Electron Configuration for Manganese (Mn, Mn2+, Mn4+)
Manganese is the 25th element in the periodic table and its symbol is ‘Mn’. In this article, I have discussed in detail how to easily write the complete electron configuration of manganese.
What is the electron configuration of manganese?
The total number of electrons in manganese is twenty-five. These electrons are arranged according to specific rules in different orbitals.
The arrangement of electrons in manganese in specific rules in different orbits and orbitals is called the electron configuration of manganese.
The electron configuration of manganese is [Ar] 3d5 4s2, 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.
Manganese 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 2n2.
Shell Number (n) | Shell Name | Electrons Holding Capacity (2n2) |
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 2n2 = 2 × 12 = 2. - For L orbit, n = 2.
The maximum electron holding capacity in L orbit is 2n2 = 2 × 22 = 8. - n=3 for M orbit.
The maximum electron holding capacity in M orbit is 2n2 = 2 × 32 = 18. - n=4 for N orbit.
The maximum electron holding capacity in N orbit is 2n2 = 2 × 42 = 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 manganese is 25. That is, the number of electrons in manganese is twenty-five. Therefore, the manganese atom will have two electrons in the first shell and eight in the 2nd orbit.
According to Bohr’s formula, the third orbit will have fifteen electrons but the third orbit of manganese will have thirteen electrons and the remaining two electrons will be in the fourth orbit.
Therefore, the order of the number of electrons in each shell of the manganese(Mn) atom is 2, 8, 13, 2. 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 manganese through orbital
Atomic energy shells are subdivided into sub-energy levels. These sub-energy levels are also called orbital. The most probable region of electron rotation around the nucleus is called the orbital.
The sub-energy levels depend on the azimuthal quantum number. It is expressed by ‘l’. The value of ‘l’ is from 0 to (n – 1). The sub-energy 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 | 1s2 |
2 | 0 1 | 2 | 1 3 | 2s 2p | 2 6 | 2s2 2p6 |
3 | 0 1 2 | 3 | 1 3 5 | 3s 3p 3d | 2 6 10 | 3s2 3p6 3d10 |
4 | 0 1 2 3 | 4 | 1 3 5 7 | 4s 4p 4d 4f | 2 6 10 14 | 4s2 4p6 4d10 4f14 |
For example,
- If n = 1,
(n – 1) = (1–1) = 0
Therefore, the value of ‘l’ is 0. So, the sub-energy level is 1s. - If n = 2,
(n – 1) = (2–1) = 1.
Therefore, the value of ‘l’ is 0, 1. So, the sub-energy levels are 2s, and 2p. - If n = 3,
(n – 1) = (3–1) = 2.
Therefore, the value of ‘l’ is 0, 1, 2. So, the sub-energy 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 sub-energy 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 sub-shells 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.
Sub-shell 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 s-subshell is one, three in the p-subshell, five in the d-subshell and seven in the f-subshell. Each orbital can have a maximum of two electrons.
The sub-energy 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 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.
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 manganese 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 the remaining five electrons will enter the 3d orbital. Therefore, the manganese full electron configuration will be 1s2 2s2 2p6 3s2 3p6 3d5 4s2.
Note: The abbreviated electron configuration of manganese is [Ar] 3d5 4s2. When writing an electron configuration, you have to write serially.
Electron configuration of manganese in the excited state
Atoms can jump from one orbital to another orbital in an excited state. This is called quantum jump.
The ground-state electron configuration of manganese is 1s2 2s2 2p6 3s2 3p6 3d5 4s2. In the manganese ground-state electron configuration, the five electrons of the 3d orbital are located in the dxy, dyz, dzx, dx2-y2 and dz2 orbitals.
We already know that the d-subshell has five orbitals. The orbitals are dxy, dyz, dzx, dx2-y2 and dz2 and each orbital can have a maximum of two electrons.
Then the correct electron configuration of manganese in the ground state will be 1s2 2s2 2p6 3s2 3p6 3dxy1 3dyz1 3dzx1 3dx2-y21 3dz21 4s2. This electron configuration shows that the manganese atom has five unpaired electrons.
So the oxidation state of manganese is +5. When a manganese atom is excited, then the manganese atom absorbs energy. As a result, an electron in the 4s orbital jumps to the 4px orbital.
We already know that the p-subshell has three orbitals. The orbitals are px, py, and pz and each orbital can have a maximum of two electrons.
Therefore, the electron configuration of manganese(Mn*) in an excited state will be 1s2 2s2 2p6 3s2 3p6 3dxy1 3dyz1 3dzx1 3dx2-y21 3dz21 4s1 4px1.
The valency of the element is determined by electron configuration in the excited state. Here, manganese has seven unpaired electrons. Therefore, the oxidation state of manganese is +7.
From the above information, we can say that manganese exhibits variable valency. Therefore, the valency of manganese is 5, and 7. Manganese also exhibits +2, +3, +4 and +6 oxidation states.
Manganese ion(Mn2+, Mn3+, Mn4+) electron configuration
The electron configuration of manganese shows that the last shell of manganese has two electrons and the d-orbital has a total of five electrons. Therefore, the valence electrons of manganese are seven.
There are three types of manganese ions. The manganese atom exhibits Mn2+, Mn3+ and Mn4+ ions. The manganese atom donates two electrons from the last shell to form the manganese ion(Mn2+).
Mn – 2e– → Mn2+
Here, the electron configuration of manganese ion(Mn2+) is 1s2 2s2 2p6 3s2 3p6 3d5. The manganese atom donates two electrons in the 4s orbital and an electron in the 3d orbital to convert to a manganese ion(Mn3+).
