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. \(\frac{1}{3}\) ; 4
2. 2.5 ; \(\frac{1}{3}\)
3. \(-\frac{1}{3}\) ; 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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MnO42- undergoes disproportionation reaction in acidic medium but MnO4- does not. It is:

1.  Due to the highest oxidation state of Mn in  MnO42-
2.  Due to the highest oxidation state of Mn in  MnO4-
3.  Due to the endothermic nature of the disproportionation reaction.
4.  Due to the exothermic nature of the disproportionation reaction.

Subtopic:  Introduction to Redox and Oxidation Number |
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The reaction that does not represent auto redox or disproportionation is: 

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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