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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'''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==
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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.
 
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.
  
==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==

Revision as of 19:31, 24 December 2015

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.

Physical

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

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.[1]

See also

References

  1. Perchlorate in the Environment (2000), Edward Todd Urbansky, pag. 106

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

Relevant Sciencemadness threads