Question

The electronic configuration of the element M is $[Ar]3{d^{10}}4{s^2}4{p^3}$. Then M belongs to
(A) V B Group
(B) VIII Group
(C) V A Group
(D) 0 Group

Answer 1

From the electronic configuration of the element M, belongs to p block element. p-block elements will have electronic configuration $n{s^2}n{p^{0 - 6}}$. The element can belong to any of the groups from Group VA to Group VIIIA. Use the clue that that number of valence electrons decides the group.

Complete Solution :
- First, what is an electronic configuration? Electronic configuration is the arrangement or distribution of the electrons present in an atom or molecules in the atomic or molecular orbital. There are three rules for filling of the electrons in the orbitals. Those rules are Pauli’s exclusion principle, Hund’s rule and Aufbau’s principle.
- The electronic configuration of the element M is $[Ar]3{d^{10}}4{s^2}4{p^3}$. The element M is filled in these orbitals by following all the three rules. For the element M, the outermost orbital is 4p. Hence the element M belongs to the p block element. Therefore, M can belong to any of the groups from Group IIIA to Group VIIIA.
- When we see the element, M = $[Ar]3{d^{10}}4{s^2}4{p^3}$, we can understand that it belongs to period 4 of the periodic table. The outer electronic configuration of M is $4{s^2}4{p^3}$ similar to the form $n{s^2}n{p^3}$. The $n{s^2}n{p^3}$ is the general electronic configuration of the element of Group V A. So, the element, thus belongs to Group V A.

So, the correct answer is “Option B”.

Additional Information:
Characteristics of p-block element:
- When the last electron of an atom is present in the p-orbital, it comes under the p-block element.
- There are three p-orbitals present and it can accommodate a total of six electrons.
- The outer electronic configuration of the p-block element is $n{s^2}n{p^{0 - 6}}$.
- The groups belonging to p-block are group 13 to 18.
- Boron, Carbon, Nitrogen, Oxygen, Fluorine and Helium head those groups.

Note: Electrons will follow three rules while filling the orbital.

These three rules are:
- Pauling’s exclusion principle:
According to this principle, no two electrons in an orbital will have all four quantum numbers equal.
- Hund’s rule:
Hund’s rule states that every orbital in the subshells should be singly filled, before doubly filled. All the singly filled electrons should have the same spin.
- Aufbau’s principle:
According to Aufbau’s principle, filling of the electron in the orbital of an atom takes place according to the increasing energy of their orbitals.