This means that the elements with the lowest ionization energies would be in the bottom left-hand corner of the periodic table. The change in ionization energies is also bigger going down the periodic table (by change within a group) than going across the periodic table (by change within a period).
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So let”s start from the bottom of the periodic table:#Pb# is the element that is in the lowest period at 6 (and lowest group at 14) in the periodic table; it”s the smallest ionization energy.
The period above (5) has two of the elements: Sn and Te. Well, since ionization energy increases across a period, Sn will have a smaller ionization energy than Te.#Pb, Sn, Te#
Now, let”s go to the third period, where #S# and #Cl# are. Since #S# is before #Cl,# #S# has a lower ionization energy than #Cl#.#Pb, Sn, Te, S, Cl#
Nov 15, 2016
The order is #”Sn .
You have learned that ionization energy increases from top to bottom and from left to right in the Periodic Table.
You probably saw a diagram something like this.
Here”s the portion of the Periodic Table that includes the elements in this question.
(Adapted from ZON PENA)
You would naturally predict the order to be
This is almost correct, but the correct order is #”Sn , as shown in the image below.
Why is this so?
The electron configuration of #”Sn”# is #”
The electron configuration of #”Pb”# is #”
The #”4f”# electrons in #”Pb”# are poor at shielding the outermost electrons.
Thus the outer electrons experience a greater effective nuclear charge, and it is more difficult to remove them.
Hence #”Pb”# has a higher ionization than #”Sn”#, and the correct order is #”Sn .
I hope that your instructor told you about this phenomenon before asking you to make a prediction.
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