Oxidation
Reduction
dissociation
ionisation
`HNO_3`
`K_2Cr_2O_7`
`KMnO_4`
All of these
ionisation
oxidation
reduction
nuclear reaction
I and IV
II and Ill
Only I
Only IV
`I^(-) > Cl^(-) > Br^(-)`
`Cl^(-) > Br^(-) > I^(-)`
`I^(-) > Br^(-) > Cl^(-)`
`Br^(-) > I^(-) > Cl^(-)`
Oxidation
reduction
autoxidation
None of these
increases the oxidation number of an element in a given substance
decreases the oxidation number of an element in a given substance
is oxidised itself in an oxidation reduction reaction
loses electrons in an oxidation reduction reaction
only I
only II
Both I and II
Neither I nor II
water is oxidised
silver is oxidised
silver is reduced
it is not a redox reaction
`HNO_3`
`H_2S`
`H_2SO_3`
`SnCl_2`
`NaNO_2`
`NaNO_3`
`HI`
`SnCl_2`
`Na`
`Ca`
`Sr`
`Ba`
`F^-`
`Cl^-`
`Br^-`
`F`
It is redox reaction
Metallic iron is a reducing agent
`Fe^(3+)` is an oxidising agent
Metallic iron is reduced to `Fe^(3+)`
`AsH_3`
`BiH_3`
`NH_3`
`PH_3`
accept electrons
donate electrons
accept protons
donate protons
`CuO + H_2 rightarrow Cu + H_2O`
`Fe_2O_3 + 3CO rightarrow2Fe+ 3CO_2`
`2K+ F_2rightarrow 2KF`
`BaCl_2+ H_SO_4 rightarrow BaSO_4 + 2HCl`
bromine is oxidised and carbonate is reduced
bromine is the both reduced and oxidised
bromine is neither reduced nor oxidised
bromine is reduced and water is oxidised
Cu is more easily reduced than Ag
Ag is more easily reduced than Cu
nitrate ion acts as an oxidising agent
nitrate ion acts as a reducing agent
(This question may have multiple correct answers)
`Br_2`
`Br^-`
`H^+`
`Cr_2O_7^(2-)`
Both the statements are true and Statement II is the correct explanation of Statement I
Both the statements are true but Statement II is not the correct explanation of Statement I.
Statement I is true, but Statement II is false
Statement I is false, but Statement II is true.
(This question may have multiple correct answers)
Column I | Column II | ||
---|---|---|---|
(A) | Ions having positive charge | (1) | +7 |
(B) | The sum of oxidation number of all atoms in a neutral molecule | (2) | -1 |
(C) | Oxidation number of hydrogen ion `(H^(+))` | (3) | +1 |
(D) | Oxidation number of fluorine in NaF | (4) | 0 |
(E) | Ions having negative charge | (5) | Cation |
`quad` | `quad` | (6) | Anion |
`+2`
`0`
`+4`
`-8`
`0`
`-2`
`+2`
`-6`
-1
+1
-2
None of these
`H_2O_2`
`OF_2`
`H_2O`
`SO_2`
`CrO_2^(-) ; ClO_3^(-); CrO_4^(2-);. MnO_4^(-)`
`ClO_3^(-), CrO_4^(2-); MnO_4^(-), CrO_2^(-)`
`CrO_2^(-), ClO_3^(-), MnO_4^(-), CrO_4^(2-)`
`CrO_4^(2-), MnO_4^(-), CrO_2^(-). ClO_3^(-)`
`-1/2`
`-1`
`-2`
`0`
+2
+1
+3
+4
-3 and +5
+3 and -5
-3 and +3
-5 and +5
Column I | Column II | ||
---|---|---|---|
(A) | `Cr_2O_7^(2-)` | (P) | `+3` |
(B) | `MnO_4^(-)` | (Q) | `+4` |
(C) | `VO_3^(-)` | (R) | `+5` |
(D) | `FeF_6^(3-)` | (S) | `+6` |
`quad` | `quad` | (T) | `+7` |
+5 to -2
+6 to +2
+7 to +2
+7 to +3
`XY_1Z_2`
`X_2 (YZ_3)_2`
`X_3 (YZ_4)_2`
`X_3 (Y_4 Z)_2`
The oxidation number of hydrogen is always+ 1
The algebraic sum of all the oxidation numbers in a compound is zero
An element in the free or the uncombined state bears oxidation number zero
In all its compounds, the oxidation number of fluorine is -1
+8
-6
+6
+4
+2
+3
`8/3`
`2/3`
Oxidation state of bromine varies from -1 to +6
Among `IO_4^- , ClO_4^-` and `BrO_4^-` the last one `(BrO_4^-)` is the strongest oxidising agent
`HNO_3` is an oxidising agent
All of the above
Both the statements are true and Statement II is the correct explanation of Statement I
Both the statements are true but Statement II is not the correct explanation of Statement I.
