Question

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Answer 1

The answer is: The electronic configuration of Nitrogen is $1s^22s^22p^3$.

Electronic configuration: The electronic configuration is defined as the distribution of electrons of an atom in the atomic or molecular orbitals and is written using the labels for the subshell.

How to decide which orbital is filled first?

• The order in which electrons are filled in atomic orbitals as:

(Shown in image)

• Just follow the arrows to select the orbitals, s orbital can have 2 electrons, p can have 6 electrons, d can have 10 electrons and f can 14 electrons.

• The electronic configuration in which the outer shell is completely filled is known as noble-gas configuration as they are similar to electronic configurations of noble gases.
• Now, the given element is nitrogen ($N$). The atomic number of Nitrogen is 7. Thus, these 7 electrons are filled as-

         $1s^22s^22p^3$

• Therefore, the electronic configuration of Nitrogen is $1s^22s^22p^3$.

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Answer 2

Nitrogen's complete electron configuration is 12s2s22p3.

The shorthand electron configuration for noble gases is [He] 2s22p3. Nitrogen has an atomic number of 7. The nitrogen atoms' nucleus contain this many protons. An atom that is neutral has an equal number of protons and electrons. Thus, the ground state electron configuration will consist of 7 electrons in the suitable s and p orbitals (state of lowest energy). For nitrogen, the entire electron configuration is 1s22s22p. Scientists may easily express and explain how the electrons are organized around the nitrogen atom's nucleus by using the configuration notation for nitrogen (N). As a result, it is simpler to comprehend and forecast how atoms will cooperate to form chemical bonds.

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