Isotopic shift

The isotopic shift (also called isotope shift) is the shift in various forms of spectroscopy that occurs when one nuclear isotope is replaced by another.

NMR spectroscopy

In NMR spectroscopy, Isotopic effects on chemical shifts are typically small, far less than 1 ppm the typical unit for measuring shifts. The ¹
H NMR signals for ¹
H
_² and ¹
H²
H ("HD") are readily distinguished in terms of their chemical shifts. The asymmetry of the signal for the "protio" impurity in CD
_²Cl
_² arises from the differing chemical shifts of CDHCl
_² and CH
_²Cl
_².

H NMR spectrum of a solution of HD (labeled with red bars) and H₂ (blue bar). The 1:1:1 triplet arises from the coupling of the H nucleus (I = 1/2) to the H nucleus ( I = 1).

Vibrational spectra

Isotopic shifts are best known and most widely used in vibration spectroscopy where the shifts are large, being proportional to the ratio of the square root of the isotopic masses. In the case of hydrogen, the "H-D shift" is (1/2)^1/2 or 1/1.41. Thus, the (totally symmetric) C-H vibration for CH
_⁴ and CD
_⁴ occur at 2917 cm⁻¹ and 2109 cm⁻¹, respectively. ^[1] This shift reflects the differing reduced mass for the affected bonds.

Atomic spectra

Isotope shifts in atomic spectra are minute differences between the electronic energy levels of isotopes of the same element. They are the focus of a multitude of theoretical and experimental efforts due to their importance for atomic and nuclear physics. If atomic spectra also have hyperfine structure the shift refers to the center of gravity of the spectra.

From a nuclear physics perspective, isotope shifts combine different precise atomic physics probes for studying nuclear structure, and their main use is nuclear-model-independent determination of charge-radii differences.

Two effects contribute to this shift:

Mass effects

The mass difference (mass shift), which dominates the isotope shift of light elements. ^[2] It is traditionally divided to a normal mass shift (NMS) resulting from the change in the reduced electronic mass, and a specific-mass-shift (SMS) which is present in multi-electron atoms and ions.

The NMS is a purely kinematical effect, studied theoretically by Hughes and Eckart. ^[3] It can be formulated as follows:

In a theoretical model of atom, which have a infinitely massive nucleus, the energy (in wavenumbers) of a transition can be calculated from Rydberg formula

$${\displaystyle {\tilde {\nu }}_{\infty }=R_{\infty }\left({\frac {1}{n^{2}}}-{\frac {1}{n^{\prime 2}}}\right),}$$

where ${\displaystyle n}$ and ${\displaystyle n^{\prime }}$ are principal quantum numbers, and ${\displaystyle R_{\infty }}$ is Rydberg constant.

However, for a nucleus with finite mass ${\displaystyle M_{N}}$, reduced mass is used in the expression of Rydberg constant instead of mass of electron:

$${\displaystyle {\tilde {\nu }}={\tilde {\nu }}_{\infty }{\frac {M_{N}}{m_{e}+M_{N}}}}$$

With two isotopes with atomic mass approximately ${\displaystyle A^{\prime }M_{p}}$ and ${\displaystyle A^{\prime \prime }M_{p}}$, then the difference in the energies of the same transition is

$${\displaystyle \Delta {\tilde {\nu }}={\tilde {\nu }}_{\infty }\left({\frac {1}{1+{\frac {m_{e}}{A^{\prime \prime }M_{p}}}}}-{\frac {1}{1+{\frac {m_{e}}{A^{\prime }M_{p}}}}}\right)\approx {\tilde {\nu }}_{\infty }\left[1-{\frac {m_{e}}{A^{\prime \prime }M_{p}}}\left(1-{\frac {m_{e}}{A^{\prime }M_{p}}}\right)\right]\approx {\frac {m_{e}}{M_{p}}}{\frac {A^{\prime \prime }-A^{\prime }}{A^{\prime }A^{\prime \prime }}}{\tilde {\nu }}_{\infty }}$$

The above equations imply that such mass shift is greatest for hydrogen and deuterium since their mass ratio is the largest ${\displaystyle A^{\prime \prime }=2A^{\prime }}$.

