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**Hint:**The maximum number of electrons that can be accommodated in a shell is given by the formula ${ 2n }^{ 2 }$, where n denotes the shell number.

**Complete answer:**

As we know,

For l = ${ 0 }$, s subshell = 2 electrons

For l = ${ 1 }$, p subshell = 6 electrons

For l = ${ 2 }$, d subshell = 10 electrons

For l = ${ 3 }$, f subshell = 14 electrons and so on.

So, For n = ${ 2 }$, The values of l will be ${ n-1 }$ = ${ 2-1 }$ = 1 and 0.

It means that the second shell has only s and p- orbitals and there is no d-orbital present.

Hence, the maximum number of electrons that can be present in ${ 2d }$ orbitals is X, then X is 0.

This is a hypothetical condition.

**Additional Information:**

A quantum number portrays the energies of electrons in particles. Every quantum number indicates the estimation of a saved amount in the elements of the quantum framework.

The principal quantum number (n): It tells us about the size of the orbital.

The angular quantum number (l): It tells us about the shape of the orbital.

The magnetic quantum number (m): It tells us about the orientation in space of a particular orbital.

The spin quantum number (s) is a value (of $\dfrac { 1 }{ 2 } $): It tells us about the angular momentum of an electron.

**Note:**The possibility to make a mistake is that you in d-orbital there are ${ 10 }$ electrons present but in reality, ${ 2d }$ doesn’t exist in nature, so the number of electrons present will be zero, not ${ 10 }$.

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