Nickel(II) hydroxide (original) (raw)

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Nickel(II) hydroxide

Nickel(II) hydroxide
Nickel(II) hydroxide
Names
IUPAC name Nickel(II) hydroxide
Other namesNickel hydroxide, Theophrastite
Identifiers
CAS Number 12054-48-7 checkY36897-37-7 (monohydrate) ☒N
3D model (JSmol) Interactive image
ChemSpider 55452 checkY
ECHA InfoCard 100.031.813 Edit this at Wikidata
EC Number 235-008-5
PubChem CID 61534
RTECS number QR648000
UNII L8UW92NW6J checkY
CompTox Dashboard (EPA) DTXSID90274011 Edit this at Wikidata
InChI InChI=1S/Ni.2H2O/h;2*1H2/q+2;;/p-2 checkYKey: BFDHFSHZJLFAMC-UHFFFAOYSA-L checkYInChI=1/Ni.2H2O/h;2*1H2/q+2;;/p-2Key: BFDHFSHZJLFAMC-NUQVWONBAJ
SMILES [Ni+2].[OH-].[OH-]
Properties
Chemical formula Ni(OH)2
Molar mass 92.724 g/mol (anhydrous) 110.72 g/mol (monohydrate)
Appearance green crystals
Density 4.10 g/cm3
Melting point 230 °C (446 °F; 503 K) (anhydrous, decomposes)
Solubility in water 0.0015 g/L[1]
Solubility product (_K_sp) 5.48×10−16[2]
Magnetic susceptibility (χ) +4500.0·10−6 cm3/mol
Structure[3]
Crystal structure hexagonal, hP3
Space group P3m1, No. 164
Lattice constant a = 0.3117 nm, b = 0.3117 nm, c = 0.4595 nmα = 90°, β = 90°, γ = 120°
Thermochemistry
Std molar entropy (_S_⦵298) 79 J·mol−1·K−1[4]
Std enthalpy of formation (Δf_H_⦵298) −538 kJ·mol−1[4]
Hazards
GHS labelling:[5]
Pictograms GHS07: Exclamation markGHS08: Health hazard
Signal word Danger
Hazard statements H302, H315, H317, H332, H334, H341, H350, H360, H372
Precautionary statements P201, P260, P280, P284, P405, P501
Lethal dose or concentration (LD, LC):
LD50 (median dose) 1515 mg/kg (oral, rat)
Safety data sheet (SDS) External SDS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). ☒N verify (what is checkY☒N ?) Infobox references

Chemical compound

The test tube in the middle contains a precipitate of nickel(II) hydroxide

Nickel(II) hydroxide is the inorganic compound with the formula Ni(OH)2. It is a lime-green solid that dissolves with decomposition in ammonia and amines and is attacked by acids. It is electroactive, being converted to the Ni(III) oxy-hydroxide, leading to widespread applications in rechargeable batteries.[6]

Nickel(II) hydroxide has two well-characterized polymorphs, α and β. The α structure consists of Ni(OH)2 layers with intercalated anions or water.[7][8] The β form adopts a hexagonal close-packed structure of Ni2+ and OH− ions.[7][8] In the presence of water, the α polymorph typically recrystallizes to the β form.[7][9] In addition to the α and β polymorphs, several γ nickel hydroxides have been described, distinguished by crystal structures with much larger inter-sheet distances.[7]

The mineral form of Ni(OH)2, theophrastite, was first identified in the Vermion region of northern Greece, in 1980. It is found naturally as a translucent emerald-green crystal formed in thin sheets near the boundaries of idocrase or chlorite crystals.[10] A nickel-magnesium variant of the mineral, (Ni,Mg)(OH)2 had been previously discovered at Hagdale on the island of Unst in Scotland.[11]

Nickel(II) hydroxide is frequently used in electrical car batteries.[8] Specifically, Ni(OH)2 readily oxidizes to nickel oxyhydroxide, NiOOH, in combination with a reduction reaction, often of a metal hydride (reaction 1 and 2).[12][13]

