Final answer:
Bond energies increase and bond lengths decrease as the number of bonds between two nitrogen atoms increases; the highest bond energy and shortest bond length go to the triple bond, while the lowest bond energy and longest bond length are characteristic of the single bond.
Step-by-step explanation:
The assignment given involves organizing bond energies and bond lengths for nitrogen-nitrogen single, double, and triple bonds. To complete this task, we need to understand that as the number of bonds between two nitrogen atoms increases, the bond itself becomes stronger and the bond length becomes shorter. This means a triple bond (N≡N) will have the highest bond energy and the shortest bond length, a double bond (N=N) will have an intermediate bond energy and bond length, and a single bond (N-N) will have the lowest bond energy and the longest bond length.
The correct way to arrange the given data is:
- Bond Energy for N-N (single bond) is least, thus 167 kJ/mol
- Bond Energy for N≡N (triple bond) is greatest, thus 942 kJ/mol
- Bond Energy for N=N (double bond) would therefore be 418 kJ/mol
- Bond Length for N-N (single bond): 145 pm
- Bond Length for N≡N (triple bond): 110 pm
- Bond Length for N=N (double bond): 125 pm
This arrangement follows the trend that a stronger bond has a shorter bond length, and a weaker bond has a longer bond length. It is important to remember these relationships when determining unknown values for bond lengths and energies.