Nickel Dmg

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Apr 15, 2004  Herein, the colorimetric nickel(II) reagent dimethylglyoxime (DMG) is immobilized on a solid support and released as the sample passes through the support. As one of the most selective nickel(II) reagents, DMG reacts to form a pink flocculent precipitate, in solution which is collected on the surface of an extraction disk. The analyte is then quantified with a diffuse reflectance.

  1. Nickel Dmg Complex Structure
  2. Nickel Dmg Complex Iupac Name
  3. Nickel Dmg Reaction
  1. Pour half the nickel ethylene diamine solution into a small hydrometer and add the DMG solution dropwise to form the red precipitate. Hint: Any green precipitate formation is due to Ni(OH)2 precipitate. (Add more ammonia to make it go away.) Make the ethylene diamine solution fresh if there are crystals present in the solution or if it’s more.
  2. The Ni(DMG) 2 complex (MW 288.9 g/mole) is stable to heat and is unusually hydrophobic; it will dry quickly in an oven at 110-120 o C to yield a pure substance whose weight can be used to calculate the nickel content of the original sample.
Nickel(II) hydroxide
Names
IUPAC name
Other names
Nickel hydroxide, Theophrastite
Identifiers
  • 12054-48-7
  • 36897-37-7 (monohydrate)
ChemSpider
ECHA InfoCard100.031.813
EC Number
  • 235-008-5
RTECS number
CompTox Dashboard(EPA)
  • Key: BFDHFSHZJLFAMC-UHFFFAOYSA-L
  • Key: BFDHFSHZJLFAMC-NUQVWONBAJ
  • [Ni+2].[OH-].[OH-]
Properties
Ni(OH)2
Molar mass92.724 g/mol (anhydrous)
110.72 g/mol (monohydrate)
Appearancegreen crystals
Density4.10 g/cm3
Melting point 230 °C (446 °F; 503 K) (anhydrous, decomposes)
0.13 g/L
+4500.0·10−6 cm3/mol
Structure[1]
hexagonal, hP3
P3m1, No. 164
α = 90°, β = 90°, γ = 120°
Thermochemistry
79 J·mol−1·K−1[2]
Std enthalpy of
formation(ΔfH⦵298)
−538 kJ·mol−1[2]
Hazards
Safety data sheetExternal SDS
GHS pictograms[3]
GHS Signal wordDanger[3]
H302, H332, H315, H334, H317, H341, H350, H360, H372[3]
P260, P284, P201, P280, P405, P501[3]
Lethal dose or concentration (LD, LC):
1515 mg/kg (oral, rat)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references
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 an apple-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.[4]

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Properties[edit]

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.[5][6] The β form adopts a hexagonal close-packed structure of Ni2+ and OH− ions.[5][6] In the presence of water, the α polymorph typically recrystallizes to the β form.[5][7] 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.[5]

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.[8] A nickel-magnesium variant of the mineral, (Ni,Mg)(OH)2 had been previously discovered at Hagdale on the island of Unst in Scotland.[9]

Reactions[edit]

Nickel(II) hydroxide is frequently used in electrical car batteries.[6] 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).[10]

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.[7]

Synthesis[edit]

The synthesis entails treating aqueous solutions of nickel(II) salts with potassium hydroxide.[11]

Toxicity[edit]

Nickel Dmg Complex Structure

The Ni2+ ion is a known carcinogen. Toxicity and related safety concerns have driven research into increasing the energy density of Ni(OH)2 electrodes, such as the addition of calcium or cobalt hydroxides.[4]

See also[edit]

References[edit]

