Consider the two statements below. Which of the following best explains (I) and (II)? (I) the Ka of HXO2 is greater than the Ka of HYO2, but (II) the Ka of HX is less than the Ka of HY
(A) (I) X is more electronegative than Y, and (II) the H—X bond is shorter than the H—Y bond
(B) (I) X is less electronegative than Y, and (II) the H—X bond is longer than the H—Y bond
(C) (I) the H—X bond is weaker than the H—Y bond, and (II) X is more electronegative than Y
(D) (I) the H—X bond is stronger than the H—Y bond, and (II) X is less electronegative than Y

(D) (I) the H—X bond is stronger than the H—Y bond, and (II) X is less electronegative than Y.

Explanation:

A large Ka value indicates a strong acid because it means the acid is largely dissociated into its ions. A large Ka value also means the formation of products in the reaction is favored. As the electronegativity of an atom increases from left to right across a row, the acidity increases.

The higher the electronegativity of an atom, greater is its tendency to pull towards itself the pair of electrons that form the bond. This, in true effect, leads to a reduction in the bond length and therefore makes it harder cleave.