Reaction 1 Ni(OH)2 + OH− → NiO(OH) + H2O + e−

Reaction 2 M + H2O + e− → MH + OH−

Net Reaction (in H2O)Ni(OH)2 + M → NiOOH + MH

Of the two polymorphs, α-Ni(OH)2 has a higher theoretical capacity and thus is generally considered to be preferable in electrochemical applications. However, it transforms to β-Ni(OH)2 in alkaline solutions, leading to many investigations into the possibility of stabilized α-Ni(OH)2 electrodes for industrial applications.[9]

The synthesis entails treating aqueous solutions of nickel(II) salts with potassium hydroxide. When the same reaction is conducted in the presence of bromine, the product is Ni3O2(OH)4.[14]

The Ni2+ ion is a carcinogen when inhaled.

  1. ^ CRC Handbook of Chemistry and Physics (84 ed.). CRC press. 2003. pp. 4–71. ISBN 0849304849.
  2. ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–189. ISBN 978-1138561632.
  3. ^ Enoki, Toshiaki; Tsujikawa, Ikuji (1975). "Magnetic Behaviours of a Random Magnet, NipMg(1-p)(OH2)". Journal of the Physical Society of Japan. 39 (2): 317. Bibcode:1975JPSJ...39..317E. doi:10.1143/JPSJ.39.317.
  4. ^ a b Zumdahl, Steven S. (2009). Chemical Principles (6 ed.). Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7.
  5. ^ "Nickel Hydroxide". American Elements. Retrieved 2018-08-30.
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  7. ^ a b c d Oliva, P.; Leonardi, J.; Laurent, J.F. (1982). "Review of the structure and the electrochemistry of nickel hydroxides and oxy-hydroxides". Journal of Power Sources. 8 (2): 229–255. Bibcode:1982JPS.....8..229O. doi:10.1016/0378-7753(82)80057-8.
  8. ^ a b c Jeevanandam, P.; Koltypin, Y.; Gedanken, A. (2001). "Synthesis of Nanosized α-Nickel Hydroxide by a Sonochemical Method". Nano Letters. 1 (5): 263–266. Bibcode:2001NanoL...1..263J. doi:10.1021/nl010003p.
  9. ^ a b Shukla, A.K.; Kumar, V.G.; Munichandriah, N. (1994). "Stabilized α-Ni(OH)2 as Electrode Material for Alkaline Secondary Cells". Journal of the Electrochemical Society. 141 (11): 2956–2959. Bibcode:1994JElS..141.2956V. doi:10.1149/1.2059264.
  10. ^ Marcopoulos, T.; Economou, M. (1980). "Theophrastite, Ni(OH)2, a new mineral from northern Greece" (PDF). American Mineralogist. 66: 1020–1021.
  11. ^ Livingston, A.; Bish, D. L. (1982). "On the new mineral theophrastite, a nickel hydroxide, from Unst, Shetland, Scotland" (PDF). Mineralogical Magazine. 46 (338): 1. Bibcode:1982MinM...46....1L. doi:10.1180/minmag.1982.046.338.01. S2CID 8381523.
  12. ^ Ovshinsky, S.R.; Fetcenko, M.A.; Ross, J. (1993). "A nickel metal hydride battery for electric vehicles". Science. 260 (5105): 176–181. Bibcode:1993Sci...260..176O. doi:10.1126/science.260.5105.176. PMID 17807176. S2CID 9523468.
  13. ^ Young, Kwo (2016). Nickel Metal Hydride Batteries. MDPI. doi:10.3390/books978-3-03842-303-4. ISBN 978-3-03842-303-4.
  14. ^ O. Glemser (1963). "Nickel (II) Hydroxide and Nickel (II,III) Hydroxide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2. New York: Academic Press. p. 1549-1551.