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Nitrogen-Nitrogen bonds inside larger molecules are never quite stable because 1) nitrogen “wants” to form stable di-nitrogen (N2) molecules containing a very s

Nitrogen-Nitrogen bonds inside larger molecules are never quite stable because 1) nitrogen “wants” to form stable di-nitrogen (N2) molecules containing a very stable triple bond (an exothermic reaction) and 2) the result of such decompositions is nitrogen gas increasing the amount of entropy released (due to more molecules being created). Reactions are driven both by the amount of heat released (enthalpy) and the amount of “disorder” created (entropy). Explosive reactions tend to be the ones where both factors add to the driving force.

morpheuskafka 5y ago
Does the same apply to oxygen? Since it also likes to be in a diatomic form.
- masklinn 5y ago
  The opposite, or oxygen wouldn't be such a strong oxidiser, which implies it readily and energetically leaves its double bond behind for either single bonds (H2O) or double bonds with non-oxygen atoms (CO2).
- G3rn0ti 5y ago
  Oh, yes. Every substance carrying a „peroxo“ in its name is usually nasty stuff. Concentrated hydrogenperoxide for example can explode creating gaseous water (aka steam) and dioxygen (aka oxygen) in the process. While O2 is a corrosive, it is quite inert under normal conditions (which is why our clothes don’t burst into flames spontaneously).
- opportune 5y ago
  Diatomic oxygen is less stable than many other oxygen-containing compounds like CO2 (that is why charcoal burns) but diatomic nitrogen is pretty much as stable as nitrogen can get.
- lmilcin 5y ago
  Hydrogen peroxide at sufficient concentration can be used as rocket fuel. https://en.wikipedia.org/wiki/Hydrogen_peroxide https://en.wikipedia.org/wiki/Hydrogen_peroxide "High-concentration H2O2 is referred to as "high-test peroxide" (HTP). It can be used either as a monopropellant (not mixed with fuel) or as the oxidizer component of a bipropellant rocket."
- jldugger 5y ago
  I mean, pure oxygen envs are pretty dangerous on their own, compared to pure N2.

morpheuskafka 5y ago

Does the same apply to oxygen? Since it also likes to be in a diatomic form.

masklinn 5y ago
The opposite, or oxygen wouldn't be such a strong oxidiser, which implies it readily and energetically leaves its double bond behind for either single bonds (H2O) or double bonds with non-oxygen atoms (CO2).
G3rn0ti 5y ago
Oh, yes. Every substance carrying a „peroxo“ in its name is usually nasty stuff. Concentrated hydrogenperoxide for example can explode creating gaseous water (aka steam) and dioxygen (aka oxygen) in the process. While O2 is a corrosive, it is quite inert under normal conditions (which is why our clothes don’t burst into flames spontaneously).
opportune 5y ago
Diatomic oxygen is less stable than many other oxygen-containing compounds like CO2 (that is why charcoal burns) but diatomic nitrogen is pretty much as stable as nitrogen can get.
lmilcin 5y ago
Hydrogen peroxide at sufficient concentration can be used as rocket fuel. https://en.wikipedia.org/wiki/Hydrogen_peroxide https://en.wikipedia.org/wiki/Hydrogen_peroxide "High-concentration H2O2 is referred to as "high-test peroxide" (HTP). It can be used either as a monopropellant (not mixed with fuel) or as the oxidizer component of a bipropellant rocket."
jldugger 5y ago
I mean, pure oxygen envs are pretty dangerous on their own, compared to pure N2.