Explain the reason for the variation of the first ionisation energies of the third period elements
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Hi, Here is your answer
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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 I.E should increase.
Third period elements are :
Na, Mg, Al, Si, P, S , Cl, Ar
Order of I.E 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 I.E than Al.
Mg>Al
due too its stable ns2 configuration of Mg.
Case 2:
P has more I.E 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.
Hope it is helpful.....
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