Rydberg+Equation

=Rydberg Equation=

History
In the late nineteenth century and early twentieth century with classical physics at it’s peak, one of the few mysteries that remained was understanding line spectra. With classical physics unable to explain line spectra scientists turned to empirically derived formulas to predict line emissions. Although nearly all spectra were too complex to mathematically model scientists were able to model Hydrogen’s spectra using the Rydberg equation:



Where λ is wavelength, n1 and n2 are integers such that n2 > n1, and R is the Rydberg constant of R=1.097x107 m-1. Although the rational for such a relationship was unknown, the Rydberg equation did predict correct hydrogen line spectra.

Quantum mechanics would later provide such a rational. Essentially the Rydberg equation is a classical approximation of an electron orbiting the nucleus. Other atom’s spectra cannot be approximated likewise because such a model ignores electron – electron interactions, so only an atom like H or He+ with only one electron can be accurately described this way.

Applications
The Balmer series makes up the visible Hydrogen spectra. All energy level transitions for this series go from n2>2 and end at n1=2.

Visible Balmer Series (n1=2)


 * n2 || Wavelength (nm) ||
 * 3 || 649 ||
 * 4 || 481 ||
 * 5 || 429 ||
 * 6 || 406 ||

Links
Bohr’s Derivation of the Ryberg Equation: []