Groups and atomic structureIf we now look at the electron arrangement in the Groups, we'll find that they too are:
- Similar for the different elements in each Group
Select each Group to find out more
Group I
While lithium and sodium from Group I have different numbers of electrons (3 and 11 respectively), they do have one thing in common:
- Both have only one electron in the outermost shell
This is true of all the elements in Group I.
Group II
While beryllium and magnesium from Group II have different numbers of electrons (4 and 12, respectively), they do have one thing in common:
- Both have two electrons in the outermost shell
This is true of all the elements in Group II.
Group 0
While neon and argon from Group 0 have different numbers of electrons (10 and 18, respectively), they do have one thing in common:
- Both have outermost shells that are completely filled
This is true of all the elements in Group 0.
Results
The reason why the elements in Group I are so reactive is that they have a lone electron in their outer shells.
Conversely, the reason the Group 0 elements are so unreactive is that they have completely filled outer electron shells.
