5.2: The Equation for a HarmonicOscillator Model of a Diatomic Molecule Contains the Reduced Mass of the Molecule
 Page ID
 13414
For studying the energetics of molecular vibration we take the simplest example, a diatomic heteronuclear molecule \(\ce{AB}\). Let the respective masses of atoms \(\ce{A}\) and \(\ce{B}\) be \(m_A\) and \(m_B\). For diatomic molecules, we define the reduced mass \(\mu_{AB}\) by:
\[ \mu_{AB}=\dfrac{m_A\, m_B}{m_A+m_B} \label{5.2.1}\]
Reduced mass is the representation of a twobody system as a singlebody one. When the motion (displacement, vibrational, rotational) of two bodies are only under mutual interactions, the inertial mass of the moving body with respect to the body at rest can be simplified to a reduced mass.
Reduced Mass
Viewing the multibody system as a single particle allows the separation of the motion: vibration and rotation, of the particle from the displacement of the center of mass. This approach greatly simplifies many calculations and problems.
This concept is readily used in the general motion of diatomics, i.e. simple harmonic oscillator (vibrational displacement between two bodies, following Hooke's Law), the rigid rotor approximation (the moment of inertia about the center of mass of a twobody system), spectroscopy, and many other applications.
Determine the reduced mass of the two body system of a proton and electron with \(m_{proton} = 1.6727 \times 10^{27}\, kg\) and \(m_{electron} = 9.110 \times 10^{31}\, kg\)).
 Answer

\[\begin{align*} \mu_{pe} &= \dfrac{(1.6727 \times 10^{27})(9.110 \times 10^{31})}{1.6727 \times 10^{27} + 9.110 \times 10^{31}} \\[4pt] &= 9.105 \times 10^{31} kg \end{align*}\]
The Quantum Harmonic Oscillator
The classical Harmonic Oscillator approximation is a simple yet powerful representation of the energetics of an oscillating spring system. Central to this model is the formulation of the quadratic potential energy
\[V(x) \approx \dfrac {1}{2} kx^2 \label{potential}\]
One problem with this classical formulation is that it is not general. We cannot use it, for example, to describe vibrations of diatomic molecules, where quantum effects are important. This require the formulation for Schrödinger Equation using Equation \ref{potential}.
\[ \hat{H}  \psi \rangle = \left[ \dfrac {\hbar^2}{2\mu} \dfrac {d^2 }{d x^2} + \dfrac {1}{2}kx^2 \right ]  \psi \rangle = E\psi \rangle\]
Solving this quantum harmonic oscillator is appreciably harder than solving the Schrödinger Equation for the simpler particleinthebox model and is outside the scope of this text. However, as with most quantum modules (and in contrast to the classical harmonic oscillator), the energies are quantized in terms of a quantum number (\(v\) in this case):
\[ \begin{align} E_v &= \hbar \left(\sqrt {\dfrac {k}{\mu}} \right) \left(v + \dfrac {1}{2} \right) \\[4pt] &= h \nu \left(v+\dfrac {1}{2} \right) \end{align} \]
with the natural vibrational frequency of the system given as
\[\nu = \dfrac{1}{2 \pi}\sqrt {\dfrac {k}{\mu}} \label{freq}\]
and the mass, \(\mu\), is the reduced mass of the system (Equation \ref{5.2.1}).
Be careful to distinguish \(\nu\), the symbol for the natural frequency (as a Greek nu) from \(v\) the quantum harmonic oscillator quantum number (Latin v).
The vibrational frequencies given by Equation \ref{freq} depend on the force constants (\(k\)) and the atomic masses of the vibrating nuclei via the reduced mass (\(\mu\)). It should be clear that the substitution of one isotope of an atom in a molecule for another isotope will affect the atomic masses and therefore the reduced mass (via Equation \ref{5.2.1}) and therefore the vibrational frequencies (via Equation \ref{freq}).
It is important to remember that the Periodic Table gives only atomic weights of elements, which are scaled averages of atoms normally encountered in the laboratory (Table 5.2.1 ). To properly discuss vibrational frequencies of molecules, we need to know (or denote) the specific isotopes in the molecule. Check Table A4 for that information.
atomic mass (in amu) 
isotopic abundance (%) 


