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The element is darmstadtium (Ds), which has 110 electrons.

Assumption- All the electrons are put into the shells one by one and electron-electron interaction is neglected.

An atom is a particle of a substance that specifically defines an achemical element. An atom consists of a central nucleus usually surrounded by one or more electrons.

The electronic state is defined by the configuration of the electron system, as well as the quantum numbers of each electron that contribute to that configuration. Each electronic state corresponds to one of the molecular energy levels

Using the concept of the electron states, the values of the electrons are to be accommodated in each shell with the different quantum numbers ranging from 1,2,3,4,5, and other higher orders. Thus, the order of the subshells is named as s,p,d,f,g, and to the higher values.

Formula:

The number of electron states presents in the shell for each given value of is,

$N=2n^2$ 鈥�.. (1)

If ignore the electron-electron interaction, the element notation with electrons using equation (1). Thus, the two electrons are in the n=1 shell, eight electrons in the shell, in the n=2 shell 18, in the n=3 shell 32, and the n=4 remaining 50(=110-2-8-18-32) in the n=5 shell. The electrons would be placed in the subshells in the order according to the concept and thus the resulting configuration is

$5s^{2}5p^{6}5d^{10}5f^{14}5g^{18}$.

Hence, the spectroscopic notation for the quantum number of the last electron would be g.

However, for considering the electron-electron interaction, the ground-state electronic configuration of the element is $\left[Rn\right]5f^{14}6d^{9}7s^1$.

Where $\left[Rn\right]:1s^{2}2s^{2}3s^{2}3p^{6}3d^{1}04s^{2}4p^{6}4d^{10}4f^{14}5s^{2}5p^{6}5d^{10}6s^{2}6p^6$represents the inner-shell electrons.