To compare the bond strength of the nitrogen-hydrogen bond in ammonia NH3 and hydrazine N2H4 , we can consider the electronegativity values and bond lengths of the molecules.Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. The electronegativity values for nitrogen N and hydrogen H are 3.04 and 2.20, respectively. The difference in electronegativity values between N and H in both molecules is the same 3.04 - 2.20 = 0.84 , which indicates that the polarity of the N-H bonds in both ammonia and hydrazine is similar.Bond length is another factor that can influence bond strength. In general, shorter bond lengths correspond to stronger bonds. The bond length of the N-H bond in ammonia is approximately 1.012 angstroms , while the bond length of the N-H bond in hydrazine is approximately 1.020 . The difference in bond lengths is small, but the N-H bond in ammonia is slightly shorter, suggesting that it may be slightly stronger.However, it is important to note that bond strength is also influenced by factors such as bond order and resonance structures. In the case of ammonia and hydrazine, the bond order for the N-H bonds is 1 in both molecules, and there are no resonance structures to consider.Taking all these factors into account, we can conclude that the bond strength of the nitrogen-hydrogen bond in ammonia NH3 is likely to be slightly stronger than the nitrogen-hydrogen bond in hydrazine N2H4 due to the slightly shorter bond length in ammonia. However, the difference in bond strength is expected to be small, as the electronegativity values and bond orders are similar in both molecules.