Hund S Law Electron Configuration
The three rules are.
Hund s law electron configuration. Hund s rule 2 for a given multiplicity the term with the largest value of l lies lowest in energy. Aufbau principle electrons fill orbitals starting at the lowest available energy state before filling higher states 1s before 2s.
Under the orbital approximation we let each electron occupy an orbital which can be solved by a single wavefunction. In the configuration p 2 we expect the order 3 p 1 d 1 s.
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. Hunds rule of maximum multiplicity rule states that for a given electron configuration the term with maximum multiplicity falls lowest in energy.
The electron configuration is the standard notation used to describe the electronic structure of an atom. In atomic physics hund s rules refers to a set of rules that german physicist friedrich hund formulated around 1927 which are used to determine the term symbol that corresponds to the ground state of a multi electron atom the first rule is especially important in chemistry where it is often referred to simply as hund s rule.
In doing so we obtain three quantum numbers n l m l which are the same as the ones obtained from solving the schrodinger s equation for bohr s hydrogen atom. Example 1 consider the different ways in which a pair of electrons might be arranged in p orbitals.
The two 2s electrons will fill the similar orbital whereas the two 2p electrons will be in various orbital and aligned in the same direction in accordance with hund s rule. For a given electron configuration the term.
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. An orbital can hold 0 1 or 2 electrons only and if there are two electrons in the orbital they must have opposite paired spins.
Oxygen has 8 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.
Consider the electron configuration for carbon atoms. This implies that if two or more orbitals of equal energy are.
Considering also the electron configuration of oxygen. 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.
There are a few rules for the box and arrow configurations. Consider also the electron configuration of oxygen.
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.
