The bond enthalpies of N–N, N=N and N≡N bonds are not in the ratio 1:2:3. Explain the reason
Answers
The bond energies of N-N, N=N and N≡N are not in the ratio of 1:2:3 because the strength of bond is different in all three examples. The sigma bonds are stronger than the pie bonds.
Explanation:
The stronger is the bond as in N≡N, the more energy gets released during the formation of bond. Bond energy is the amount of energy stored in a bond between atoms of the molecule.
The presence of sigma bonds increases the bond energy so.
N-N has one pie bond so low bond energy
N=N has one pie and one sigma so bond energy increases
N≡N has stronger bonds between them hence larger bond energy.
Hence, they are not in the ratio of 1:2:3
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Answer:
A Nitrogen molecule, two bonds are a sigma bond and a pi bond; a pi bond is stronger between nitrogen atoms than a sigma bond. The difference in the strength of sigma and pi bonds is due to the large charge of the nucleus of the nitrogen atom. When only one sigma bond is formed, the nuclei of the nitrogen atoms repel each other more strongly and the N – N bond is less strong. When sigma and pi bonds are formed simultaneously, the electron clouds shield the charges of the nuclei and the nuclei begin to be attracted to zones of increased electron density, and nitrogen nuclei with a large charge are attracted more strongly. A stronger bond N = N is formed.The large difference in the strengths of the single and triple nitrogen-nitrogen bonds is the reason that this element does not have a tendency to form chains.