Photographic recording of Kα and Kβ X-ray emission lines for a range of elements; note that for the dispersive element used, the line position is proportional to the wavelength (not energy)

Moseley's law is an empirical law concerning the characteristic X-rays emitted by atoms. The law had been discovered and published by the English physicist Henry Moseley in 1913–1914.^[1][2] Until Moseley's work, "atomic number" was merely an element's place in the periodic table and was not known to be associated with any measurable physical quantity.^[3] In brief, the law states that the square root of the frequency of the emitted X-ray is approximately proportional to the atomic number:

$${\displaystyle {\sqrt {\nu }}\varpropto Z.}$$

History

Henry Moseley, holding an X-ray tube

The historic periodic table was roughly ordered by increasing atomic weight, but in a few famous cases the physical properties of two elements suggested that the heavier ought to precede the lighter. An example is cobalt having the atomic weight of 58.9 and nickel having the atomic weight of 58.7.

Henry Moseley and other physicists used X-ray diffraction to study the elements, and the results of their experiments led to organizing the periodic table by proton count.

Apparatus

Since the spectral emissions for the lighter elements would be in the soft X-ray range (absorbed by air), the spectrometry apparatus had to be enclosed inside a vacuum.^[4] Details of the experimental setup are documented in the journal articles "The High-Frequency Spectra of the Elements" Part I^[1] and Part II.^[2]

Results

Moseley found that the ${\displaystyle K\alpha }$ lines (in Siegbahn notation) were indeed related to the atomic number, Z.^[2]

Following Bohr's lead, Moseley found that for the spectral lines, this relationship could be approximated by a simple formula, later called Moseley's Law.^[2]

$${\displaystyle \nu =A\cdot \left(Z-b\right)^{2}}$$

where:

• ${\displaystyle \nu }$ is the frequency of the observed X-ray emission line
• ${\displaystyle A}$ and ${\displaystyle b}$ are constants that depend on the type of line (that is, K, L, etc. in X-ray notation)
• ${\displaystyle A=\left({\frac {1}{1^{2}}}-{\frac {1}{2^{2}}}\right)\cdot }$ Rydberg frequency and ${\displaystyle b\ }$= 1^[2] for ${\displaystyle K\alpha }$ lines, and ${\displaystyle A=\left({\frac {1}{2^{2}}}-{\frac {1}{3^{2}}}\right)\cdot }$ Rydberg frequency and ${\displaystyle b=7.4}$^[2] for ${\displaystyle L\alpha }$ lines.

Derivation

Moseley derived his formula empirically by fitting the square root of the X-ray frequency plotted against the atomic number.^[2] This formula can be explained based on the Bohr model of the atom, namely,

$${\displaystyle E=h\nu =E_{\text{i}}-E_{\text{f}}={\frac {m_{\text{e}}q_{\text{e}}^{2}q_{Z}^{2}}{8h^{2}\varepsilon _{0}^{2}}}\left({\frac {1}{n_{\text{f}}^{2}}}-{\frac {1}{n_{\text{i}}^{2}}}\right),}$$

where

• ${\displaystyle \varepsilon _{0}}$ is the permittivity of free space
• ${\displaystyle m_{\text{e}}}$ is the mass of an electron
• ${\displaystyle q_{\text{e}}}$ is the charge of an electron
• ${\displaystyle q_{Z}}$ is an effective charge of the nucleus, expressed as ${\displaystyle (Z-b)q_{e}}$
• ${\displaystyle n_{\text{f}}}$ is the quantum number of final energy level
• ${\displaystyle n_{\text{i}}}$ is the quantum number of initial energy level (${\displaystyle n_{\text{i}}>n_{\text{f}}}$)

Taking into account the empirically found b constant that reduced (or "screened") the nucleus charge, Bohr's formula for ${\displaystyle K\alpha }$ transitions becomes^[2]

$${\displaystyle E=h\nu =E_{\text{i}}-E_{\text{f}}={\frac {m_{\text{e}}q_{\text{e}}^{4}}{8h^{2}\varepsilon _{0}^{2}}}\left({\frac {1}{1^{2}}}-{\frac {1}{2^{2}}}\right)(Z-1)^{2}\approx {\frac {3}{4}}(Z-1)^{2}\times 13.6\ \mathrm {eV} .}$$

Dividing both sides by h to convert to the frequency units, one obtains

$${\displaystyle \nu ={\frac {E}{h}}={\frac {m_{\text{e}}q_{\text{e}}^{4}}{8h^{3}\varepsilon _{0}^{2}}}{\frac {3}{4}}(Z-1)^{2}\approx (Z-1)^{2}\times (2.47\cdot 10^{15}\ \mathrm {Hz} ).}$$

Screening

A simplified explanation for the effective charge of a nucleus being one less than its actual charge is that an unpaired electron in the K-shell screens it.^[5][6] An elaborate discussion criticizing Moseley's interpretation of screening can be found in a paper by Whitaker^[7] which is repeated in most modern texts.

A list of experimentally found and theoretically calculated X-ray transition energies is available at NIST.^[8] Nowadays, theoretical energies are computed with a much greater accuracy than what Moseley's law provides, using modern computational models such as the Dirac–Fock method (the Hartree–Fock method with the relativistic effects accounted for).

See also

• Moseley's periodic law, concerning the modern periodic table.
• Auger electron spectroscopy, a similar phenomenon with increased X-ray yield from species of higher atomic number.
• Discovery of the neutron Mosley's law was an important step in the delvelopment of the understanding of the atom.

References

External links

• Oxford Physics Teaching - History Archive, "Exhibit 12 - Moseley's graph Archived 2016-03-03 at the Wayback Machine" (Reproduction of the original Moseley diagram showing the square root frequency dependence)