Rydberg formula
In atomic physics, the Rydberg formula calculates the wavelengths of a spectral line in many chemical elements.
The formula was primarily presented as a generalization of the Balmer series for all atomic electron transitions of hydrogen.
It was first empirically stated in 1888 by the Swedish physicist Johannes Rydberg,[1] then theoretically by Niels Bohr in 1913, who used a primitive form of quantum mechanics.
The formula directly generalizes the equations used to calculate the wavelengths of the hydrogen spectral series.
In 1890, Rydberg proposed on a formula describing the relation between the wavelengths in spectral lines of alkali metals.
[2]: v1:376 He noticed that lines came in series and he found that he could simplify his calculations using the wavenumber (the number of waves occupying the unit length, equal to 1/λ, the inverse of the wavelength) as his unit of measurement.
Finding that the resulting curves were similarly shaped, he sought a single function which could generate all of them, when appropriate constants were inserted.
Rydberg therefore rewrote Balmer's formula in terms of wavenumbers, as
This suggested that the Balmer formula for hydrogen might be a special case with
was found to be a universal constant common to all elements, equal to 4/h.
As stressed by Niels Bohr,[3] expressing results in terms of wavenumber, not wavelength, was the key to Rydberg's discovery.
The fundamental role of wavenumbers was also emphasized by the Rydberg-Ritz combination principle of 1908.
The fundamental reason for this lies in quantum mechanics.
Modern and legitimate understanding is that Rydberg's findings were a reflection of the underlying simplicity of the behavior of spectral lines, in terms of fixed (quantized) energy differences between electron orbitals in atoms.
Rydberg's 1888 classical expression for the form of the spectral series was not accompanied by a physical explanation.
Walther Ritz's pre-quantum 1908 explanation for the mechanism underlying the spectral series was that atomic electrons behaved like magnets and that the magnets could vibrate with respect to the atomic nucleus (at least temporarily) to produce electromagnetic radiation,[4] but this theory was superseded in 1913 by Niels Bohr's model of the atom.
is a constant for all spectral series and elements, and the remaining values,
In Bohr's conception of the atom, the integer Rydberg (and Balmer) n numbers represent electron orbitals at different integral distances from the atom.
A frequency (or spectral energy) emitted in a transition from n1 to n2 therefore represents the photon energy emitted or absorbed when an electron makes a jump from orbital 1 to orbital 2.
Later models found that the values for n1 and n2 corresponded to the principal quantum numbers of the two orbitals.
run from 2 to infinity, the spectral lines known as the Lyman series converging to 91 nm are obtained, in the same manner: The formula above can be extended for use with any hydrogen-like chemical elements with
where This formula can be directly applied only to hydrogen-like, also called hydrogenic atoms of chemical elements, i.e. atoms with only one electron being affected by an effective nuclear charge (which is easily estimated).
But the Rydberg formula also provides correct wavelengths for distant electrons, where the effective nuclear charge can be estimated as the same as that for hydrogen, since all but one of the nuclear charges have been screened by other electrons, and the core of the atom has an effective positive charge of +1.
Finally, with certain modifications (replacement of Z by Z − 1, and use of the integers 1 and 2 for the ns to give a numerical value of 3⁄4 for the difference of their inverse squares), the Rydberg formula provides correct values in the special case of K-alpha lines, since the transition in question is the K-alpha transition of the electron from the 1s orbital to the 2p orbital.
This is analogous to the Lyman-alpha line transition for hydrogen, and has the same frequency factor.
Because the 2p electron is not screened by any other electrons in the atom from the nucleus, the nuclear charge is diminished only by the single remaining 1s electron, causing the system to be effectively a hydrogenic atom, but with a diminished nuclear charge Z − 1.
This formula of f = c / λ = (Lyman-alpha frequency) ⋅ (Z − 1)2 is historically known as Moseley's law (having added a factor c to convert wavelength to frequency), and can be used to predict wavelengths of the Kα (K-alpha) X-ray spectral emission lines of chemical elements from aluminum to gold.
See the biography of Henry Moseley for the historical importance of this law, which was derived empirically at about the same time it was explained by the Bohr model of the atom.
For other spectral transitions in multi-electron atoms, the Rydberg formula generally provides incorrect results, since the magnitude of the screening of inner electrons for outer-electron transitions is variable and cannot be compensated for in the simple manner above.
The correction to the Rydberg formula for these atoms is known as the quantum defect.
