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Question

1. how do you calculate ionization energies for elements in kj/mol, i need to find out what element has the first ionization energy of 600kj/mol, 2nd ionization energy of 1800. please explain what the formula is and how to solve it.

2. why does nitrogen have higher ionization enery than oxygen. is it because of
a. effective nuclear charge
b.greater penetration of the nitrogen p orbitals
c. a crowding effect of the electrons
d. the extra neutrons of oxygen
e. or the half filled subshell of nitrogen
im guessing its either b. or e.

Answer 1

1. There really is no way to calculate it; it is determined experimentally.

2. The answer is e. There is extra stability from having a half-filled subshell. In order for oxygen to have the extra electron, it has to reverse the spin of one electron and pair it up with another electron in a 2p orbital, which costs energy, so oxygen is more willing to give that electron up that nitrogen is, despite the higher nuclear charge.

Answer 2

Ionization energies are calculated experimentally. It is not possible to guess the element from its ionization energy values always.

Nitrogen has greater ionisation energy than oxygen. It is becoz, nitrogen has relatively stable electronic configuration due to half filled sub-shell.

Answer 3

i'm not sure how to calculate the first question, but if you look at table "s" in the new york state chemistry reference tables for the new york state regents exams, there is a chart with the ionization energies for most elements. as far as question 2 goes, the question must be wrong, because oxygen definitely has a greater ionization energy than nitrogen because oxygen has greater effective nuclear charge. hope this helped.