(i) Electronic configuration

The general electronic configuration for lanthanoids and actinoids  is  ns² (n-1)d^0-1 (n-2)f^1-14

Lanthanoids has 4f and actinoids has 5f, unlike 4f orbitals, the 5f orbitals are not deeply buried and participate in bonding to a greater extent.

(ii) Oxidation states

The principal oxidation state of lanthanoids is (+3). However, sometimes we also

encounter oxidation states of + 2 and + 4. This is because of the extra stability of fully-filled

and half-filled orbitals. Actinoids exhibit a greater range of oxidation states. This is because

the 5f, 6d, and 7s levels are of comparable energies. Again, (+3) is the principal oxidation

state for actinoids. Actinoids such as lanthanoids have more compounds in +3 state than

in +4 state.

(iii). Chemical reactivity

In the lanthanide series, the earlier members of the series are more reactive. They have reactivity that is comparable to Ca. With an increase in the atomic number, the lanthanides start behaving similarly to Al.

Actinoids, on the other hand, are highly reactive metals, especially when they are finely divided. When they are added to boiling water, they give a mixture of oxide and hydride.

Actinoids combine with most of the non-metals at moderate temperatures.

Alkalies have no action on these actinoids. In the case of acids, they are slightly affected by nitric acid (because of the formation of a protective oxide layer).