Mn – 3e– → Mn3+
Here, the electron configuration of manganese ion(Mn3+) is 1s2 2s2 2p6 3s2 3p6 3d4. The manganese atom donates two electrons in the 4s orbital and two electrons in the 3d orbital to convert to a manganese ion(Mn4+).
Again, Mn – 4e– → Mn4+
The electron configuration of manganese ion(Mn4+) is 1s2 2s2 2p6 3s2 3p6 3d3. From the above information, we can say that manganese exhibits +2, +3, and +4 oxidation states. The oxidation state of the element changes depending on the bond formation.
Video for Electron Configuration for Mn, Mn2+, Mn3+, and Mn4+
Compound formation of manganese
Manganese atoms participate in the formation of bonds through valence electrons. This valence electron participates in the formation of bonds with atoms of other elements.
The electron configuration of oxygen shows that the valence electrons of oxygen are six. The manganese atom donates its valence electrons to the oxygen atom and the oxygen atom receives those electrons.
As a result, oxygen acquires the electron configuration of neon. Manganese(III) oxide (Mn2O3) is formed by the exchange of electrons between two atoms of manganese and three atoms of oxygen. Manganese(III) oxide (Mn2O3) is ionic bonding.
FAQs
What is the symbol for manganese?
Ans: The symbol for manganese is ‘Mn’.
How many electrons does manganese have?
Ans: 25 electrons.
How do you write the full electron configuration for manganese?
Ans: The full electron configuration for manganese is 1s2 2s2 2p6 3s2 3p6 3d5 4s2.
How many valence electrons does manganese have?
Ans: Seven valence electrons.
What is the valency of manganese?
Ans: The valency of manganese is 2, 4, and 7.
What is the electron configuration of a mn atom in the ground state?
Ans: The electron configuration of a mn atom in the ground state is 1s2 2s2 2p6 3s2 3p6 3d5 4s2.
What is the complete ground state electron configuration for the manganese atom?
Ans: The complete ground state electron configuration for the manganese atom is 1s2 2s2 2p6 3s2 3p6 3dxy1 3dyz1 3dzx1 3dx2-y21 3dz21 4s2.
How many electrons are in d-orbital of ground state mn atom?
Ans: The ground state mn atom has five electrons in its d-orbital.
What is the abbreviated electron configuration of mn2+?
Ans: The abbreviated electron configuration of mn2+ is [Ar] 3d5.
What is the ground state electron configuration of mn+?
Ans: The ground state electron configuration of mn+ is [Ar] 3d5 4s1.
How many 3d electrons does the manganese(ii) ion (mn2+) have?
Ans: The electron configuration of manganese ion(Mn2+) is 1s2 2s2 2p6 3s2 3p6 3d5. Manganese(ii) ion (mn2+) has a total of five electrons in its 3d orbital.
How many s electrons and p electrons does mn possess?
Ans: The sub-energy level ‘s’ can hold a maximum of two electrons, ‘p’ can hold a maximum of six electrons. A manganese atom has a total of four s-subshells and two p-subshells. They are 1s, 2s, 3s, 4s and 2p, 3p. These subshells of manganese atom are filled with electrons.
What is the electronic configuration of mn2+?
Ans: The electron configuration of manganese ion(Mn2+) is 1s2 2s2 2p6 3s2 3p6 3d5.
How many electrons are in the 3d sublevel for manganese?
Ans: A manganese atom has a total of five electrons in its 3d subshell.
How many unpaired electrons are in the manganese atom?
Ans: Five unpaired electrons. Because the electron configuration of manganese in the ground state will be 1s2 2s2 2p6 3s2 3p6 3dxy1 3dyz1 3dzx1 3dx2-y21 3dz21 4s2. Here, the 4s orbital is full of two electrons. Only 3d orbital has five unpaired electrons.
What is the electron configuration of mn3+ ion?
Ans: The electron configuration of manganese ion(Mn3+) is 1s2 2s2 2p6 3s2 3p6 3d4.
What is the total number of principle energy levels that are present in at atom of manganese?
Ans: The total number of principle energy levels in a manganese atom is four. The order of the number of electrons in each energy levels of the manganese(Mn) atom is 2, 8, 13, 2.
How many electrons are unpaired in the 3d orbital of manganese?
Ans: Five unpaired electrons. The electron configuration of manganese in the ground state will be 1s2 2s2 2p6 3s2 3p6 3dxy1 3dyz1 3dzx1 3dx2-y21 3dz21 4s2. Here, the 4s orbital is full of two electrons. Only 3d orbital has five unpaired electrons.
How many d electrons are in the ground state electron configuration of mn2+?
Ans: The electron configuration of manganese ion(Mn2+) is 1s2 2s2 2p6 3s2 3p6 3d5. Here, the 3d orbital has five electrons.
What is the abbreviated electron configuration for manganese?
Ans: The abbreviated electron configuration for manganese is [Ar] 3d5 4s2.
How many unpaired electrons are present in the ground state electron configuration of mn3+ ion?
Ans: The electron configuration of manganese ion(Mn3+) is 1s2 2s2 2p6 3s2 3p6 3d4. Here, The mn3+ ion has four unpaired electrons in its ground state electron configuration.
How many energy levels does manganese have?
Ans: Manganese has four energy levels.
How many unpaired electrons are in the ground state electron configuration for mn?
Ans: The correct electron configuration of manganese in the ground state will be 1s2 2s2 2p6 3s2 3p6 3dxy1 3dyz1 3dzx1 3dx2-y21 3dz21 4s2. This electron configuration shows that the manganese atom has five unpaired electrons.
How many electrons does a mn atom have in its 3d subshell?
Ans: Five electrons.
How many electron shells does manganese have?
Ans: Four shells.