Question

arrange the following elements in order of decreasing ionization energy. rank values from highest to lowest ionization energy. to rank items as equivalent, overlap ci s pb sn te highest lowest submit request answer current temp

Explanation:

Ionization energy generally increases across a period (left to right) and decreases down a group (top to bottom) in the periodic table.

1. Cl and S are in Period 3; Cl is to the right of S, so Cl has higher ionization energy than S.
2. Te is in Period 6, Group 16; it is below S, so its ionization energy is lower than S.
3. Sn and Pb are in Group 14; Sn is above Pb, but due to the lanthanide contraction, Pb has a slightly higher ionization energy than Sn, both lower than Te.

Answer:

highest: Cl

1. S
2. Te
3. Pb
4. Sn (lowest)