Question

Based on the Lewis electron-dot diagrams of n2 and n2h4, compare the strength of the nitrogen-to-nitrogen bond in n2 with the strength of the nitrogen-to-nitrogen bond in n2h4.​

Answer 1

Answer:N2 is weaker

Explanation: Because N2 shares more valence electrons together than the nitrogen-to-nitrogen bonds in N2H4, the valence electrons make it weaker.

Answer 2

Answer:

Nitrogen to nitrogen bond in $N_{2}$ higher in strength than nitrogen to nitrogen bond in $N_{2}H_{4}$

Explanation:

• Lewis dot structure of $N_{2}$ reveals that there exist a triple bond between two N atoms.
• Lewis dot structure of $N_{2}H_{4}$ reveals that there exist one single bond between two N atoms.
• For covalent bond between two given atoms, force constant of a triple bond is almost 3 times higher than force constant of a single bond.
• As bond energy is proportional to force constant of a bond therefore strength of triple bond is higher than strength of single bond.
• So nitrogen to nitrogen bond in $N_{2}$ higher in strength than nitrogen to nitrogen bond in $N_{2}H_{4}$
• Lewis dot structures are given below.