Complete Electron Configuration for Xenon (Xe)
Xenon is the 54th element in the periodic table and its symbol is ‘Xe’. Xenon is a classified noble gas. In this article, I have discussed in detail how to easily write the complete electron configuration of xenon.
What is the electron configuration of xenon?
The total number of electrons in xenon is fiftyfour. These electrons are arranged according to specific rules in different orbitals.
The arrangement of electrons in xenon in specific rules in different orbits and orbitals is called the electron configuration of xenon.
The electron configuration of xenon is [Kr] 4d^{10} 5s^{2} 5p^{6}, if the electron arrangement is through orbitals. Electron configuration can be done in two ways.
 Electron configuration through orbit (Bohr principle)
 Electron configuration through orbital (Aufbau principle)
Electron configuration through orbitals follows different principles. For example Aufbau principle, Hund’s principle, and Pauli’s exclusion principle.
Xenon atom electron configuration through orbit
Scientist Niels Bohr was the first to give an idea of the atom’s orbit. He provided a model of the atom in 1913. The complete idea of the orbit is given there.
The electrons of the atom revolve around the nucleus in a certain circular path. These circular paths are called orbit(shell). These orbits are expressed by n. [n = 1,2,3,4 . . . The serial number of the orbit]
K is the name of the first orbit, L is the second, M is the third, and N is the name of the fourth orbit. The electron holding capacity of each orbit is 2n^{2}.
Shell Number (n)  Shell Name  Electrons Holding Capacity (2n^{2}) 
1  K  2 
2  L  8 
3  M  18 
4  N  32 
For example,
 n = 1 for K orbit.
The maximum electron holding capacity in K orbit is 2n^{2} = 2 × 1^{2} = 2.  For L orbit, n = 2.
The maximum electron holding capacity in L orbit is 2n^{2} = 2 × 2^{2} = 8.  n=3 for M orbit.
The maximum electron holding capacity in M orbit is 2n^{2} = 2 × 3^{2 }= 18.  n=4 for N orbit.
The maximum electron holding capacity in N orbit is 2n^{2} = 2 × 4^{2} = 32.
Therefore, the maximum electron holding capacity in the first shell is two, the second shell is eight and the 3rd shell can have a maximum of eighteen electrons. The atomic number is the number of electrons in that element.
The atomic number of xenon is 54. That is, the number of electrons in xenon is fiftyfour. Therefore, a xenon atom will have two electrons in the first shell, eight in the 2nd orbit, and eighteen electrons in the 3rd shell.
According to Bohr’s formula, the fourth shell will have twentysix electrons but the fourth shell of xenon will have eighteen electrons and the remaining eight electrons will be in the fifth shell.
Therefore, the order of the number of electrons in each shell of the xenon(Xe) atom is 2, 8, 18, 18, 8. Electrons can be arranged correctly through orbits from elements 1 to 18.
The electron configuration of an element with an atomic number greater than 18 cannot be properly determined according to the Bohr atomic model. The electron configuration of all the elements can be done through the orbital diagram.
Electron configuration of xenon through orbital
Atomic energy shells are subdivided into subenergy levels. These subenergy levels are also called orbital. The most probable region of electron rotation around the nucleus is called the orbital.
The subenergy levels depend on the azimuthal quantum number. It is expressed by ‘l’. The value of ‘l’ is from 0 to (n – 1). The subenergy levels are known as s, p, d, and f.
Orbit Number  Value of ‘l’  Number of subshells  Number of orbital  Subshell name  Electrons holding capacity  Electron configuration 
1  0  1  1  1s  2  1s^{2} 
2  0 1  2  1 3  2s 2p  2 6  2s^{2} 2p^{6} 
3  0 1 2  3  1 3 5  3s 3p 3d  2 6 10  3s^{2} 3p^{6} 3d^{10} 
4  0 1 2 3  4  1 3 5 7  4s 4p 4d 4f  2 6 10 14  4s^{2} 4p^{6} 4d^{10} 4f^{14} 
For example,
 If n = 1,
(n – 1) = (1–1) = 0
Therefore, the value of ‘l’ is 0. So, the subenergy level is 1s.  If n = 2,
(n – 1) = (2–1) = 1.
Therefore, the value of ‘l’ is 0, 1. So, the subenergy levels are 2s, and 2p.  If n = 3,
(n – 1) = (3–1) = 2.
Therefore, the value of ‘l’ is 0, 1, 2. So, the subenergy levels are 3s, 3p, and 3d.  If n = 4,
(n – 1) = (4–1) = 3
Therefore, the value of ‘l’ is 0, 1, 2, 3. So, the subenergy levels are 4s, 4p, 4d, and 4f.  If n = 5,
(n – 1) = (n – 5) = 4.
Therefore, l = 0,1,2,3,4. The number of subshells will be 5 but 4s, 4p, 4d, and 4f in these four subshells it is possible to arrange the electrons of all the elements of the periodic table.
