Question

explain the formation of Nitrogen molecule by using valence bond theory

Answer 1

The electronic configuration of ‘N’ atom is 2, 5 and to have Octet in the valence shell it requires three more electrons.When two nitrogen atoms approach each other, each atom contributes 3 electrons for bonding.There are six electrons shared between two nitrogen atoms in the form of three pairs.Therefore, there is a triple bond between two nitrogen atoms in $N _{ 2 }$ molecules.

Answer 2

Answer:

Nitrogen's electronic configuration is $1s^{2} 2s^{2} 2px^{2} 2py^{1} 2pz^{1}$, Both nitrogen atoms will share three electrons, resulting in three covalent bonds and the formation of a nitrogen molecule ($N_{2}$).

Explanation

Each nitrogen atom may count on $8$electrons in its outer shell by sharing $6$ electrons where the shells touch.

The $3$pairs of electrons, i.e. $6$ electrons, are now shared by the N-atoms. Each electron pair represents a single bond. Nitrogen has three links between its atoms. This is referred to as a triple bond. This triple bond is extremely strong, which is why nitrogen is so unreactive (i.e., stable)

In nitrogen gas, there are no ions (no + or – charges) because electrons are shared rather than moved from one atom to another.