Rules For Filling Of Electrons In Various Orbitals
Category : JEE Main & Advanced
The atom is built up by filling electrons in various orbitals according to the following rules, (1) Aufbau?s principle This principle states that the electrons are added one by one to the various orbitals in order of their increasing energy starting with the orbital of lowest energy. The increasing order of energy of various orbitals is \[1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f\] \[<5d<6p<7s<\,5f<6d<7p.........\] (2) (n+l) Rule In neutral isolated atom, the lower the value of (n + l) for an orbital, lower is its energy. However, if the two different types of orbitals have the same value of (n + l), the orbitals with lower value of \[n\] has lower energy. (3) Pauli?s exclusion principle According to this principle ?no two electrons in an atom will have same value of all the four quantum numbers?. If one electron in an atom has the quantum numbers \[n=1\], \[l=0\], \[m=0\] and \[s=+1/2\], no other electron can have the same four quantum numbers. In other words, we cannot place two electrons with the same value of \[s\] in a \[1s\] orbital.
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