[Basic Theory.1] Basic Theory
Energy Units and Molecular Spectra
Plane Polarized electromagetic radiation
![plane polarization](https://upload.wikimedia.org/wikipedia/commons/9/99/EM-Wave.gif)
[Figure. 1] illustrates a wave of polarized electromagnetic radiation traveling in the x-direction. The electric component is y-direction and magnetic is z-direction.
Hereafter, we consider only the former. (Don’t involve magnetic phenomena). The electric field strength (E) at a given time (t) is expressed by
\(E_0\) is the amplitude, \(\nu\) is the frequency of radiation.
The distance between two points of the same phase in successive waves is called the “wavelength” , \(\lambda\), which us measured in units.(\(\mathring{A}\)(angstrom), \(nm\)(nanometer), \(m\mu\)(millimicron), and \(cm\)(centimeter)). The relationships between them are:
Frequency
The frequency, \(\nu\) is the number of waves in the distance light travels in one second. Thus,
\[\nu = \frac{c}{\lambda} \tag{3}\]\(c\) is the velocity of light \((3 \times 10^{10} cm/s)\). And if \(\lambda\) is in the unit of centimeters, its dimension is \((cm/s)/(cm) = 1/s\). This “reciporal second” unit is also called the “hertz” \((Hz)\). There’s another parameter is the “wavenumber”, \(\tilde{\nu}\) defined by
\[\tilde{\nu} = \frac{\nu}{c} \tag{4}\]The difference between \(\nu\) and \(\tilde{\nu}\) is obvious. It has the dimension of \((1/s)/(cm/s) = 1/cm.\) By combining Eq.(3),Eq.(4) we have
\[\tilde{\nu} = \frac{\nu}{c} = \frac{1}{\lambda}(cm^{-1}) \tag{5}\]Also, we can express by \(v\)
\[\nu = \frac{c}{\lambda} = c \tilde{\nu} \tag{6}\]As shown earlier, the wavenumber\((\tilde{\nu})\) and frequency \((\nu)\) are different parameters, yet these two terms are often used interchangeably. Thus, we can express by IR and Raman spectrosopists such as “frequency shift of \(10 \;cm^{-1}\)”.
Interacts with an electromagetic field
We can know a transfer energy from the field to the molecule and it can occur only when Bohr’s frequency condition is satisfied.(If a molecule interacts with an electromagetic field).
\[\Delta E = h\nu = h\frac{c}{\lambda} = hc\tilde{\nu} \tag{7}\]Here \(h\) is Planck’s constant \((6.62 \times 10^{-27}erg\; s)\) and \(\Delta E\) is the difference in energy between two quantized states. Thus, \(\tilde{v}\) is directly proportional to the energy of transition.
Let’s Suppose that
\[\Delta E = E_2 - E_1 \tag{8}\]\(E_2\) : Energy of the exicted states, \(E_1\) : Energy of the gound states.
Then, the molecule absorbs \(\Delta E\) when it is exited from \(E_1\) to \(E_2\) ( \(E_1 \rightarrow E_2\) ) and emits \(\Delta E\) when it reverts from \(E_2\) to \(E_1\) ( \(E_2 \rightarrow E_1\) ).
We can express \(\Delta E\) in terms of various energy units. Thus, \(1 cm^{-1}\) is :
\[\begin{align} \Delta E &= E^2 - E^1 = hc\tilde{\nu} \\ &=[6.62 \times 10^{-27} (erg \; s)][3 \times 10^{10} (cm/s)][1(1/cm)] \\&= 1.99 \times 10^{-16} &\; (erg/molecule) \\ &= 1.99 \times 10^{-23} &\; (joule/molecule)\\ &= 2.86 &\; (cal/mole) \\ &=1.24 \times 10^{-4} &\; (eV/molecule) \end{align}\]Observed Region
We mainly concern with vibrational transitions which are observed in infrared(IR) or Raman Spectra. They appear in the \(10^{-4} \sim 10^2 \; (cm^{-1}) \;\) region and originate from vibrations of nuclei constituting the molecule. Raman spectra are related to electronic transitions. Thus, it is important to know the relationship between electronic and vibrational states.
