- 1(current)
Q. No.
Consider the following data
Eo Cl2/Cl– = +1.36, Eo I2/I– =+ 0.53, Eo Ag+ /Ag = +0.79, Eo Na+/Na = –2.71 and Li+ /Li is – 3.04.
Arrange the following ionic species in decreasing order of reducing strength:
I–, Ag, Cl–, Li, Na.
1. Li > Na > I– > Ag > Cl–
2. Cl– > Na > I– > Ag > Li
3. Li < Na < I– < Ag < Cl–
4. Li > Na = I– > Ag > Cl–
KO2 is paramagnetic in nature ,It is because -
1. K+ ion contains unpaired electron
2. \(O_{2}^{2-}\) ion contains unpaired electron
3. \(O_{2}^{-}\) ion contains unpaired electron in \( \pi^{*}\) MO
4. \(O_{2}^{-}\) ion contains unpaired electron in \( \pi\) MO
The solubility of alkaline earth metal hydroxides in water increases down the group because-
| 1. | Down the group both lattice and hydration energy increase. |
| 2. | Down the group lattice energy increases and hydration energy decreases |
| 3. | Down the group lattice enthalpy decreases much more than the hydration enthalpy |
| 4. | None of the above |
The correct statement above the following is -
| 1. | The solubility of alkaline earth metal carbonates and sulphates in water decrease down the group |
| 2. | The solubility of alkaline earth metal carbonates increase and sulphates in water decrease down the group |
| 3. | The solubility of alkaline earth metal carbonates decreases and sulphates in water increases down the group |
| 4. | The solubility of alkaline earth metal carbonates and sulphates in water increases down the group |
- 1(current)
Q. No.
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