Tris(ethylenediamine)nickel perchlorate

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Tris(ethylenediamine)nickel perchlorate
Tris(ethylenediamine) nickel(II) perchlorate by woelen.jpg
The nickel complex in solid form.
Properties
C6H24O8N6Cl2Ni
[Ni(en)3](ClO4)2
Molar mass 437.89 g/mol
Appearance Violet solid
Melting point Decomposes
Boiling point Detonates
Poorly soluble
Solubility Reacts with strong acids
Hazards
Safety data sheet None
Related compounds
Related compounds
Bis(ethylenediamine)copper(II) perchlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Tris(ethylenediamine)nickel perchlorate is a coordination complex with ethylenediamine to nickel ions. It is easy to prepare and is highly energetic, deflagrating easily in a flame.

Properties

Chemical

Tris(ethylenediamine)nickel perchlorate is highly explosive, though its oxygen balance is not optimal, with excess ethylenediamine in the structure. Although it is energetic, it can be stored indefinitely. It is poorly soluble in water, and this can be used to aid in its production.

It dissolves in acetone and methyl ethyl ketone, and will slowly react with the ketones to form a macrocyclic compound.[1][2][3]

Physical

Unlike its nickel perchlorate precursor, tris(ethylenediamine)nickel perchlorate has a strongly purple hue.

Explosive

Tris(ethylenediamine)nickel perchlorate will explode in contact with an open flame.

Preparation

Tris(ethylenediamine)nickel perchlorate can be prepared by dissolving nickel(II) oxide, hydroxide, or carbonate in perchloric acid and then adding ethylenediamine until the solution turns purple. After a day it will precipitate and the crystals can be collected.

Handling

Safety

Keep away from open flames.

Storage

It can be stored in closed containers.

Disposal

It can be safely neutralized by detonating it.

Residual perchlorates can be destroyed by adding metallic iron under UV light, in the absence of air.[4]

See also

References

  1. D. A. House and N. F. Curtis, Chem. Ind. (London), 42, 1708 (1961)
  2. http://pubs.acs.org/doi/pdf/10.1021/ja00999a008
  3. Coordination Chemistry of Macrocyclic Compounds, Gordon Melson, p. 39
  4. Perchlorate in the Environment (2000), Edward Todd Urbansky, pag. 106

http://woelen.homescience.net/science/chem/exps/Ni_en_complexes/index.html

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