Nickel(II) hydroxide

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Nickel(II) hydroxide
Nickel(II) hydroxide Hydroxid nikelnaty.PNG
Nickel(II) hydroxide
Nickel(II) hydroxide Kristallstruktur Cadmiumiodid.png
Nickel(II) hydroxide
Names
IUPAC name
Nickel(II) hydroxide
Other names
Nickel hydroxide, Theophrastite
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.031.813 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 235-008-5
PubChem CID
RTECS number
  • QR648000
UNII
  • InChI=1S/Ni.2H2O/h;2*1H2/q+2;;/p-2 Yes check.svgY
    Key: BFDHFSHZJLFAMC-UHFFFAOYSA-L Yes check.svgY
  • InChI=1/Ni.2H2O/h;2*1H2/q+2;;/p-2
    Key: BFDHFSHZJLFAMC-NUQVWONBAJ
  • [Ni+2].[OH-].[OH-]
Properties
Ni(OH)2
Molar mass 92.724 g/mol (anhydrous)
110.72 g/mol (monohydrate)
Appearancegreen crystals
Density 4.10 g/cm3
Melting point 230 °C (446 °F; 503 K) (anhydrous, decomposes)
0.0015 g/L [1]
5.48×10−16 [2]
+4500.0·10−6 cm3/mol
Structure [3]
hexagonal, hP3
P3m1, No. 164
a = 0.3117 nm, b = 0.3117 nm, c = 0.4595 nm
α = 90°, β = 90°, γ = 120°
Thermochemistry
Std molar
entropy (S⦵298)
79 J·mol−1·K−1 [4]
−538 kJ·mol−1 [4]
Hazards
GHS labelling: [5]
GHS-pictogram-exclam.svg GHS-pictogram-silhouette.svg
Danger
H302, H315, H317, H332, H334, H341, H350, H360, H372
P201, P260, P280, P284, P405, P501
Lethal dose or concentration (LD, LC):
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).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)
The test tube in the middle contains a precipitate of nickel(II) hydroxide DSC01973 - Nickel (II) reactions.JPG
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]

Contents

Properties

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]

Reactions

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 1Ni(OH)2 + OH− → NiO(OH) + H2O + e−

Reaction 2M + 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]

Synthesis

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]

Toxicity

The Ni2+ ion is a carcinogen when inhaled.

See also

References

  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. 1 2 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.
  6. ↑ Chen, J.; Bradhurst, D.H.; Dou, S.X.; Liu, H.K. (1999). "Nickel Hydroxide as an Active Material for the Positive Electrode in Rechargeable Alkaline Batteries". Journal of the Electrochemical Society. 146 (10): 3606–3612. Bibcode:1999JElS..146.3606C. doi:10.1149/1.1392522. S2CID   33058220.
  7. 1 2 3 4 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. 1 2 3 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. 1 2 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.
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