Question

\(O - O\) bond length in \(H _2 O _2\) is X than the \(O - O\) bond length in \(F _2 O _2\)The \(O - H\) bond length in \(H _2 O _2\)is Y than that of the\(O - F\) bond in \(F _2 O _2\)Choose the correct option for \(\underline{X} and \underline{Y}\) from those given below :

• A. X-shorter, Y-shorter
• B. X - shorter, Y - longer
• C. X - longer, Y - shorter
• D. X-longer,  Y-longer

Hint:

Electronegativity and atomic size influence bond lengths. Higher electronegativity differences lead to shorter bonds, and smaller atomic radii also contribute to shorter bond lengths.

Answer 1

The Correct Option is C

The question asks about the comparative bond lengths in \(H_2O_2\) (hydrogen peroxide) and \(F_2O_2\) (dioxydifluoride), aiming to determine for which compound the bond lengths \(O-O\) and \(O-H\) differ. Let's analyze this step-by-step: 

Understanding Bond Lengths: The bond length is the distance between the nuclei of two bonded atoms. It is influenced by various factors like atomic size, bond order, and electronegativity of the atoms involved.

Comparing \(O-O\) Bond Lengths:

• In \(H_2O_2\), the \(O-O\) bond is a single bond.
• In \(F_2O_2\), the \(O-O\) bond is also a single bond, but the electronegativity of attached atoms influences this bond.

Comparing \(O-H\) and \(O-F\) Bond Lengths:

• The \(O-H\) bond in \(H_2O_2\) is typically shorter because hydrogen atoms have smaller radii compared to fluorine.
• The \(O-F\) bond in \(F_2O_2\) is longer because the larger fluorine atom increases the bond length, despite its higher electronegativity.

Conclusion: Based on the above analysis:

• \(X\) is longer (the \(O-O\) bond in \(H_2O_2\) is longer than in \(F_2O_2\)).
• \(Y\) is shorter (the \(O-H\) bond in \(H_2O_2\) is shorter than the \(O-F\) bond in \(F_2O_2\)).

Therefore, the correct option is: X - longer, Y - shorter.