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Q : 1. (1!) (1!) (1!)(1!)( ) 2. (1!) (1!) (1)(1) (1) 3. (1!) (1!) (1)(!)(1) here one (1) is the upper arrow and (!) this is the downward arrow...... among these above mentioned electronic configuration ,which one is correct ? tell me why 2 is correct?? |
The electronic configuration corresponds to 1S2 2S2 2Px 2Py 2Pz orbitals. Filling of orbitals follow Hunds rule of maximum multiplicity. Hund's Rule states that:
Look at the correct electron configuration of Nitrogen(Z = 7): 1s2 2s2 2p3 We can clearly see that p orbitals are half filled as there are three electrons and three p orbitals. This is because the three electrons in the 2p subshell will fill all the empty orbitals first before pairing with electrons in them. If we look at the element after Nitrogen in the same period, Oxygen (Z = 8) its electron configuration is: 1s2 2s2 2p4 Oxygen has one more electron than Nitrogen and as the orbitals are all half filled the electron must pair up. |