![electromagnetic spectrum](https://www.researchgate.net/profile/Rekha-Gautam/publication/320505957/figure/fig1/AS:551293086965760@1508449922411/Overview-of-various-imaging-modalities-within-the-electromagnetic-spectrum.png)
Furthermore, vibrational spectra of small molecules in the gaseous state exhibit rotational fine structures. Thus, it’s also important to know the relationship between vibrational and rotational states. [Figure. 3]
![Energy levels of a diatomic molecule](https://www.researchgate.net/profile/Charles-Geiger/publication/239968471/figure/fig5/AS:341802461745158@1458503465601/Schematic-representation-of-various-energy-levels-of-a-diatomic-molecule-An-absorption.png)
Vibration of a Diatomic Molecule
Classical treatment
Consider the vibartion of a diatomic molucule in which two atoms are connected by a chemical bond.[Figure. 4]
![Energy levels of a diatomic molecule](/assets/images/posts/raman/two_atoms.png)
Each masses of atom 1 and 2 are \(m_1\) and \(m_2\) and \(r_1\) and \(r_2\) are the distances from the center of gravity (C.G.) to the atoms designated. Thus, \(r_1 + r_2\) is the equilibrium distance. Then, the conservation requires the ralationships:
Eq.9 and Eq.10 combine
\[x_1 = \Big(\frac{m_2}{m_1}\Big)x_2 \quad \text{or} \quad x_2=\Big(\frac{m_1}{m_2}\Big)x_1 \tag{11}\]In the classical treatment, we can regard the chemical bond as a spring. It obeys the Hooke’s law, so we can express the restoring force, \(f\) :
\[f = -K(x_1 + x_2) \tag{12}\]Where K is the force constant, and the directions of the force are opposite to each other. Now, combining the Eq.11 and Eq.12, we obtain :
\[f = -K \Big(\frac{m_1 + m_2}{m_1}\Big) = -K \Big(\frac{m_1 + m_2}{m_2}\Big) \tag {13}\]Using Newton’s equation of motion, we obtain for each atom as :
\[\begin{align} m_1\frac{d^2 x_1}{dt^2} = -K \Big(\frac{m_1 + m_2}{m_2}\Big)x1 \\ m_2\frac{d^2 x_2}{dt^2} = -K \Big(\frac{m_1 + m_2}{m_2}\Big)x2 \tag{14} \end{align}\]Multiply for each atom \(\Big(\frac{m_2}{m_1 + m_2} \Big)\) and adding, we obtain :
\[\frac{m_1 m_2}{m_1 + m_2} \Big(\frac{d^2 x_1}{dt^2} + \frac{d^2 x_2}{dt^2}\Big) = -K(x_1 + x_2) \tag{15}\]Introducing the reduced mass \((\mu)\) and the displacement \((q = x_1 + x_2)\), the Eq.15 is written as :
\[\mu \frac{d^2 q}{dt^2} = -Kq \tag{16}\]Here, the solution of thie differential equation is
\[q=q_0 sin(2\pi \nu_0 t + \varphi) \tag{17}\]where \(q_0\) is the maximum displacement and \(\varphi\) is the phase constant.(depends on the inital conditions.) \(v_0\) is the classical vibrational frequency given by
\[\nu_0 = \frac{1}{2\pi} \sqrt{\frac{K}{\mu}} \tag{18}\]We can calculate the potential energy \((V)\) and the kinetic energy \((T)\) as :
\[\begin{align*} dV &= -f\;dq = Kq\;dq \\ V &= \frac{1}{2}Kq^2 \\ &=\frac{1}{2} Kq^2_0 sin^2(2\pi \nu_0 t + \varphi) \\ &=2\pi^2 \nu_0^2 \mu q^2_0 sin^2(2\pi\nu_0 t + \varphi) \tag{19}\\ \\ T &= \frac{1}{2} m_1 \Big(\frac{dx_1}{dt}\Big)^2 + \frac{1}{2} m_2 \Big(\frac{dx_2}{dt} \Big)^2 \\ &= \frac{1}{2}\mu \Big(\frac{dq}{dt}\Big)^2 \\ &= 2\pi^2 \nu^2_0 \mu q_0^2 cos^2(2\pi \nu_0 t + \varphi) \tag{20} \end{align*}\]Thus, the total energy \((E)\) is :
\[\begin{align*} E &= T + V \\ &=2\pi^2\nu^2_0q_0^2 \quad (\because sin^2 x + cos^2 x = 1) \\ &= constant \tag{21} \end{align*}\]![Potentail energy diagram](/assets/images/posts/raman/Potential energy diagram.png)
[Figure. 5] is based on the book. It shows the plot of \(V\) as a function of \(q\) and looks like a vibrator called a harmonic oscillator.
