Question

What is the electronic configuration of nitrogen in ground state?

Answer 1

Hint: We also remember that the atomic number of the atom is equal to the number of protons or the number of electrons. In every atom the number of protons and the number of electrons are equal. The electrons in the atom are filled by the lower energy level to the higher energy level. In modern periodic table elements are arranged in the table depending on the atomic number. In this way only periods and rows are arranged in the modern periodic table.

Complete step by step answer:
We must know that the atomic number of nitrogen is \[{\text{ 7 }}\] and the total number of electrons is\[7\]and the symbol of nitrogen is \[{\text{N}}\]. In this seven electrons, first two electrons are going to filled in the first energy level \[1{s^2}\], remaining five electron are going to filled in the second energy level, in these five electrons two electrons are going to filled in \[2{s^2}\] and three electrons are filled each electron in \[2p_x^12p_y^12p_z^1\].
According to Pauli principle, Aufbau principle and Hund’s rule, the electronic configuration of nitrogen in ground state is \[1{s^2},2{s^2}2p_x^12p_y^12p_z^1\].

Note: We have to remember that the number of electrons in the atom is equal to the atomic number of the atom. The electron fills in the atomic orbital of the atom. The electron filling in the atomic orbital is followed by the three important principles. There are Pauli exclusion principle, Aufbau principle and Hund’s rule. In Aufbau principle, the electrons are filled in the orbital in the order of increasing the energy level of the orbital. First lower energy orbital filled followed by higher energy orbital are filled. In Pauli principle, no two electrons in the same orbital have the same quantum number. In Hund’s rule, the orbital must have more multiplicity than the pairing effect. Electrons are filled each electron in one orbital in the same energy level then it goes to a pair of electrons in the orbital.