Hund S Rule Maximum Multiplicity
For a given electron configuration the term with maximum multiplicity has the lowest energy.
Hund s rule maximum multiplicity. Hunds rule of maximum multiplicity rule states that for a given electron configuration the term with maximum multiplicity falls lowest in energy. Hund s rule of maximum multiplicity.
The rule states that for a given electron configuration the lowest energy term is the one with the greatest value of spin multiplicity. This is known as hund s rule of maximum multiplicity.
Total no of 6 electrons is disposed over 1s 2s and 2p orbitals. It states that when electrons enter sub levels of fixed n 1 values available orbitals are singly occupied table.
According to this principle for a given electronic configuration the paring of the particle is done after each subshell is filled with a single electron. Pairing of electrons requires energy.
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. 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.
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. Therefore no pairing occurs until all orbitals of a given sub level are half filled.
Hund s rule states that. In other words the under subshell should have maximum multiplicity.
Every orbital in a sublevel is singly occupied before any orbital is doubly occupied. The hund rule of maximum multiplicity states.
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 three rules are.
The first rule is especially important in chemistry where it is often referred to simply as hund s rule. All of the electrons in singly occupied orbitals have the same spin to maximize total spin.
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. When two or more orbitals of equal energy or very close energy are available electrons will fill the orbitals singly before filling doubly.
But both of these rules does not tell any thing how electrons would be arrange in p orbital or d orbital. The answer to this question involves hund s rule.
S orbitals can hold two electrons and p orbital holds 2 electrons by following hund s rule of highest multiplicity.
