Neon (Ne) Electron Configuration

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Orbit Electron Configuration of Neon (Ne) atom is two electrons in first orbit (K) and 8 electrons in second orbit (L)

Orbital Electron Configuration of Neon (Ne) atom is 1s2 2s2 2p6 which means Neon atom have two electrons inside 1s orbital, two electron in 2s orbital and 6 electrons in 2p orbitals

Also we can replace 1s2 with [He], therefore electron configuration of Neon (Ne) is [He] 2s2 2p6

Ne is the symbol for the element Neon, which is located at second place from top of group 18 of periodic table. Neon have total of ten electrons in its atomic structure. Name neon is derived from Greek word neos which means new

Although Neon is fifth most abundant element in the universe. But in the Earth’s atmosphere it’s concentration is just 18 parts per million.

Due to very low concentration of Neon in the air, its extremely hard to extract and isolate it from air.

Most common process to isolate it is Fractional Distillation which involves warming up air under controlled environment, even through this process almost 40,000 kg of air need to be processed to just extract 0.5 kg of Neon.

Neon is not reactive at all and it barely react with any other element that too under extreme conditions like really high temperature. Due to it’s inertness, its mostly found in elemental form in the universe.

Existence of Neon was discovered by British chemists Sir William Ramsay and Morris W. Travers in 1898.
Most common uses of Neon are
– In discharge tubes

– Fluorescent bulbs for advertisement display purposes

– Neon lamps are used in botanical gardens and in greenhouses as they stimulate growth and are effective in the formation of chlorophyll, a compound which helps plants to absorb energy

– Neon is also used in voltage regulators and indicators

– Light emitted from ionised neon can pass through water fog that’s why it is used in cold regions and in airports

Talking about physical properties of Neon, in both liquid and gaseous form is colourless, odourless and non-combustible. Under low pressure if neon gas is electrified then it glows reddish-orange.

There are three common stable isotopes of Neon
20Ne (neon-20)
21Ne (neon-21)
22Ne (neon-22)
Amongst all of these 20Ne is most abundant.

Electron configuration refers to the arrangement of electrons in different orbits and orbitals of an atom in a certain order. Depending upon whether electrons are being arranged in Orbits or Orbitals there are two types of electron configurations – Orbit Electron Configuration and Orbital Electron Configuration.

In this article, I’ve discussed both Orbit and Orbital Electron Configurations of Neon (Ne) atom.

How do you write the electron configuration for Neon?

Neon atom in total have ten electrons, to write down the electron configuration of Neon, the first two electrons would go into the 1s orbital. Because the 1s orbital can only accommodate two electrons, next two electrons are placed in the 2s orbital. The remaining six electrons would go in the 2p subshell orbitals. Putting all this together, electron configuration of Neon is 1s2 2s2 2p6. Which can also be written as [He] 2s2 2p6 where [He] represents electron configuration of noble gas Helium.

Electron configuration of elements whose atomic number is more than 10 but less than 18 is usually written as [Ne] ………..

Orbit Electron Configuration of Neon (Ne)

Niels Bohr, a Danish scientist, was the first to propose the concept of an orbit around an atom. In 1913, he presented a model of the atom to the scientific community. As per this model, the electrons in an atom follow a set path as they go around the nucleus in circular motion.

These set paths are called “Orbits” and are numbered as 1, 2, 3, ……… depending upon their closeness to nucleus of atom. So first circular path around nucleus is numbered as 1, second as 2 and so no. Moreover orbits are also denoted by English letters.

  • First orbit – K and have n = 1
  • Second orbit – L and have n = 2
  • Third orbit – M and have n = 3
  • Fourth orbit – N and have n = 4
  • and so on.

How many electrons any of these orbits can hold is determined by using formula 2n2 where n is number of orbit. Based upon this formula, different orbits in the atom can hold electrons as following.

  • First orbit – K (n = 1) can hold 2n2 = 2 (1)2 = 2 electrons
  • Second orbit – L and have n = 2 can hold 2n2 = 2 (2)2 = 2 (4) = 8 electrons
  • Third orbit – M and have n = 3 can hold 2n2 = 2 (3)2 = 2 (9) = 18 electrons
  • Fourth orbit – N and have n = 4 can hold 2n2 = 2 (4)2 = 2 (16) = 32 electrons
  • and so on.

