earth’s core, comprising about 7%. The most common nickel ores are pentlandite, (Ni,Fe)9S16, limonite, (Fe,Ni)O(OH)?nH2O, and garnierite, (Ni,Mg)6Si4O10(OH)8. Other ores that are of rare occurrence are the sulfide ores, millerite, NiS, polydymite Ni3S4 and siegenite, (Co,Ni)3S4; the arsenide ores niccolite, NiAs, gersdorffite, NiAsS, and annabergite, Ni3As2O8?8H2O; and the antimonide ore, NiSb.
2. Discovered by Cronstedt in 1751 in kupfernickel (niccolite). Nickel is found as a constituent in most meteorites and often serves as one of the criteria for distinguishing a meteorite from other minerals. Iron meteorites, or siderites, may contain iron alloyed with from 5 to nearly 20% nickel. Nickel is obtained commercially from pentlandite and pyrrhotite of the Sudbury region of Ontario, a district that produces much of the world’s nickel. It is now thought that the Sudbury deposit is the result of an ancient meteorite impact. Large deposits of nickel, cobalt, and copper have recently been developed at Voisey’s Bay, Labrador. Other deposits of nickel are found in Russia, New Caledonia, Australia, Cuba, Indonesia, and elsewhere. Nickel is silvery white and takes on a high polish. It is hard, malleable, ductile, somewhat ferromagnetic, and a fair conductor of heat and electricity. It belongs to the iron-cobalt group of metals and is chiefly valuable for the alloys it forms. It is extensively used for making stainless steel and other corrosion- resistant alloys such as Invar?, Monel?, Inconel?, and the Hastelloys?. Tubing made of a copper-nickel alloy is extensively used in making desalination plants for converting sea water into fresh water. Nickel is also now used extensively in coinage and in making nickel steel for armor plate and burglar-proof vaults, and is a component in Nichrome?, Permalloy?, and constantan. Nickel added to glass gives a green color. Nickel plating is often used to provide a protective coating for other metals, and finely divided nickel is a catalyst for hydrogenating vegetable oils. It is also used in ceramics, in the manufacture of Alnico magnets, and in batteries. The sulfate and the oxides are important compounds. Natural nickel is a mixture of five stable isotopes; twenty-five other unstable isotopes are known. Nickel sulfide fume and dust, as well as other nickel compounds, are carcinogens. Nickel metal (99.9%) is priced at about $2/g or less in larger quantities.

Uses

Different sources of media describe the Uses of 7440-02-0 differently. You can refer to the following data:
1. The most important applications of nickel metal involve its use in numerous alloys. Such alloys are used to construct various equipment, reaction vessels, plumbing parts, missile, and aerospace components. Such nickel-based alloys include Monel, Inconel, Hastelloy, Nichrome, Duranickel, Udinet, Incoloy and many other alloys under various other trade names. The metal itself has some major uses. Nickel anodes are used for nickel plating of many base metals to enhance their resistance to corrosion. Nickel-plated metals are used in various equipment, machine parts, printing plates, and many household items such as scissors, keys, clips, pins, and decorative pieces. Nickel powder is used as porous electrodes in storage batteries and fuel cells. Another major industrial use of nickel is in catalysis. Nickel and raney nickel are used in catalytic hydrogenation or dehydrogenation of organic compounds including olefins, fats, and oils.
2. Nickel-plating; for various alloys such as new silver, Chinese silver, German silver; for coins, electrotypes, storage batteries; magnets, lightning-rod tips, electrical contacts and electrodes, spark plugs, machinery parts; catalyst for hydrogenation of oils and other organic substances. See also Raney nickel. manufacture of Monel metal, stainless steels, heat resistant steels, heat and corrosion resistant alloys, nickel-chrome resistance wire; in alloys for electronic and space applications.
3. Nickel is used in various alloys, such asGerman silver, Monel, and nickel–chrome;for coins; in storage batteries; in spark plugs;and as a hydrogenation catalyst.
4. The most common use of nickel is as an alloy metal with iron and steel to make stainlesssteel, which contains from 5% to 15% nickel. The higher the percentage of nickel in stainlesssteel, the greater the steel’s resistance to corrosion—particularly when exposed to seawater.Nickel is also alloyed with copper to make Monel metal, which was widely used before stainless steel became more economical and practical. It was used for many purposes as varied ashousehold appliances and general manufacturing. Nickel is also used to electroplate othermetals to provide a noncorrosive protective and attractive finish.

Production

Nickel usually is recovered from its sulfide ore, pentlandite (Ni,Fe)9S16. Although laterite type oxide ores sometimes are used as starting materials, pentlandite is used in many commercial operations. Pentlandite often is found in nature associated with other sulfide minerals, such as pyrrhotite, Fe7S8,and chalcopyrite, CuFeS2. The ores are crushed and powdered. Sulfides are separated from gangue by froth flotation or magnetic separation processes. After this, the ore is subjected to roasting and smelting. These steps are carried out initially in rotary kilns or multihearth furnaces and then smelting is done in either blast furnaces or reverberatory, or arc furnaces. Most sulfur is removed as sulfur dioxide. Iron and other oxides produced in roasting are also removed along with siliceous slag during smelting. A matte obtained after smelting usually contains impure nickel-iron-copper sulfides and sulfur. The molten matte is treated with silica and an air blower in a converter in the Bessemerizing stage to remove all remaining iron and sulfur. Copper-nickel matte obtained in this stage is allowed to cool slowly over a few days to separate mineral crystals of copper sulfide, nickel sulfide and nickel-copper alloy. The cool matte is pulverized to isolate sulfides of nickel and copper by froth flotation. Nickel-copper alloy is extracted by magnetic separation. Nickel metal is obtained from the nickel sulfide by electrolysis using crude nickel sulfide cast into anodes and nickel-plated stainless steel cathodes. Alternatively, nickel sulfide is roasted to nickel oxide, which then is reduced to crude nickel and is electrorefined as above. Two other refining processes are also frequently employed. One involves hydrometallurgical refining in which sulfide concentrates are leached with ammonia solution to convert the copper, nickel, and cobalt sulfides into their complex amines. Copper is precipitated from this solution upon heating. Under such conditions, the sulfide-amine mixture of nickel and cobalt are oxidized to their sulfates. The sulfates then are reduced to metallic nickel and cobalt by heating with hydrogen at elevated temperatures under pressure. The metals are obtained in their powder form. The more common carbonyl refining process involves reaction of crude nickel with carbon monoxide under pressure at 100°C to form nickel tetracarbonyl, Ni(CO)4. The liquid tetracarbonyl upon heating at 300°C decomposes to nickel metal and carbon monoxide. Very pure nickel can be obtained by the carbonyl refining processes, as no other metal forms a similar carbonyl under these conditions.

Reactions

At ordinary temperatures, bulk nickel in compact form has no perceptible reactivity with air or water. However, in finely-divided state, the metal reacts readily and can be pyrophoric under certain conditions. When heated in air at 400°C or with steam, nickel converts to its oxide, NiO. When heated with bromine vapors or chlorine gas, nickel catches fire forming nickel bromide, NiBr2, and yellow nickel chloride, NiCl2, respectively. Finely divided nickel combines with carbon monoxide to form zero valent nickel tetracarbonyl, Ni(CO)4. The reaction occurs at 50°C and one atmosphere, although it is usually carried out at 200°C under high CO pressure between 100 to 400 atm for high yield of carbonyl, and to prevent product decomposition. Carbon monoxide at ordinary pressure may be passed over freshly reduced metal to form the tetracarbonyl. Finely divided nickel absorbs a large volume of hydrogen at high temperatures. Even at ordinary temperatures, considerable occlusion of hydrogen occurs on to the metal surface and no definite composition of any hydride formed is known. The metal activates molecular hydrogen to its atomic state, contributing to its catalytic action in hydrogenation of unsaturated compounds. Dilute mineral acids attack nickel to a varying extent. The metal dissolves readily in dilute nitric acid. Evaporation of the solution forms emerald green crystals of nickel nitrate hexahydrate, Ni(NO3)2?6H2O. Actions of dilute hydrochloric and sulfuric acid on nickel are relatively slow: slower than on iron. Concentrated nitric acid passivates the metal, oxidizing it and forming a protective film on its surface which prevents any further reaction. Nickel is stable in caustic alkalies. At moderate temperatures, it decomposes gaseous ammonia into hydrogen and nitrogen. Nickel combines with sulfur, phosphorus, carbon, arsenic, antimony, and aluminum at elevated temperatures. Fusion of nickel powder with molten sulfur yields nickel sulfide, NiS. Reaction with aluminum can be explosive at 1,300°C, forming nickelaluminum intermetallic products of varying compositions. Nickel powder combines with carbon dioxide in ammonia solution forming nickel carbonate. Boiling the solution to expel ammonia precipitates pure carbonate, NiCO3. Fine nickel powder reacts with sulfamic acid in hot aqueous solution under controlled conditions, forming nickel sulfamate tetrahydrate, Ni(SO3NH2)2?4H2O, used in electroplating baths.

Toxicity

Skin contact can cause dermatitis and a type of chronic eczema, known as “nickel itch”, caused by hypersensitivity reactions of nickel on the skin (Patnaik, P. 1999. A Comprehensive Guide to the Hazardous Properties of Chemical Substances, 2nd ed. pp. 621-622, New York: John Wiley & Sons.) Although oral toxicity of the metal is very low, ingestion may cause hyperglycemia and depression of the central nervous system. Chronic inhalation of nickel dust can cause lung and sinus cancers in humans. Nickel and certain of its compounds are listed by IARC under Group 2B carcinogens as “possibly carcinogenic to humans” (International Agency for Research on Cancer. 1990. IARC Monograph, Vol. 49: Geneva.)