  1. ^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. doi:10.1143/JPSJ.39.317.
  2. ^ abZumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN978-0-618-94690-7.
  3. ^ abcd'Nickel Hydroxide'. American Elements. Retrieved 2018-08-30.
  4. ^ abChen, 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'. J. Electrochem. Soc. 146 (10): 3606–3612. doi:10.1149/1.1392522.
  5. ^ abcdOliva, 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. doi:10.1016/0378-7753(82)80057-8.
  6. ^ abcJeevanandam, P.; Koltypin, Y.; Gedanken, A. (2001). 'Synthesis of Nanosized α-Nickel Hydroxide by a Sonochemical Method'. Nano Letters. 1 (5): 263–266. doi:10.1021/nl010003p.
  7. ^ abShukla, A.K.; Kumar, V.G.; Munichandriah, N. (1994). 'Stabilized α-Ni(OH)2 as Electrode Material for Alkaline Secondary Cells'. J. Electrochem. Soc. 141 (11): 2956–2959. doi:10.1149/1.2059264.
  8. ^Marcopoulos, T.; Economou, M. (1980). 'Theophrastite, Ni(OH)2, a new mineral from northern Greece'(PDF). American Mineralogist. 66: 1020–1021.
  9. ^Livingston, A.; Bish, D. L. (1982). 'On the new mineral theophrastite, a nickel hydroxide, from Unst, Shetland, Scotland'(PDF). Mineralogical Magazine. 46 (338): 1. doi:10.1180/minmag.1982.046.338.01.
  10. ^Ovshinsky, S.R.; Fetcenko, M.A.; Ross, J. (1993). 'A nickel metal hydride battery for electric vehicles'. Science. 260 (5105): 176–181. doi:10.1126/science.260.5105.176. PMID17807176.
  11. ^Glemser, O. (1963) 'Nickel(II) Hydroxide' in 'Handbook of Preparative Inorganic Chemistry, 2nd ed. G. Brauer (ed.), Academic Press, NY. Vol. 1. p. 1549.

External links[edit]

Retrieved from 'https://en.wikipedia.org/w/index.php?title=Nickel(II)_hydroxide&oldid=904764643'
Dimethylglyoxime
Names
IUPAC name
Other names
  • Dimethylglyoxime
  • Diacetyl dioxime
  • Butane-2,3-dioxime
  • Chugaev's reagent
Identifiers
  • 95-45-4
ChEMBL
ChemSpider
  • 10606175
ECHA InfoCard100.002.201
EC Number
PubChemCID
RTECS number
  • EK2975000
UNII
  • InChI=1S/C4H8N2O2/c1-3(5-7)4(2)6-8/h7-8H,1-2H3/b5-3-,6-4+
  • InChI=1/C4H8N2O2/c1-3(5-7)4(2)6-8/h7-8H,1-2H3/b5-3-,6-4+
  • CC(=NO)C(C)=NO
Properties
C4H8N2O2
Molar mass116.120 g·mol−1
AppearanceWhite/Off White Powder
Density1.37 g/cm3
Melting point 240 to 241 °C (464 to 466 °F; 513 to 514 K)
Boiling pointdecomposes
low
Structure
0
Hazards
Main hazardsToxic, Skin/Eye Irritant
Safety data sheetExternal MSDS
GHS pictograms
GHS Signal wordDanger
H228, H301
P210, P240, P241, P264, P270, P280, P301+310, P321, P330, P370+378, P405, P501
NFPA 704 (fire diamond)
Related compounds
Hydroxylamine
salicylaldoxime
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Dimethylglyoxime is a chemical compound described by the formula CH3C(NOH)C(NOH)CH3. Its abbreviation is dmgH2 for neutral form, and dmgH for anionic form, where H stands for hydrogen. This colourless solid is the dioxime derivative of the diketone butane-2,3-dione (also known as diacetyl). DmgH2 is used in the analysis of palladium or nickel. Its coordination complexes are of theoretical interest as models for enzymes and as catalysts. Many related ligands can be prepared from other diketones, e.g. benzil.

Preparation[edit]

How to download netflix shows mac. Dimethylglyoxime can be prepared from butanone first by reaction with ethyl nitrite to give biacetyl monoxime. The second oxime is installed using sodium hydroxylamine monosulfonate:[1]

Complexes[edit]

Dimethylglyoxime is used to detect and quantify nickel, which forms the bright red complex nickel bis(dimethylglyoximate) (Ni(dmgH)2). The reaction was discovered by L. A. Chugaev in 1905.[2]

Cobalt complexes have also received much attention. In chloro(pyridine)cobaloxime[3] the macrocycle [dmgH]22− mimics the macrocyclic ligand found in vitamin B12.

Structure of chloro(pyridine)cobaloxime.

References[edit]

Nickel Dmg Complex Iupac Name

  1. ^Semon, W. L.; Damerell, V. R. (1930). 'Dimethylglyoxime'. Organic Syntheses. 10: 22. doi:10.15227/orgsyn.010.0022.CS1 maint: multiple names: authors list (link)
  2. ^Lev Tschugaeff (1905). 'Über ein neues, empfindliches Reagens auf Nickel'. Berichte der Deutschen Chemischen Gesellschaft. 38 (3): 2520–2522. doi:10.1002/cber.19050380317.
  3. ^Girolami, G. S.; Rauchfuss, T.B.; Angelici, R. J. (1999). Synthesis and Technique in Inorganic Chemistry: A Laboratory Manual (3rd ed.). pp. 213–215.

Nickel Dmg Reaction

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