Quantum Numbers Class 11 Chemistry
In this video, all four quantum numbers are explained very
easily in the Hindi language.
A large number of orbitals are possible in an atom.
Qualitatively these orbitals can be distinguished by their size, shape, and
orientation. An orbital of smaller size means there is more chance of finding
the electron near the nucleus. Similarly, shape and orientation mean that there
is more probability of finding the electron along with certain directions than
along others. Atomic orbitals are precisely distinguished by what is known as
quantum numbers. Each orbital is designated by three quantum numbers labeled as
n, l, and ml.
There are four Quantum numbers, which are as follows.
1. The principal quantum number ‘n’
2. Azimuthal quantum number. ‘l’
3. Magnetic orbital quantum number. ‘ml’
4. Electron spin quantum number (ms)
i) n defines the shell, determines the size of the orbital
and also to a large extent the energy of the orbital.
ii) There are n subshells in the nth shell. l identifies the
subshell and determines the shape of the orbital. There are (2l+1) orbitals of
each type in a subshell, that is, one s orbital (l = 0), three p orbitals (l =
1), and five d orbitals (l = 2) per subshell. To some extent l also determines
the energy of the orbital in a multi-electron atom.
iii) ml designates the orientation of the orbital. For a
given value of l, ml has (2l+1) values, the same as the number of orbitals per
subshell. It means that the number of orbitals is equal to the number of ways
in which they are oriented.
iv) ms refers to the orientation of the spin of the
electron.
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