Arsenic(As) electron configuration and orbital diagram

Arsenic is the 33rd element in the periodic table and its symbol is ‘As’. The total number of electrons in arsenic is thirty-three. These electrons are arranged according to specific rules of different orbits. The arrangement of electrons in different orbits and orbitals of an atom in a certain order is called electron configuration. The electron configuration of arsenic(As) atom 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. The electron configuration and orbital diagram of arsenic is the main topic in this article. Also, valency and valence electrons of arsenic, and compound formation, bond formation have been discussed. Hopefully, after reading this article you will know in detail about this.

Table of Contents

Arsenic 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, N is the name of the fourth orbit. The electron holding capacity of each orbit is 2n².

Arsenic atom electron configuration — Arsenic(As) electron configuration (Bohr model)

For example,

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.
n=3 for M orbit.
The maximum electron holding capacity in M orbit is 2n² = 2 × 3²= 18 electrons.
n=4 for N orbit.
The maximum electron holding capacity in N orbit is 2n² = 2 × 4² = 32 electrons.

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 arsenic(As) is 33. That is, the number of electrons in arsenic is thirty-three.

Therefore, the arsenic atom will have two electrons in the first shell, eight in the 2nd orbit, eighteen electrons in the 3rd shell, and the remaining five electrons will be in the fourth shell. Therefore, the order of the number of electrons in each shell of the arsenic atom is 2, 8, 18, 5.

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 arsenic 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 1s.
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.

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. The German physicist Aufbau first proposed the idea of electron configuration through sub-orbits.

Electron configuration via Aufbau principal

The Aufbau method is to do electron configuration through the sub-energy 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. These orbitals are named s, p, d, f. The Aufbau electron configuration method is 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d.

The first two electrons of arsenic enter the 1s orbital. The s-orbital can have a maximum of two electrons. Therefore, the next two electrons enter the 2s orbital. The p-orbital 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 of the third orbit and the next six electrons will be in the 3p orbital. The 3p orbital is now full. So, the next two electrons will enter the 4s orbital and ten electrons will enter the 3d orbital. The 3d orbital is now full. So, the remaining three electrons enter the 4p orbital. Therefore, the arsenic(As) electron configuration will be 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p³.

How to write the orbital diagram for arsenic?

To create an orbital diagram of an atom, you first need to know Hund’s principle and Pauli’s exclusion principle. Hund’s principle is that electrons in different orbitals with the same energy would be positioned in such a way that they could be in the unpaired state of maximum number and the spin of the unpaired electrons will be one-way.

And Pauli’s exclusion principle is that the value of four quantum numbers of two electrons in an atom cannot be the same. To write the orbital diagram of arsenic(As), you have to do the electron configuration of arsenic. Which has been discussed in detail above. 1s is the closest and lowest energy orbital to the nucleus. Therefore, the electron will first enter the 1s orbital.

According to Hund’s principle, the first electron will enter in the clockwise direction and the next electron will enter the 1s orbital in the anti-clockwise direction. The 1s orbital is now filled with two electrons. Then the next two electrons will enter the 2s orbital just like the 1s orbital.

The next three electrons will enter the 2p orbital in the clockwise direction and the next three electrons will enter the 2p orbital in the anti-clockwise direction. Then next two electrons will enter the 3s orbital just like the 1s orbital and then the next six electrons will enter the 3p orbital just like the 2p orbital. The 3p orbital is now full. So, the next two electrons will enter the 4s orbital just like the 1s orbital. The 4s orbital is now full.

Therefore, the next five electrons will enter the 3d orbital in the clockwise direction and the next five electrons will enter the 3d orbital in the anti-clockwise direction. The 3d orbital is now full. so, the remaining three electrons will enter the 4p orbital in the clockwise direction. This is clearly shown in the figure of the orbital diagram of arsenic.

Atomic Orbital Diagram for Arsenic

Arsenic ion(As^3-) electron configuration

The ground state electron configuration of arsenic is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p³. This electron configuration shows that the last shell of arsenic has five electrons. Therefore, the valence electrons of arsenic are five.

The elements that have 5, 6, or 7 electrons in the last shell receive the electrons in the last shell during bond formation. The elements that receive electrons and form bonds are called anions. During the formation of a bond, the last shell of arsenic receives three electrons and turns into an arsenic ion(As^3-). That is, arsenic is an anion element.

As + 3e^– → As^3-

The electron configuration of arsenic ion(As^3-) is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶. This electron configuration shows that the arsenic ion(As^3-) acquired the electron configuration of krypton. Arsenic atom exhibits -3, +3, +5 oxidation state. The oxidation state of the element changes depending on the bond formation.