Redox Reactions...

Out of the following, select species with different oxidation states of the underlined atoms.
$$I:CaO\underline { { Cl }_{ 2 } } $$;  

Bleaching powder ($$CaO{Cl}_{2}$$) has two types of chlorine atoms with oxidation number of $$+1$$ and $$-1$$. It can be represented as :

$${ Fe }^{ 2+ }$$ is oxidised by $$Mn{ O }_{ 4 }^{ - }$$ or $${ Cr }_{ 2 }{ O }_{ 7 }^{ 2- }$$ in acidic medium. What is new oxidation number of Fe?

Oxidation number of oxygen in superoxide ion, $${O}_{2}^{-}$$ is :

In $$\left[ Cr({ O }_{ 2 }){ \left( { NH }_{ 3 } \right)}_{ 4 }{ (H }_{ 2 }O) \right] { Cl }_{ 2 }$$, oxidation number of $$Cr$$ is $$+3$$ then, $${O}_{2}$$ will be in the form of :

What is the oxidation number of sulphur in $${ H }_{ 2 }{ S }_{ 2 }{ O }_{ 8 }$$?

Strongest conjugate base is :

When $${Cl}^{-}$$ is converted into $${Cl}_{2}$$, change in oxidation number is :

Prussian blue has two types of iron with oxidation number as shown below:
$$\overset { III }{ Fe } \left[ \overset { II }{ Fe } { \left( CN \right)  }_{ 6 } \right] $$
What is the net charge on prussian blue?

$${ H }_{ 2 }{ S }_{ 2 }{ O }_{ 8 }$$ and $${ H }_{ 2 }S{ O }_{ 5 }$$, both have $$+6$$ oxidation state of sulphur. It is due to the :