Final answer:
The electronic structure of a nitrogen molecule, N₂, consists of two nitrogen atoms, each with five electrons in its outer shell, arranged with three lone pairs and one shared pair of electrons forming a triple bond between the two atoms.
Step-by-step explanation:
The electronic structure of a nitrogen molecule, N₂, involves two nitrogen atoms, each with five valence electrons in its outer shell. Nitrogen's atomic number is 7, indicating that it has five electrons in its outermost shell. The electronic configuration of nitrogen is 1s² 2s² 2p³, with three electrons in the 2p orbital. In the formation of a nitrogen molecule, each nitrogen atom contributes three of its five valence electrons to form a triple covalent bond (N≡N). This bond is formed by the overlap of the 2p orbitals from each nitrogen atom, resulting in the sharing of six electrons, creating the triple bond between them. Consequently, both nitrogen atoms attain a stable octet configuration by sharing electrons, fulfilling the octet rule.
The Lewis structure of nitrogen molecule, N≡N, illustrates this bonding arrangement. Each nitrogen atom has three lone pairs and shares one pair of electrons, forming the triple bond. The triple bond consists of one sigma bond (σ) and two pi bonds (π), resulting from the overlap of the sp² hybridized orbitals. This arrangement leads to the formation of a stable N₂ molecule where both nitrogen atoms have achieved a full outer shell configuration, resembling the noble gas configuration of neon (2s² 2p⁶).
The triple bond in the nitrogen molecule is strong due to the presence of three shared electron pairs. This configuration contributes to the stability of the molecule and its properties as a gas at room temperature. The triple bond's strength results in limited movement and separation between nitrogen molecules in the gaseous state, explaining why nitrogen gas consists of molecules that are spread far apart and move randomly at high speeds, consistent with the principles of kinetic theory.