Rules For Filling Electrons In Orbitals Notes For NCERT Chemistry Class 11

For L- orbit, n = 2, l can have two values (= 0 and 1 which corresponds to s and p sub shells respectively), m will have three values (=-1, 0, +1) which corresponds to three orbitals of p sub shell and s can have two values +1/2 or -1/2. From this information, following combination will be obtained:

n = 2; l = 0; m = 0; s = +1/2
n = 2; l = 0; m = 0; s = -1/2

n = 2; l = 1; m = -1; s = +1/2

n = 2; l = 1; m = 0; s = +1/2
n = 2; l = 1; m =+1; s = +1/2
n = 2; l = 1; m = -1; s = -1/2

n = 2; l = 1; m = 0; s = -1/2
n = 2; l = 1; m =+1; s = -1/2

Therefore, L orbit where n = 2 can accommodate total of eight electrons, two in s sub shell and six in p sub shell. Likewise, the M orbit with n = 3 can accommodate 18 electrons; 2 in s sub shell (l = 0), 6 in p sub shell (l= 1) and 10 in d sub shell (l= 2).

As we pass from one element to another (one of next higher atomic number), one electron is added every time to the atom.

Remember:

The maximum number of electrons in any orbit or shell is 2n2, where n is a principal quantum number or the number of the orbit.
The maximum number of electrons in a subshell (s, p, d or f) is equal to 2(2l + 1), where l is an azimuthal quantum number) and has the value 0, 1, 2 or 3. Thus, these subshells can have a maximum of 2, 6, 10 and 14 electrons respectively.
Orbitals are filled up in order of their increasing energy. The orbital with lower energy is filled up first, then the orbital with higher energy starts filling up. A new electron enters the orbital where (n + l) is minimum. When (n + l) has the same value for two or more orbitals, the new electron enters the orbital where n is minimum.

Continue complete chapter click Rules For Filling Electrons In Orbitals Notes

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