Na requires the least amount of energy to remove the most loosely held electron.
Why does Na have the least ionization enthalpy among the given elements?
Electronic configuration of the elements:
Na - [Ne] 3s¹
P - [Ne] 3s² 3p³
Ar - [Ne] 3s² 3p⁶
Cl - [Ne] 3s² 3p⁵
- As it can be seen, Na after losing one electron from its outermost subshell attains a stable noble gas configuration. So, it will require a very less amount of energy i.e., ionization enthalpy, to remove that electron.
- P, which already has a half-filled subshell, will not readily lose the electrons and hence requires more amount of energy.
- Ar has the noble gas configuration i.e., all its subshells are fully filled. A very large amount of energy will be required to remove its electron.
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