Question

What is the abbreviated electron configuration of $Sn$ ?

Answer 1

Hint :We know that to answer this question the information of tin atomic number must be known. The tin has an atomic number of $50,$ which means tin has $50$ electrons. Thus, Aufbau’s principle will be utilized to solve the question.

Complete Step By Step Answer:
The electronic configuration can be described via Aufbau’s principle. This principle states that the electrons of an atom or ions, that are in ground state, For example, the electrons first enter to $1sthen2sthen2p,3s,3p,4s,3d$ . The atom or ions are most stable when the s, p, d, f orbital are fully or half filled with electrons.
Thus, tin $(Sn)$ has an atomic number $50.$ It means it has $50$ electrons. Tin $(Sn)$ has an atomic number 50. Here, as the electron of tin reaches and fulfill the vacant orbitals it would be filling the vacant orbitals it would be $1s,2s,2p,3s,3p,4s,3d,4p,5s,4dand5p$ orbitals.
The noble gas Krypton has an electron configuration of $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d105p^2$
So we can replace this portion of tin's electron configuration with the noble gas notation $\left[Kr\right]$
 $\therefore \left[Kr\right]=5s^{2}4d^{10}5p^2.$
Therefore, the abbreviated electron configuration of $Sn$ is $5s^{2}4d^{10}5p^2$ .

Note :
Aufbau’s principle describes the manner of electrons filled in an atomic orbital of an atom in the ground state configuration. The principle stated that, based on the energy level of atomic orbital electron fills happen. The electron fills to the respective atomic orbital happens with the fact that lowest energy orbitals are first occupied by electrons, if they are completely filled then in the higher energy level orbitals start to be occupied by electrons.