Rotational–vibrational spectroscopy

Rotational–vibrational spectroscopy is a branch of molecular spectroscopy concerned with infrared and Raman spectra of molecules in the gas phase. Transitions involving changes in both vibrational and rotational states can be abbreviated as rovibrational (or ro-vibrational) transitions. When such transitions emit or absorb photons (electromagnetic radiation), the frequency is proportional to the difference in energy levels and can be detected by certain kinds of spectroscopy. Since changes in rotational energy levels are typically much smaller than changes in vibrational energy levels, changes in rotational state are said to give fine structure to the vibrational spectrum. For a given vibrational transition, the same theoretical treatment as for pure rotational spectroscopy gives the rotational quantum numbers, energy levels, and selection rules. In linear and spherical top molecules, rotational lines are found as simple progressions at both higher and lower frequencies relative to the pure vibration frequency. In symmetric top molecules the transitions are classified as parallel when the dipole moment change is parallel to the principal axis of rotation, and perpendicular when the change is perpendicular to that axis. The ro-vibrational spectrum of the asymmetric rotor water is important because of the presence of water vapor in the atmosphere.

Overview

Ro-vibrational spectroscopy concerns molecules in the gas phase. There are sequences of quantized rotational levels associated with both the ground and excited vibrational states. The spectra are often resolved into lines due to transitions from one rotational level in the ground vibrational state to one rotational level in the vibrationally excited state. The lines corresponding to a given vibrational transition form a band.[1]

In the simplest cases the part of the infrared spectrum involving vibrational transitions with the same rotational quantum number (ΔJ = 0) in ground and excited states is called the Q-branch. On the high frequency side of the Q-branch the energy of rotational transitions is added to the energy of the vibrational transition. This is known as the R-branch of the spectrum for ΔJ = +1. The P-branch for ΔJ = −1 lies on the low wavenumber side of the Q branch. The appearance of the R-branch is very similar to the appearance of the pure rotation spectrum, and the P-branch appears as a nearly mirror image of the R-branch.[note 1]

The appearance of rotational fine structure is determined by the symmetry of the molecular rotors which are classified, in the same way as for pure rotational spectroscopy, into linear molecules, spherical-, symmetric- and asymmetric- rotor classes. The quantum mechanical treatment of rotational fine structure is the same as for pure rotation.

A general convention is to label quantities that refer to the vibrational ground and excited states of a transition with double prime and single prime, respectively. For example, the rotational constant for the ground state is written as ${\displaystyle B^{\prime \prime },}$ and that of the excited state as ${\displaystyle B^{\prime }.}$ Also, these constants are expressed in the molecular spectroscopist's units of cm⁻¹. so that ${\displaystyle B}$ in this article corresponds to ${\displaystyle {\bar {B}}=B/hc}$ in the definition of rotational constant at Rigid rotor.

Method of combination differences

Numerical analysis of ro-vibrational spectral data would appear to be complicated by the fact that the wavenumber for each transition depends on two rotational constants, ${\displaystyle B^{\prime \prime }}$ and ${\displaystyle B^{\prime }}$. However combinations which depend on only one rotational constant are found by subtracting wavenumbers of pairs of lines (one in the P-branch and one in the R-branch) which have either the same lower level or the same upper level.[2][3] For example, in a diatomic molecule the line denoted P(J + 1) is due to the transition (v = 0, J + 1) → (v = 1, J), and the line R(J − 1) is due to the transition (v = 0, J − 1) → (v = 1, J). The difference between the two wavenumbers corresponds to the energy difference between the (J + 1) and (J − 1) levels of the lower vibrational state and denoted by ${\displaystyle \Delta _{2}}$ since it is the difference between levels differing by two units of J. If centrifugal distortion is included, it is given by[4]

${\displaystyle \Delta _{2}^{\prime \prime }F(J)={\bar {\nu }}[R(J-1)]-{\bar {\nu }}[P(J+1)]=(2B^{\prime \prime }-3D^{\prime \prime })\left(2J+1\right)-D^{\prime \prime }\left(2J+1\right)^{3}}$

The rotational constant of the ground vibrational state B′′ and centrifugal distortion constant, D′′ can be found by least-squares fitting this difference as a function of J. The constant B′′ is used to determine the internuclear distance in the ground state as in pure rotational spectroscopy. (See Appendix)

Similarly the difference R(J) − P(J) depends only on the constants B′ and D′ for the excited vibrational state (v = 1), and B′ can be used to determine the internuclear distance in that state (which is inaccessible to pure rotational spectroscopy).

