Question

Write Some Similarities And Differences Between Lanthanide And Actinide.

Answer 1

Hint :The f-block consists of elements in which the 4f and 5f orbitals are gradually filled. These elements are technically members of group 3, although they are represented independently in the periodic table as the f-block. Inner transition elements are also known as f-block elements.

Complete Step By Step Answer:
The element is considered to belong to the first series of inner transition elements when differentiating electrons enter one of the 4f orbitals. This series includes fourteen elements following lanthanum (La). These are known as lanthanides or lanthanoids because they appear in the periodic table just after lanthanum. Despite the fact that lanthanum has no 4f electrons, it is frequently included in lanthanides since it closely resembles lanthanoids. Actinides or actinides are electrons generated by successively filling 5f orbitals. They get their name from the fact that they follow actinium (Ac) in the periodic table. The actinide series, which includes 14 elements ranging from Th(90) to Lw(103), is also known as the second inner transition series. Despite the fact that actinium (Z=89) has no 5f electrons, it is common to investigate actinium using actinoids.
Difference-

Lanthanides	Actinides
The last electron enters a 4f orbital	The last electron enters a 5f orbital.
Electronic setup in general $ 4{f^{0 - 14}}5{d^{0 - 1}}6{s^2} $	Electronic setup in general $ \;5{f^{0 - 14}}6{d^{0 - 17}}{s^2} $
The atomic size drop is not as regular as the size decline of tripositive ions ( $ L{n^{3 + }} $ ).	The atomic and ionic (tripositive ion) sizes are gradually shrinking.
They don't readily form complexes.	They have a far higher proclivity for forming complexes.
Their compounds have a lower level of basicity.	Their compounds are highly basic.
Except for promethium, none of these elements are radioactive.	All of them are radioactive.

Similarities
The lanthanides and actinides are both classified as inner transition metals.
(ii) They both have 14 elements in common.
(iii) Both demonstrate radii shrinkage.
(iv) Both have a predominantly +3 oxidation state and are electropositive and highly reactive.

Note :
Transition elements are unusual in that they may contain an interior subshell that is incomplete, allowing valence electrons to be deposited in a shell other than the one on the exterior. The outer shell of certain elements contains exclusively valence electrons. It allows for the formation of transition metals in a variety of oxidation states.