Question

Rank the Ionization Energies from highest to lowest for: Be, S , Li , Li+ .

Explain why S has a higher Ionization energy than Be.

Answer 1

The energy which is required to remove an electron from a gaseous atom or ion is known as Ionization energy. Generally, in the periodic table; in a period from left side to right side, the first ionization energy increases, due to decrease of atomic radius on the other hand first ionization energy decrease in going down a group due to increase of atomic radius. Li(g)? Li+(g)+e- 1=520.2 Li+(g)? Li2+(g)+e- I=7298.2 Be(g)? Be+(g)+e- I= 899.5 S(g)? S(g)+e- =999.6 the Ionization Energies from highest to lowest for: Be, S., Li, Lit is as follows: Li+>S>Be > Li Li+ has highest ionization energy because electron is removed from positive charge S has a higher Ionization energy than Be because Be present on the left side while S present on the right side of table and from left side to right side, the first ionization energy increases The electron configuration of Be and S is as follows: Be -4: 182 2s2 S-16: 152 282 2p6 382 3p4