Question

The N₂S₂ is a square molecule with nitrogen atoms at opposite corners and sulfur atoms at opposite corners. In other words, there are no S-S nor N-N bonds.

a) True
b) False

Answer 1

The question concerns the molecular structure and electron configurations of nitrogen and sulfur in hypothetical and real compounds, focusing on hybridization states, bond angles, and bond orders.

Step-by-step explanation:

The question is about the molecular geometry and electron configuration of the hypothetical square molecule N₂S₂. In the context of molecular orbital theory and VSEPR theory, it's apparent that the question covers the hybridization states of nitrogen and sulfur, the bond angles in molecules like NO2+ and NO2−, and the comparison of bond order and strength between diatomic nitrogen (N₂) and diatomic sulfur (S₂). For N₂, it is noted that nitrogen is sp² hybridized, and generally in molecules with a nitrogen, the geometry tends to be bent with a bond angle of approximately 120° when engaging in sp² hybridization.

The nitrogen-nitrogen triple bond in N₂ is significantly stronger and shorter than the single bond in F₂, as evidenced by molecular structure data. On the other hand, for a molecule of S₂, the valence electrons are distributed between bonding and antibonding orbitals to predict the electron configuration, bond order, and number of unpaired electrons.