The first ionization enthalpy of carbon atom is greater than that of boron whereas the reverse is true for the second ionization enthalpy.
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Electronic Configuration of C : 1s2, 2s2, 2p2
Electronic Configuration of B : 1s2, 2s2, 2p1
The first ionization energy of C will be higher than that of B, this is simply because the size of C is smaller than that of B. Due to the smaller size of C atom, the valence electron of atom feels greater nuclear charge as compare to the valence electron of B. Due to the greater nuclear force, it requires higher energy to remove the valence electron of C atom as compare to that of B. this can also be justified by the trend of variation of ionization energy along the period.
After removal of one electron:
Electronic Configuration of C+ : 1s2, 2s2, 2p1
Electronic Configuration of B+ : 1s2, 2s2
Now the next electron is to be removed from partially filled 2p1orbital of C + while a fully filled 2s2orbital of B+. As we know that fully filled orbitals have extra stability, so it would require more energy to remove an electron from B+ as compare to that of C+.
Hence, the 2nd ionization energy of B is higher than that of C.
Electronic Configuration of B : 1s2, 2s2, 2p1
The first ionization energy of C will be higher than that of B, this is simply because the size of C is smaller than that of B. Due to the smaller size of C atom, the valence electron of atom feels greater nuclear charge as compare to the valence electron of B. Due to the greater nuclear force, it requires higher energy to remove the valence electron of C atom as compare to that of B. this can also be justified by the trend of variation of ionization energy along the period.
After removal of one electron:
Electronic Configuration of C+ : 1s2, 2s2, 2p1
Electronic Configuration of B+ : 1s2, 2s2
Now the next electron is to be removed from partially filled 2p1orbital of C + while a fully filled 2s2orbital of B+. As we know that fully filled orbitals have extra stability, so it would require more energy to remove an electron from B+ as compare to that of C+.
Hence, the 2nd ionization energy of B is higher than that of C.
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