Justify that the following reaction is redox reaction; identify the species oxidized/reduced, Which acts as an oxidant and which acts as a reductant?

$2{\mathrm{Cu}}_2\mathrm{O}\left(\mathrm{s}\right) +{\mathrm{Cu}}_2\mathrm{S}\left(\mathrm{s}\right)\to 6\mathrm{Cu}\left(\mathrm{s}\right) + {\mathrm{SO}}_2\left(\mathrm{g}\right)$

Justify that the following reactions are redox reaction; identify the species oxidised/reduced, Which acts as an oxidant and which act as a reductant.

Justify that the following reactions are redox reaction; identify the species oxidized/reduced, Which acts as an oxidant and which act as a reductant?

${\mathrm{I}}_2\left(\mathrm{aq}\right)+2{\mathrm{S}}_2{{\mathrm{O}}_3}^{2⊝}\left(\mathrm{aq}\right)\underset{}{\to } {\mathrm{S}}_4{\mathrm{O}}_6^{2-} \left(\mathrm{aq}\right)+2{\mathrm{I}}^{⊝}\left(\mathrm{aq}\right)$

What is oxidation? Which one of the following pairs of species is in its oxidized state?

$$\begin{gathered} \mathrm{a}. \mathrm{Mg}/{\mathrm{Mg}}^{2\oplus } \mathrm{b}. \mathrm{Cu}/{\mathrm{Cu}}^{2\oplus } \\ \mathrm{c}. {\mathrm{O}}_2/{\mathrm{O}}^{2⊝} \mathrm{d}. {\mathrm{Cl}}_2/{\mathrm{Cl}}^{⊝} \end{gathered}$$

Justify the following reaction as redox reaction.

$2\mathrm{Na}\left(\mathrm{s}\right) + \mathrm{S}\left(\mathrm{s}\right) \to {\mathrm{Na}}_2\mathrm{S}\left(\mathrm{s}\right)$

Find out the oxidizing and reducing agents.

Assign oxidation number to each atom in the following species : 

$\mathrm{Cr}(\mathrm{OH}{{)}_4}^{⊝}$

Assign oxidation number to each atom in the following species : 

Assign oxidation number to each atom in the following species : 

${\mathrm{H}}_3{\mathrm{BO}}_3$