Statement-I: $∆_{f}^{0} H of H_{2} O and H_{2} S$ is negative
Statement-II: ${TeO}_{2}$ is an oxidizing agent

A
Both statements-I and II are correct
B
Statement-I is correct and statement-II is incorrect
C
Statement-I is incorrect and statement-II is correct
D
Both statements-I and II are incorrect

Solution:

I) Thermal stability of $H_{2} O > H_{2} S > H_{2} Se > H_{2} Te > H_{2} Po .$

$∆_{f}^{0} H of H_{2} O and H_{2} S$ is negative indicating their high thermal stability.

II) ${TeO}_{2} ({Te}^{+ 4})$ is an oxidizing agent because ${Te}^{+ 4}$ has a great tendency to reduce to ${Te}^{+ 2}$ .

Down the group lower oxidation states become stable.

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