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Question
Explain the following, give an appropriate reason.
First ionisation potential of the C-atom is greater than that of the B atom, whereas the reverse is true is for the second ionisation potential.
Solution
C (Z = 6) 1s2 2s2 2px1 2py1. The electron removal from p orbital is very difficult. So carbon has the highest first ionization potential. B (Z = 5) 1s2 2s2 2p1. In boron nuclear charge is less than that of carbon, so boron has the lowest first ionization potential.
I.E1C > I.E1B
But it is reversed in the case of second ionization energy. Because in the case of B+ the electronic configuration is 1s2 2s2, which is completely filled and has high ionization energy. But in C+ the electronic configuration is 1s2 2s2 2p1, one electron removal is easy so it has low ionization energy.
I.E2B > I.E2C
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