( l = ) per subshell. To some extent l also determines the energy of the orbital in a multi-electron atom. iii) m l designates the orientation of the orbital. For a given value of l , m l has ( l + ) values, the same as the number of orbitals per subshell.
It means that Orbit, orbital and its importance Orbit and orbital are not synonymous. An orbit, as proposed by Bohr, is a circular path around the nucleus in which an electron moves. A precise description of this path of the electron is impossible according to Heisenberg uncertainty principle. Bohr orbits, therefore, have no real meaning and their existence can never be demonstrated experimentally.
An atomic orbital, on the other hand, is a quantum mechanical concept and refers to the one electron wave function ψ in an atom. It is characterized by three quantum numbers ( n, l and m l ) and its value depends upon the coordinates of the electron. ψ has, by itself, no physical meaning. It is the square of the wave function i.e., | ψ | which has a physical meaning.
| ψ | at any point in an atom gives the value of probability density at that point. Probability density (| ψ | ) is the probability per unit volume and the product of | ψ | and a small volume (called a volume element) yields the probability of finding the electron in that volume (the reason for specifying a small volume element is that | ψ | varies from one region to another in space but its value can be assumed to be constant within a small volume element). The total probability of finding the electron in a given volume can then be calculated by the sum of all the products of | ψ | and the corresponding volume elements. It is thus possible to get the probable distribution of an electron in an orbital.
the number of orbitals is equal to the number of ways in which they are oriented. iv) m s