Silicon(Si) is the 14th element in the periodic table and its symbol is ‘Si’. Silicon is a semiconductor material. The electron configuration of silicon and the orbital diagram is the main topic of this article. Also, valency and valence electrons of silicon, various reactions, and compound formation, bond formation have been discussed. Hopefully, after reading this article you will know in detail about this.
The total number of electrons in silicon is fourteen. 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 silicon(Si) atoms can be done in two ways.
- Electron configuration through orbit
- Electron configuration through orbital
Electron configuration through orbitals follows different principles. For example Aufbau principle, Hund’s principle, Pauli’s exclusion principle. There is an article published on this site detailing the electron configuration, you can read it if you want.
Silicon(Si) 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.
- 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 silicon(Si) is 14. That is, the number of electrons in silicon is fourteen. Therefore, the silicon atom will have two electrons in the first shell, eight in the 2nd orbit, and four electrons in the 3rd shell. Therefore, the order of the number of electrons in each shell of a silicon atom is 2, 8, 4.
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 orbital diagrams.
Electron configuration of silicon(Si) through orbital
The German physicist Aufbau first proposed an 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 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d.
The first two electrons of silicon(Si) 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 remaining two electrons will be in the 3p orbital. Therefore, the silicon(Si) electron configuration will be 1s2 2s2 2p6 3s2 3p2.
How to write the orbital diagram for silicon(Si)?
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 silicon(Si), you have to do the electron configuration of silicon. 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. 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. The next two electrons will enter the 3s orbital and the remaining two electrons will enter the 3p orbital in a clockwise direction. This is clearly shown in the figure of the orbital diagram of silicon(Si). The last orbit of a silicon atom has four electrons. So, the valence electrons of silicon are four.
Silicon(Si) excited state electron configuration
Atoms can jump from one orbital to another by excited state. This is called quantum jump. Ground state electron configuration of silicon is 1s2 2s2 2p6 3s2 3p2. The valency of the element is determined by electron configuration in the excited state. The p-orbital has three sub-orbitals. The sub-orbitals are px, py and pz. Each sub-orbital can have a maximum of two electrons.
In the silicon ground-state electron configuration, the two electrons of the 3p orbital are located in the px and py sub-orbitals and the spin of the two electrons is the same. Then the correct electron configuration of silicon in ground state will be 1s2 2s2 2p6 3s2 3px1 3py1. This electron configuration shows that the last shell of the silicon atom has two unpaired electrons(3px1 3py1). So the valency of silicon is 2. When silicon atoms are excited, silicon atoms absorb energy. As a result, an electron in the 3s orbital jumps to the 3pz sub-orbital. The second orbit of the silicon atom is filled with electrons.
So the electron of the third orbit jumps and goes to another sub-orbital of the third orbit. Then the electron configuration of silicon(Si*) in excited state will be 1s2 2s2 2p6 3s1 3px1 3py1 3pz1. This electron configuration shows that the last shell of the silicon atom has four unpaired electrons(3s1 3px1 3py1 3pz1). So the valency of silicon is 4.
How do you write the electron configuration for silicon(Si)?
Ans: Silicon(Si) electron configuration is 1s2 2s2 2p6 3s2 3p2.
How many electrons does silicon(Si) have?
Ans: 14 electrons.
How many valence electrons does silicon(Si) have?
Ans: Four valence electrons.
What is the symbol for silicon?
Ans: The symbol for silicon is ‘Si’.