As Neon atom have ten electrons, therefore it’s Orbit Electron Configuration will be two electrons in K orbit and eight electrons in L orbit.

Electron Configuration of Neon (Ne) Atom showing 2 electrons in K shell and 8 electrons in L shell

How many electron shells does Neon have?

Neon have electron configuration 2, 8 which means it have 2 electrons in K shell and 8 electrons in L shell. Therefore Neon have 2 electron shells.

Does Neon have a full valence shell?

Neon has electron configuration 2, 8 which means it have 2 electrons in K shell and 8 electrons in L shell. Valence shell is most outermost shell, so in case of Neon L is valence shell. As maximum capacity of L shell is to just accomodate 8 electrons. Therefore neon have a full valence shell.

How many electrons does Neon have in K shell?

2 electrons

How many electrons does Neon have in L shell?

8 electrons

Orbital Electron Configuration of Neon (Ne)

Niels Bohr proposed the idea that electrons revolve around nucleus in specific circular paths called Orbits, but later on Heisenberg found out that it’s impossible to determine position and velocity of an electron inside the atom at same time, so how it’s possible that electrons do circular motion on specific paths in an atom.

In later years, Erwin Schrodinger developed a mathematical formula to compute the probability of finding the location of an electron inside an atom.

On the basis of this probability, the location of an electron inside an atom could be represented as the chances of that electron being located in a certain three-dimensional area surrounding the nucleus.

As 3D region can be explained only using 3 parameters, therefore in order to describe where an electron is? inside the atom.

We need three numbers – Principle Quantum Number (n), Angular Momentum Number (l) and Magnetic Momentum Number (m).

Therefore Orbits(this concept was proposed by Neils Bohr) are further divided into sub-energy levels called subshells. How many subshells an orbit have is equal to Principle Quantum Number (n) of orbit.

Therefore

  • First Orbit (K and n = 1) have 1 subshell
  • Second Orbit (L and n = 2) have 2 subshell
  • Third Orbit (M and n = 3) have 3 subshell
  • Fourth Orbit (N and n = 4) have 4 subshell

These sub-energy levels/subshells have specific regions where probability of finding electrons is maximum. These subshells are names as s, p, d, f and have angular momentum numbers as 0, 1, 2 and 3 respectively.

Which type of subshell an orbit have can be determined using Angular Momentum Number (I).
So
If Principle Quantum Number of an orbit is n
Then subshells in that orbit are 0 to (n – 1)

If
Angular Momentum Number(l) = 0 that means it’s s orbital
Angular Momentum Number(l) = 1 that means it’s p orbital
Angular Momentum Number(l) = 2 that means it’s d orbital
Angular Momentum Number(l) = 3 that means it’s f orbital

First Orbit (K and n = 1)
Angular Momentum Number (l) = 0 to (1 – 1) = 0 (0 to 0)
Which means first orbit just have one subshell which is s

Second Orbit (L and n = 2)
Angular Momentum Number (l) = 0 to (2 – 1) = 1 (0 to 1)
Which means second orbit have two subshells which are s and p

Third Orbit (M and n = 3)
Angular Momentum Number (l) = 0 to (3 – 1) = 2 (0 to 2)
Which means third orbit have three subshells (0, 1, 2) which are s, p and d

Fourth Orbit (N and n = 4)
Angular Momentum Number (l) = 0 to (4 – 1) = 3 (0 to 3)
Which means fourth orbit have four subshells (0, 1, 2, 3) which are s, p, d and f

OrbitPrinciple Quantum NumberNumber of SubshellsSubshells
First Orbit (K)n = 111s
Second Orbit (L)n = 222s
2p
Third Orbit (M)n = 333s
3p
3d
Fourth Orbit (N)n = 444s
4p
4d
4f

These s, p, d and f subshells further have subregions which are called Orbitals, orbitals are just regions inside a subshell where probability of existence of an electron is quite high.

How many orbitals a subshell have depends upon it’s Angular Momentum Number (l) and can be calculated using formula.
Number of orbitals in a subshell = 2l + 1 where I is Angular Momentum Number of a subshell.