Description

Nickel is a hard, silvery white, malleable metal chunk or grey powder. Nickel powder is pyrophoric – can ignite spontaneously. It may react violently with titanium, ammonium nitrate, potassium perchlorate, and hydrazoic acid. It is incompatible with acids, oxidising agents, and sulphur. The industrially important nickel compounds are nickel oxide (NiO), nickel acetate (Ni(C2H3O2), nickel carbonate (NiCO3), nickel carbonyl (Ni(CO)4), nickel subsulphide (NiS2), nickelocene (C5H5)2Ni, and nickel sulphate hexahydrate (NiSO4 · 6H2O). Nickel compounds have been well established as human carcinogens. Investigations into the molecular mechanisms of nickel carcinogenesis have revealed that not all nickel compounds are equally carcinogenic: certain water-insoluble nickel compounds exhibit potent carcinogenic activity, whereas highly water-soluble nickel compounds exhibit less potency. The reason for the high carcinogenic activity of certain water-insoluble nickel compounds relates to their bioavailability and the ability of the nickel ions to enter cells and reach chromatin. The water-insoluble nickel compounds enter cells quite efficiently via phagocytic processes and subsequent intracellular dissolution. Nickel is classified as a borderline metal ion because it has both soft and hard metal properties and it can bind to sulphur, nitrogen, and oxygen groups. Nickel ions are very similar in structure and coordination properties to magnesium.

Chemical Properties

Different sources of media describe the Chemical Properties of 7440-02-0 differently. You can refer to the following data:
1. silver white, hard, malleable metal chunks or grey powder
2. RANEY NICKEL is a hard, ductile, magnetic metal with a silver-white color.

Physical properties

Nickel metal does not exist freely in nature. Rather, it is located as compounds in ores ofvarying colors, ranging from reddish-brown rocks to greenish and yellowish deposits, andin copper ores. Once refined from its ore, the metallic nickel is a silver-white and hard butmalleable and ductile metal that can be worked hot or cold to fabricate many items. Nickel,located in group 10, and its close neighbor, copper, just to its right in group 11 of the periodictable, have two major differences. Nickel is a poor conductor of electricity, and copper is anexcellent conductor, and although copper is not magnetic, nickel is. Nickel’s melting point is1,455°C, its boiling point is 2,913°C, and its density is 8.912 g/cm3.

Isotopes

There are 31 isotopes of nickel, ranging from Ni-48 to Ni-78. Five of these arestable, and the percentage of their contribution to the element’s natural existence onEarth are as follows: Ni-58 = 68.077%, Ni-60 = 26.223%, Ni-61 = 1.140%, Ni-62 =3.634%, and Ni 64 = 0.926%. All of the other 26 isotopes of nickel are artificially madeand radioactive with half-lives ranging from a few nanoseconds to 7.6×104 years.

Origin of Name

The name is derived from the ore niccolite, meaning “Old Nick,” referred to as the devil by German miners. The niccolite mineral ore was also called “kupfernickel,” which in German stands for two things; first, it is the name of a gnome (similar to Cobalt), and second, it refers to “Old Nick’s false copper.”

Occurrence

Nickel is the 23rd most abundant element found in the Earth’s crust. It is somewhat plentiful but scattered and makes up one-hundredth of 1% of igneous rocks. Nickel metal is foundin meteorites (as are some other elements). It is believed that molten nickel, along with iron,makes up the central sphere that forms the core of the Earth.There are several types of nickel ores. One is the major ore for nickel called pentlandite(NiS ? 2FeS), which is iron/nickel sulfide. Another is a mineral called niccolite (NiAs), discovered in 1751 and first found in a mining area of Sweden. By far, the largest mining area fornickel is located in Ontario, Canada, where it is recovered from what is thought to be a verylarge meteorite that crashed into the Earth eons ago. This large nickel deposit is one reasonfor the theory of the Earth’s core being molten nickel and iron, given that both the Earth andmeteorites were formed during the early stages of the solar system. Some nickel ores are alsofound in Cuba, the Dominican Republic, and Scandinavia. Traces of nickel exist in soils, coal,plants, and animals.

Characteristics

As mentioned, nickel is located in group 10 (VIII) and is the third element in the specialtriad (Fe, Co, Ni) of the first series of the transition elements. Nickel’s chemical and physicalproperties, particularly its magnetic peculiarity, are similar to iron and cobalt.Some acids will attack nickel, but it offers excellent protection from corrosion from air andseawater. This quality makes it excellent for electroplating other metals to form a protectivecoating. Nickel is also an excellent alloy metal, particularly with iron, for making stainless steelas well as a protective armor for military vehicles. It is malleable and can be drawn throughdies to form wires. About one pound of nickel metal can be drawn to about 200 miles of thinwire.

Production Methods

Nickel is obtained by processing sulfide and laterite ore concentrates using pyrometallurgic and hydrometallurgic processes. The resultant nickel matte obtained by roasting and smelting is subjected to further cleaning by electro-, vapo-, and hydrometallurgic refining methods. Some portion of the matte is roasted to obtain commercial nickel oxide agglomerate. Pure, 99.9% nickel can be obtained by electrolytic refining process. The most pure, 99.97%, nickel is obtained by vapometallurgy. In this process, known also as the Mond method,nickel and copper sulfide blend is converted to oxides and then reduced by heating with water gas at 350–400°C. The resultant active form of nickel is treated with carbon monoxide to give volatile nickel carbonyl [Ni(CO)4]. The latter reaction is reversible; heating results in pure nickel and carbon monoxide.

Preparation

The carbonyl process is most commonly employed when very pure nickel is required. The impure metal is reacted with pure carbon monoxide at 50° and the carbonyl produced fractionated several times prior to pyrolysis at around 200°. The nickel thus obtained has a purity of 99.90-99.99% depending upon the materials used. Electrolytic methods for producing high purity nickel depend upon the production of high purity nickel salts. The nickel obtained by the electrolysis of pure nickel chloride solution with inert platinum-iridium anodes is 99.99% pure.

Definition

Different sources of media describe the Definition of 7440-02-0 differently. You can refer to the following data:
1. A transition metal that occurs naturally as the sulfide and silicate. It is extracted by the Mond process, which involves reduction of nickel oxide using carbon monoxide followed by the formation and subsequent decomposition of volatile nickel carbonyl. Nickel is used as a catalyst in the hydrogenation of alkenes, e.g. margarine manufacture, and in coinage alloys. Its main oxidation state is +2 and these compounds are usually green. Symbol: Ni; m.p. 1453°C; b.p. 2732°C; r.d. 8.902 (25°C); p.n. 28; r.a.m. 58.6934.
2. nickel: Symbol Ni. A malleable ductilesilvery metallic transition element;a.n. 28; r.a.m. 58.70; r.d. 8.9;m.p. 1450°C; b.p. 2732°C. It is foundin the minerals pentlandite (NiS),pyrrhoite ((Fe,Ni)S), and garnierite((Ni,Mg)6(OH)6Si4O11.H2O). Nickel isalso present in certain iron meteorites(up to 20%). The metal isextracted by roasting the ore to givethe oxide, followed by reductionwith carbon monoxide and purificationby the Mond process. Alternativelyelectolysis is used. Nickel metalis used in special steels, in Invar, and,being ferromagnetic, in magnetic alloys,such as Mumetal. It is also aneffective catalyst, particularly for hydrogenation reactions (see also raneynickel). The main compounds areformed with nickel in the +2 oxidationstate; the +3 state also exists (e.g.the black oxide, Ni2O3). Nickel wasdiscovered by Axel Cronstedt(1722–65) in 1751.
3. ChEBI: Chemical element (nickel group element atom) with atomic number 28.

General Description

Nickel catalyst, is extremely fine powdered nickel. Nickel is grayish colored. Insoluble in water. Nickel catalyst is used to promote the chemical action in manufacturing synthetics and to process vegetable oil and petroleum. If exposed to air or moisture, Nickel may become hot enough to ignite. Nickel is insoluble in water and does not react with larger volumes of water.

Air & Water Reactions

Pyrophoric, Ignites spontaneously in the presence of air; during storage, H2 escapes with fire and explosion hazards; reacts violently with acids forming H2. [Handling Chemicals Safely 1980. p. 807].

Reactivity Profile

Metals, such as METAL CATALYST, are reducing agents and tend to react with oxidizing agents. Their reactivity is strongly influenced by their state of subdivision: in bulk they often resist chemical combination; in powdered form they may react very rapidly. Thus, as a bulk metal Nickel is somewhat unreactive, but finely divided material may be pyrophoric. The metal reacts exothermically with compounds having active hydrogen atoms (such as acids and water) to form flammable hydrogen gas and caustic products. The reactions are less vigorous than the similar reactions of alkali metals, but the released heat can still ignite the released hydrogen. Materials in this group may react with azo/diazo compounds to form explosive products. These metals and the products of their corrosion by air and water can catalyze polymerization reactions in several classes of organic compounds; these polymerizations sometimes proceed rapidly or even explosively. Some metals in this group form explosive products with halogenated hydrocarbons. Can react explosively with oxidizing materials.

Hazard

Nickel dust and powder are flammable. Most nickel compounds, particularly the salts, aretoxic. NiSO4 is a known carcinogen.Although nickel is not easily absorbed in the digestive system, it can cause toxic reactionsand is a confirmed carcinogen in high concentration in the body. Nickel workers can receivesevere skin rashes and lung cancer from exposure to nickel dust and vapors.Nickel is stored in the brain, spinal cord, lungs, and heart. It can cause coughs, shortnessof breath, dizziness, nausea, vomiting, and general weakness.

