The compound AgF2 (unstable) acts as a/ an:
1. Oxidising agent.
2. Reducing agent.
3. Both oxidising and reducing agent.
4. Neither oxidising and reducing agent.
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 oxidation number of sulphur and nitrogen in H2SO5 and NO3- are respectively-
1. | +6, +5 | 2. | -6, -6 |
3. | +8, +6 | 4. | -8, -6 |
The correct statement(s) about the given reaction is -
\(\mathrm{{X} eO_{6 (aq)}^{4 -} + 2 F^{- 1}_{(aq)} + 6 H^{+}_{(aq )} \rightarrow}~\mathrm{{X} eO_{3 (g)} + {F}_{2 (g)} + 3 H_{2} O_{(l)}}\)
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.
Which element exhibits both positive and negative oxidation states?
1. Cs
2. Ne
3. I
4. F
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. \(\dfrac{1}{3}\) ; 4
2. 2.5 ; \(\dfrac{1}{3}\)
3. \(-\dfrac{1}{3}\) ; 2.5
4. 2.5 ; 3