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State hund\'s rule |
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Answer» Hund’s rule\tAccording to this rule, the\xa0electrons are filled in the degenerate orbitals of the same subshell.\tElectron pairing in p, d and f orbitals cannot be done until each sub-shell is occupied singly.\tThis is because electrons are the same in charge and they repel each other. This repulsion is minimized if two electrons move away from each other by acquiring different degenerate orbitals.\tAll the orbitals which are singly occupied have parallel spins which can be either clockwise or anticlockwise.\tIf the electrons have parallel spin then there will be less inter-electronic repulsions and high spin multiplicity.\tSo in order to maximize spin multiplicity, the pairing of electrons in a sub-shell does not take place until each sub-shell is singly occupied. Every orbital in a sublevel is singly occupied before any orbital is doubly occupied |
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