CHEMISTRY · Multi-part · CBSE · Chemistry · Chemical Bonding and Molecular Structure · Chemical Bonding and Molecular Structure
Problem
Nitrous oxide, N₂O(g), is used as an anesthetic and propellant. Because more than one plausible electron arrangement exists, chemists often analyze multiple Lewis structures to predict properties.
(a) Calculate the total number of valence electrons for N₂O.
(b) Draw every distinct Lewis structure that obeys the octet rule (or duet for H) and places the atoms in a linear order. Clearly indicate all lone pairs and multiple bonds.
(c) For each structure from part (b), assign formal charges to all atoms.
(d) Using the formal-charge data and any other relevant considerations, identify which structure is predicted to make the greatest contribution to the resonance hybrid. Justify your choice thoroughly.
(e) Based on your preferred structure, predict the relative lengths of the two N–N or N–O bonds in the molecule (if they are equivalent or not) and explain your reasoning.