ionisation energy is the energy required to remove one electron from an element
electronic configuration of atoms
Atom 1 - 1s2 2s2 2p6 3s2
Atom 2 - 1s2 2s2 2p6 3s2 3p4
Atom 3 - 1s2 2s2 2p6 3s2 3p6
elements configuration after removal of one electron( after first ionisation energy)
Atom 1 - 1s2 2s2 2p6 3s1
Atom 2 - 1s2 2s2 2p6 3s2 3p3
Atom 3 - 1s2 2s2 2p6 3s2 3p5
elements configuration after removal of one electron( after second ionisation energy)
Atom 1 - 1s2 2s2 2p6
Atom 2 - 1s2 2s2 2p6 3s2 3p2
Atom 3 - 1s2 2s2 2p6 3s2 3p4
now in Third ionisation energy,
From above configuration,for
Atom 1 - electron will be taken out from a fully filled p orbital
Atom 2- electron will be taken out from a incompletely filled p orbital
Atom 3- electron will be taken out from a incompletely filled p orbital
So,less energy is required to take out electron from partially filled orbitals than a fully filled orbitals as half filled and fully filled orbitals are stable
therefore Atom 1 will have highest third ionisation energy
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