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QUESTION

# How would you arrange the following elements in order of increasing ionization energy: Te, Pb, Cl, S, Sn?

Pb, Sn, Te, S, Cl

The ionization energy increases across a period but decreases down a group.

This means that the with the lowest ionization energies would be in the bottom left-hand corner of . 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).

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