How do you write the noble gas electron configuration for manganese?

Hint:To write the noble gas electron configuration for manganese we need to know what is meant by noble gas configuration. A noble gas configuration of an atom comprises the elemental symbol of the last noble gas which is present prior to that atom, then which is followed by the configuration of the remaining electrons. The elements that are found in the last column of the periodic table are called the noble gases which comprises helium, neon, argon, krypton, xenon, and radon.

Complete answer:
We know that Atomic number of manganese is $25$.
Hence, ${Z_{manganese}} = 25$
The noble gas nearest to manganese is Argon which has $18$ electrons hence there is no need to specify the configuration.
Therefore, ${Z_{\arg on}} = 18$
The electronic configuration of argon is given by;
$1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}$
Hence for manganese the electronic configuration is given by;
$1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^5}4{s^2}$
So the noble gas configuration for manganese is given by
$[Ar]3{d^5}4{s^2}$

Note: The noble gas configuration system allows some shortening of the total electron configuration by using the symbol for the noble gas of the previous period as part of the pattern of electrons. We must be careful in knowing the difference between noble gas electron configuration and electron configuration. By electron configuration we mean the organization of electrons within energy levels and orbitals. In simple words noble gas electron configuration, we write the symbol of noble gases followed by the configuration of the remaining electrons whereas if the question is to write the electronic configuration, we simply write the configuration of all the electrons without mentioning the noble gases.