Hund S Rule Example
Hund s rule 2 for a given multiplicity the term with the largest value of l lies lowest in energy.
Hund s rule example. All of the electrons in separately occupied orbitals have an equivalent spin to maximize total spin. Hund s rule states that.
In the configuration p 2 we expect the order 3 p 1 d 1 s. 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.
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.
Each orbital in a sublevel is separately occupied before any orbital is doubly occupied. As an example consider the ground state of silicon the electronic configuration of si is 1s 2 2s 2 2p 6 3s 2 3p 2 see spectroscopic notation we need to consider only the outer 3p 2 electrons for which it can be shown see term symbols that the possible terms allowed by the pauli exclusion principle are 1 d 3 p and 1 s hund s first rule now states that the ground state term is 3 p.
Hund s rule states that a larger total spin state of an atom sometimes makes the atom more stable. All of the electrons in singly occupied orbitals have a similar spin to maximize total spin.
According to hund s rule. This implies that if two or more orbitals of equal energy are.
Consider also the electron configuration of oxygen. All of the electrons in singly occupied orbitals have the same spin.
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. 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.
Every orbital in a sublevel is singly occupied before any orbital is doubly occupied. Example 1 consider the different ways in which a pair of electrons might be arranged in p orbitals.
1s 2 2s 2 2p 2. 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.
