Question

How does the electronic configuration of an atom relate to its position in the modern periodic table?​

Answer 1

Answer:

the no. of valence electrons in the outermost shell decide it's place in which group it should be.

for eg there is 1 valence electron in the elements of group one.

Answer 2

Answer

In the modern periodic table, the electronic configuration can be used to determine the position of the element.

The number of shells the atom has, determines the period of the element in the modern periodic table.

Ex :- Na = 2, 8, 1 has 3 shells, so it belongs to the 3rd period of modern periodic table

The electronic configuration(spdf configuration) helps in determining the group of the element in the modern periodic table.

For s block elements, the group is equal to the number of their outermost electrons.

Example, Li = 2, 1

Its spdf configuration would be = 1s2 2s1

It belongs to s block, hence its group number = number of thier outermost electrons = 1

For p block, its group number is equal to (10 + number of electrons in their outermost shell)

Example, C = 2, 4

Its spdf configuration would be = 1s2 2s2 2p2

It belongs to p block, hence its group number = 10 + number of electrons in their outermost shell = 10 + 4 = 14

For d block, the group number is equal to number of electrons in (n - 1) d subshell + number of electrons in n s subshell

(n = number of shells)

Example, Fe = 2, 8, 14, 2

Its spdf configuration = 1s2 2s2 2p6 3s2 3p6 4s2 3d6

Here, n = 4 so n - 1 = 3

number of electrons in 3d subshell = 6

number of electrns in 4s subshell = 2

So group = 6 + 2