Correct Answer - Option 4 : n = 2, l = 2, m = 0;
Concept:
Atomic orbitals are precisely distinguished by what are known as quantum numbers.
Each orbital is designated by three quantum numbers labelled as n, l and ml.
Principal quantum number (n): It is a positive integer with value of n = 1, 2, 3.... The principal quantum number determines the size and to large extent the energy of the orbital.
All the orbitals of a given value of ‘n’ constitute a single shell of atom and are represented by the following letters n = 1 (K), 2 (L), 3 (M), 4 (N)…
Azimuthal quantum number (l): It is also known as orbital angular momentum or subsidiary quantum number.
For a given value of n, l can have n values ranging from 0 to n – 1, that is, for a given value of n, the possible value of l are : l = 0, 1, 2, .......... (n–1);
Each shell consists of one or more subshells or sub-levels. The number of subshells in a principal shell is equal to the value of n.
Sub-shells corresponding to different values of l are represented by the following symbols,
l = 0 (s), 1(p), 2(d), 3(f), 4(g),5(h)…
Magnetic orbital quantum number (ml): It gives information about the spatial orientation of the orbital with respect to standard set of co-ordinate axis.
For any sub-shell (defined by ‘l’ value), 2l+1 values of ml are possible and these values are given by,
ml = - l, - (l-1), - (l-2)... 0,1... (l -2), (l-1), l;
Explanation:
All the options are following the quantum model criteria except option 4.
In option 4, the set of quantum numbers is n = 2, l = 2, m = 0;
Now for n = 2, possible values of l are 0 and 1, 2 is not possible
∴ 4th option is not possible
