Mn²⁺ compounds are more stable than Fe²⁺ compounds towards oxidation in their +3 state because :

1.	3d5 configuration is more stable than 3d6 configuration.
2.	3d6 configuration is more stable than 3d5 configuration.
3.	3p5 configuration is less stable than 3p6 configuration.
4.	3p6 configuration is less stable than 3p5 configuration.

The oxo metal anions of the 3d series in which the metal exhibits an oxidation state equal to its group number is /are -

1. ${\mathrm{VO}}_3^{-}$

2. ${\mathrm{CrO}}_4^{2-}$

3. ${\mathrm{MnO}}_4^{-}$

4. All of the above.

What is the electronic configuration of transition elements?

Give below are some atomic numbers:

29, 59, 74, 95, 102, 104
The atomic numbers of the inner transition elements among the above are :

The electronic configuration of the last element of actinoids is :

1. Thorium, Th: $\left[\mathrm{Rn}\right]5{\mathrm{f}}^{14}6{\mathrm{d}}^{1}7{\mathrm{s}}^2$

2. Lawrencium, Lr: $\left[\mathrm{Rn}\right]5{\mathrm{f}}^{14}6{\mathrm{d}}^{1}7{\mathrm{s}}^2$

3. Neptunium, Np: $\left[\mathrm{Rn}\right]5{\mathrm{f}}^{14}6{\mathrm{d}}^{1}7{\mathrm{s}}^2$

4. Protactinium, Pa: $\left[\mathrm{Rn}\right]5{\mathrm{f}}^{14}6{\mathrm{d}}^{1}7{\mathrm{s}}^2$

The correct statement regarding Ag is 

The enthalpy of atomization of transition metals is high due to :

1. High effective nuclear charge

2. A large number of valence electrons

3. Very strong metallic bonds

4. All of the above

The transition metals generally form coloured compounds due to :

Transition metals and their many compounds act as good catalysts due to :

Transition metals show paramagnetic behaviour due to: