Bond Energies

  1. 1. The problem statement, all variables and given/known data
    Nitrogen trifluoride, NF3, is relatively stable toward decomposition to its elements. In contrast, NCl3 can be dangerous to work with because of its tendency to decompose to N2 + Cl2, Use bond energies to rationalize.

    2. Relevant equations

    Bond energies for N-F is 278 kJ/mol, N-Cl is 193 kJ/mol, N≡N is 942 kJ/mol, Cl-Cl is 240 kJ/mol and F-F is 154 kJ/mol.

    3. The attempt at a solution

    I don't really know what we are supposed to be explaining. Rationalizing the formation of N2 and Cl2 has more to do with attraction than bonding energies right? I'm so lost :(
  2. jcsd
  3. i think its because when the bonds decompose, it releases energy, given off in some form...that could make it dangerous...i have not done the calculations, you should try that...see if NCl3 has more or less energy than N2 + Cl2
  4. Borek

    Staff: Mentor

    And do the same for NF3. It doesn't have to give the answer, but that's the most obvious thing to try.
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