Since the valence shell is n = 3 it is in Period 3. Since there are 4 valence electrons (2 in 3s and 2 in 3p) it is in Group 4A (14).

You are watching: An element that has the valence electron configuration 6s26p6 belongs to which period and group?

For 4s2 4p1, the valence shell in n = 4 so this is in Period 4 and there are 3 valence electrons putting it in group 3A (13)


If you take a look at a periodic table that shows orbitals1 you can see what elements have which configurations. An element with the valence shell configuration 3s23p2 has a full s-orbital (because s-orbitals can hold at most two electrons) and two electrons in the p-orbitals. The table linked below shows which row (or period) on the table has elements with valence 3p orbitals. Because there are two electrons in the p-orbital, the column (or group) that this element is in will be the second in the 3p row.

The element in the second column of the p-orbitals and third row would be silicon (Si). It"s not shown in the linked table, but the group that this element is in is shown at the top of the table; it"s also just the number of the column counting from left to right. So silicon is in the third row and fourteenth column, or third period and fourteenth group.

The same exact logic goes to find that Gallium is in the fourth period and the thirteenth group.

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This video uses the periodic table to give you a really helpful visual understanding of how orbital notation works. I hope this helps. :)

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