| Direction (11 - 13): The hydrides of oxygen family are : \[{{H}_{2}}O\], \[{{H}_{2}}S\], \[{{H}_{2}}Se\], \[{{H}_{2}}Te\] and \[{{H}_{2}}Po\]. The acidic nature, thermal stability and reducing character of these hydrides depend on the strength of M-H bond. Smaller the size of central atom (M), greater is the strength of M-H bond. These hydrides are angular, involves \[s{{p}^{3}}\] hybridisation and their comparative bond angle depends upon the repulsions between the bond pairs. |
A) \[{{H}_{2}}Te\]
B) \[{{H}_{2}}Se\]
C) \[{{H}_{2}}O\]
D) \[{{H}_{2}}S\]
Correct Answer: A
Solution :
\[{{H}_{2}}Te\] is the most acidic because HTe bond can break most readily due to maximum bond length value.
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