The bond order between nitrogen atoms in a nitrogen gas molecule N2 can be determined by looking at its molecular orbital diagram or using the formula:Bond order = Number of electrons in bonding orbitals - Number of electrons in antibonding orbitals / 2Nitrogen has 5 valence electrons, so in a nitrogen gas molecule N2 , there are a total of 10 valence electrons. The molecular orbital diagram of N2 shows that there are 8 electrons in bonding orbitals 2 in the sigma 1s, 2 in the sigma 2s, 2 in the pi 2px, and 2 in the pi 2py orbitals and 2 electrons in antibonding orbitals 2 in the sigma 2s* orbital .Using the bond order formula:Bond order = 8 - 2 / 2 = 6 / 2 = 3The bond order between nitrogen atoms in a nitrogen gas molecule is 3, which means there is a triple bond between the two nitrogen atoms.This bond order affects the properties of the nitrogen gas molecule in several ways:1. Stability: The triple bond makes N2 a very stable molecule, as breaking the bond requires a significant amount of energy. This is why nitrogen gas is relatively unreactive under normal conditions.2. Bond length: The triple bond between nitrogen atoms results in a shorter bond length approximately 1.10 compared to single or double bonds. This is because the more bonds there are between atoms, the closer they are held together.3. Bond strength: The triple bond in N2 is stronger than a single or double bond, which means it takes more energy to break the bond. This contributes to the stability and unreactivity of nitrogen gas.4. Reactivity: Due to the high bond strength and stability of the triple bond, nitrogen gas is generally unreactive at room temperature. However, under certain conditions e.g., high temperatures, pressures, or in the presence of a catalyst , nitrogen gas can react with other elements to form various compounds.