^{1}H 
1.007825 
99.985 
^{2}H 
2.0140 
0.015 
^{35}Cl 
35.968852 
75.77 
^{37}Cl 
36.965903 
24.23 
^{79}Br 
78.918336 
50.69 
^{81}Br 
80.916289 
49.31 
What are the reduced mass for \(\ce{^1H^35Cl}\) and \(\ce{^1H^37Cl}\)? If the spring constants for vibrations of both molecules are equal and estimated at \(478 \,N/m\), what are the natural vibrational frequencies of these two molecules?
Solution
The periodic table gives an atomic weight of 35.45 amu for chlorine, but remember this is the the average of the natural abundances of different chlorine isotopes which is dictated primary by two isotopes: \(\ce{^35Cl}\) and \(\ce{^37Cl}\). For this problem, we need the exact mass of the \(\ce{^1H}\), \(\ce{^35Cl}\), and \(\ce{^37Cl}\) isotopes. Check Table A4 for that information.
For \(\ce{^1H^35Cl}\):
\[\begin{align*} \text{Reduced mass} &= \dfrac{m_1m_2}{m_1+m_2} \\[4pt] &= \dfrac{m_\ce{H}m_\ce{^35Cl}}{m_\ce{H}+m_\ce{^35Cl}} \\[4pt] &= \dfrac{(1.0078)(34.9688)}{1.0078 + 34.9688)}\, amu \\[4pt] &= 0.9796\,amu\end{align*}\]
or when converted into kg is \(1.629 \times 10^{27}\,kg\).
For \(\ce{^1H^37Cl}\):
\[\begin{align*} \text{Reduced mass} &= \dfrac{m_1m_2}{m_1+m_2} \\[4pt] &= \dfrac{m_\ce{H}m_\ce{^37Cl}}{m_\ce{H}+m_\ce{^37Cl}} \\[4pt] &= \dfrac{(1.0078)(36.965)}{1.0078 + 36.965)}\, amu \\[4pt] &= 0.9810\,amu\end{align*}\]
or when converted into kg is \(1.6291 \times 10^{27}\,kg\). This is only 0.29% bigger.
Equation \ref{freq} is used to predict the respective vibrational frequencies of these two molecules.
For \(\ce{^1H^35Cl}\):
\[\begin{align*} \nu &= \dfrac{1}{2 \pi}\sqrt {\dfrac {k}{\mu}} \\[4pt] &= \dfrac{1}{2 \pi}\sqrt {\dfrac {478 \,N/m}{1.629 \times 10^{27}\,kg}} \\[4pt] &= 8.6394×10^{13} s^{1} \end{align*}\]
For \(\ce{^1H^37Cl}\):
\[\begin{align*} \nu &= \dfrac{1}{2 \pi}\sqrt {\dfrac {k}{\mu}} \\[4pt] &= \dfrac{1}{2 \pi}\sqrt {\dfrac {478 \,N/m}{1.629 \times 10^{27}\,kg}} \\[4pt] &= 8.621×10^{13} s^{1} \end{align*}\]
As with the differences in the reduced masses, the differences in the vibrational frequencies of these two molecules is quite small. However, high resolution IR spectroscopy can easily distinguish the vibrations between these two molecules. Exercise 5.2.1 will demonstrate that this "isotope effect" is not always a small effect.
The force constant is weakly sensitive to the specific isotopes in a molecule (and we typically assume it is isotope independent). If the \(k = 478 \,N/m\) for both \(\ce{H^{35}Cl}\) and \(\ce{H^{37}Cl}\). What are the vibration frequencies in these two diatomic molecules.
 Answer

\(\ce{H^{35}Cl}\): 2886 cm^{1}
\(\ce{D^{35}Cl}\): 2081 cm^{1}
Contributors and Attributions
 Eugene Lee