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

The +2 oxidation state becomes more stable in the first half of the first-row transition elements with increasing atomic number because:

1. s-orbital is becoming more and more half-filled.

2. f-orbital is becoming more and more half-filled.

3. d-orbital is becoming more and more half-filled.

4. p-orbital is becoming more and more half-filled.

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.

The d-block elements that may not be regarded as transition elements are :

What is the electronic configuration of transition elements?

The "Disproportionation" reaction means that :

In the 3d series, a metal with a +1 oxidation state is:

The number of unpaired electrons in the gaseous ions ${\mathrm{Mn}}^{3+},$ ${\mathrm{Cr}}^{3+},$ ${\mathrm{V}}^{3+,}$ $\mathrm{and}$ ${\mathrm{Ti}}^{3+ }$ are, respectively:

The number of 3d electrons in the Cr³⁺ ions will be:

The correct statement regarding Ag is