The molecule exhibiting maximum number of non-bonding electron pairs (l.p.) around the central atom — Chemical Bonding Chemistry Question

💡 Solution & Explanation

Step 1: Calculate the lone pairs on Xenon for each species: - XeOF4: 8 valence e^-, 2 for O, 4 for F, leaving 2 e^- (1 lp). - XeO2F2: 8 valence e^-, 4 for 2 O, 2 for F, leaving 2 e^- (1 lp). - XeF3^-: 8 valence e^-, plus 1 for the negative charge = 9. Three form bonds with F, leaving 6 e^- (3 lps). - XeO3: 8 valence e^-, 6 for 3 O, leaving 2 e^- (1 lp). Step 2: Compare the number of lone pairs: XeF3^- has 3 lone pairs on the central Xe atom, while the others have 1 lone pair. Step 3: Thus, XeF3^- has the maximum number of lone pairs around the central atom, matching option (c).