Below are the ionization energies (IE) of an element in the second row of the pe

Question

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_4 and IE_5? 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 SPCl, 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

Q1.

2nd row...

identify the larges dop in energy

that is, form 4th to 5th

this must be therefore in family IV A

if it is the second row, the it mustbe CARBON with n = 6 b)

the large jump is due to the fact that the 5th electorn sia ctually a "core" electron, it is NOT a valence electron, so the energy required is much stronger because of the proton attraction to the core electron

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