YEAR 11 CHEMISTRY QUESTION
Hi all! Having a bit of trouble with chemistry, and this question in particular
Find the identity of an atom given the following electronic configuration.
1s^2 2s^2 2p^6 3s^2 3p^4
I know that the number of valence electrons is equal to the group number. So in this case, it's group 4? But per my understanding, Sulfur is in group 6?
I am incredibly confused- please help out!
In schrodinger's model, each orbital can hold upto a maximum of two electrons.
s has 1 orbital
p has 3 orbitals
d has 5 orbitals
f has 7 orbitals
The litlle subscript at the top tells you the amount of electrons the sub shell holds. (E.g. 3p^5 holds 5 electrons)
In your case, the first shell holds 2 electrons, the seconds one holds 8 (2s^2 and 2p^6), and finally the third one holds 6 electrons (3s^2 and 3p^4)
You would add the amount of electrons there are in all your shells, and in your case, you would have 16 electrons.
There are 6 valence electrons (as there are 6 electrons in the
third shell), therefore it would be found in Group 6 (or 16...), and your atom would be Sulfur.