The effect of the specific mass shift was first observed in the spectrum of neon isotopes by Nagaoka and Mishima. ^[4]

Considering the kinetic energy operator in Schrödinger equation of multi-electron atoms,

$${\displaystyle T={\frac {p_{n}^{2}}{2M_{N}}}+\sum _{i}{\frac {p_{i}^{2}}{2m_{e}}}}$$

For a stationary atom, the conservation of momentum gives

$${\displaystyle p_{n}=-\sum _{i}p_{i}}$$

Therefore, the kinetic energy operator becomes

$${\displaystyle T={\frac {\left(\sum _{i}p_{i}\right)^{2}}{2M_{N}}}+{\frac {\sum _{i}p_{i}^{2}}{2m_{e}}}={\frac {\sum _{i}p_{i}^{2}}{2M_{N}}}+{\frac {1}{M_{N}}}\sum _{i>j}p_{i}\cdot p_{j}+{\frac {\sum _{i}p_{i}^{2}}{2m_{e}}}}$$

Ignoring the second term, then the rest two terms in equation can be combined and original mass term need to be replaced by the reduced mass ${\displaystyle \mu ={\frac {m_{e}M_{N}}{m_{e}+M_{N}}}}$, and this gives the normal mass shift formulated above.

The second term in the kinetic term gives an additional isotope shift in spectral lines known as specific mass shift, giving

$${\displaystyle {\frac {1}{M_{N}}}\sum _{i>j}p_{i}\cdot p_{j}=-{\frac {\hbar ^{2}}{M_{N}}}\sum _{i>j}\nabla _{i}\cdot \nabla _{j},}$$

Using perturbation theory, the first order energy shift can be calculated as

$${\displaystyle \Delta E=-{\frac {\hbar ^{2}}{M}}\sum _{i>j}\int \psi ^{*}\nabla _{i}\cdot \nabla _{j}\psi \,d^{3}r,}$$

which requires the knowledge of accurate many-electron wave function. Due to the ${\displaystyle {\frac {1}{M_{N}}}}$ term in the expression, the specific mass shift also decrease as ${\displaystyle {\frac {1}{M_{N}^{2}}}}$ as mass of nucleus increase, same as normal mass shift.

Volume effects

The volume difference (field shift) dominates the isotope shift of heavy elements. This difference induces a change in the electric charge distribution of the nucleus. The phenomenon was described theoretically by Pauli and Peierls. ^{[5] [6] [7]} Adopting a simplified picture, the change in an energy level resulting from the volume difference is proportional to the change in total electron probability density at the origin times the mean-square charge radius difference.

For a simple nuclear model of an atom where the nuclear charge is distributed uniformly in a sphere with radius ${\displaystyle R=r_{0}A^{\frac {1}{3}}}$ where A is the atomic mass number and ${\displaystyle r_{0}\approx 1.2\times 10^{-15}m}$ is a constant.

Similarly, calculating the electrostatic potential of an ideal charge density uniformly distributed in a sphere, the nuclear electrostatic potential is

$${\displaystyle V(r)={\begin{cases}{\frac {Ze^{2}}{(4\pi \epsilon _{0})2R}}\left({\frac {r^{2}}{R^{2}}}-3\right),&r\leq R\\-{\frac {Ze^{2}}{(4\pi \epsilon _{0})r}},&r\geq R\end{cases}}}$$

Then the unperturbed Hamiltonian is subtracted, the perturbation is the difference of the potential in the above equation and Coulomb potential ${\displaystyle -{\frac {Ze^{2}}{(4\pi \epsilon _{0})r}}}$.

$${\displaystyle H^{\prime }={\begin{cases}{\frac {Ze^{2}}{(4\pi \epsilon _{0})2R}}\left({\frac {r^{2}}{R^{2}}}+{\frac {2R}{r}}-3\right),&r\leq R\\0,&r\geq R\end{cases}}}$$

