Oxidation States of Group 16 Elements
The outer shell configuration of group 16 elements is ns2np4, and they can acquire noble gas configuration by acquiring two electrons, producing the M-2 ion, or by sharing two electrons, establishing two covalent bonds. As a result, both negative and positive oxidation states are represented by these elements. The oxidation states of the elements in group 16 are 2, +2, +4, and +6.
Elements |
Atomic Number |
Electronic Configuration |
Oxidation State |
---|---|---|---|
Oxygen |
8 |
[He] 2s2 2p4 |
-2,-1,+1,+2 |
Sulphur |
16 |
[Ne] 3s2 3p4 |
-2,+2,+4,+6 |
Selenium |
34 |
[Ar] 3d10 4s2 4p4 |
-2,+2,+4,+6 |
Tellurium |
52 |
[Kr] 4d10 5s2 5p4 |
-2,+2,+4,+6 |
Polonium |
84 |
[Xe] 4f14 5d10 6s2 6p4 |
+2,+4,+6 |
Group 16 Elements
Group 16 Elements refer to those elements which are arranged in the 16th group of the Modern Periodic Table. Group 16 accommodates five elements in total from the second to sixth period. If we carefully observe the periodic table, we find that in the case of Group 16 Elements, the last electrons enter the p-orbital and hence the Group 16 Elements are also called p-block elements. Also, Group 16 is located on the left side of the periodic table. Group 16 Elements are primarily non-metal in nature. The p-block extends from Group 13 to Group 18. The p-block does not include helium, which is found at the top of column 8A. The p orbital can only store six electrons, which is why the p-block has six columns. The p-block is the only block that contains all three categories of elements: metals, nonmetals, and metalloids, and it has the greatest diversity of elements. In this article, we will learn about the Group 16 Elements, their electronic configuration and properties in detail.