Therefore
s subshell (Angular Momentum Number l = 0)
Number of orbitals = 2(0) + 1 = 1
So s subshell just have one orbital

p subshell (Angular Momentum Number l = 1)
Number of orbitals = 2(1) + 1 = 3
So p subshell have three orbitals

d subshell (Angular Momentum Number l = 2)
Number of orbitals = 2(2) + 1 = 4 + 1 = 5
so d subshell have five orbitals

f subshell (Angular Momentum Number l = 3)
Number of orbitals = 2(3) + 1 = 6 + 1 = 7
so f subshell have seven orbitals

Moreover electron holding capacity of a subshell can be calculated using formula
Number of electrons which a subshell can hold = 2(2I + 1) where I is Angular Momentum Number of subshell

Therefore
s subshell (Angular Momentum Number l = 0)
Number of electrons it can hold = 2(2(0) + 1) = 2(1) = 2
So s subshell can hold maximum two electrons

p subshell (Angular Momentum Number l = 1)
Number of electrons it can hold = 2(2(1) + 1) = 2(3) = 6
So p subshell can hold maximum six electrons

d subshell (Angular Momentum Number l = 2)
Number of electrons it can hold = 2(2(2) + 1) = 2(4 + 1) = 2(5) = 10
so d subshell can hold maximum ten electrons

f subshell (Angular Momentum Number l = 3)
Number of electrons it can hold = 2(2(3) + 1) = 2(6 + 1) = 2(7) = 14
so f subshell can hold maximum fourteen electrons

SubshellAngular Momentum Number (I)Number of Orbitals in
Subshell (2l + 1)
Maximum Electrons Subshell can hold 2(2l + 1)
s012
p136
d2510
f3714

Summarising all this we can write energy levels in an atom as

1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f 5g

But next question which arises is “in which order these orbitals should be filled in to figure out electron configuration of an atom?”.

Like should 2 electrons be filled in 1s orbital first or 3p orbital first???

Well answer to this question is Aufbau Principle.

According to the Aufbau Principle, in the ground state of an ion or an atom, electrons first occupy the atomic orbitals of lowest energy levels before filling up in higher energy levels. What this indicates is that the orbital with the lower energy will be filled first, followed by the orbital with the greater energy.

As per this principle energy of any orbital depends upon sum of Principle Quantum Number (n) and Angular Quantum Number (l).
Therefore
Energy of Orbital = n + l

So lower the value of n + l is lower its energy.

OrbitalnIEnergy (n + l)
1s101
2s202
2p213
3s303
3p314
3d326
4s404
4p415
4d426
4f437

From the above table its clear that 4s have less energy than 3d, so it should be filled first.
Based upon the energies of orbitals as per Aufbau Principle, order of filling of orbitals is 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p 8s and so on.

It’s tricky to remember what’s order of filling of orbitals as per Aufbau Principle, so you can use below diagram for easily filling up orbitals. Just follow the arrows from top right corner to bottom left corner diagonally.

Order of filling orbitals in an atom as per Aufbau Principle
Aufbau Principle Filling Of Orbitals Order

Order of filling of orbitals as per Aufbau Principle is 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p 8s and so on.

As Neon atom have ten electrons, therefore it’s electron configuration is 1s2 2s2 2p6. Which means Neon atom have 2 electrons each in its 1s, 2s orbitals and 6 electrons in 2p orbitals.

Electron Configuration of Neon (Ne) Atom showing 1s2 2s2 2p6
NeonElectron Configuration
1s2 2s2 2p6

How many orbitals are in Neon Atom?

Electron Configuration of neon atom is 1s2 2s2 2p6 which means
Neon Atom have
– 2 electrons in 1s subshell
– 2 electrons in 2s subshell
– 6 electrons in 2p subshell

1s subshell have just one orbital
2s subshell also just have one orbital
2p subshell have 3 orbitals

So in total nitrogen atom 1 + 1 + 3 = 5 orbitals

Therefore Neon atom have 5 orbitals.

Valence Electrons of Neon (Ne)

Number of electrons in the last orbit of an element’s atom are called valence electrons.

As Neon have electron configuration 1s2 2s2 2p6 so it’s last orbit is 2 (L shell which have Principle Quantum Number n = 2), as last orbit of Neon have 8 electrons (2 in 2s and 6 in 2p subshell), therefore number of valence electrons in Neon is eight.

