Difference between revisions of "Tris(ethylenediamine)nickel perchlorate"

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'''Tris(ethylenediamine)nickel perchlorate''' is a coordination complex with [[ethylenediamine]] to [[nickel]] ions. It is easy to prepare and is highly energetic, deflagarating easily in a flame.
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| Name = Tris(ethylenediamine)nickel perchlorate
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| ImageFile = Tris(ethylenediamine) nickel(II) perchlorate by woelen.jpg
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| ImageCaption = The nickel complex in solid form.
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| Appearance = Violet solid
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| BoilingPt_notes = Detonates
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| Formula = C<sub>6</sub>H<sub>24</sub>O<sub>8</sub>N<sub>6</sub>Cl<sub>2</sub>Ni<br>[Ni(en)<sub>3</sub>](ClO<sub>4</sub>)<sub>2</sub>
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| MolarMass = 437.89 g/mol
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| MeltingPt_notes = Decomposes
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| OtherCompounds = [[Bis(ethylenediamine)copper(II) perchlorate]]
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'''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==
 
==Properties==
 
===Chemical===
 
===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.
 
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.
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It dissolves in [[acetone]] and [[methyl ethyl ketone]], and will slowly react with the ketones to form a macrocyclic compound.<ref>D. A. House and N. F. Curtis, Chem. Ind. (London), 42, 1708 (1961)</ref><ref>http://pubs.acs.org/doi/pdf/10.1021/ja00999a008</ref><ref>[https://books.google.ro/books?id=fgXrBwAAQBAJ&pg=PA39&lpg=PA39&dq=Tris%28ethylenediamine%29nickel+perchlorate&source=bl&ots=KMtlNyvJLJ&sig=_iGMBJsPc4UTKXGxpT_4Rifu8Yg&hl=ro&sa=X&ved=0ahUKEwi_j9eFmdfUAhWjdpoKHe3iAMcQ6AEIqAEwEw#v=onepage&q=Tris%28ethylenediamine%29nickel%20perchlorate&f=false Coordination Chemistry of Macrocyclic Compounds, Gordon Melson, p. 39]</ref>
  
 
===Physical===
 
===Physical===
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Unlike its [[nickel perchlorate]] precursor, tris(ethylenediamine)nickel perchlorate has a strongly purple hue.
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Unlike its [[nickel(II) perchlorate]] precursor, tris(ethylenediamine)nickel perchlorate has a strongly purple hue.
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===Explosive===
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Tris(ethylenediamine)nickel perchlorate will explode in contact with an open flame.
  
 
==Preparation==
 
==Preparation==
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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.
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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.
  
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==Safety==
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==Handling==
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===Safety===
 
Keep away from open flames.
 
Keep away from open flames.
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===Storage===
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It can be stored in closed containers.
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===Disposal===
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It can be safely neutralized by detonating it.
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Residual perchlorates can be destroyed by adding metallic [[iron]] under UV light, in the absence of air.<ref>[https://books.google.ro/books?id=gjfSBwAAQBAJ&pg=PA106&lpg=PA106&dq=perchlorate+neutralization&source=bl&ots=ztEPz18eE-&sig=oHHZzByFHPVjYIVxbvzGl4SC_xQ&hl=en&sa=X&ved=0ahUKEwi5gpTJm_XJAhVBURoKHb3LB4o4ChDoAQguMAc#v=onepage&q=perchlorate%20neutralization&f=false Perchlorate in the Environment (2000), Edward Todd Urbansky, pag. 106]</ref>
  
 
==See also==
 
==See also==
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[[Category:Perchlorates]]
 
[[Category:Perchlorates]]
 
[[Category:Coordination complexes]]
 
[[Category:Coordination complexes]]
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[[Category:Nickel complexes]]
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[[Category:Energetic materials]]
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[[Category:Primary explosives]]

Latest revision as of 17:35, 26 September 2020

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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(II) 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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