Such a purterbation of the atomic system neglects all other potential effect like relativistic corrections. Using the perturbation theory (quantum mechanics), the first-order energy shift due to such perturbation is

$${\displaystyle \Delta E=\langle \psi _{nlm}|H^{\prime }|\psi _{nlm}\rangle }$$

Since the wave function ${\displaystyle \psi _{nlm}=R_{nl}(r)Y_{lm}(\theta ,\phi )}$ has radial and angular parts, and the perturbation has no angular dependence so the spherical harmonic normalize integral over the unit sphere

$${\displaystyle \Delta E={\frac {Ze^{2}}{(4\pi \epsilon _{0})2R}}\int _{0}^{R}|R_{nl}(r)|^{2}\left({\frac {r^{2}}{R^{2}}}+{\frac {2R}{r}}-3\right)r^{2}\,dr}$$

Since the radius of nuclues ${\displaystyle R}$ is small, and within such a small region ${\displaystyle r\leq R}$, the following approximation is valid ${\displaystyle R_{nl}(r)\approx R_{nl}(0)}$. And at ${\displaystyle r\approx 0}$, only the s sublevel is left, so ${\displaystyle l=0}$. Integration gives

$${\displaystyle \Delta E\approx {\frac {Ze^{2}}{(4\pi \epsilon _{0})}}{\frac {R^{2}}{10}}|R_{n0}(0)|^{2}={\frac {Ze^{2}}{(4\pi \epsilon _{0})}}{\frac {2\pi }{5}}R^{2}|\psi _{n00}(0)|^{2}}$$

The explicit form for hydrogenic wave function gives ${\displaystyle |\psi _{n00}(0)|^{2}={\frac {Z^{3}}{\pi a_{\mu }^{3}n^{3}}}}$.

$${\displaystyle \Delta E\approx {\frac {e^{2}}{(4\pi \epsilon _{0})}}{\frac {2}{5}}R^{2}{\frac {Z^{4}}{a_{\mu }^{3}n^{3}}}}$$

In an real experiment, the difference of this energy shift of different isotopes ${\displaystyle \delta E}$ is measured. These isotopes have nuclear radius difference ${\displaystyle \delta R}$. Differentiation of the above equation gives the first order in ${\displaystyle \delta R}$.

$${\displaystyle \delta E\approx {\frac {e^{2}}{(4\pi \epsilon _{0})}}{\frac {4}{5}}R^{2}{\frac {Z^{4}}{a_{\mu }^{3}n^{3}}}{\frac {\delta R}{R}}}$$

The above equation confirms that the volume effect is more significant for hydrogenic atoms with larger Z, which explains why volume effects dominates the isotope shift of heavy elements.

See also

• Kinetic isotope effect
• Magnetic isotope effect

References

1. Takehiko Shimanouchi (1972). "Tables of Molecular Vibrational Frequencies Consolidated" (PDF). National Bureau of Standards. NSRDS-NBS-39. Archived from the original (PDF) on 2016-08-04. Retrieved 2017-07-13.
2. King, W. H. (1984), "Isotope Shifts in X-Ray Spectra", Isotope Shifts in Atomic Spectra, Springer US, pp. 55–61, doi:10.1007/978-1-4899-1786-7_5, ISBN   9781489917881
3. Hughes, D. J.; Eckart, C. (1930). "The Effect of the Motion of the Nucleus on the Spectra of Li I and Li jII". Phys. Rev. 36 (4): 6s94–698. Bibcode:1930PhRv...36..694H. doi:10.1103/PhysRev.36.694.
4. H. Nagaoka and T. Mishima, Sci. Pap. Inst. Phys. Chem. Res. (Tokyo) 13, 293 (1930).
5. W. Pauli, R. E. Peierls, Phys. Z. 32 (1931) 670
6. Brix, P.; Kopfermann, H. (1951). "Neuere Ergebnisse zum Isotopieverschiebungseffekt in den Atomspektren". Festschrift zur Feier des Zweihundertjährigen Bestehens der Akademie der Wissenschaften in Göttingen. Springer. pp. 17–49. doi:10.1007/978-3-642-86703-3_2. ISBN   978-3-540-01540-6.
7. Kopfermann, H. (1958). Nuclear Moments . Academic Press.