What is the relationship between the electronic configuration of elements and their position in the periodic table? Explain with examples.

Hint: At the point when components are submitted at the request of their expanding nuclear number, the components having a similar number of valence shell electrons are rehashed in such a manner, in order to fall under a similar gathering. Since the electronic arrangement of the valence shell electrons is the same they show comparable properties.

Complete step by step solution: At the point when components are organized by their atomic number, there is a periodicity in the properties of components. The oddities found in Mendeleev's occasional table were taken out. The isotopes were given positions. The atomic weights are arranged altogether.
The electronic setup of components and their situation in the occasional table are identified with one another. From the electronic setup of components, we can decide the period and gathering to which the components have a place. Think about sodium with nuclear number 11. K, L, and M shells have 2, 8, and 1 electron each. Since there are 3 head energy levels, sodium has a place in the third period. M shell (valence shell) has just 1 electron. So sodium has a place with bunch 1 or IA. Presently think about chlorine with nuclear number 17. K, L, and M shells have 2,8 and 7 electrons each. Since there are 3 head energy levels, chlorine has a place in the third period. M shell (valence shell) has 7 electrons. So, chlorine has a place with bunch 7.

Note: A table of the chemical components orchestrated arranged by atomic number, ordinarily in rows, so components with comparative nuclear structure (and consequently comparative compound properties) show up in vertical columns.