# Give reasons for the following : Acidic character decreases from $N_2O_3$ to $Bi_2O_3$ All the P – Cl bonds in $PCl_5$ are not equivalent. HF is a weaker acid than HCl in an aqueous solution.

(a) Acidic character decreases from $N_2O_3$ to $Bi_2O_3$ because of decrease in electronegativity down the group.

(b) The three halogen atoms occupy equitorial position while the other two occupy axial positions. Since the three equatorial E-X bonds are repelled by two 'electron pairs but the two axial E-X bonds are repelled by three electron pairs, therefore axial bonds are usually longer than the equitorial bonds.

(c) It is due to high bond dissociation enthalpy of HF than $HCl$, it does not release hydrogen easily hence a weaker acid than $HCl$.

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