Transition metals show variable oxidation states due to tendency of ‘d’ as well as ‘s’ electrons to take part In bond formation:- Why do actinoids,in general, exhibit a greater range of oxidatln states than the lanthanoids?

Transition metals show variable oxidation states due to tendency of ‘d’ as well as ‘s’ electrons to take part In bond formation:- Which element in the first series of transition elements does not exhibit variable oxidation states and why?

The actinoids exhibit more number of oxidation states in general than the lanthanoids. This is because

Transition elements generally have high enthalpy of atomisation and they show variable oxidation states Which element of the 3d series shows the largest number of oxidation states? Explain the reason for it.

Transition elements generally have high enthalpy of atomisation and they show variable oxidation states Why do transition elements exhibit higher enthalpies of atomisation?

The outer most subshell electronic configuration of an element is 3d^54s^2 : This element shos variable oxidation state. Why?

The outer most subshell electronic configuration of an element is 3d^(5)4s^2 . (d) This element shows variable oxidation state. Why?

Transition elements are d-block elements, with some exceptions. Usually they are paramagnetic. They show variable oxidation states. They and their compounds show catalytic property Zn (atomic number 30) is not a transition element, though it is a d-block element. Why?