a). Explain the reason for the variation of the first ionization energies of the third period elements.

Md Ariful Islam

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Md Ariful Islam

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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 too 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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