The oxidation number of the atom (in bold) in the following species is given. Identify, which one is incorrectly related?

1. \(\mathbf{Cu}_{2} O\) is \(- 1\)

2. \(\mathbf{Cl} O_{3}^{-}\) is \(+ 5\)

3. \(K_{2} \mathbf{Cr}_{2} O_{7}\) is \(+ 6\)

4. \(H \mathbf{Au} Cl_{4}\) is \(+ 3\)

$\mathrm{}$

In the given reaction, what is the name of the species that bleaches the substances due to its oxidising action?

Cl₂(g) + 2OH^-(aq) → ClO^-(aq) + Cl^-(aq) + H₂O(l)

1. ClO^- 

2. Cl₂

3. Cl^-

4. Both ClO^- and Cl^-

${\mathrm{MnO}}_4^{2-}$ undergoes disproportionation reaction in acidic medium but ${\mathrm{MnO}}_4^{-}$ does not. It is:

Nitric acid reacts with PbO but does not react with PbO₂ , because -

1. PbO is a base while PbO₂ is a strong oxidizing reagent

2. PbO is a base while PbO₂ is a weak oxidizing reagent

3. PbO is neutral while PbO₂ is a strong oxidizing reagent

4. PbO is acid while PbO₂ is a strong oxidizing reagent

The oxidation state of P in ${\mathrm{HPO}}_3^{2-}$ is-

The oxidation state of two S-atoms in ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3$ is -

1. +2 and +4

2. +3 and -2

3. +4 and -2

4. +6 and -2

Among the following, identify the species with an atom in +6 oxidation state-

1. MnO₄^-

2. Cr(CN)₆^3-

3. NiF₆^2-

4. CrO₂Cl₂

Which of the following does not represent a redox reaction?

1. Cr₂O₇^2- + 2OH^- $\to$CrO₄^2- + H₂O

2. SO₄^2- + 2I^- + 2H⁺ $\to$I₂ + H₂S + H₂O

3. Ca + 2H₂O → Ca(OH)₂ + H₂

4. PCl₅ $\to$PCl₃ + Cl₂

The oxidation number of phosphorous in ATP (adenosine triphosphate) is -

Based on standard electrode potentials given above, the correct arrangement for increasing order of reducing power of
elements is: