Neon Electron Configuration with Full Orbital Diagram

Neon electron configuration is 1s2 2s2 2p6. The symbol for neon is ‘Ne’. The electron configuration of neon shows that neon is an inert element and the period of neon is 2. Neon electron configuration with an orbital diagram is the main topic of this article.

The tenth element in the periodic table is neon. The atomic number of neon is ten and, the total number of electrons in the neon atom is 10. These electrons are arranged according to specific rules of different orbits. The position of the electrons in different energy levels of the atom and the orbital in a certain order is called electron configuration.

Electron configuration is done in 2 ways of all the elements of the periodic table. That’s why neon electron configuration can be done in 2 ways.

  1. Electron configuration through orbit.
  2. Electron configuration through orbital.

Neon 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. These orbits are expressed by n. [ n = 1,2 3 4 . . .]

K is the name of the first orbit, L is the second, M is the third, N is the name of the fourth orbit. The electron holding capacity of each orbit is 2n2. [Where, n = 1,2 3,4. . .]

Now,
n = 1 for K orbit.
The electron holding capacity of K orbit is 2n2 = 2 × 12 = 2 electrons.

For L orbit, n = 2.
The electron holding capacity of the L orbit is 2n2 = 2 × 22 = 8 electrons.

neon electron configuration

n=3 for M orbit.
The maximum electron holding capacity in M orbit is 2n2 = 2 × 3= 18 electrons.

n=4 for N orbit.
The maximum electron holding capacity in N orbit is 2n2 = 2 × 32 = 32 electrons.

The atomic number is the number of electrons in that element. The atomic number of neon is ten. That is, the number of electrons in neon is 10.

Therefore, the maximum electron holding capacity in the first orbit is two. And the maximum electron holding capacity in the second orbit is eight. In the electron configuration of neon, The total number of electrons in a neon atom is ten.

Therefore, the two electrons of neon will be in the first orbit. And the other eight electrons will be in the second orbit. The order of electron configuration of neon atom through orbits is 2, 8. Therefore, neon has electrons per shell 2, 8.

The electron configuration of Neon atom through orbital

Atomic energy levels are subdivided into sub-energy levels. These sub-energy levels are called orbital. The sub energy levels are expressed by ‘l’. The value of ‘l’ is from 0 to (n – 1). The sub-energy levels are known as s, p, d, f.

Determining the value of ‘l’ for different energy levels is-

If n = 1,
(n – 1) = (1–1) = 0
Therefore, the orbital number of ‘l’ is 1; And the orbital is 1 s.

If n = 2,
(n – 1) = (2–1) = 1.
Therefore, the orbital number of ‘l’ is 2; And the orbital is 2s, 2p.

If n = 3,
(n – 1) = (3–1) = 2.
Therefore, the orbital number of ‘l’ is 3; And the orbital is 3s, 3p, 3d.

If n = 4,
(n – 1) = (4–1) = 3
Therefore, the orbital number of ‘l’ is 4; And the orbital is 4s, 4p, 4d, 4f.

If n = 5,
(n – 1) = (n – 5) = 4.

neon electron configuration
Neon Electron Configuration

Therefore, l = 0,1,2,3,4. The number of orbitals will be 5 but 4s, 4p, 4d, 4f in these four orbitals it is possible to arrange the electrons of all the elements of the periodic table. The electron holding capacity of these orbitals is s = 2, p = 6, d = 10 and f = 14.

Neon electron configuration in the Aufbau principle

The German physicist Aufbau first proposed the idea of electron configuration through sub-orbits. The Aufbau method is to do electron configuration through the sub-energy level. These sub-orbitals are expressed by ‘l’. 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. These orbitals are named s, p, d, f. The electron holding capacity of these orbitals is s = 2, p = 6, d = 10 and f = 14. 

The Aufbau electron configuration method is 1 s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d. The neon electron configuration in the Aufbau principle is 1s2 2s2 2p6.

The electron configuration of Neon in Hund principle

The German physicist Friedrich Hund provided a guideline for the entry of electrons into different orbitals of equal power. Which is known as the Hund principle. The Hund principle is that when electrons enter the orbitals of equal power, the electrons will randomly enter the orbital as long as the orbital is empty. And the spin of these unpaired electrons will be one-sided.  In Hund principle, the neon electron configuration is 1s2 2s2 2p6. The last orbit of neon is always full of eight electrons. From the electron configuration of neon, it is seen that neon has no unpaired electrons.

Determination of group and period through the neon electron configuration

The neon electron configuration is 1s2 2s2 2p6. The last orbit of an element is the period of that element. The electron configuration of neon atom shows that the last orbit of the neon atom is 2(2s 2p). So, the period of neon is 2.

