though both nitrogen and oxygen are diatomic gases, nitrogen is far less reactive than oxygen. Why?
The bond energy for the NtriplebondN is much higher than the O-O (Oxygen to oxygen bond is a little more than a single bond but a little less than a double bond).
The difference in reactivity between nitrogen and oxygen is primarily due to their atomic structures.
To understand why nitrogen is less reactive than oxygen, we need to consider their electron configurations. Nitrogen (N) has atomic number 7, and its electron configuration is 1s² 2s² 2p³. As you can see, nitrogen has three unpaired electrons in its outermost energy level (2p). These unpaired electrons make nitrogen relatively stable because they contribute to a half-filled or partially-filled electron configuration, which is energetically favorable.
On the other hand, oxygen (O) has atomic number 8, and its electron configuration is 1s² 2s² 2p⁴. Oxygen has two unpaired electrons in its outermost energy level (2p), which means it is close to having a fully filled electron configuration. Having unpaired electrons makes oxygen more reactive because it only requires two more electrons to achieve a stable, fully filled configuration.
This difference in the number of unpaired electrons between nitrogen and oxygen accounts for the variance in reactivity. Nitrogen is less likely to engage in chemical reactions because it is already relatively stable with its partially-filled electron configuration. Oxygen, on the other hand, eagerly reacts with other elements, seeking to gain two electrons and attain a more stable configuration.
It's also important to note that the strength of the bond between the two nitrogen atoms in a nitrogen molecule (N₂) is stronger than the bond between the two oxygen atoms in an oxygen molecule (O₂). This increased bond strength further contributes to nitrogen's lower reactivity compared to oxygen.