Hund S Rule Why
This implies that if two or more orbitals of equal energy are.
Hund s rule why. According to the first rule electrons always enter an empty orbital before they pair up. Hunds rule of maximum multiplicity rule states that for a given electron configuration the term with maximum multiplicity falls lowest in energy.
This rule deals with reducing the repulsion between electrons. 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 first rule now states that the ground state term is 3 p which has s 1. The diagram shows the state of this term with m l 1 and m s 1.
Electrons are negatively charged and as a result they repel each other. Hund s rule 2 for a given multiplicity the term with the largest value of l lies lowest in energy.
Hund s rule states that a larger total spin state of an atom sometimes makes the atom more stable. All of the electrons in separately occupied orbitals have an equivalent spin to maximize total spin.
Focusing on the outer shell hund s rule determines how the electrons are arranged in the orbitals or their configuration. Electrons tend to minimize repulsion by occupying their own orbitals rather than sharing an orbital with another electron.
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. According to hund s rule.
Building off of the concepts that only two electrons can occupy a given orbital and electrons in the same orbital spin in opposite directions hund s rule states that electrons must always fill up all the empty orbitals in a subshell before pairing with electrons. Each orbital in a sublevel is separately occupied before any orbital is doubly occupied.
