Hund S Law Of Multiplicity
Pauli exclusion rule shows that we cannot have more than 2 electrons in orbital and also aufbau rules tells us that electron are filled up in increasing order of energy level.
Hund s law of multiplicity. Hund s rule is also known as the rule of maximum multiplicity. Consider the electron configuration for carbon atoms.
Hund s rule of maximum multiplicity. The diagram shows the state of this term with m l 1 and m s 1.
Pairing of electrons requires energy. 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.
Therefore no pairing occurs until all orbitals of a given sub level are half filled. Learn hund s rule of maximum multiplicity with examples.
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. This implies that if two or more orbitals of equal energy are.
It can be understood from the classical picture that if all electrons are orbiting in the same direction higher orbital angular momentum they. 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. According to hund s rule electrons are placed into separate orbitals before going into an orbital this is already occupied.
Hund s rule of maximum multiplicity states that in filling p d or f orbitals as many unpaired electrons as possible are placed before pairing of electrons with opposite spin is allowed. Hund s rule of maximum multiplicity.
Consider also the electron configuration of oxygen. The superscript 3 is the value of the multiplicity 2s 1 3.
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.
