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The electronic configuration with the highest ionization enthalpy is
Across period 3 the ionization enthalpy increases from Al ($$3p^1$$) to Si ($$3p^2$$) to P ($$3p^3$$), and P has an extra-stable half-filled $$3p$$ subshell. An element with a $$p^3$$ configuration further down the group (such as arsenic) is larger and has a lower ionization enthalpy than P. So $$[\text{Ne}]3s^2 3p^3$$ has the highest value.
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