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In atomic physics, the principal quantum number symbolized as n is the first of a set of quantum numbers (which includes: the principal quantum number, the azimuthal quantum number, the magnetic quantum number, and the spin quantum number) of an atomic orbital.

[edit] Derivation

There are a set of quantum numbers associated with the energy states of the atom. The four quantum numbers n, ℓ, m, and s specify the complete and unique quantum state of a single electron in an atom called its wavefunction or orbital. Two electrons belonging to the same atom can not have the same four quantum numbers which is shown in the Pauli exclusion principle. The wavefunction of the Schrödinger wave equation reduces to the three equations that when solved lead to the first three quantum numbers. Therefore, the equations for the first three quantum numbers are all interrelated. The principal quantum number arose in the solution of the radial part of the wave equation as shown below.

The Schrödinger wave equation describes energy eigenstates having corresponding real numbers E_n with a definite total energy which the value of E_n defines. The bound state energies of the electron in the hydrogen atom are given by:

$E_n = \frac {E_1}{n^2} = \frac {-13.6eV}{n^2}, \quad n=1,2,3,\ldots$

The parameter n can take only positive integer values. This idea of energy levels and notation was borrowed from the earlier Bohr model of the atom and expanded in Schrödinger's equation from the flat two-dimensional Bohr atom to the three-dimensional wavefunction model of the atom. In the Bohr model, the allowed orbits were derived from quantized (discrete) values of orbital angular momentum, L according to the equation

$\mathbf{L} = n \cdot \hbar = n \cdot {h \over 2\pi}$

where n = 1, 2, 3, … and is called the principal quantum number, and h is Planck's constant. This formula is not correct in quantum mechanics as the angular momentum magnitude is described by the azimuthal quantum number, but the energy levels are accurate and classically they correspond to the sum of potential and kinetic energy of the electron.

The principal quantum number n represents the relative overall energy of each orbital and the energy of each orbital increases as the distance from the nucleus increases. The sets of orbitals with the same n-value are often referred to as electron shells or energy levels.

The minimum energy exchanged during any wave-matter interaction is the wave frequency multiplied by Planck's constant. This causes the wave to display particle-like packets of energy called quanta. The difference between energy levels that have different n determine the Emission spectrum of the element.

In the notation of the periodic table, the main shells of electrons are labeled:

K (n = 1), L (n = 2), M (n = 3), etc.

based on the principal quantum number.

The principal quantum number is related to the radial quantum number, n_r, by:

$n = n_r + \ell + 1 \,$

where ℓ is the azimuthal quantum number and n_r is equal to the number of nodes in the radial wavefunction.

[edit] See also

[edit] External references

Periodic Table Applet: showing principal and azimuthal quantum number for each element