A) \[{{H}_{2}}O>{{H}_{2}}S>{{H}_{2}}Se>{{H}_{2}}Te\]
B) \[{{H}_{2}}O<{{H}_{2}}S<{{H}_{2}}Se<{{H}_{2}}Te\]
C) \[{{H}_{2}}S>{{H}_{2}}O>{{H}_{2}}Se>{{H}_{2}}Te\]
D) \[{{H}_{2}}Se>{{H}_{2}}S>{{H}_{2}}O>{{H}_{2}}Te\]
Correct Answer: B
Solution :
The acidic nature increases from \[{{H}_{2}}O\] to\[{{H}_{2}}Te.\] The increase in acidic character of hydrides on moving down the group may be explained in terms of bond length of \[H-M\] bond, larger is bond-length, lesser is bond energy and thus easier is ionisation of \[H-M\] bond or easier is proton donor nature. Hence, \[{{H}_{2}}O<{{H}_{2}}S<{{H}_{2}}Se<{{H}_{2}}Te\]
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