CHEM101 Lecture : Chem 101 Lecture September 23.docx

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graymoose214

8 Jul 2014

School

University of Alberta

Department

Chemistry

Course

CHEM101

Professor

Yoram Apelblat

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CHEM101 Full Course Notes

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Document Summary

Ionization energy: first ionization energy corresponds to outermost electron as it is the easiest to remove, second ionization energy corresponds to second outermost electron, etc, each successive energy will increase, ie1< ie2 < ie3, boron example ie3, b2+ b3+ + e , b3+ has configuration of he noble gas = very stable, ie4: b3+ b4+ + e requires much more energy because we are trying to remove an electron from a very stable configuration, this explains the large jump in ie when trying to remove electrons form noble gas configurations for any ions, any time an electron is removed from a noble gas configuration, the ionization. Periodic trend of ionization energy: energy is very large!: going across (l r), zeff increases, radius decreases, electrons held tighter, more energy necessary to remove electron, ie increases, small decreases at start of new orbitals (s p, p d, etc.

Related Questions

When trying to remove electrons from Be, which of the following sets of ionization energy makes the most sense going from first to
third ionization energy? Explain your answer.

a. First IE 900 KJ/m01, second IE 1750 kJ/m01, third IE 15,000 kJ/mol
b. First IE 1750 KJ/m01, second IE 900 kJ/m01, third IE 15,000 kJ/mol
c. First IE 15,000 KJ/m01, second IE 1750 kJ/m01, third IE 900 kJ/mol
d. First IE 900 KJ/m01, second IE 15,000 kJ/m01, third IE 22,000 kJ/mol
e. First IE 900 KJ/m01, second IE 1750 kJ/m01, third IE 1850 kJ/mol