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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