In which one of the following arrangements the given sequence is...

$1 )$ $HF < HCl < HBr < HI$ bond strength decreases therefore, acidic strength increases.
$2 )$ ${H}_{2}O < {H}_{2}S < {H}_{2}Se < {H}_{2}Te$ from going down the group bond length increase so bond strength decreases therefore, acidic nature of these will increase but ${pK}_{a}$ will decrease.
So, this given order is wrong.
$3 )$ ${NH}_{3} < {PH}_{3} < {AsH}_{3} < {SbH}_{3}$ from going down the group bond length increases, so bond strength decreases therefore, acidic nature of these will increase
$4 )$ ${CO}_{2} < {SiO}_{2} < {SnO}_{2} < {PbO}_{2}$ From going down the group stability of higher oxidation state decreases due to inert pair effect therefore, their tendency to reduce will increase, so their oxidizing power will increase.