The oxidation states of the central atom in the given species are, respectively:
1. | 0 and +6 | 2. | +3 and +4 |
3. | +4 and +2 | 4. | +5 and +6 |
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
undergoes disproportionation reaction in acidic medium but 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. |
The reaction that does not represent auto redox or disproportionation is:
1.
2.
3.
4.
Which of the following reactions does not represent a redox change?
1. CaCO3 CaO + CO2
2. 2H2 + O2 2H2O
3. Na + H2O NaOH + \(\frac{1}{2}\)H2
4. MnCl3 MnCl2 + \(\frac{1}{2}\)Cl2
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. |
The formulas for the following compounds are:
(a) Mercury(II) chloride and (b) Thallium(I) sulphate
1. HgCl2, Tl2SO4
2. Hg2Cl2, Tl2SO4
3. HgCl2, TlSO4
4. HgCl2, Tl3SO4
The correct statement(s) about the given reaction is -
1. oxidises F-
2. The oxidation number of F increases from -1 to zero
3. is a stronger oxidizing agent that
4. All of the above.