How does electron configuration relate to the periodic table?

Hint: Electronic configuration was utilized to group components with similar valence electrons together. They likewise will, in general, have similar properties

Complete step by step answer:
For simple clarification, I will discuss just a delegate element for example,
\[11Na:\] \[1{s^2}2{s^2}2{p^6}3{s^1}\]
\[19K:\] \[1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}4{s^1}\]
You can see that \[Na\] and \[K\] were in a similar group on the grounds that their valence electron was in s orbital and just has \[1\] electron.
So in the event that you do electron configuration with column \[2\] of the periodic table you will likewise get 2 valence electrons in s orbital for \[Mg\] and \[Ca\] and so forth.
The association of electrons in molecules clarifies the shape of the periodic table as well as the way that elements in a similar column of the periodic table have comparative chemistry.
A similar idea applies to different sections of the periodic table. Elements in every column have a similar valence shell electron configuration, and the elements have some comparative chemical properties.

Note:
This is carefully valid for all elements in the s and p blocks. In the d and f blocks, on the grounds that there are special cases for the request for filling of subshells with electrons, comparable valence shells are not absolute in these blocks. Nonetheless, many similarities do exist in these blocks, so similarity in chemical properties is expected.
Similarly of valence shell electron configuration infers that we can decide the electron configuration of an atom exclusively by its situation on the periodic table
The electrons in the outermost or valence shell are particularly significant in light of the fact that they can participate in the sharing and that is responsible for chemical reactions.