Subshell name  Name source  Value of ‘l’  Value of ‘m’ (0 to ± l)  Number of orbital (2l+1)  Electrons holding capacity 2(2l+1) 
s  Sharp  0  0  1  2 
p  Principal  1  −1, 0, +1  3  6 
d  Diffuse  2  −2, −1, 0, +1, +2  5  10 
f  Fundamental  3  −3, −2, −1, 0, +1, +2, +3  7  14 
The orbital number of the ssubshell is one, three in the psubshell, five in the dsubshell and seven in the fsubshell. Each orbital can have a maximum of two electrons.
The subenergy level ‘s’ can hold a maximum of two electrons, ‘p’ can hold a maximum of six electrons, ‘d’ can hold a maximum of ten electrons, and ‘f’ can hold a maximum of fourteen electrons.
Aufbau is a German word, which means building up. The main proponents of this principle are scientists Niels Bohr and Pauli. The Aufbau method is to do electron configuration through the subenergy level.
The Aufbau principle is that the electrons present in the atom will first complete the lowest energy orbital and then gradually continue to complete the higher energy orbital.
The energy of an orbital is calculated from the value of the principal quantum number ‘n’ and the azimuthal quantum number ‘l’. The orbital for which the value of (n + l) is lower is the low energy orbital and the electron will enter that orbital first.
Orbital  Orbit (n)  Azimuthal quantum number (l)  Orbital energy (n + l) 
3d  3  2  5 
4s  4  0  4 
Here, the energy of 4s orbital is less than that of 3d. So, the electron will enter the 4s orbital first and enter the 3d orbital when the 4s orbital is full. The method of entering electrons into orbitals through the Aufbau principle is 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d.
The first two electrons of xenon enter the 1s orbital. The sorbital can have a maximum of two electrons. Therefore, the next two electrons enter the 2s orbital.
The porbital can have a maximum of six electrons. So, the next six electrons enter the 2p orbital. The second orbit is now full. So, the remaining electrons will enter the third orbit.
Then two electrons will enter the 3s orbital and the next six electrons will be in the 3p orbital of the third orbit. The 3p orbital is now full of electrons. So, the next two electrons will enter the 4s orbital and ten electrons will enter the 3d orbital.
Then the next six electrons enter the 4p orbital. The 4p orbital is now full. So, the next two electrons will enter the 5s orbital and the next ten electrons will enter the 4d orbital.
The 4d orbital is now full. So, the remaining six electrons enter the 5p orbital. Therefore, the xenon complete electron configuration will be 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{10} 4s^{2} 4p^{6} 4d^{10} 5s^{2} 5p^{6}.
Note: The unabbreviated electron configuration of xenon is [Kr] 4d^{10} 5s^{2} 5p^{6}. When writing an electron configuration, you have to write serially.
Video for writing the electron configuration for Xenon (Xe)
Why is xenon an inert gas?
The groundstate electron configuration of xenon is 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{10} 4s^{2} 4p^{6} 4d^{10} 5s^{2} 5p^{6}.
This electron configuration shows that the last shell of xenon has eight electrons. Therefore, the valence electrons of xenon are eight. The elements in group18 of the periodic table are inert gases.
The inert gases of Group18 are helium(He), neon(Ne), argon(Ar), krypton(Kr), xenon(Xe), and radon(Rn). We know that the element in group18 is xenon. The electron configuration shows that the orbit at the end of the xenon atom is filled with electrons.
Xenon does not want to exchange or share any electrons because the last orbit is full of electrons. And xenon does not form any compounds because it does not share any electrons. They do not participate in chemical bonding and chemical reactions.
For this, they are called inert elements. The inert elements are in the form of gases at normal temperatures. For this inert elements are called inert gases. Again for this same reason, inert gas is called a noble gas.
FAQs

What is the symbol for xenon?
Ans: The symbol for xenon is ‘Xe’.

How many electrons does xenon have?
Ans: 54 electrons.

How do you write the full electron configuration for xenon?
Ans: 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{10} 4s^{2} 4p^{6} 4d^{10} 5s^{2} 5p^{6}.

How many valence electrons does xenon have?
Ans: Eight valence electrons.

What is the valency of xenon?
Ans: The valency of xenon is 0.