Health Hazard

Ingestion of nickel can cause hyperglycemia,depression of the central nervous system,myocardial weakness, and kidney damage.A subcutaneous lethal dose in rabbits isin the range 10 mg/kg. The oral toxicityof the metal, however, is very low. Skincontact can lead to dermatitis and “nickelitch,” a chronic eczema, caused by dermalhypersensitivity reactions. Nickel itch mayresult from wearing pierced earrings. Inhalationof metal dusts can produce irritation ofthe nose and respiratory tract. Nickel andsome of its compounds have been reportedto cause lung cancer in experimental animals.It may also induce cancer in nose,stomach, and possibly the kidney. The experimentaldata on the latter, are not fully confirmative.Nickel refinery flue dust, nickelsulfide (Ni3S2) , and nickeloxide (NiO) produced localizedtumors in experimental animals wheninjected intramuscularly. IARC has classifiednickel and its compounds as carcinogenicto humans (IARC 1990). Inhalation ofmetal dusts can produce lung and sinus cancersin humans, with a latent period of about25 years. Nickel is susceptible to cross human placentaand produce teratogenesis and embroytoxicity. In vitro study on lipid peroxidationindicated that nickel induced peroxidativedamage to placental membrane causing decreased placental viability, altered permeabilityand subsequent embroy toxicity (Chenand Lin 1998). In a latter study, Chen et al.(2003) evaluated nickel-induced oxidativestress and effects of antioxidants in humanlymphocytes. The levels of intracellular reactiveoxygen species, lipid peroxidation andhydroxyl radicals were examined for one hourfollowing acute treatment with Nicl2. Thestudy showed that glutathione, catalase andmannitol each provided protection against theoxidative stress induced by Ni. The efficacy of organic chelating ligandsin cleaning human skin contaminated withnickel has been investigated (Healy et al.1998). Commercial liquid soap added withL-histidine was found to be more effectivethan the untreated soap. Similarly sodiumethylenediamine tetraacetic acid (EDTA)salt or L-histidine added to phosphate buffersaline solution was more effective in cleaningnickel contaminated human skin than thephosphate saline alone.

Fire Hazard

Flammable/combustible material. May ignite on contact with moist air or moisture. May burn rapidly with flare-burning effect. Some react vigorously or explosively on contact with water. Some may decompose explosively when heated or involved in a fire. May re-ignite after fire is extinguished. Runoff may create fire or explosion hazard. Containers may explode when heated.

Agricultural Uses

Nickel (Ni) is a silver-white, ductile, malleable, yet tough metallic element of Group 10 (formerly Group VIII) of the Periodic Table. Mostly, nickel goes into the making of steel and other corrosion resistant alloys. Finely divided nickel is used as a hydrogenation catalyst. Nickel is a beneficial trace element for plants. Its presence in the urease enzyme underlines its importance as a functional element. It is essential for grain viability, in barley and at concentrations less than 100 μg/kg, the grain level and the germination frequency decrease progressively. The quantity of Ni in a few fertilizers is as given: 2 ppm in nitrochalk, 13 ppm in superphosphate and 10 ppm in FYM. Nickel is the metal component of urease that hydrolyzes urea to give ammonia and carbon dioxide. Compounds that react with nickel in the urease molecule inhibit the hydrolysis of urea. Nickel enhances the nodule weight and the seed yield of soybeans, chickpeas and temperate cereals. It is present in plants in the range of 0.1 to 1O ppm of the dry weight. High levels of Ni may induce Zn or Fe deficiency because of cation competition, and may create nickel toxicity. The browning and necrosis of the leaf tips and margins are the toxicity symptoms on the plant. High Ni content also causes the distortion of young leaves and the death of the terminal shoots of the plant. The emerging leaves may fail to unroll and become necrotic, with the necrosis starting from near the base and spreading toward the leaf tip. Nickel toxicity in cereals and grasses varies in the intensity of chlorosis along the length of the leaf with a series of transverse bands. Sewage sludge contains heavy metals like Ni, Cd, etc. that are absorbed by plants grown in soils contaminated with these heavy metals. The toxicity caused by these metals is in turn, passed on to animals that feed on such plants. Any regulation for sludge use should ensure that the soil pH is not lower than 6.5, as heavy metals are insoluble at pH greater than 6.5.

Safety Profile

Confirmed carcinogen with experimental carcinogenic, neoplastigenic, and tumorigenic data. Poison by ingestion, intratracheal, intraperitoneal, subcutaneous, and intravenous routes. An experimental teratogen. Ingestion of soluble salts causes nausea, vomiting, and diarrhea. Mutation data reported. Hypersensitivity to nickel is common and can cause allergic contact dermatitis, pulmonary asthma, conjunctivitis, and inflammatory reactions around nickel-containing medcal implants and prostheses. Powders may ignite spontaneously in air. Reacts violently with F2, NH4NO3, hydrazine, NH3, (H2 + dioxane), performic acid, P, Se, S, (Ti + KCLO3). Incompatible with oxidants (e.g., bromine pentafluoride, peroxyformic acid, potassium perchlorate, chlorine, nitryl fluoride, ammonium nitrate), Raney-nickel catalysts may initiate hazardous reactions with ethylene + aluminum chloride, pdioxane, hydrogen, hydrogen + oxygen, magnesium silicate, methanol, organic solvents + heat, sulfur compounds. Nickel catalysts have caused many industrial accidents.

Potential Exposure

Nickel is used as an alloy additive in steel manufacture; in the production of coins and other utensils. Nickel forms alloys with copper, manganese, zinc, chromium, iron, molybdenum, etc. Stainless steel is the most widely used nickel alloy. An important nickel copper alloy is Monel metal, which contains 66% nickel and 32% copper and has excellent corrosion resistance properties. Permanent magnets are alloys chiefly of nickel, cobalt, aluminum, and iron. Elemental nickel is used in electroplating, anodizing aluminum casting operations for machine parts; and in coinage; in the manufacture of acid-resisting and magnetic alloys; magnetic tapes; surgical and dental instruments; nickel cadmium batteries; nickel soaps in crankcase oil; in ground-coat enamels; colored ceramics; and glass. It is used as a catalyst in the hydrogenation synthesis of acrylic esters for plastics. Exposure to nickel may also occur during mining, smelting, and refining operations. The route by which most people in the general population receive the largest portion of daily nickel intake is through food. Based on the available data from composite diet analysis, between 300 and 600 μg nickel per day are ingested. Fecal nickel analysis, a more accurate measure of dietary nickel intake, suggests about 300 μg per day. The highest level of nickel observed in water was 75 μg/L. Average drinking water levels are about 5 μg/L. A typical consumption of 2 L daily would yield an additional 10 μg of nickel, of which up to 1 μg would be absorbed.

Carcinogenicity

Metallic nickel is reasonably anticipated to be a human carcinogenbased on sufficient evidence of carcinogenicity from studies in experimental animals.

Environmental Fate

Nickel and its compounds are naturally present in the Earth’s crust, and nickel can be released into the atmosphere via natural discharges such as windblown dust and volcanic eruptions. It is estimated that 8.5 million kilograms of nickel are emitted into the atmosphere from natural sources such as windblown dust, volcanoes, and vegetation each year. Anthropogenic activities constitute significant discharge into the environment, particularly in the form of particulate matter and nickel compounds not normally found naturally; these sources comprise five times the quantity estimated to come from natural sources. Nickel releases are mainly in the form of aerosols that cover a broad spectrum of sizes. Particulates from power plants tend to be associated with smaller particles than those from smelters. Atmospheric aerosols are removed by gravitational settling and dry and wet deposition. Submicrometer particles may have atmospheric half-lives as long as 30 days. Monitoring data confirm that nickel can be transported far from its source, and that the form of nickel emitted to the atmosphere will vary according to the type of source. Species associated with combustion, incineration, and metals smelting and refining are often complex nickel oxides, nickel sulfate, metallic nickel, and in more specialized industries, nickel silicate, nickel subsulfide, and nickel chloride. Nickel may be transported into streams and waterways from the natural weathering of soil as well as from anthropogenic discharges and runoff. This nickel can accumulate in sediment, with the adsorption of the metal to the soil depending on pH, redox potential, ionic strength of the water, concentration of complexing ions, and the metal concentration and type. Soluble nickel compounds such as nickel chloride would be expected to release divalent nickel into moist environments. Since these compounds quickly dissolve upon exposure to water, and partially due to the ubiquity of nickel in soil, water, and air, tracking the course of these compounds through the environment is difficult. This is particularly due to nickel’s ability to complex with anionic species other than chloride to form nickel oxide, sulfate, nitrate, carbonate, or acetate, among others. Industrial uses of nickel result in nickel being distributed mainly at soil surfaces and through surrounding waterways and water tables. Once distributed to the soil, nickel(II) ions can potentially form inorganic crystalline minerals or precipitates, can complex or adsorb onto organic and inorganic surfaces, can participate in cation exchange, and can exist as free-ion or chelated metal complexes in soil solution.

Shipping

UN3089 Metal powders, flammable, n.o.s., Hazard Class: 4.1; Labels: 4.1-Flammable solid. UN3077 Environmentally hazardous substances, solid, n.o.s., Hazard Class: 9; Labels: 9-Miscellaneous hazardous material, Technical Name Required.

Toxicity evaluation

Skin sensitization is believed to occur as a result of nickel binding to proteins (particularly on the cell surface) and hapten formation. The nickel–protein complex is recognized as foreign and an immune reaction follows. For example, sweat may react with the nickel in plated jewelry that comes in direct contact with skin; dissolved metal may penetrate and react with proteins in the skin, leading to immune sensitization. Nickel may substitute for certain other metals (especially zinc) in metal-dependent enzymes, leading to altered protein function. High nickel content in serum and tissue may interfere with both copper and zinc metabolism. It also readily crosses the cell membrane via calcium channels and competes with calcium for specific receptors. Nickel can alter the sodium balance and lipid metabolism and can induce metallothionein synthesis. Dissolved nickel also affects the T-cell system and suppresses the activity of natural killer cells. If given orally or by inhalation, nickel chloride has been reported to decrease iodine uptake by the thyroid gland. The lipid peroxidation properties of nickel can introduce potential malignancies in humans, as DNA strand gaps and breaks in DNA–protein cross-links can form. The down-regulation of glycoprotein metabolism by nickel ions may produce nephrotoxicity in humans as well. Nickel carbonyl can cross-link amino acids to DNA and lead to formation of reactive oxygen species. Nickel carbonyl can also suppress natural killer cell activity and production of some interferons. Responses in many of these assays were weak and occurred at toxic doses, and were affected by tissue culture conditions modifying uptake by the cell. The mechanism of nickel carcinogenesis is controversial, and is likely to vary with the form of nickel. The nickel ion (Ni2+) alone does not form premutagenic DNA lesions, suggesting that nickel causes indirect DNA damage, perhaps due to oxidative stress or blocking DNA repair mechanisms. Nickel is an essential trace nutrient in plants and certain animal species (e.g., rat and chick); however, it has not been shown to be essential in humans.

