These are a way of describing the locations of the electrons.
They are how the shells split up.
There is a degree-level explanation as to why the following numbers are the way they are, but I doubt you want me to go into that much detail.
The first one is the s orbital, it can hold 2 electrons. Elements filling this orbital are hydrogen, helium and the s block elements.
The second is the p orbital, it can hold 6 electrons. Elements that are filling up this orbital go in the p block.
The third is the d orbital; it can hold 10 electrons and gives rise to the transition metals.
The fourth is the f block. It can hold, as I remember, 12 electrons and gives rise to the lanthanides and actinides, at the bottom of the table.
eg. 2s^2 means that the s orbital in the 2nd shell has 2 electrons in it.
Argon is 1s^2 2s^2 2p^6. If you add them together you get 2 electrons in the first shell and 8 in the 2nd.
Electron affinity/electronegativity values only apply across bonds. If a more electronegative atom is bonded to a less electronegative atom, the electrons forming the bond spend more time nearer the more electronegative nucleus.What are the S and P numbers in the periodic table for?
I study Chemistry a level:
in the atomic structure, there are energy shells, but in between these are sub-shells - which lie electrons.
each element has a different electronic configuration e.g
1s2 2s2 etc..
s can have a maximum of 2 electrons
p '; '; 6
d '; '; 10
these are what you need to know for chemsitry as level.
hope this helps!
S and P numbers???
Are you by any chance refering to the S and P block elements???
