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Hunds Rule - Definition, Examples, Uses, Spin Multiplicity, FAQs

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Hunds Rule - Definition, Examples, Uses, Spin Multiplicity, FAQs

Edited By Team Careers360 | Updated on Jun 25, 2022 09:24 AM IST

State Hund's Rule of Maximum Multiplicity Class 11

The Aufbau principle tells us that the lowest energy orbitals will get filled up by electrons first. Thereafter, the electrons move on to energetically higher orbitals. The problem with this rule is that it does not tell about the order in which they will be filled in three 2p orbitals and five 3d orbitals consequently. Hund's Rule of Maximum Multiplicity depicts the perfect order of electrons filled up in energetically higher orbitals with higher principal numbers such as 2,3,4.. so on.. It states that for a particular electronic configuration, the term with maximum multiplicity is of lowest energy. By this rule pairing of electrons in p, d and f orbitals cannot occur until each orbital of a given subshell contains one electron each or becomes singly occupied.

What is Hund's rule?

Hund's rule states that:

1. For a particular electronic configuration, the electron having maximum spin multiplicity has the lowest energy. The multiplicity can be depicted as ( 2S+1), where S represents total spin angular momentum of the electrons.

2. For a particular multiplicity, the term with the maximum value of total orbital angular momentum quantum number (L) occupies the lowest energy.

3. In an atom having the outermost subshell half-filled or less, for a particular term, the level with the lowest value of the total angular momentum quantum number (J) lies in lowest energy. If the outermost shell is more than half-filled, the level with the highest value of J is lowest in energy.

Where, total angular momentum quantum number, J = L + S

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Explain Hund's rule of maximum multiplicity with an example.

Hund's rule of maximum multiplicity was discovered by Friedrich Hund in the year 1925. Hund's principle states that, for a particular electronic configuration, the greatest value of spin multiplicity has the lowest energy term. It says if two or more than two orbitals having the same amount of energy are unoccupied then the electrons will start occupying them individually before they get paired up during filling up. This statement depends on the observation of atomic spectra, which is helpful in predicting the ground state of a molecule or an atom with one or more than one open electronic shells.

The electrons enter into an empty orbital before it gets paired up. While considering the 1st statement, there comes a problem that The electrons repel each other as they are negatively charged. Hence, The electrons will not share orbitals to reduce repulsion. But when we consider the 2nd statement, the spins of unpaired electrons in singly occupied orbitals are the same. The spin of initial electrons in the sub-level decides what the spin of the upcoming electrons would be.

Example of hund's rule (example of hund's rule of maximum multiplicity)

For example, a nitrogen atom’s electronic configuration would be 1s22s22p3. The same orbital will be occupied by the two 2s electrons although different orbitals will be occupied by the three 2p electrons in accordance to Hund’s rule.

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Let's consider carbon as an example.

The electronic configuration for carbon atoms: 1s22s22p2:

Here, The two 2s electrons will occupy the same orbital, whereas the two 2p electrons will be in different orbital (and aligned the same direction) in accordance with Hund's rule. Consider also the electronic configuration of oxygen. Oxygen has 8 electrons.

The electronic configuration can be written as 1s22s22p4.

The first two electrons will be paired up in the 1s orbital; the next two electrons will be paired up in the 2s orbital. The remaining 4 electrons, which must be placed in the 2p orbitals. According to Hund’s rule, all orbitals will be singly occupied before being doubly occupied. Therefore, two p orbital get one electron and one will have two electrons. Hund's rule also stipulates that all of the unpaired electrons must have the same spin. In keeping with convention, the unpaired electrons are drawn as "spin-up".

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Spin Multiplicity Meaning

In spectroscopy and in quantum chemistry, the multiplicity of an energy level can be calculated by using 2S+1, where S indicates the total spin angular momentum. States of electrons with multiplicity 1, 2, 3, 4, 5 are respectively called singlets, doublets, triplets, quartets and quintets.

Spin Multiplicity Rule

According to the spin multiplicity rule, for a given electron configuration, the lowest energy term is the one with the greatest value of spin multiplicity. This indicates that if two or more orbitals of equal energy are available, electrons will occupy them singly before filling them in pairs.

Uses of Hund’s Rule:

Hund's rule of maximum multiplicity is a rule which is based on observation of atomic spectra. This observation is used to predict the electronic configuration of the ground state of an atom or molecule with one or more open electronic shells. For example, from boron through neon, the electron filling order of the 2p orbitals follows Hund's Rule of maximum multiplicity. It has wide applications in atomic chemistry to predict the electronic configuration and spin of an electron , quantum chemistry, and spectroscopy, etc.

Also check-

NCERT Chemistry Notes:

Frequently Asked Question (FAQs)

1. Why is Hund's rule called the rule of maximum multiplicity?

hund's rule is called the rule of maximum multiplicity because out of the various possible electronic configurations, only that configuration is correct for which the total spin value is maximum.

2. What type of configurations violate Hund’s principle?

Every orbital of the same energy must have at least one electron which has identical spin before you deposit two in the same orbital.

3. What is stated at the 1st part of the hund’s rule?

The 1st part of the hund’s rule states that, for a particular electronic configuration, the electron having maximum spin multiplicity has the lowest energy. The multiplicity can be depicted as ( 2S+1), where S represents total spin angular momentum of the electrons.

The orbitals of the subshell will be singly occupied with electrons initially with parallel spin before pairing up occurs.

4. What is the nickname of the 1st part of the hund’s rule?

The nickname of the 1st part of the hund’s rule is spin-spin interaction.

5. Why is hund’s rule not applicable for all elements?

If Hund's rule is not applied the number of singly occupied orbitals or unpaired electrons will decrease gradually. Total number of unpaired electrons is 5, if Hund's rule is followed. Hence, there will be only one electron unpaired if this rule is violated. Hund’s rule is not applicable for NO molecule.

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