Question

What atom could have the electron configuration of $1{s^2}2{s^2}2{p^3}$?

Answer 1

Hint : The organization of electrons in energy levels around an atomic nucleus is known as electronic configuration or electronic structure. The electron-containing atomic subshells (with the number of electrons they possess written in superscript) are arranged in a series in the normal notation for atom electron configurations.

Complete Step By Step Answer:
The number of electrons in each shell, starting with the first, can be used to express an atom's electronic structure in the shell atomic model.
Each shell is made up of one or more subshells, each of which is made up of atomic orbitals. For eg, the first (K) shell has one subshell, 1s; the second (L) shell has two subshells, 2s and 2p; the third shell has 3s, 3p, and 3d; the fourth shell has 4s, 4p, 4d, and 4f; and the fifth shell has 5s, 5p, 5d, and 5f and can potentially keep more in the 5g subshell that is not occupied in any known element's ground-state electron configuration.
In the electron configuration mentioned in the question that is $1{s^2}2{s^2}2{p^3}$, we have $2$ electrons in $1s$ shell, $2$electrons in $2s$shell and $3$electrons in $2p$shell. So, the total number of electrons in the atom is
$= 2 + 2 + 3 \\\ = 7 \\\$
Now, The element with $7$ electrons is Nitrogen (According to the periodic table).
Hence, Nitrogen is the atom that could have the electron configuration of $1{s^2}2{s^2}2{p^3}$.

Note :
The periodic table divides atoms into blocks that conform to the filling of the ns, np, nd, and nf orbitals, resulting in distinct chemical properties for the elements in the s, p, d, and f blocks, respectively.