Statement I is true, but Statement II is false
Statement I is false, but Statement II is true.
List I (The atom for which the oxidation state is to the found ) | List II(Oxidation state) | ||
---|---|---|---|
(A) | Oxygen in `BaO_2` | (1) | `-1` |
(B) | Sulphur in `S_2O_6^(2-)` | (2) | `0` |
(C) | Carbon in `C_(12) H_(22) O_(11)` | (3) | `+7` |
(D) | Manganese in `MnO_4^-` | (4) | `-2` |
(5) | `5` |
`A →1 , B → 4, C → 2 , D → 3`
`A →1 , B → 5, C → 2 , D → 3`
`A →4 , B → 1, C → 2 , D → 3`
`A →4 , B → 5, C → 3 , D → 1`
zinc cannot displace `Cu` from `CuSO_4`
`Cu` cannot displace `Fe` from `FeSO_4`
`Zn` metal displaces `H_2` gas from `H_2SO_4`
All of the above
dissolved and blue colour is discharged
dissolved but blue colour is not discharged
not dissolved and blue colour is not discharged
not dissolved but blue colour is discharged
`Cu > Mg > Zn > Na`
`Na > Zn > Mg > Cu`
`Cu > Zn > Mg > Na`
`Na > Mg > Zn > Cu`
External source of voltage is applied to carry the chemical reaction
These cells are mainly used in laboratory and chemical industry
These cells consist of two copper strips dipped in and aqueous solution of `CuSO_4`
None of the above
Mercury
Copper
Silver
Tin
It fastly coast the surfaces of metallic object
Its examples are - Rusting of iron tamishing of silver
II does not cause damage to buildings, ship made metals especially that are made up of iron
All of the above
nitrate coating on silver
sulphide coating on silver
chloride coating on silver
oxide coating on silver
I and II
I and III
II and III
III and IV
annealing
roasting
galvanisation
smelting
oxygen forms a protective oxide layer
it is a noble metal
iron undergoes reaction easily with water
iron forms ions
`A > B > C`
`A < C > B`
`C > B > A`
`B > C > A`
Column I | Column II | ||
---|---|---|---|
(A) | Lectanche cell | (1) | Cell reaction `2H_2O+O_2 → 2H_2O` |
(B) | Ni - Cd- Cell | (2) | Does not involve any ion in solution and is used in hearing aids . |
(C) | Fuel cell | (3) | Rechargeable |
(D) | Mercury cell | (4) | Reaction at anode `Zn → Zn^(2+) +2 e^-` |
(5) | Converts energy of combustion in to electrical energy |
`A →1 , B → 2, C → 3 , 4 , D → 5`
`A → 5 , B → 2 , C → 1, 3 , D → 4`
`A → 2 , B → 3 , C → 1, 5 , D → 4`
`A → 4 , B → 3 , C → 1, 5 , D → 2`