Incompatibilities

Nickel dust is a spontaneously flammable solid and a dangerous fire hazard.

Waste Disposal

Nickel compoundsencapsulation followed by disposal in a chemical waste landfill. However, nickel from various industrial wastes may also be recovered and recycled as described in the literature.

InChI:InChI=1/Ni/q+2

Synthetic route

nickel(II) chloride hexahydrate + hydrazine hydrate (7803-57-8) + sodium hydroxide (1310-73-2) → nickel (7440-02-0)

Conditions	Yield
In water N2H4*H2O (80%) added to aq. soln. of NiCl2*6H2O (temp. increased to 65°C) under vigorous stirring, cooling to 50°C, aq. NaOH (50%)added (temp. increased to 54°C), 1 h; ppt. washed with water and dried at room temp. for 16 h;	100%
In water; ethylene glycol byproducts: N2, H2O; other Radiation; soln. of Ni compd. in ethylene glycol treated with hydrazine hydrate andNaOH under external magnetic field (0.13-0.35 T) with vigorous stirring , react at 60°C; pptd., septd., washed (ethanol), dried (vac., 40°C, 24 h), SEM, XRD;

hydrogen (1333-74-0) + nickel(II) hydroxide → nickel (7440-02-0)

Conditions	Yield
In not given at 205°C, H2 pressure 14 atm, 45 min, form of product is powder;	99.8%
In not given at 200-300°C, 10 h, form of product is powder;	85%
at 270-320°C;

sodium (7440-23-5) + nickel dichloride → nickel (7440-02-0)

Conditions	Yield
Na-emulsion in organic solvent, at 220°C, form of product is powder;	99.2%
Na-emulsion in organic solvent, at 220°C, form of product is powder;	99.2%
explosive reaction;

((CO)NiNCN(CH3)2)2 → nickel (7440-02-0) + NCNMe2 (1467-79-4)

Conditions	Yield
byproducts: CO; thermal dissociation in high vacuum;	A 99% B 99%

{(CO)NiNCN(CH2)4}2 → pyrrolidine-1-carbonitrile (1530-88-7) + nickel (7440-02-0)

Conditions	Yield
byproducts: CO; thermal dissociation in high vacuum;	A 99% B 99%

{(CO)NiNCN(CH2)2O(CH2)2}2 → N-cyanomorpholine (1530-89-8) + nickel (7440-02-0)

Conditions	Yield
byproducts: CO; thermal dissociation in high vacuum;	A 99% B 99%

{(CO)NiNCN(CH2)4C(CH3)H}2 → 2-methylpiperidine-1-carbonitrile (5321-87-9) + nickel (7440-02-0)

Conditions	Yield
byproducts: CO; thermal dissociation in high vacuum;	A 99% B 99%

{(CO)NiNCN(CH2)2C6H4(CH2)}2 → 3,4-dihydro-2(1H)-isoquinolinecarbonitrile (1705-22-2) + nickel (7440-02-0)

Conditions	Yield
byproducts: CO; thermal dissociation in high vacuum;	A 99% B 99%

{(CO)NiNCN(CH2)6}2 → hexahydroazepin-1-yl cianide (5321-89-1) + nickel (7440-02-0)

Conditions	Yield
byproducts: CO; thermal dissociation in high vacuum;	A 99% B 99%

[((C6H5)3P)3NiCl]2 → bis(triphenylphosphine)nickel(II) chloride (14264-16-5, 53996-95-5, 62075-39-2, 39716-73-9) + nickel (7440-02-0) + nickel dichloride

Conditions	Yield
In neat (no solvent) byproducts: triphenylphosphine; Ar-atmosphere; 140-180°C, 1 h; extn. (ether, CH2Cl2, H2O), evapn. of extract;	A 97.7% B 94.7% C 87.5%

nickel(II) sulfate hexahydrate → nickel (7440-02-0)

Conditions	Yield
With sodium carbonate; hydrazine hydrate; sodium dodecylbenzenesulfonate In water mixt. heated at 90 °C at pH 9.6 (Na2CO3) with hydrazine:nickel 2:1 molar ratio, Ni(2+) conc. 0.25 M, sodium citrate:Ni ratio 1:4 for 18 min; metal powder filtered, washed (H2O, ethanol, acetone), dried in vac. at 40 °C; detd. by XRD;	96%
With sodium carbonate; hydrazine hydrate; sodium dodecylbenzenesulfonate In water mixt. heated at 90 °C at pH 9.6 (Na2CO3) with hydrazine:nickel 2:1 molar ratio, Ni(2+) conc. 0.25 M, sodium citrate:Ni ratio 1:4 for 120 or 160 min or without citrate for 90 min; metal powder filtered, washed (H2O, ethanol, acetone), dried in vac. at 40 °C; detd. by XRD;	95%
With sodium carbonate; hydrazine hydrate; sodium dodecylbenzenesulfonate In water mixt. heated at 90 °C at pH 9.6 (Na2CO3) with hydrazine:nickel 2:1 molar ratio, Ni(2+) conc. 0.25 M, sodium citrate:Ni ratio 1:4 for 140 min; metal powder filtered, washed (H2O, ethanol, acetone), dried in vac. at 40 °C; detd. by XRD;	94%

bis(1,5-cyclooctadiene)nickel (0) (1295-35-8) → Cyclooctan (292-64-8) + nickel (7440-02-0)

Conditions	Yield
With hydrogen In hexane 1 atm., 20°C, vigorous reaction after induction period;	A 96% B n/a
With hydrogen In hexane 1 atm., 20°C, vigorous reaction after induction period;	A 96% B n/a

bis(1,5-cyclooctadiene)nickel (0) (1295-35-8) → nickel (7440-02-0) + tetracarbonyl nickel (13463-39-3, 71564-36-8) + 1,5-dicyclooctadiene (5259-72-3, 10060-40-9, 111-78-4)

Conditions	Yield
With carbon monoxide In hexane -40°C, warming within 1 h to 0-20°C;	A 0% B 93% C 80.6%
With carbon monoxide In hexane -40°C, warming within 1 h to 0-20°C;	A 0% B 93% C 80.6%

ethylmagnesium bromide (925-90-6) + nickel dibromide → ethane (74-84-0) + ethene (74-85-1) + nickel (7440-02-0) + magnesium bromide

Conditions	Yield
In tetrahydrofuran To a soln. of anhydrous salt is added C2H5MgBr at 20°C with stirring. The reaction mixture is left for 5 - 6 h at room temp.; decantation, washing with THF, water and ethanol; electron diffraction;	A n/a B n/a C 90% D n/a

tris[bis(pentane-2,4-dionato)nickel(II)] + sodium tetraphenyl borate (143-66-8) → nickel (7440-02-0)

Conditions	Yield
In 1,2-dimethoxyethane Irradiation (UV/VIS); under Ar; ratio B(3+) : Ni(2+) = 2 : 1; irradn. (254 nm) for 8 h gave deposition of Ni; deposit sepd., washed with acetone and water, and dried in vac. to give pure Ni;	90%

trans-,trans-,trans-C12H18NiC(N2)(C6H5)2 → [Ni(1,5,9-cyclododecatriene)] (548757-70-6, 33154-75-5, 12126-69-1, 548757-71-7, 39330-67-1) + benzophenone hydrazone (5350-57-2) + nickel (7440-02-0)

Conditions	Yield
In diethyl ether byproducts: N2; heating cautiously to 20°C;	A 89% B n/a C n/a

nickel(II) oxide (1313-99-1) → nickel (7440-02-0)

Conditions	Yield
With hydrogen In neat (no solvent) Kinetics; 1000 h, NiO calcinated at 1000°C;;	85%
With H2 In neat (no solvent) Kinetics; 1000 h, NiO calcinated at 1000°C;;	85%
With hydrogen In neat (no solvent) Kinetics; 180°C, 70 h, NiO prepared be H2O elimination of Ni(OH)2 in vacuum;;	>99

tetracarbonyl nickel (13463-39-3, 71564-36-8) → nickel (7440-02-0)

Conditions	Yield
introducing of liq. Ni(CO)4 into heavy oil, vigorous mixing at 250°C, after filtration keep under petroleum ether or N2;	85%
Sonication; at 240-260°C;
150-250°C. 1-2 at, high-frequency technic, diphenyl and diphenyl oxide used as germ;

trans-,trans-,trans-C12H18NiC(N2)(C6H5)2 → 1,5,9-cyclodecatriene + nickel (7440-02-0) + benzonitrile (100-47-0)

Conditions	Yield
byproducts: N2; -30°C;	A 80.9% B n/a C 13.5%

nickel(II) chloride hexahydrate → nickel (7440-02-0)

Conditions	Yield
With N2H4*H2O; poly(vinyl pyrrolidone) In ethylene glycol byproducts: NH3, N2, H2; ethylene glycol refluxed for 5 min, treated dropwise with hydrazine monohydrate, treated with Ni salt in ethylene glycol and poly(vinyl pyrrolidone) in ethylene glycol under vigorous stirring, refluxed for 60 min; centrifuged, washed (abs. ethanol) 6 times, evapd.(vac.) at 80°C,XRD;	80%
In water Electrolysis; platinum anode and copper cathode were used; the composition of the bath: 50 g/dm3 NiCl2*6H2O, 50 g/dm3(NH4)2SO4 and 250 mol/dm3 NH4OH; the pH of the soln. was 9.5-10.2; at 25°C; the plating time was 15 min;;
With (NH2)2CSO2 In pentan-1-ol; water Kinetics; isothermal redn. of Ni-salt with thiourea dioxide, 15 mol-% alcohol, pH4.0 (Britton-Robinson buffer), 1 h, 313+/-0.5 K; gravimetric anal.;

sodium tetraphenyl borate (143-66-8) + nickel dibromide → nickel (7440-02-0)

