A) \[HF<HCl<HBr,HI\]: increasing acidic strength
B) \[{{H}_{2}}O<{{H}_{2}}S<{{H}_{2}}Se<{{H}_{2}}Te\]: increasing \[p{{K}_{a}}\]values
C) \[N{{H}_{3}}<p{{H}_{3}}<As{{H}_{3}}<Sb{{H}_{3}}\]: increasing acidic character
D) \[C{{O}_{2}}<Si{{O}_{2}}<Sn{{O}_{2}}<Pb{{O}_{2}}\]: increasing oxidising power
Correct Answer: B
Solution :
(b) As we move from top to bottom in a group, acidic strength of hydrides increases. Therefore, order of acidic strength of hydrides of V A and group elements is \[N{{H}_{3}}<P{{H}_{3}}<As{{H}_{3}}<Sb{{H}_{3}}\] \[HF<HCl<HBr<HI\] (b) As we move from top to bottom in a group, acidic nature \[({{K}_{a}})\]increases. Therefore, \[p{{K}_{a}}\] decreases. Thus order of \[p{{K}_{a}}\] values of hydrides of VI A group elements is \[{{H}_{2}}O>{{H}_{2}}S>{{H}_{2}}Se>{{H}_{2}}Te\] (d) On moving form top to bottom, oxidising power of oxides increases. Thus order of oxidising power of oxides of IVA group elements is \[C{{O}_{2}}<Si{{O}_{2}}<Sn{{O}_{2}}<Pb{{O}_{2}}\]
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