The oxidation states of the central atom in the given species are, respectively:

H4P2O7  and H2S2O7

1. 0 and +6 2. +3 and +4
3. +4 and +2 4. +5 and +6
Subtopic:  Introduction to Redox and Oxidation Number |
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KI3, H2S4O6

The oxidation numbers of iodine and sulphur in the above compounds are, respectively:

1. \(\dfrac{1}{3}\) ; 4
2. 2.5 ; \(\dfrac{1}{3}\)
3. \(-\dfrac{1}{3}\) ; 2.5
4. 2.5 ; 3

Subtopic:  Introduction to Redox and Oxidation Number |
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The oxidation state of P in HPO32- is-

1. +3 2. +4
3. +2 4. +5
Subtopic:  Introduction to Redox and Oxidation Number |
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Why does the MnO₄²⁻ ion undergo disproportionation in an acidic medium, whereas the MnO₄⁻ ion does not?
1.  Due to manganese being in its highest oxidation state in MnO₄²⁻.
2.  Due to manganese being in its highest oxidation state in MnO₄⁻
3.  Because the disproportionation reaction of MnO₄²⁻ is endothermic.
4.  Because the disproportionation reaction of MnO₄²⁻ is exothermic.
Subtopic:  Introduction to Redox and Oxidation Number |
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Which of the following reactions does not involve disproportionation process?

1. Cl2+OH-Cl-+ClO3-+H2O

2. 2H2O2H2O+O2

3. 2Cu+Cu2++Cu

4. NH42Cr2O7N2+Cr2O3+4H2O

Subtopic:  Introduction to Redox and Oxidation Number |
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Assertion (A): In the presentation 
\( \mathrm{E}_{\mathrm{Fe}^{3+}}^{\ominus} /_{ \mathrm{Fe}^{2+}}\) \( \text { and } \mathrm{E}_{\mathrm{Cu}^{2+}}^{\ominus} / _{\mathrm{Cu}^{\prime}} \mathrm{Fe}^{3+} / \mathrm{Fe}^{2+} \) and\(\text { } \mathrm{Cu}^{2+} / \mathrm{Cu}\) are reodox couples.
Reason (R): A redox couple is the combination of the oxidised and reduced forms of a substance involved in an oxidation or reduction half cell.
 
1. Both (A) and (R) are True and (R) is the correct explanation of (A).
2. Both (A) and (R) are True but (R) is not the correct explanation of (A).
3. (A) is True but (R) is False.
4. (A) is False but (R) is True.
Subtopic:  Introduction to Redox and Oxidation Number |
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The oxidation number of sulphur and nitrogen in H2SO5 and NO3- are respectively-

1. +6, +5 2. -6, -6
3. +8, +6 4. -8, -6
Subtopic:  Introduction to Redox and Oxidation Number |
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Which of the following reactions does not represent a redox change?

1. CaCO3 CaO + CO2

2. 2H2 + O2 2H2O

3. Na + H2 NaOH + \(\frac{1}{2}\)H2

4. MnCl3  MnCl2 + \(\frac{1}{2}\)Cl2

Subtopic:  Introduction to Redox and Oxidation Number |
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Fluorine reacts with ice as per the following reaction

H2O(s) + F2(g) → HF(g) + HOF(g)

This reaction is a redox reaction because-

1. F2 is getting oxidized. 2. F2 is getting reduced.
3. Both (1) and (2) 

4. None of the above.
Subtopic:  Introduction to Redox and Oxidation Number |
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Which element exhibits both positive and negative oxidation states?
1. Cs
2. Ne
3. I
4. F

Subtopic:  Introduction to Redox and Oxidation Number |
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