Conditions	Yield
In 1,2-dimethoxyethane Irradiation (UV/VIS); under Ar; mole ratio NaBPh4 : NiBr2 = 2 : 1; irradn. (254 nm) for 8 h gave deposition of Ni; deposit sepd., washed with acetone and water, and dried in vac. to give pure Ni;	80%

sodium tetraphenyl borate (143-66-8) + copper(ll) bromide (7789-45-9) + nickel dibromide → nickel (7440-02-0) + copper (12775-96-1, 15158-11-9, 15721-63-8, 16941-75-6, 17493-86-6, 19498-52-3, 20499-83-6, 20499-84-7, 20499-85-8, 20499-86-9, 20573-10-8, 20573-11-9, 21595-51-7, 21595-52-8, 22206-52-6, 26445-28-3, 28959-95-7, 37362-93-9, 39417-05-5, 54603-16-6, 54603-23-5, 54603-32-6, 54603-40-6, 54603-48-4, 54603-81-5, 54603-89-3, 56316-56-4, 95985-91-4, 122297-32-9, 7440-50-8)

Conditions	Yield
In 1,2-dimethoxyethane Irradiation (UV/VIS); under Ar; mole ratios NaBPh4 : NiBr2 : CuBr2 = 8 : 3 : 1; irradn. (254 nm) for 10 h gave deposition of Ni and Cu;	A 73% B 24%
In 1,2-dimethoxyethane Irradiation (UV/VIS); under Ar; mole ratios NaBPh4 : NiBr2 : CuBr2 = 4 : 1 : 1; irradn. (254 nm) for 10 h gave deposition of Ni and Cu;	A 48% B 49%

bis(1,5-cyclooctadiene)nickel (0) (1295-35-8) + 3,6-dimethylene-1,7-octadiene (3382-59-0) + tris(1-methylethyl)phosphine (6476-36-4) → (η(2),η(2)-3,6-dimethylene-1,7-butadiene)NiPiPr3 (163976-20-3) + nickel (7440-02-0)

Conditions	Yield
In diethyl ether stirring (-30°C, 48 h); filtering (-30°C), crystn. (-78°C), washing (pentane, -78°C); elem. anal.;	A 71% B 1%

Ni[η(1),η(2)-C5H5C2(CO2Me)2]Cp → nickel (7440-02-0) + cyclopenta-1,3-diene (542-92-7)

Conditions	Yield
With hydrogen In ethanol byproducts: C7H9(C(O)OCH3); room temp.; normal pressure;	A n/a B 70%
With H2; catalyst: Pt In ethanol byproducts: C7H9(C(O)OCH3); room temp.; normal pressure;	A n/a B 70%
With hydrogen In ethanol byproducts: C7H9(C(O)OCH3); room temp.; normal pressure;	A n/a B 70%

bis(4-acetyl-1-ethyl-3-methyl-5-pyrazolonato)nickel(II) → formaldehyd (50-00-0) + C3N2(CH3)(C2H5)(OH)C(O)CH3 + nickel (7440-02-0)

Conditions	Yield
With methanol; benzophenone In neat (no solvent) Kinetics; Irradiation (UV/VIS); photolysis (mercury lamp, 300 nm lamps, merry-go-round unit), irradn. under N2 through a pyrex filter; centrifugation, filtration through a pipette (Celite), detd. by UV;	A 56% B 68% C n/a

nickel(II) sulphate → nickel (7440-02-0)

Conditions	Yield
With Na3C6H5O7*2H2O In water Electrolysis; Ni(II):Cit=1:1, potentiostatic condditions, -1.1 V vs. SHE, Ag/AgCl immersed in 3.3 M KCl used as reference, Cu plate as working, Pt sheet as counter electrodes; soln. stirred at 500 rpm with magnet; temp. 298 K; X-ray fluorometry;	65%
With Na or K or Ca or Ba hypophosphite; Na acetate or Na formate In not given 90-92°C , pH=5.0-6.5;
Electrolysis; form of product is powder;

bis(acetylacetonate)nickel(II) → nickel (7440-02-0) + nickel(0)(1,5-cyclooctadiene)2

Conditions	Yield
With n-hexyllithium In toluene byproducts: n-hexane, hex-1-en, LiH; under Ar, reduction at room temp. with n-hexyllithium in presence of cyclooctadiene (Li:Ni=4); further byproduct: Ph-Ph, hex-Ph, cycloocta-1,3-diene, cycloocta-1,4-diene, cyclooctene; protolysis of liquid phase with MeOH (H2), gas chromy. of volatile compds.;	A n/a B 65%

dodecacarbonyl triosmium (15696-40-9) + [Ni(cyclopentadienyl)(μ-CO)]2 → (C5H5)3Ni3Os3(CO)9 + (η5-C5H5)NiOs3(μ-H)3(CO)9 + nickel (7440-02-0)

Conditions	Yield
With hydrogen In octane Os3(CO)12 refluxed in octane with (CpNi(CO))2 for 30 min under H2 flow,cooled; filtered, evapd. in vac., purified by TLC (Kiselgel PF Merck, light petroleum-Et2O), crystd. from CHCl3/heptane at -10°C; elem. anal.;	A 10% B 60% C n/a

magnesium-1,3-butadiene * 2 THF + ((CH3)2C2N2(C6H3(CH3)2)2)NiClBr → bisacetylbis(2,6-dimethylphenylimin)(1,3-butadiene)nickel (129616-15-5) + Ni(1,4-bis(2,6-dimethylphenyl)-2,3-dimethyl-1,4-diazabuta-1,3-diene)2 (74779-91-2) + nickel (7440-02-0)

Conditions	Yield
In tetrahydrofuran (N2), dry solvents; addn. of Mg compd. to suspn. of Ni compd. in THF room temperature, stirring overnight;	A 40% B 60% C n/a

2,3,5,6-tetrafluorobenzaldehyde (19842-76-3) + nickel (7440-02-0) + 1,2-dichloro-benzene (95-50-1) → (2,3,5,6-tetrafluorophenyl)methanol (4084-38-2)

Conditions	Yield
	100%

1,4-dioxane (123-91-1) + nickel (7440-02-0) + 1,2-dichloro-benzene (95-50-1) + 2,3,5,6-tetrafluoroterephthalaldehyde (3217-47-8) → 2,3,5,6-tetrafluoro-1,4-benzenedimethanol (92339-07-6)

Conditions	Yield
	100%

nickel (7440-02-0) + phthalonitrile (91-15-6) → nickel(II) phthalocyanine (14055-02-8)

Conditions	Yield
With sodium methylate In methanol pyrophoric Ni under water layer added to a methanol soln. containing an equivalent quantity of phthalonitrile and 5 drops of 30% soln of CH3ONa in methanol; flask maintained at 25°C for 24-72 h; blue product separated from unreacted metal by shaking and decanting with the solvent, washed with ethanol in Soxhlet equipment and dried in air; purity of 95-97%; elem. anal.;	100%
With sodium methylate In methanol; water pyrophoric metal:phthalonitrile=1:4 and few drops of CH3ONa under water layer treated for 24 h at 25°C; septd., washed (ethanol), dried in air, elem. anal.;	100%
With sodium methylate In ethanol pyrophoric Ni under water layer added to an ethanol soln. containing an equivalent quantity of phthalonitrile and 5 drops of 30% soln of CH3ONa in methanol; flask maintained at 25°C for 24-72 h; blue product separated from unreacted metal by shaking and decanting with the solvent, washed with ethanol in Soxhlet equipment and dried in air; purity of 95-97%; elem. anal.;	100%

triphenylphosphine diiodide (6396-07-2) + nickel (7440-02-0) → {(C6H5)3PI}(1+)*{Ni(P(C6H5)3)I3}(1-)={(C6H5)3PI}{Ni(P(C6H5)3)I3} (152442-02-9)

Conditions	Yield
In diethyl ether under N2: dissoln. of (C6H5)3PI2 (2 equivalents) in dry diethyl ether in a rotoflow tube; addn. of coarse-grain unactivated Ni, 60°C; stirring, 7d;; isolation by standard Schlenk technique; drying in vac.; elem. anal.;	100%

diiodo tri-n-butylphosphorane (21473-75-6) + nickel (7440-02-0) → {(C4H9)3PI}(1+)*{Ni(P(C4H9)3)I3}(1-)={(C4H9)3PI}{Ni(P(C4H9)3)I3} (152386-23-7)

Conditions	Yield
In diethyl ether under N2: dissoln. of (C4H9)3PI2 (2 equivalents) in dry diethyl ether in a rotoflow tube; addn. of coarse-grain unactivated Ni, 60°C; stirring, 7d;; isolation by standard Schlenk technique; drying in vac.; elem. anal.;	100%

diiodotriethylphosphorane (98961-77-4) + nickel (7440-02-0) → {(C2H5)3PI}(1+)*{Ni(P(C2H5)3)I3}(1-)={(C2H5)3PI}{Ni(P(C2H5)3)I3} (152386-25-9)

