Hello, looking for some help with problem #2. Ignore #1 and #3 please. Thank you

Question

Hello, looking for some help with problem #2. Ignore #1 and #3 please. Thank you!!

Below are the ionization energies (IE) of an element in the second row of the periodic table. What is the element? Why is there a large jump in ionization energy between IE_1 and IE_s? The electron affinity of C is -122 kJ/mol and N is >0 kJ/mol. Explain the difference in electron affinity using electron configuration/orbital diagrams in your argument. Draw the Lewis structure for the molecule SPCI, where P is the central atom and the octet rule is satisfied on all atoms and the formal charges on all atoms is zero.

Explanation / Answer

Electron affinity is defined as energy released when electron is added to atom

C has electronic configuration 1s2 2s2 2p2.

So when electron is added we get 1s2 2s2 2p3 which is stable configuration since p orbital is half filled.

Hence energy is relased as we get stability by adding e-.

N has electronic configuraton 1s2 2s2 2p3.

Here N already has stable electornic configuration. Hence addition of electron causes destabilisation. Hence we need energy to supply to N for adding electron. Hence electron affinity of N > 0

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