Identify the correct statement (s) in relation to the following reaction.
$$\mathrm{Zn}+2 \mathrm{HCl} \longrightarrow \mathrm{ZnCl}_2+\mathrm{H}_2$$
The exhibition of various oxidation states by an element is also related to the outer orbital electronic configuration of its atom. Atom (s) having which of the following outermost electronic configurations will exhibit more than one oxidation state in its compounds.
Identify the correct statements with reference to the given reaction
$$\mathrm{P}_4+3 \mathrm{OH}^{-}+3 \mathrm{H}_2 \mathrm{O} \longrightarrow \mathrm{PH}_3+3 \mathrm{H}_2 \mathrm{PO}_2^{-}$$
Which of the following electrodes will act as anodes, which connected to Standard Hydrogen Electrode ?
The reaction $\mathrm{Cl}_2(g)+2 \mathrm{OH}^{-}(a q) \rightarrow \mathrm{ClO}^{-}(a q)+\mathrm{Cl}^{-}(a q)+\mathrm{H}_2 \mathrm{O}(l)$ represents the process of bleaching. Identify and name the species that bleaches the substances due to its oxidising action.
$$\mathop {C{l_2}}\limits^0 (g) + \mathop {2O{H^ - }}\limits^{ - 2\,\,\, + 1} (aq) \to \mathop {Cl{O^ - }}\limits^{ + 1\,\,\, - 2} (aq) + \mathop {C{l^ - }}\limits^{ - 1} (aq) + \mathop {{H_2}O}\limits^{ + 1\,\,\,\, - 2} (l)$$
In this reaction, $\mathrm{O} . \mathrm{N}$. of Cl increases from $0\left(\right.$ in $\left.\mathrm{Cl}_2\right)$ to 1 (in $\left.\mathrm{ClO}^{-}\right)$as well as decreases from 0 (in $\mathrm{Cl}_2$ ) to -1 (in $\mathrm{Cl}^{-}$). So, it acts both reducing as well as oxidising agent. This is an example of disproportionation reaction. In this reaction, $\mathrm{ClO}^{-}$species bleaches the substances due to its oxidising action. [In hypochlorite ion $\left(\mathrm{ClO}^{-}\right) \mathrm{Cl}$ can decrease its oxidation number from +1 to 0 or -1 .]