Conditions	Yield
In diethyl ether under N2: dissoln. of (C2H5)3PI2 (2 equivalents) in dry diethyl ether in a rotoflow tube; addn. of coarse-grain unactivated Ni, 60°C; stirring, 7d;; isolation by standard Schlenk technique; drying in vac.; elem. anal.;	100%

antimony (7440-36-0) + zirconium (7440-67-7) + nickel (7440-02-0) → ZrNiSb

Conditions	Yield
In neat (no solvent) Electric Arc; heating (650°C, 4 d; dynamic Ar atm., arc melting), annealing (5 h, 1050-1200°C);	100%
In neat (no solvent) vac. (5E-3 mbar); stoichiometric ratio, heating (1 week, 1100°C);
In melt Electric Arc; arc melted under Ar gettered with Ti; 5 wt.-% of Sb required to compensate evaporative losses during arc-melting; ingots sealed in evacuated fused-silica tubes and annealed at 870 K for 720 h; quenched in cold water; XRD; EDX;

tin (7440-31-5) + nickel (7440-02-0) + sulfur (7704-34-9) + 1,2-diaminopropan (78-90-0, 10424-38-1) → [Ni(1,2-diaminopropane)3]2Sn2S6*2H2O

Conditions	Yield
In further solvent(s) High Pressure; prepd. under solvothermal conditions; reactants weighted in ratio of 1 Ni:1 Sn:3 S, heated in sealed Teflon-lined steel autoclave in pure 1,2-diaminopropane for 7 d at 140°C; elem. anal.;	100%

P(CH2CH2C6H5)3I2 (149683-89-6) + nickel (7440-02-0) → {(C6H5CH2CH2)3PI}(1+)*{Ni(P(C6H5CH2CH2)3)I3}(1-)={(C6H5CH2CH2)3PI}{Ni(P(C6H5CH2CH2)3)I3} (152386-19-1)

Conditions	Yield
In diethyl ether under N2: dissoln. of (C6H5CH2CH2)3PI2 (2 equivalents) in dry diethyl ether in a rotoflow tube; addn. of coarse-grain unactivated Ni, 60°C; stirring, 7d;; isolation by standard Schlenk technique; drying in vac.; elem. anal.;	100%

(C2H5)2(CH3)PI2 (147274-44-0) + nickel (7440-02-0) → {(C2H5)2(CH3)PI}(1+)*{Ni(P(C2H5)2(CH3))I3}(1-)={(C2H5)2(CH3)PI}{Ni(P(C2H5)2(CH3))I3} (152386-28-2)

Conditions	Yield
In diethyl ether under N2: dissoln. of (C2H5)2(CH3)PI2 (2 equivalents) in dry diethyl ether in a rotoflow tube; addn. of coarse-grain unactivated Ni, 60°C; stirring, 7d;; isolation by standard Schlenk technique; drying in vac.; elem. anal.;	100%

nickel (7440-02-0) + tris(dimethylamino)diiodophosphorane (82859-40-3) → {((CH3)2N)3PI}(1+)*{Ni(P(N(CH3)2)3)I3}(1-)={((CH3)2N)3PI}{Ni(P(N(CH3)2)3)I3} (152386-30-6)

Conditions	Yield
In diethyl ether under N2: dissoln. of (N(CH3)2)3PI2 (2 equivalents) in dry diethyl ether in a rotoflow tube; addn. of coarse-grain unactivated Ni, 60°C; stirring, 7d;; isolation by standard Schlenk technique; drying in vac.; elem. anal.;	100%

hafnium + antimony (7440-36-0) + nickel (7440-02-0) → HfNiSb

Conditions	Yield
In neat (no solvent) Electric Arc; heating (650°C, 4 d; dynamic Ar atm., arc melting);	100%
In neat (no solvent) Electric Arc; repeated remelting, annealing in evac. quartz tube for 250 h at 800°C, quenching (cold water);

samarium (7440-19-9) + tin (7440-31-5) + nickel (7440-02-0) → Sm2NiSn4

Conditions	Yield
In neat (no solvent, solid phase) mixt. of Sm, Ni, Sn loaded into Ta tube, heated at 970°C for 36 h, quenched in water, annealed at 700°C for 15 d;	99%
In neat (no solvent, solid phase) mixt. of Sm, Ni, Sn loaded into Nb tube, heated under dynamic vac. at 300°C for 1 d, heated at 950°C for 5 d, cooled to room temp.at 15°C/h;

thiazolidine-2-one (2682-49-7) + nickel (7440-02-0) → Ni(C3NS2H4)2 (28872-21-1, 158907-11-0)

Conditions	Yield
In acetonitrile byproducts: H2; Electrochem. Process; electrolyse of a soln. of the ligand in acetonitrile (NH4BF4) with a Nianode at room temp. under N2; filtered, washed with acetonitrile, dried in vac.; elem. anal.;	99%

tellurium + sulfuryl dichloride (7791-25-5) + nickel (7440-02-0) + acetonitrile (75-05-8) → [Ni(NCCH3)6](2+)*[Te2Cl10](2-) = [Ni(NCCH3)6][Te2Cl10] (368867-42-9)

Conditions	Yield
In acetonitrile under dry Ar; Ni and Te mixed in CH3CN; SO2Cl2 added; stirred (2 h); evapd. to dryness (vac.); recrystd. from CH3CN (room temp.); elem. anal.;	99%

nickel (7440-02-0) + trimethylarsine diiodide (17756-08-0) → [NiI3(As(CH3)3)2] (174094-63-4)

Conditions	Yield
In diethyl ether byproducts: I2; (N2); 60°C, ca. 4 d; drying (vac.), recrystn. (Et2O); elem. anal.;	99%

tellurium + sulfur dioxide (7446-09-5) + arsenic pentafluoride (7784-36-3) + nickel (7440-02-0) → [Ni(SO2)6](2+)*Te6(4+)*6AsF6(1-)=[Ni(SO2)6][Te6][AsF6]6

Conditions	Yield
In neat (no solvent) byproducts: AsF3; all manipulations under Ar atm.; SO2 and AsF5 condensed on Ni and Te (external cooling bath of liq. N2), stirred for 5 h; SO2 distd. slowly;	99%

(2S)-2-[1-(diethoxymethyl)cyclopropyl]-2-{[(1S)-1-phenylethyl]amino}acetonitrile (400709-89-9) + nickel (7440-02-0) → N-{2-amino-(1S)-1-[1-(diethoxymethyl)cyclopropyl]ethyl}-N-[(1S)-1-phenylethyl]amine

Conditions	Yield
With sodium hydroxide In ethanol; chloroform; water; hydrogen	98.4%

3,5-dimethyl-1-(carbethoxymethylene)cyclohexane (85120-26-9) + nickel (7440-02-0) → (3,5-dimethyl-cyclohexyl)-acetic acid ethyl ester (85120-28-1)

Conditions	Yield
In methanol	98%

Octanoic acid (124-07-2) + nickel (7440-02-0) → nickel(II) bis(octanoate)

Conditions	Yield
In acetonitrile Electrolysis; 4 h, initial voltage 30 V; washed with acetonitrile and dried in vacuo for 3-4 h at room temp.;elem.anal;	98%
With tetrabutyl-ammonium chloride In acetonitrile for 8h; Electrolysis;

nickel (7440-02-0) + 2-Mercaptobenzothiazole (149-30-4) → bis-[2-mercaptobenzothiazolatonickel(II)] (77321-77-8, 119203-46-2)

Conditions	Yield
In acetonitrile byproducts: H2; Electrochem. Process; electrolyse of a soln. of the ligand in acetonitrile (NH4BF4) with a Nianode at room temp. under N2; filtered, washed with acetonitrile, dried in vac.; elem. anal.;	98%

Upstream product

• 1313-99-1 nickel(II) oxide 
• 10039-56-2 sodium hypophosphite 
• 373-02-4 nickel diacetate 
• 14701-22-5 nickel(II) 
• 719261-06-0 nickel(II) carbonate 
• 83864-14-6 nickel dichloride 
• 7732-18-5 water 
• 13462-88-9 nickel dibromide 
• 12255-80-0 nickel arsenide 

Downstream Products

• 151450-18-9 3-cyclopentyloxy-4-methoxy-benzylamine 
• 433977-33-4 2-(3-Aminophenoxy)-N-(3,5-dichlorophenyl)acetamide 
• 68-94-0 1,7-dihydro-6H-purin-6-one 
• 4084-38-2 (2,3,5,6-tetrafluorophenyl)methanol 
• 3217-47-8 2,3,5,6-tetrafluoroterephthalaldehyde 
• 92339-07-6 2,3,5,6-tetrafluoro-1,4-benzenedimethanol 
• 1709-52-0 N-methyl-4-aminobenzenesulfonamide 
• 34155-39-0 2-methyl-1-(pyrrolidin-1-yl)propan-2-amine 
• 101952-26-5 5-(2-methoxy-benzyl)-imidazolidine-2,4-dione 
• 6318-42-9 5-(4-methoxy-benzyl)-hydantoin 
• 51221-36-4 5-(3,4,5-trimethoxy-benzyl)-imidazolidine-2,4-dione 
• 62285-98-7 5-(2,6,6-trimethylcyclohexenyl)-3-methyl-2,4-pentadienyltriphenylphosphonium bromide 
• 110225-00-8 2-hexyl-1-dodecanol 
• 5333-42-6 2-octyldodecan-1-ol 

Relevant articles and documents

Kinetic regularities of the chemical vapor deposition of nickel layers from bis-(ethylcyclopentadienyl)nickel

Physicochemical regularities of the nickel layers chemical vapor deposition from bis-(ethylcyclopentadienyl)nickel were studied. Dependences of the growth rate of nickel layers on the deposition temperature, gas-fl ow linear rate, partial pressures of reagents, and substrate roughness, and also dependences of the thickness of a grown layer on time and on the position of a substrate on a susceptor were obtained.

Magnetic properties of nanometric nickel particles

We have prepared nickel metal fine particles with mean diameters as low as 4 nanometers and we have studied their magnetic properties. A superparamagnetic behaviour is found for the smallest particles even at helium temperature.