On the other hand, the number of electrons present in the last orbit of an element is the number of groups in that element. But in the case of p-block elements, group diagnosis is different. To determine the group of p-block elements, the group has to be determined by adding 10 to the total number of electrons in the last orbit.

The total number of electrons in the last orbit of the neon atom is eight. That is, the group number of neon is 8 + 10 = 18. Therefore, we can say that the period of the neon element is 2 and the group is 18.

Determining the block of neon by electron configuration

The elements in the periodic table are divided into 4 blocks based on the electron configuration of the element. The block of elements is determined based on the electron configuration of the element. If the last electron enters the p-orbital after the electron configuration of the element, then that element is called the p-block element.

The neon electron configuration is 1s2 2s2 2p6. The electron configuration of neon(Ne) shows that the last electron of neon enters the p-orbital. Therefore, neon is the p-block element.

Determination of the valency(valence) and valence electrons of neon

The ability of one atom of an element to join another atom during the formation of a molecule is called valency(valence) .

The number of unpaired electrons in the last orbit of an element is the valency(valence) of that element. The electron configuration of neon 1s2 2s2 2p6. The electron configuration of neon(Ne) shows that neon is an inert element. There are eight electrons in the last orbit of a neon atom. The neon atom has no unpaired electrons. Therefore, the valency of the neon(Ne) atom is 0.

valence electrons of neon
Valence Electrons of Neon

Again, the number of electrons in the last orbit of an element, the number of those electrons is the valence electrons of that element. In the electron configuration for neon, we see that 8 electrons exist in the last orbit of the neon. Therefore, the valence electrons of the neon are 8. Finally, we can say that the valency (valence) of the neon is 0, and the valence electrons of the neon are 8.

Reasons for placing neon in group-18 of the periodic table

Neon electron configuration is 1s2 2s2 2p6. The electron configuration of neon shows that the number of electrons in the last orbit of the neon atom is 8. We know that the number of electrons in the last orbit of an element is the number of groups in that element. Accordingly, the group of neon is ten but neon is an inert element. All inert elements are placed in group number 18 in the periodic table. Therefore, neon is placed in group-18 instead of group-10.

Why is neon an inert gas?

The elements in group-18 of the periodic table are inert gases. The inert gases of Group-18 are helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn). We know that the element in group-18 is neon(Ne). The electron configuration of neon shows that the orbit at the end of neon is filled with electrons. Neon does not want to exchange or share any electrons because the last orbit of neon is full of electrons.

And neon 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.

Properties of Neon Atoms

  • The atomic number of neon atoms is ten. The atomic number of an element is the number of electrons and protons in that element. That is, the number of electrons and protons in the neon atom is ten.
  • The active atomic mass of the neon atom is 20.1797.
  • Neon is a inert element.
  • The valency(valence) of a neon atom is zero and the valence electrons of a neon atom are 8.
  • Neon atoms are the 2nd period of the periodic table and an element of the 18-group.
  • The electron configuration of neon ends in a p-orbital. Therefore, it is a p-block element.
  • The melting point of a neon atom is 24.56 K ​(−248.59 °C, ​−415.46 °F) and the boiling point is 27.104 K ​(−246.046 °C, ​−410.883 °F).
  • The value electronegativity of neon atoms is 0.
  • The oxidation state of neon is 0.
  • Neon atom van der Waals radius is 154 pm.
  • Ionization energies of neon atoms are 1st: 2080.7 kJ/mol, 2nd: 3952.3 kJ/mol, 3rd: 6122 kJ/mol.
  • The covalent radius of the neon atom is 58 pm.
  • Neon atoms do not participate in any chemical reaction.
  • The atomic radius of the neon atom is 38pm.
  • Neon is normally in the form of gas.

Conclusion of Neon Electron configuration

The tenth element of the periodic table is neon. Which is an inert gas. The atomic number of an element is the number of electrons in that element. Therefore, the number of electrons in the neon are ten. Neon electron configuration is 1s2 2s2 2p.  The main topic of this article is the neon electron configuration with orbital diagrams. Neon is the 2nd period of the periodic table and the group-18 element. Electron configuration of neon atoms , period and group , valence and valence electrons, properties of neon are discussed in this article.

FAQ of Neon Electron configuration

How do you write the electron configuration for neon?
Ans: Neon Electron configuration is Ne(10) = 1s2 2s2 2p6.

How many electron does neon have?
Ans: Ten electrons.

What is electron configuration of neon 10?
Ans: electron configuration of neon 10 is 1s2 2s2 2p6.

How many valence electron in Neon?
Ans: Eight valence electrons.

What is the symbol for neon?
Ans: The symbol for neon is ‘Ne’.

References

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