Explain the variation of ionization energies of third elements
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Ionization energy is the amount of energy required to remove an electron from neutral gaseous electrons.
Across period, in a periodic table from left to right ionization energy should increase.
Third period elements are:
Na, Mg, Al, Si, P, S , Cl, Ar
Order of ionization energy in third period:
Na<Mg>Al<Si<P>S<Cl<Ar
In third period element with highest ionization energy is argon due to stable octet configuration.
Case 1:
Mg has more ionization energy than Al.
Mg>Al
Due to its stable ns2 configuration of Mg.
Case 2:
P has more ionization energy than sulphur (S) a because phosphorous has half filled p sub shell in its valence shell that gives extra stability and hence more energy is required to remove the electron.
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