Supercapacitor electrodes with high-energy and power densities prepared from monolithic NiO/Ni nanocomposites

Impressive energy storage and delivery: A simple, cost-effective, and potentially scalable technique is described for fabricating support- and additive-free NiO/Ni nanocomposite electrodes (see picture) for electrochemical supercapacitors. Maximum performances of energy storage and delivery were simultaneously achieved by developing a slow-charging and fast-discharging procedure. Copyright

Effect of nickel precursors on the performance of Ni/AlMCM-41 catalysts for n-dodecane hydroconversion

The bifunctional Ni/AlMCM-41 catalysts with 2.0 wt.% nickel loading were prepared by means of the wetness impregnation technique using three nickel precursors: nickel nitrate, alkaline tetraamine nickel nitrate and nickel citrate. The texture, crystal pha

Fabrication and magnetic properties of nickel dodecahedra

Here we report a one-pot route for the synthesis of nickel dodecahedra with 52.3 ± 0.1 emu g-1 of saturation magnetization. The procedure is very simple, and only three chemicals (NiCl2·6H 2O, isopropanol and polyvinylpyrrolidone) are used throughout the entire synthetic process. During the reaction, it is believed that the application of isopropanol and the amount of polyvinylpyrrolidone play an essential role in forming the dodecahedral morphology of the final product. Furthermore, a formation process of twinning and the influence of reaction kinetic factors were proposed to explain the formation of nickel dodecahedra.

One-step synthesis of carbon nanotubes with Ni nanoparticles as a catalyst by the microwave-assisted polyol method

Carbon nanotubes (CNTs) were firstly synthesized by the microwave-assisted polyol method and magnetic Ni nanoparticles were employed as a catalyst in the process. The structures, morphologies and magnetic properties of the as-synthesized samples were investigated by using X-ray diffraction (XRD), transmission electron microscopy (TEM) and vibrating sample magnetometer (VSM), respectively. Our results indicated that CNTs can be synthesized after the observation of a small electric spark with Ni particles used as a catalyst. TEM showed that the length of the hollow carbon nanotubes was of the order of micron. VSM demonstrated that Ni/CNTs composite was ferromagnetic characteristic with hysteretic behavior at room temperature.

Cyclic voltammetry study of the NiP electrodeposition

Cyclic voltammetry was used to investigate the deposition mechanism of NiP amorphous alloys. Whatever the cathodic potential for the deposition, the anodic going scan presents two well-formed anodic peaks preceded by a small current plateau. The two peaks are related to two alloys of different phosphorus content, and therefore in two different structural states. The formation of the first peak is controlled by a very slow kinetic process.

Comparison of the magnetic properties of metastable hexagonal close-packed Ni nanoparticles with those of the stable face-centered cubic Ni nanoparticles

We report the first magnetic study of pure and metastable hexagonal close-packed (hep) Ni nanoparticles (sample 1). We also produced stable face-centered cubic (fcc) Ni nanoparticles, as mixtures with the hcp Ni nanoparticles (samples 2 and 3). We compared the magnetic properties of the hcp Ni nanoparticles with those of the fcc Ni nanoparticles by observing the evolution of magnetic properties from those of the hcp Ni nanoparticles to those of the fcc Ni nanoparticles as the number of fcc Ni nanoparticles increased from sample 1 to sample 3. The blocking temperature (TB) of the hcp Ni nanoparticles is ～12 K for particle diameters ranging between 8.5 and 18 nm, whereas those of the fcc Ni nanoparticles are 250 and 270 K for average particle diameters of 18 and 26 nm, respectively. The hcp Ni nanoparticles seem to be antiferromagnetic for T B and paramagnetic for T > TB. This is very different from the fcc Ni nanoparticles, which are ferromagnetic for T B and superparamagnetic for T > T B. This unusual magnetic state of the metastable hcp Ni nanoparticles is likely related to their increased bond distance (2.665 A), compared to that (2.499 A) of the stable fcc Ni nanoparticles.

Enhanced electrochemical performance of nanoplate nickel cobaltite (NiCo2O4) supercapacitor applications

Well-ordered, unique interconnected nanostructured binary metal oxides with lightweight, free-standing, and highly flexible nickel foam substrate electrodes have attracted tremendous research attention for high performance supercapacitor applications owing to the combination of the improved electrical conductivity and highly efficient electron and ion transport channels. In this study, a unique interconnected nanoplate-like nickel cobaltite (NiCo2O4) nanostructure was synthesized on highly conductive nickel foam and its use as a binder-free material in energy storage applications was assessed. The nanoplate-like NiCo2O4 nanostructure electrode was prepared by a simple chemical bath deposition method under optimized conditions. The NiCo2O4 electrode delivered an outstanding specific capacitance of 2791 F g?1 at a current density of 5 A g?1 in a KOH electrolyte in a three-electrode system as well as outstanding cycling stability with 99.1% retention after 3000 cycles at a current density of 7 A g?1. The as-synthesized NiCo2O4 electrode had a maximum energy density of 63.8 W h kg?1 and exhibited an outstanding high power density of approximately 654 W h kg?1. This paper reports a simple and cost-effective process for the synthesis of flexible high performance devices that may inspire new ideas for energy storage applications.

Magnetic field effects in electrochemical reactions

The influence of an external magnetic field B on the electrochemical behaviour of the systems Cu2+/Cu, Ni2+/Ni, and [IrCl 6]2-/[IrCl6]3- has been studied. In the case of Cu depositions in an electrochemical cell with a large ratio of the electrode area and the cell volume the increase of the limiting current density with B can be explained with the interplay of natural convection and the Lorentz force acting on the resulting flow profile (magneto hydrodynamic or MHD effect). Ni depositions also show an MHD effect as well as a tendency to form more fine grained material in the presence of a magnetic field. The results on the homogeneous redox system [IrCl6]2-/[IrCl 6]3- at 50μm diameter micro electrodes are in qualitative agreement with recently proposed relationships to describe the influence of a B field on the limiting current density.

Electrocodeposition of nickel nanocomposites using an impinging jet electrode

The electrocodeposition of nickel alumina nanocomposites was investigated using an impinging jet electrode. The effects of jet flow rate, particle loading, and current density on the particle incorporation were studied. The amount of codeposited particles was determined using both electrogravimetric measurements and energy dispersive X-ray analysis. A maximum particle incorporation of about 5 wt % was found for a flow rate of 2.5 L min-1 and a current density of 10 A dm-2. The microstructure of the coatings was investigated via X-ray diffraction. As a result of increasing current density and particle incorporation, a loss of (100) texture and a relative enhancement of the (111), (220), and (311) reflections appeared. The microhardness of the nickel films increased significantly with the inclusion of alumina nanoparticles.

Magnetophoresis behaviour at low gradient magnetic field and size control of nickel single core nanobeads

Magnetic separation of organic compounds, proteins, nucleic acids and other biomolecules, and cells from complex reaction mixtures is becoming the most suitable solution for large production in bioindustrial purification and extraction processes. Optimal magnetic properties can be achieved by the use of metals. However, they are extremely sensitive to oxidation and degradation under atmospheric conditions. In this work Ni nanoparticles are synthesised by conventional solution reduction process with the addition of a non-ionic surfactant as a surface agent. The nanoparticles were surfacted in citric acid and then coated with silica to form single core Ni nanobeads. A magnetophoresis study at different magnetic field gradients and at the different steps of synthesis route was performed using Horizontal Low Gradient Magnetic Field (HLGMF) systems. The reversible aggregation times are reduced to a few seconds, allowing a very fast separation process.

Aqueous solutions of colloidal nickel: Radiation-chemical preparation, absorption spectra, and properties

Radiation-chemical reduction of Ni2+ ions in aqueous solutions of Ni(ClO4)2 containing sodium formate or isopropyl alcohol was studied, γ-Irradiation of deaerated solutions in the presence of polyethyleneimine, polyacrylate, or polyvinyl sulfate gives stable metal sols containing spherical particles 2-4 nm in diameter. The optical absorption spectra of nickel nanoparticles exhibit a band with a maximum at 215±5 nm (ε215 = 4.7 · 103 L mol-1 cm-1) and a shoulder at 350 nm. A mechanism for the radiation-chemical reduction of Ni2+ ions by hydrated electrons and organic radicals (CO2- radical anions in the case of HCOONa and Me2COH radicals in the case of Pr1OH). The redox potentials of the Ni2+/Ni0 and Ni+/Ni0 pairs (Ni0 is a nickel atom) are approximately -2.2 and -1.7 V, respectively. The nanoparticles are readily oxidized by O2, H2O2, and other oxidants. The reactions of these species with silver ions yield relatively stable nanoaggregates containing both nickel and silver in addition to silver nanoparticles.

Amperometric detection of hydrogen peroxide at nano-nickel oxide/thionine and celestine blue nanocomposite-modified glassy carbon electrodes

A simple procedure was developed to prepare a glassy carbon (GC) electrode modified with nickel oxide (NiOx) nanoparticles and water-soluble dyes. By immersing the GC/NiOx modified electrode into thionine (TH) or celestine blue (CB) solutions for a short

SURFACE STATE,CATALYTIC ACTIVITY AND SELECTIVITY OF NICKEL CATALYSTS IN HYDROGENATION REACTIONS

The X-ray photoelectron spectroscopic study of Raney and Urushibara nickel catalysts activatede under various conditions was undertaken to chyrycterize the surface state of the catalysts including thecatalists' structure.Raney nickel catalysts contain both oxidized and metallic aluminium in the activated phase.As for Urushibara nickel catalystsdigested with acetic acid or sodium hydroxide, metallic and oxidized zinc were observed in the catalysts surface.Based on the X.p.s. peak intensities for the catalysts, the structure of Urushibara nickel catalysts was found to be that of a supported catalysts, whereas Raney nickel catalysts showed X.p.s. features consistent with those expected for skeletal nickel catalysts.

