explain the reasons for the variation of the first ionization energies of the third period elements
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Hey dear,
# Ionisation energy -
- It is the minimum amount of energy required to remove the valence electron of an isolated neutral gaseous atom or molecule.
● For third period element -
- Usually ionization enthalpy increases from left to right in period.
- But for third period elements, increasing order of ionization enthalpy is different -
Na < Al < Mg < SI < S < P < Cl < Ar
This is due to -
- Mg is more stable than Al due to its filled s-orbital (3s2).
- P is more stable than S due to its half-filled p-orbital.
Hope this helps you...
# Ionisation energy -
- It is the minimum amount of energy required to remove the valence electron of an isolated neutral gaseous atom or molecule.
● For third period element -
- Usually ionization enthalpy increases from left to right in period.
- But for third period elements, increasing order of ionization enthalpy is different -
Na < Al < Mg < SI < S < P < Cl < Ar
This is due to -
- Mg is more stable than Al due to its filled s-orbital (3s2).
- P is more stable than S due to its half-filled p-orbital.
Hope this helps you...
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