Explain why the ionization energy of S slightly lower than P when we would expec

Question

Explain why the ionization energy of S slightly lower than P when we would expect it to be higher based on the general trend. Explain why there is a decrease in ionization energy form Zn to Ga. Answer the questions below using plots of electron affinity for groups IA, IIIA, and VIIA. a. Define electron affinity. b. Explain why the electron affinities for groups IIA and VIIIA are-0 kJ/mol. c. Explain why the electron affinities for group VILA is so high compared to the other groups. d. Explain why the electron affinity for F is less than for Cl.

Explanation / Answer

d. P has half filled 3p shell and S has two half filled shells and one complete confriguration in 3p shell,
   Sulfur tries to get rid of that one extra counter spinning electron in the first sub-shell of 3p shell
   whereas phosphorous is stable. This is the reason why ionzation energy of S is slightly lower than P.
e. Zinc has full stable configuration in its outer orbital whereas Ga has partially filled outer orbital
   and therefore Zinc's ability to lose electrons is not as quick as Ga as Zn is more stable. This is
   the reason why there is decrease in ionzation energy from Zn to Ga
22.
a) When an atom is added to neutral atom in gaseous state, energy will evolve or be absorbed.
Such energy change involved in that process is called Electron affinity.
b) IIA (alkali group elements) and VIIIA ( noble gases) do not form stable negative ions.
   For energy to be released or spent there must involve this change into negative ion.
   This is the reason why IIA and VIIIA elements have 0kJ/mol
c) As you move down the group VII A elements, aka halogens there will be an extra addition of
   electron in in an already filled shell. That is why it has high EA
d) F has smaller atomic size and its anion is pretty much unstable due to high q/m ratio.
   This is the reason why F has lower EA than Cl
  
   

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