Redox Reactions...

Balance the following equation and choose the quantity which is the sum of the coefficients of reactants and products:
             ......... $$ PtCl_4 $$ + ........... $$ XeF_4 \rightarrow PtF_{6} $$ +  ....$$ClF $$ + ....$$Xe $$ 

Oxidation number of carbon in $$CH_2Cl_2$$ is:

The value of coefficients to balance the following reaction are
$$Cr(OH)_3+ClO^-+OH^- \rightarrow CrO_4^{2-}+Cl^-+H_2O$$

Oxidation number of iodine in $$IO_3^-, IO_4^- , KI$$ and $$I_2$$ respectively is:

Oxidation state of Osmium (Os) in $$ \mathrm{OsO}_{4} $$ is

The reaction, $$ 3 \mathrm{ClO}^{-}(a q) \rightarrow $$ $$ \mathrm{ClO}_{3}^{-}(a q)+2 \mathrm{Cl}^{-}(a q) $$ is an example of

Oxidation number of sodium in sodium amalgam is

The oxidation number of phosphorus in $$ \mathrm{Ba}\left(\mathrm{H}_{2} \mathrm{PO}_{2}\right)_{2} \ \mathrm{is} $$

If a half cell reaction, $$ A+e^{-} \longrightarrow A^{-} $$ has a large negative reduction potential, it follows that

In which of the following pairs, there is the greatest difference in the oxidation number of the underlined elements?