Properties[change | change source]
Physical properties[change | change source]
Nickel is a silver-white metal. It is easily polished (made shiny). It is magnetic. It is not magnetic when heated above 355 °C (671 °F). It is not soft like many other metals. It can be stretched into wires easily. It is not radioactive.
Chemical properties[change | change source]
Chemical compounds[change | change source]
Nickel is found in two oxidation states: +2, nickel(II); and +3, nickel(III). Nickel(II) is more common. Nickel in its +2 oxidation state is green. Nickel(II) chloride is a common +2 oxidation state compound. Nickel(II) oxide is normally dark green, but sometimes it is gray. This is because some of the nickel is in the +3 oxidation state (nickel(III). Nickel(III) compounds are oxidizing agents. They also are grayish. Nickel compounds can be green, blue, gray, or black.
- Nickel(II) compounds
Nickel(II) compounds are not highly reactive. They are normally green or blue. They are toxic and irritate skin. Some of them are carcinogens.
- Nickel(II) carbonate, green
- Nickel(II) chloride, greenish
- Nickel(II) hydroxide, light green
- Nickel(II) nitrate, greenish
- Nickel(II) oxide, gray or light green
- Nickel(II) sulfate, blue-green
- Nickel(III) compounds
Nickel(III) compounds are black or gray.
Isotopes[change | change source]
History[change | change source]
Nickel was found when an ore that looked like copper did not make copper metal. Later it was found that the ore actually had a new metal, called nickel. Nickel was isolated as a metal and classified as a chemical element by Axel Fredrik Cronstedt in 1751. At first, the copper colored nickel ore was the only source. Later, it was made as a byproduct of cobalt blue making.
Occurrence[change | change source]
Nickel is normally found as a mineral, and not as a metal in the ground. Sometimes meteorites have nickel and iron metal in them. The most common nickel mineral is pentlandite. Most of the nickel on Earth is thought to be in the Earth's Earth's outer and inner cores. There are sulfidic and lateritic nickel ores. Philippines mines the most nickel. Other major mining countries are Russia, Canada and Australia. All the older rocks on Earth have some rare metals. They are got by mining where the ores are most plentiful.
Preparation[change | change source]
Nickel is found in both laterite and sulfide ores. They are heated to melt them and concentrate them. They are also separated by oils. Nickel is made from its sulfide by heating it in air. This oxidizes the sulfide to sulfur dioxide, leaving liquid nickel behind. This nickel is not yet pure and not ready for use.
Pure nickel with a nickel content greater than 99% is made in an electrolytic process. In this process, the nickel is dissolved in bath of sulfuric acid. When the pure nickel sticks to cathodes hanging into the bath, the impurities remain in the sulfuric acid or at the bottom of the bath. These impurities are very interesting, as they can contain precious metals.
Production[change | change source]
Nickel is got by mining: the ore is roasted and reduced. This gives a metal of over 75% purity. In many stainless steel applications, 75% pure nickel is usable.
Uses[change | change source]
Sixty-eight percent of all nickel produced is used to make stainless steel. Nickel is also used in nichrome, a name for a nickel-chromium alloy, and other alloys. Nickel is used in magnets. Nickel is used in special expensive alloys called superalloys.
Nickel sulphate is used in rechargeable batteries. A lithium ion battery contains up to 15% of nickel while the lithium content is less than 1%. A nickel cadmium battery also uses nickel. Nickel compounds are also used to electroplate nickel on items. Nickel and some of its compounds are also used as a catalyst. Nickel is used in stainless steel. It is also used in some nonferrous alloys. It is used in electroplating.
Nickel is used to make many products like stainless steel, alnico magnet, coinage, rechargeable batteries, electric guitar strings, microphone capsules and plating on plumbing fixtures. It is used as a green tint in glass.
63Ni is used in krytron devices as a beta particle emitter to make ionization by the keep-alive electrode more reliable. Raney nickel is used for hydrogenation of unsaturated oils to make margarine.
Safety[change | change source]
Nickel can irritate skin. That is why jewelry that releases nickel ions is bad for some people. Some nickel salts are carcinogens. Nickel is not as toxic as other metals such as mercury but it is still toxic.
References[change | change source]
- Audi, G.; Bersillon, O.; Blachot, J.; Wapstra, A.H. (2003). "The Nubase evaluation of nuclear and decay properties". Nuclear Physics A. 729 (1): 3–128. Bibcode:2003NuPhA.729....3A. doi:10.1016/j.nuclphysa.2003.11.001.
- "Fun facts about nickel element - Nickel Institute". www.nickelinstitute.org. Archived from the original on 2017-09-21. Retrieved 2020-09-29.
- University of California Libraries (1896). American plumbing practice. From the Engineering record (Prior to 1887 the sanitary engineer.) A selected reprint of articles describing notable plumbing installations in the United States, and questions and answers on problems arising in plumbing and house draining. With five hundred and thirty-six illustrations. New York, The Engineering record.
- Davis, J.R.; Joseph, R.; ASM International Handbook Committee (2000). Nickel, cobalt, and their alloys. Materials Park, OH: ASM International. ISBN 0-87170-685-7. OCLC 44613209.
- Kharton, Vladislav V. (2011). Solid state electrochemistry II:electrodes, interfaces and ceramic membranes. Weinheim: Wiley-VCH. ISBN 978-3-527-63558-0. OCLC 729731930.
- "Bidault PDF" (PDF). 2011-07-20. Archived from the original (PDF) on 2011-07-20. Retrieved 2020-09-29.
- Cheburaeva, R. F.; Chaporova, I. N.; Krasina, T. I. (1992). "Structure and properties of tungsten carbide hard alloys with an alloyed nickel binder". Soviet Powder Metallurgy and Metal Ceramics. 31 (5): 423–425. doi:10.1007/BF00796252. ISSN 0038-5735. S2CID 135714029.
- "Silicon Investigations Krytron Pulse Power Switch Page". 2011-07-16. Archived from the original on 2011-07-16. Retrieved 2020-09-30.
Related pages[change | change source]