How do you draw the electron configuration diagram for manganese?

Hint: Manganese is the element of group 7 of the d-block and its atomic number is 25 so, there are 25 electrons in the atom. Arrange these 25 electrons in the increasing order of the energy of the shell, since it is a d-block element, its last electron should come in the d-subshell. Now form a chart having all subshells and fill them accordingly.

Complete answer:
There are various shells in the atoms which are denoted by K, L, M, N, etc, which represents the specific energy of the shell. The shell K represents 1, the shell L represents 2, the shell M represents 3, the shell N represents 4. Each shell has specific sub-shells which are s, p, d, f, etc.
The K shell has one sub-shell (s), the L shell has two sub-shells (s, p), the M shell has three sub-shells (s, p, d), the N shell has four sub-shells (s, p, d, f).
Manganese is the element of group 7 of the d-block and its atomic number is 25 so, there are 25 electrons in the atom. Arrange these 25 electrons in the increasing order of the energy of the shell, since it is a d-block element, its last electron should come in the d-subshell.
The electronic configuration will be:
$1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{6}}4{{s}^{2}}3{{d}^{5}}$
Now, forming the chart in which all the subshells are present and the electrons are filled according to the configuration given above:



Note:
It must be noted that in the 3-d sub-shell all the orbitals have only one electron because the pairing cannot be done; all the orbitals get one electron each. This is the basis of Hund’s rule.