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The ionization energy of O2 is smaller than the ionization energy of atomic O; the opposite is true for the ionization energies of N2 and atomic N. Explain this behavior in terms of molecular orbital energy diagrams of O2 and N2.

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Patrick Suarez
Patrick SuarezLv10
14 Dec 2020

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Related questions

As one gains altitude in the atmosphere, based on the ionization energies shown below, which sequence of mole fractions is the correct one?

Given:

N2 + hv > N2 + e- =Ionization Energy is 1495kj/mol

O2 + hv > O2 + e- =Ionization Energy is 1205kj/mol

O + hv > O + e- =Ionization Energy is 1313kj/mol

NO + hv > NO + e- =Ionization Energy is 890kj/mol

1. NO > O2 > O > N2

2. N2 > O2 > O > NO

3. N2 > O > O2 > NO

4. N2 > N > NO > O2

5. All will be equal.


Answer the following questions about first ionization energies.

(a) Generally, ionization energies increase on proceeding across a period, but this is not true for magnesium (738 kJ/mol) and aluminum (578 kJ/mol). Explain this observation.Ā 

(b) Explain why the ionization energy of phosphorus (1012 kJ/mol) is greater than that of sulfur (1000 kJ/mol) when the general trend in ionization energies in a period would predict the opposite.

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