Neon (Ne)8 valence electron

How many Valence Electrons does Neon have?

Neon have 8 valence electrons as it’s Orbital Electron Configuration is 1s2 2s2 2p6. As electron configuration shows, neon have 8 valence electrons located in 2s and 2p subshells.

How many electrons does Neon require to reach an octet in it’s valence shell?

Electron configuration of Neon is 2, 8 which means it have 2 electrons in K shell and 8 electrons in L shell. As maximum capacity of L shell is to accomodate just 8 electrons and in case of Neon atom this shell already have 8 electrons. Therefore L shell is already full and it is an octet (as there are 8 electrons in L shell that’s why its called Octet).

Therefore in order to reach an octet in it’s valence shell Neon does not need to gain any electrons.

Valency of Neon (N)

Valency refers to the ability of an element to combine with other elements. Valencies are same throughout the periodic table for elements that are located in the same group. 

Which means valency is same for all of Group 1 elements (K, Na etc. have valency = 1), Group 2 elements (Ca, Mg etc. have valency = 2) and so on for other groups in the periodic table. Also valency depends upon number of electrons that are found in an element’s outer most shell.

As Neon (Ne) have electron configuration 1s2 2s2 2p6, which means there are in total eight electrons in outermost subshell (2s and 2p subshells).

As there’s no space available to accept any new electron. Therefore valency of Neon is zero.

Therefore valency of Neon (Ne) is 0.

Neon (Ne)Valency = 0

Why neon is an inert gas?

As Neon has electron configuration 1s2 2s2 2p6 which clearly shows that all of its orbitals are fully filled. Therefore it doesn’t neither need to gain nor need to loose any electrons. Thus it doesn’t react at all with other elements. That’s why its called inert gas, inert meaning no reaction.

Summary

Electron Configuration of Neon is 1s2 2s2 2p6

FAQs

What is electron configuration of ground-state Neon atom?

Ground state atom means that all electrons inside it are in least possible energy state levels, therefore net total energy of atom in ground-state is minimum out of all possible states of it. As Neon atom just have 10 electrons, therefore it’s electron configuration is 1s2 2s2 2p6. Which means Neon atom have 2 electrons each in its 1s, 2s orbitals and 6 electrons in 2p orbitals.

Valency of neon is zero explain why?

Neon has atomic number 10 which means in ground-state it just have 10 total electrons. Therefore it’s electron configuration is 2, 8. 2 electrons in K shell and 8 in L shell. As maximum capacity of L shell is to accomodate just 8 electrons, thus Neon already have an Octet Configuration. Which means it doesn’t need to either accept nor loose any electron to achieve stable noble gas configuration. Therefore valency of neon is zero.

Can Neon form Covalent bonds?

Neon has electron configuration 1s2 2s2 2p6 which means all of its orbitals are fully filled and therefore there’s no space to add new electron. As neon already have stable octet electron configuration, it doesn’t need to share any of it’s electron with other atoms to become stable. Therefore neon doesn’t form covalent bonds.

Some Properties of Neon

Element NameNeon
SymbolNe
Atomic Number10
Number of electrons10
Group in Periodic Table18
Atomic Weight20.180 u
Number of Valence Electrons8
Valency0
Melting Point– 248.67 °C (24.48 K)
Boiling Point– 246.048 °C (27.102 K)
Atomic Radius38 picometre
Electronegativity0 on Pauling Scale
Van der waals Radius154 picometre
Density0.9 g/cm3
Heat of fusion0.3317 kJ/mol
Heat of vaporization1.7326 kJ/mol
Thermal Conductivity0.5 W/mK

Some Uses of Neon

In discharge tubes
Fluorescent bulbs for advertisement display purposes
Neon lamps are used in botanical gardens and in greenhouses as they stimulate growth and are effective in the formation of chlorophyll, a compound which helps plants to absorb energy
Neon is also used in voltage regulators and indicators
Light emitted from ionised neon can pass through water fog that’s why it is used in cold regions and in airports

Physical Properties of Neon

Neon, in both liquid and gaseous form is colourless, odourless and non-combustible

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