In every atom there are principle energy levels, sub-levels and atomic orbitals. The principle energy levels are often those first taught when studying chemistry. They correspond to how close the electrons are to the nucleus. The first principle energy level is closest to the nucleus and can hold a maximum of two electrons. The second principle energy level is slightly further away from the nucleus and can hold a maximum of eight electrons. The third energy level is even further away and can hold a maximum of ten electrons.
Each principle energy level is comprised of different sub-levels: s, p, d and f. The s sub-level can hold a maximum of two electrons; , p a maximum of 6; d, a maximum of 10 and f, a maximum of 14 (although the f sub-level is only present in the lanthanide and actanide series). Sub-levels all have different energies and electrons fill sub-levels in order of lowest energy to highest. The first principle energy level has one sub-level, the 1s sub-level. The second principle energy level has two sub-levels, 2s and 2p. The third principle energy level has three sub-levels, 3s 3p and 3d. (However, the 4s sub-level is filled before the 3d sub-level, which is a different matter which cannot be explained quite so simply.)
Now, each sub-level is comprised of atomic orbitals which define the approximate boundaries of the electron orbit. Each orbital can hold up to two electrons, so a s sub-level has one orbital; a p sub-level has three orbitals; a d sub-level has five orbitals and a f sub-level has seven. This explanation is really quite brief as there is so much more information concerned with principle energy levels, sub-levels and atomic orbitals.
the orbitals of the sublevels of the same principal energy level differ in shape which describes where the electron is likely to be found.
Also the orbitals of sublevels have different energy levels.
In ascending enegy in any level
s < p < d < f < g etc
HOWEVER whether the different sublevels exist depends on the principal energy level
ie
1s
2s, 2p
3s, 3p, 3d
4s, 4p, 4d, 4f
There are 2 energy sublevels in the second principal.
1st energy has 1 sublevel -- 1 orbital -- 2 electrons 2nd energy level has 2 sublevels -- 4 orbitals -- 8 e- 3rd energy level has 3 sublevels -- 9 orbitals -- 18 e- 4th energy level has 4 sublevels -- 16 orbitals -- 32 e- Notice the pattern? number of orbitals = energy level squared Number of electrons = 2x number of orbitals
There are two sublevels in the 2nd principal energy level. They are the 2s and 2p sublevels.
some elements have unusual atomic orbitals
There are 8 sublevels, or types of orbitals in the 8th energy level. They would be s, p, d,f, g, h, i,j.
the orbitals of the sublevels of the same principal energy level differ in shape which describes where the electron is likely to be found. Also the orbitals of sublevels have different energy levels. In ascending enegy in any level s < p < d < f < g etc HOWEVER whether the different sublevels exist depends on the principal energy level ie 1s 2s, 2p 3s, 3p, 3d 4s, 4p, 4d, 4f
There are 2 energy sublevels in the second principal.
1st energy has 1 sublevel -- 1 orbital -- 2 electrons 2nd energy level has 2 sublevels -- 4 orbitals -- 8 e- 3rd energy level has 3 sublevels -- 9 orbitals -- 18 e- 4th energy level has 4 sublevels -- 16 orbitals -- 32 e- Notice the pattern? number of orbitals = energy level squared Number of electrons = 2x number of orbitals
The principal energy level is three, so there are three sublevels: 3s, 3p, and 3d. S,P and D
There are two sublevels in the 2nd principal energy level. They are the 2s and 2p sublevels.
9
There are four energy sublevels in the fourth energy levels: 4s, 4p, 4d, and 4f.
some elements have unusual atomic orbitals
There are 8 sublevels, or types of orbitals in the 8th energy level. They would be s, p, d,f, g, h, i,j.
The 2s and 2p sublevels in the second principal energy level are completely occupied in the ground state of a sodium atom.
4 (apex lol)
It depends which n since n is the row (period) number. 1st n = 1-s subshell, 1 orbital, and 2 electrons. 2nd n = 2-s subshell with 1 orbital and 2 electrons + 2-p subshell with 3 orbitals and 6 electrons.