Ammonia-assisted fabrication of flowery nanostructures of metallic nickel assembled from hexagonal platelets

A simple one-pot solution method was reported for the synthesis of metallic nickel nanostructures assembled from hexagonal nanoplatelets. The process involved the reduction of nickelous salt with hydrazine in ammonia solution, and the reaction proceeded w

Fabrication of Ni-coated Al2O3 powders by the heterogeneous precipitation method

Ni-coated Al2O3 powders were prepared by the heterogeneous precipitation method using Al2O3, Ni(NO3)2·6H2O and NH4HCO3 as the starting materials. The amorphous NiCO3·2Ni(OH)2·2H2O was uniformly coated on the surface of Al2O3 particles with the thickness of 20 nm. The amorphous coating layer was crystallized to NiO with the size of about 15 nm at 500°C for 2 hours in air, meantime, the dispersant was eliminated. NiO was completely reduced to Ni at 700°C for 4 hours in hydrogen atmosphere. Ni with the size of about 20 nm in the coating layer was spherical and weakly agglomerated. The continuous coating layer became discontinuous during heating treatment.

Electrooxidation of methanol on NiMn alloy modified graphite electrode

Nickel and nickel-manganese alloy modified graphite electrodes (G/Ni and G/NiMn) prepared by galvanostatic deposition were examined for their redox process and electrocatalytic activities towards the oxidation of methanol in alkaline solutions. The methods of cyclic voltammetery (CV), chronoamperometry (CA) and impedance spectroscopy (EIS) were employed. In CV studies, in the presence of methanol NiMn alloy modified electrode shows a significantly higher response for methanol oxidation. The peak current of the oxidation of nickel hydroxide increase is followed by a decrease in the corresponding cathodic current in presence of methanol. The anodic peak currents show linear dependency upon the square root of scan rate. This behavior is the characteristic of a diffusion controlled process. Under the CA regime the reaction followed a Cottrellian behavior and the diffusion coefficient of methanol was found to be 4 × 10-6 cm2 s-1. A mechanism based on the electro-chemical generation of Ni3+ active sites and their subsequent consumptions by methanol have been discussed and the corresponding rate law under the control of charge transfer has been developed and kinetic parameters have been derived. The charge transfer resistance accessible both theoretically and through the EIS have been used as criteria for derivation of the rate constant.

Polar symmetry and intercalation of new multilayered hybrid molybdates: [M2(pzc)2(H2O)x][Mo 5O16] (M = Co, Ni)

The layered molybdate [M2(pzc)2(H2O) x][Mo5O16] (I: M = Ni, x = 5.0; II: M = Co, x = 4.0; pzc = pyrazinecarboxylate) hybrid solids were synthesized via hydrothermal reactions at 160-165°C. The structures were determined by single-crystal X-ray diffraction data for I (Cc, Z = 4; a = 33.217(4) A, b = 5.6416(8) A, c = 13.982(2) A, β = 99.407(8)°, and V = 2585.0(6) A3) and powder X-ray diffraction data for II (C2/c, Z = 4; a = 35.42(6) A, b = 5.697(9) A, c = 14.28(2) A, β = 114.95(4)°, and V = 2614(12) A3). The polar structure of I contains new [Ni2(pzc)2(H2O)5] 2+ double layers that form an asymmetric pattern of hydrogen bonds and covalent bonds to stair-stepped [Mo5O16]2- sheets, inducing a net dipole moment in the latter. In II, however, the [Co 2(pzc)2(H2O)4]2+ double layers have one less coordinated water and subsequently exhibit a symmetric pattern of covalent and hydrogen bonding to the [Mo5O 16]2- sheets, leading to a centrosymmetric structure. Thermogravimetric analyses and powder X-ray diffraction data reveal that I can be dehydrated and rehydrated with from 0 to 6.5 water molecules per formula unit, which is coupled with a corresponding contraction/expansion of the interlayer distances. Also, the dehydrated form of I can be intercalated by ～4.3 H2S molecules per formula unit, but the intercalation by pyridine or methanol is limited to less than one molecule per formula unit.

Alkalization of the near-cathode layer in electrodeposition of nickel from a chloride electrode

Dependences of the pH at which hydrate formation begins and the pH of the near-cathode layer on the electrolysis modes (temperature, cathode current density, pH in the electrolyte bulk) and the dependence of the pH of the near-cathode layer on the distance from the cathode surface in a low-concentration chloride nickelplating electrolyte were studied. Pleiades Publishing, Ltd., 2010.

Hydrangea-like NiCo-based Bimetal-organic Frameworks, and their Pros and Cons as Supercapacitor Electrode Materials in Aqueous Electrolytes

Hydrangea-like NiCo-based bimetal-organic frameworks (NiCo-MOF) are synthesized in DMF-EtOH solution via a solvothermal method, using 4,4′-biphenyldicarboxylic acid as a ligand. NiCo-MOF having a highest capacity of 1056.6 F·g–1 at 0.5 A·g–1 and 457.7 F·g–1 even at 10 A·g–1 is achieved at a Ni/Co/BPDC molar ratio of 1:1:1, a temperature of 170 °C and a reaction time of 12 hours. It exhibits secondary 3D microsphere structures assembled by primary 2D nanosheet structures, good crystalline structure and good thermal stability below 350 °C in air. All the electrochemical data show that NiCo-MOF has the pros and cons as supercapacitor electrode materials in aqueous electrolytes. On the one hand, NiCo-MOF has a high capacity even at a high current density, low internal resistance, charge-transfer resistance and ion diffusion impendence, owing to the ordered coordination structure, 2D nanosheet structure and 3D assembled microsphere structure of NiCo-MOF. On the other hand, the cycling stability and rate capability are not ideal enough due to the hydrolysis of coordination bonds in aqueous electrolytes, especially, in alkaline solution. The good dispersion and high electrochemical activity of metal ions bring a high capacity for NiCo-MOF, but they result in the poor stability of NiCo-MOF. In the future work, finding a suitable organic electrolyte is an effective way to enhance the cycling stability of NiCo-MOF as well as deriving more stable skeleton materials from NiCo-MOF.

Magnetic nanochains of metal formed by assembly of small nanoparticles

Ni nanochains are synthesized with diameters of 150-250 nm and lengths of 0.5-2 μm by assembly of small nanoparticles, which exhibit a magnetic coercivity over two orders of magnitude larger than that of bulk Ni.

Theoretical and Experimental Evaluation of the Reduction Potential of Straight-Chain Alcohols for the Designed Synthesis of Bimetallic Nanostructures

Recently, the development of bimetallic nanoparticles with functional properties has been attempted extensively but with limited control over their morphological and structural properties. The reason was the inability to control the kinetics of the reduction reaction in most liquid-phase syntheses. However, the alcohol reduction technique has demonstrated the possibility of controlling the reduction reaction and facilitating the incorporation of other phenomena such as diffusion, etching, and galvanic replacement during nanostructure synthesis. In this study, the reduction potential of straight-chain alcohols has been investigated using molecular orbital calculations and experimentally verified by reducing transition metals. The alcohols with a longer chain exhibited higher reduction potential, and 1-octanol was found to be the strongest among alcohols considered. Furthermore, the experimental evaluation carried out via the synthesis of metallic Cu, Ni, and Co particles was consistent with the theoretical predictions. The reaction mechanism of metallic particle formation was also studied in detail in the Ni-1-octanol system, and the metal ions were confirmed to be reduced via the formation of nickel alkoxide. The results of this investigation were successfully implemented to synthesize Cu-Ni bimetallic nanostructures (core-shell, wire, and tube) via the incorporation of diffusion and etching besides the reduction reaction. These results suggest that the designed synthesis of a wide range of bimetallic nanostructures with more refined control has become possible.

Morphology-control and template-free fabrication of bimetallic Cu–Ni alloy rods for ethanol electro-oxidation in alkaline media

The design of highly efficient and stable non-noble transition metal-based electrocatalysts for the ethanol oxidation reaction (EOR) is imperative for the development of the direct ethanol fuel cells (DEFCs). In this work, we report a simple template-free method for preparing a type of rod-like Cu–Ni alloy particle with the unique porous structure and evaluate it as the electrocatalyst for the EOR in alkaline media. The pH, which was adjusted by the addition of NH3·H2O during the liquid-phase coprecipitation process, was found to be a key factor to shape Cu–Ni alloy precursor into a quasi-one-dimensional morphology. After annealing at a reducing atmosphere (H2/Ar = 5/95, v/v), well-alloyed Cu–Ni rods with the predefined molar ratio (Cu/Ni) of 1:1, a specific surface area of 6.84 m2 g?1, and the average pore size of 30.97 nm were obtained. Cyclic voltammetry (CV) and chronoamperometry (CA) test results show that the prepared Cu–Ni alloy catalyst demonstrated an anodic current peak of 86.10 mA cm?2 in the presence of 0.2 M ethanol and a 95% retention of current density after 2000 s, indicating its good electrochemical performance in terms of catalytical activity and long-term stability. This bottom-up synthesis strategy would enrich the fabrication methodologies and open up a promising avenue for preparing multiple Ni-based EOR electrocatalysts with the easy-controllable morphologies and porous structure at the industrial scale.

Self-assembled Ni/NiO impregnated polyaniline nanoarchitectures: A robust bifunctional catalyst for nitrophenol reduction and epinephrine detection

It is extremely significant to address an urgency toward the development of low-cost and efficient catalysts. Herein, for the first time, we synthesize a novel self-assembled Ni/NiO@PANI by a combustible crystallization followed polymerization method, constructed by impregnation of Ni/NiO in sulfonic acid-doped polyaniline, which can be used as a bifunctional catalyst for electrochemical sensing of epinephrine (EP) and reduction of nitro- to amino-phenol (4-NP to 4-AP). Due to the unique nanoarchitecture, ferromagnetic feature of Ni, anti-corrosion feature of PANI, and synergy between the system (metal/metaloxide@carbon) leads superior performance: it can rapidly reduce the 4-NP pollutant to environmentally friendly 4-AP within 8 min, and easy magnetic recycling; Also, it can be used as a sensor for EP neurotransmitters with a sensitivity, detection, and quantification limit of 0.117 nAμM?1, 87.2, and 290.71 μM, respectively. This work provides a strategy to design low-cost and superior catalysts applied in catalysis and electrochemical sensor.