Quantum Mechanics
Considering a motion of a single particle having mass \(\mu\), the vibration can be written for the Schrödinger equation as
\[\frac{d^2 \psi}{dq^2} + \frac{8 \pi^2 \mu }{h^2} \Big(E-\frac{1}{2}Kq^2 \Big)\psi = 0 \tag{22}\]If the \(\psi\) must be single-valued,finite and continuous, the eigenvalues are written as by solving the Eq.22 :
\[E_v = h\nu \Big(v + \frac{1}{2} \Big) = hc\tilde{\nu} \Big( v + \frac{1}{2}\Big) \tag{23}\]And the frequency of vibration is as follows seems like Eq.18
\[\nu = \frac{1}{2\pi} \sqrt{\frac{K}{\mu}} \tag{24}\]where \(v\) is the vibrational quantum number, and having the values 0,1,2… So, the corresponding eigenfunctions are :
\[\psi _v = \frac{(\alpha / \pi)^{1/4}}{\sqrt{2^{\mathrm{v}} v!}}e^{-\alpha q^2 / 2} H_v(\sqrt{\alpha q}) \tag{25}\]where \(\alpha = 2\pi \sqrt{\mu K/h} = 4\pi^2 \mu v/h\) and \(H_v(\sqrt{\alpha q})\) is a Hermite polynomial of the $\mathrm{v}^{th} $ degree.
Thus, the eigenvalues and the corresponding eigenfunctions are
\[\begin{align*} &v = 0, \quad E_0 = \frac{1}{2} hv, \quad \psi _0 = (\alpha / \pi)^{1/4} e^{-\alpha q^2 /2} \\ &v = 1, \quad E_1 = \frac{3}{2} hv, \quad \psi _1 = (\alpha / \pi)^{1/4} 2^{1/2}qe^{-\alpha q^2 /2} \tag{26} \end{align*}\] \[\vdots\]Difference of the frequency between classical & quantum-mechanical
The quantum mechanical frequency(Eq.24) is same as the classical frequency(Eq.18). However, there are some differences noted between the two treatments.
First, the zero-state Engergy. Classicaly, the energy E is zero when q is zero.
\[q=0 \rightarrow E=0 \tag{27-1}\]But, in the Quantum-mechanically, the lowest E state \((v=0)\) has the energy, \(\frac{1}{2} h\nu\) (=zero point energy). That’s because the Heisenberg’s uncertainly prinicple.
\[v=0 \rightarrow E = \frac{1}{2} h\nu \quad (\because uncertainly principle) \tag{27-2}\]Second, continuity of a vibrator. Classicaly, vibrator can change contiuosly. But In quantum mechanics, the energy, E can change only in units of \(h\nu\).
Vibrator | Continuity |
---|---|
Classical | continuous |
Quantum | units of $h\nu$ |
Thirdly, probability of breakaway from the parabola. Classically, the vibration is confined within the parabola. Because if $\vert q \vert > \vert q_0 \vert$, the T becomes negative. Contrary, in quantum-mechanics, the probability (of finding q outside the parabola) is not zero since the tunnel effect.
Hot Band
![Internuclear Distance](https://upload.wikimedia.org/wikipedia/commons/thumb/7/7a/Morse-potential.png/800px-Morse-potential.png)
Hereafter, talk about the separation between the two vibrational levels.
In the case of a harmonic oscillator, that is always same with $h\nu$. But an actual molecule is not the case. The potential is approximated by the Morse potential function shown by the solid curve like [Figure. 6].
where $D_e$ is the dissociation energy, $\beta$ is a measure of the curvature an the bottom of the potentail well.
The eigenvalues by solving with the Schrödinger equation :
where $w_e$ is the wavenumber corrected for anharmonicity, $\chi_e w_e$ indicates the magnitude of anharmonicity.
By Eq.29, the E levels of the anharmonic oscillator are no longer equidistant. And the separtion decreases with increasing $\nu$ like [Figure. 6].
