= Solution
\b[C-C is strongest; N-N is much weaker despite <nitrogen>'s smaller size.] <Carbon>'s effective nuclear attraction and good overlap of compact second-row valence orbitals favor a strong C-C <sigma bond>. The larger, more electron-deficient <boron> centres give less effective B-B bonding in the stated molecule, despite its relatively high-s-character trigonal bonding.
In hydrazine, the two neighboring <nitrogen> <lone pairs> strongly repel one another, destabilizing the N-N bond. Bond strength therefore cannot be predicted from atomic size alone; lone-pair repulsion explains the especially low N-N value.
This illustrates <bonding trends in second-period single bonds>.
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