Consider the following table regarding interhalogen compounds, XYn (where Y is more electronegative — Chemical Bonding Chemistry Question
Question
Consider the following table regarding interhalogen compounds, XYn (where Y is more electronegative than X) : [Value of n: P1, Total d-orbitals used in hybridization: 1, Polarity: Polar, Planarity: Planar], [Value of n: P2, Total d-orbitals: Q1, Polarity: Polar, Planarity: Non-Planar], [Value of n: P3, Total d-orbitals: Q2, Polarity: Non-Polar, Planarity: Non-Planar]. Then according to given information calculate value of expression P2 * (P3 - P1) / (Q1 + Q2).
💡 Solution & Explanation
Step 1: Note that hydrogen bond strength increases with the electronegativity of the highly electronegative atom bonded to hydrogen (F > O > S). Thus, HF has the strongest hydrogen bonds and H2S has the weakest. Step 2: Compare H2O and H2O2. The oxygen in H2O carries a greater partial negative charge than in H2O2 because the presence of the peroxide linkage in H2O2 reduces the electron density on each oxygen, making H2O's hydrogen bonds stronger. Step 3: This leads to the strength order: HF > H2O > H2O2 > H2S, matching option (d).