Hund S Rule With Example

Hund s rule states that a larger total spin state of an atom sometimes makes the atom more stable. For example take the electron configuration for carbon. 1s 2 2s 2 2p 2.

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Example 1 consider the different ways in which a pair of electrons might be arranged in p orbitals.

Hund s rule with example. This implies that if two or more orbitals of equal energy are. The basis for this rule is essentially that if the electrons are orbiting in the same direction and so have a large total angular momentum they meet less often than when they orbit in opposite directions.

All of the electrons in separately occupied orbitals have an equivalent spin to maximize total spin. Each orbital in a sublevel is separately occupied before any orbital is doubly occupied.

Consider also the electron configuration of oxygen. Hund s first rule now states that the ground state term is 3 p which has s 1.

Hund s rule states that each orbital in a subshell is only obtained before any orbital is double involved. According to hund s rule.

All of the electrons in singly occupied orbitals have a similar spin to maximize total spin. The correct orbital diagram obeying hund s rule will note the two 2p electrons to be unpaired in two of the three.

In the configuration p 2 we expect the order 3 p 1 d 1 s. Hund s rule states that the lowest energy electron configuration the ground state in any electron subshell is the one with the greatest number of parallel electron spins.

The diagram shows the state of this term with m l 1 and m s 1. 2 electrons will pair up in the 1s orbital 2 electrons pair up in the 2s orbital and the remaining 2 electrons will be placed into the 2p orbitals.

According to this rule electron pairing in p d and f orbitals cannot occur until each orbital of a given subshell contains one electron each or is singly occupied. Hunds rule of maximum multiplicity rule states that for a given electron configuration the term with maximum multiplicity falls lowest in energy.

Consider the electron configuration for carbon atoms. This rule deals with reducing the repulsion between electrons.

Hund s rule 2 for a given multiplicity the term with the largest value of l lies lowest in energy. Hund s rule of maximum multiplicity is a rule based on observation of atomic spectra which is used to predict the ground state of an atom or molecule with one or more open electronic shells the rule states that for a given electron configuration the lowest energy term is the one with the greatest value of spin multiplicity.

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. The superscript 3 is the value of the multiplicity 2s 1 3.