Question

Why does the reactivity of nitrogen differ from phosphorus?

Answer 1

Hint : In order to answer this question, to know the comparison of reactivity of both the given compounds, we will go through the exact reasons why one is more reactive than other. We will also discuss more about both the elements.

Complete Step By Step Answer:
Nitrogen is chemically less reactive. This is because of the high stability of its molecule, $ {N_2} $ . In $ {N_2} $ , the two nitrogen atoms form a triple bond. This triple bond has very high bond strength, which is very difficult to break. It is because of nitrogen's small size that it is able to form $ \pi - \pi $ bonds with itself. This property is not exhibited by atoms such as phosphorus. Thus, phosphorus is more reactive than nitrogen.
Given the great reactivity of atomic nitrogen, elemental nitrogen usually occurs as molecular $ {N_2} $ , di-nitrogen. This molecule is a colourless, odourless, and tasteless diamagnetic gas at standard conditions: it melts at $ - 210{\text{ }}^\circ C $ and boils at $ - 196{\text{ }}^\circ C $ .
Reaction of phosphorus with air White phosphorus shines in obscurity when presented to moist air in a cycle known as chemiluminescence. White phosphorus should be taken care of with extraordinary consideration. It spontaneously touches off in air at about room temperature to shape "phosphorus pentoxide" - really tetraphosphorus decaoxide, $ {P_4}{O_{10}} $ .
Hence, phosphorus is more reactive than nitrogen.

Note :
Nitrogen and phosphorus are group V elements in the periodic table. Having the same valence shell electrons, they share some similar properties especially when making compounds. Nitrogen is in the second period, whereas phosphorus is in the third period.