According to quantum-mechanics, Only in a harmonic oscillator, those transitions involving $\Delta v = \pm 1 $ are allowed. Else, the transitions involving $\Delta v = \pm 2, \pm 3, \dots$ (overtones). Both in IR and Raman spectra, many $\Delta v = \pm 1 $ transitions that of $v = 0 \leftrightarrow 1 $ appears most strongly. That is expected from the Maxwell-Boltzmann distribution law, which states that the population ration of the $v=1 $ and $v = 0$ states is given by
where $\Delta E$ is the energy difference between the two states, $k$ is Boltzmann’s constant $(1.3807 \times 10^{-16} \; erg/degree)$, and $T$ is the absolute temperature. Since $\Delta E = hc\tilde{v}$, the ratio is inversely proportional with $\tilde{v}$. $(\frac{P_{v=1}}{P_{v=0}} \propto \frac{1}{\tilde{v}}) $
Example, the $\tilde{v}$ of $\mathrm{H}_2$ is $4,160 \; cm^{-1}$, $T$ is room temperature $(300K)$
\[\begin{align*} kT &= 1.38 \times 10^{-6} \; (erg/degree) \quad 300 \; (degree) \\ &= [4.14 \times 10^{-14} \; (erg)] / [1.99 \times 10^{-16} \; (erg)(cm^{-1})] \\ &= 208 \; (cm^{-1}) \tag{31} \\ \end{align*}\]Then, the ratio is
\[\frac{P_{v=1}}{P_{v=0}}=e^{-hc(4,160)/208} = 2.19 \times 10^{-9} \tag{32}\]That means almost all of the molecules are at $v=0$.
If $\tilde{v} = 213 \; cm^{-1} $ ( $I_2$ molecule), the ratio is 0.36. That is abpit 27% of the $I_2$ molecules are at $v=1$ state. In this case, the transition $ v = 1 \rightarrow 2 $ should be observed on the low-frequency side of the fundamental with much less intensity. Such a transition is called a “hot band” since it tends to appear at higher temperatures.
Origin of Raman Spectra
IR absorption
Now measure the absorption of IR by the sample as a function of frequency. The molecule absorbs $\Delta E = hv$ from the IR source at each vibrational transition. The intensity of IR absorption is governed by the Beer-Lambert Law :
\[I = I_0 e^{-\varepsilon c d} \tag{33}\]In IR spectroscopy, it’s customary to plot the percentage transmission $(T)$ versus wave number $(\tilde{\nu})$:
\[T(\%) = \frac{I}{I_0} \times 100 \tag{34}\]Note : $T(\%)$ is not proportional to $c$.
For quntitative analysis, the absorbance $(A)$ defined here should be used:
Raman spectra
![Differences in mechanism of Raman vs IR](/assets/images/posts/raman/RamanIR.jpeg)
In [Figure. 7], Raman spectra is different from that of IR spectra. The scattered light from the sample is observed in the direction perpendicualr to the incident beam. That consists of two types :
- Rayleigh scattering : is strong and has the same frequency as the incident beam.
- Raman scattering : is very weak ( $ ~ 10^{-5} $ of the incident beam) and has frequencies $ \nu_0 \pm \nu_m$
At the Raman scattering, $\nu_0 - \nu_m$ is Stokes, and $\nu_0 + \nu_m$ is anti-Stokes lines. Thus, we measure the vibrational frequncy $(\nu_m)$ as a shift from the incident beam frequncy $(\nu_0)$.
In classical theory, Raman scattering follows:
If a diatomic molecule is irradiated, an electric dipole moment P is induced :
\[P = \alpha E = \alpha E_0 cos 2\pi \nu_0 t \tag{37}\]The $\alpha$ is a proportionally constant ( polarizability). Frequency of the vibrating molecule is $\nu_m$, $q_0$ is the vibrational amplitude, the nuclear displacement q:
\[q = q_0 cos 2\pi \nu_m t \tag{38}\]For a small amplitude of vibration, $\alpha$ is a linear function of q. Thus, we can write
\[\alpha = \alpha_0 + \Big(\frac{\partial \alpha}{\partial q} \Big)_0 q_0 + \cdots \tag{39}\]Combining Eq.37 & Eq.38, we obtain :
\[\begin{align} \\ P &= \alpha E_0 cos 2\pi \nu_0 t \\ &= \alpha_0 e_0 cos 2\pi \nu_0 t + \Big(\frac{\partial \alpha}{\partial q}\Big)_0 q E_0 cos 2\pi \nu_0 t \\ &= \alpha_0 E_0 cos 2\pi \nu_0 t + \Big(\frac{\partial \alpha}{\partial q}\Big)_0 q_0 E_0 cos2\pi \nu_0 t cos 2\pi \nu_m t \\ &= \alpha_0 E_0 cos 2\pi \nu_0 t + \frac{1}{2} \Big(\frac{\partial \alpha}{\partial q})_0 q_0 E_0 [cos {2\pi(\nu_0 + \nu_m)t} + cos {2\pi (\nu_0 - \nu_m)t}] \tag{39} \\ \end{align}\]
Leave a comment