${\displaystyle \Delta _{2}^{\prime }F(J)={\bar {\nu }}[R(J)]-{\bar {\nu }}[P(J)]=(2B^{\prime }-3D^{\prime })\left(2J+1\right)-D^{\prime }\left(2J+1\right)^{3}}$

Linear molecules

Heteronuclear diatomic molecules

Simulated vibration-rotation line spectrum of carbon monoxide, ¹²C¹⁶O. The P-branch is to the left of the gap near 2140 cm⁻¹, the R-branch on the right.[note 2]

Schematic ro-vibrational energy level diagram for a linear molecule

Diatomic molecules with the general formula AB have one normal mode of vibration involving stretching of the A-B bond. The vibrational term values ${\displaystyle G(v)}$,[note 3] for an anharmonic oscillator are given, to a first approximation, by

${\displaystyle G(v)=\omega _{e}\left(v+{1 \over 2}\right)-\omega _{e}\chi _{e}\left(v+{1 \over 2}\right)^{2}\,}$

where v is a vibrational quantum number, ω_e is the harmonic wavenumber and χ_e is an anharmonicity constant.

When the molecule is in the gas phase, it can rotate about an axis, perpendicular to the molecular axis, passing through the centre of mass of the molecule. The rotational energy is also quantized, with term values to a first approximation given by

${\displaystyle F_{v}(J)=B_{v}J\left(J+1\right)-DJ^{2}\left(J+1\right)^{2}}$

where J is a rotational quantum number and D is a centrifugal distortion constant. The rotational constant, B_v depends on the moment of inertia of the molecule, I_v, which varies with the vibrational quantum number, v

${\displaystyle B_{v}={h \over {8\pi ^{2}cI_{v}}};\quad I_{v}={\frac {m_{A}m_{B}}{m_{A}+m_{B}}}d_{v}^{2}}$

where m_A and m_B are the masses of the atoms A and B, and d represents the distance between the atoms. The term values of the ro-vibrational states are found (in the Born–Oppenheimer approximation) by combining the expressions for vibration and rotation.

${\displaystyle G(v)+F_{v}(J)=\left[\omega _{e}\left(v+{1 \over 2}\right)+B_{v}J(J+1)\right]-\left[\omega _{e}\chi _{e}\left(v+{1 \over 2}\right)^{2}+DJ^{2}(J+1)^{2}\right]}$

The first two terms in this expression correspond to a harmonic oscillator and a rigid rotor, the second pair of terms make a correction for anharmonicity and centrifugal distortion. A more general expression was given by Dunham.

The selection rule for electric dipole allowed ro-vibrational transitions, in the case of a diamagnetic diatomic molecule is

${\displaystyle \Delta v=\pm 1\ (\pm 2,\pm 3,{\textit {etc.}}}$[note 4]${\displaystyle ),\Delta J=\pm 1}$

The transition with Δv=±1 is known as the fundamental transition. The selection rule has two consequences.

1. Both the vibrational and rotational quantum numbers must change. The transition :${\displaystyle \Delta v=\pm 1,\Delta J=0}$ (Q-branch) is forbidden
2. The energy change of rotation can be either subtracted from or added to the energy change of vibration, giving the P- and R- branches of the spectrum, respectively.

The calculation of the transition wavenumbers is more complicated than for pure rotation because the rotational constant B_ν is different in the ground and excited vibrational states. A simplified expression for the wavenumbers is obtained when the centrifugal distortion constants ${\displaystyle D^{\prime }}$ and ${\displaystyle D^{\prime \prime }}$ are approximately equal to each other.[5]

${\displaystyle {\bar {\nu }}=\omega _{0}+(B^{\prime }+B^{\prime \prime })m+(B^{\prime }-B^{\prime \prime })m^{2}-2(D^{\prime }+D^{\prime \prime })m^{3},\quad \omega _{0}=\omega _{e}(1-2\chi _{e})\quad m=\pm 1,\pm 2\ etc.}$

Spectrum of R-branch of nitric oxide, NO, simulated with Spectralcalc,[6] showing λ-doubling caused by the presence of an unpaired electron in the molecule

where positive m values refer to the R-branch and negative values refer to the P-branch. The term ω₀ gives the position of the (missing) Q-branch, the term ${\displaystyle (B^{\prime }+B^{\prime \prime })m}$ implies an progression of equally spaced lines in the P- and R- branches, but the third term, ${\displaystyle (B^{\prime }-B^{\prime \prime })m^{2}}$shows that the separation between adjacent lines changes with changing rotational quantum number. When ${\displaystyle B^{\prime \prime }}$ is greater than ${\displaystyle B^{\prime }}$, as is usually the case, as J increases the separation between lines decreases in the R-branch and increases in the P-branch. Analysis of data from the infrared spectrum of carbon monoxide, gives value of ${\displaystyle B^{\prime \prime }}$ of 1.915 cm⁻¹ and ${\displaystyle B^{\prime }}$ of 1.898 cm⁻¹. The bond lengths are easily obtained from these constants as r₀ = 113.3 pm, r₁ = 113.6 pm.[7] These bond lengths are slightly different from the equilibrium bond length. This is because there is zero-point energy in the vibrational ground state, whereas the equilibrium bond length is at the minimum in the potential energy curve. The relation between the rotational constants is given by

${\displaystyle B_{v}=B_{eq}-\alpha \left(v+{1 \over 2}\right)}$

where ν is a vibrational quantum number and α is a vibration-rotation interaction constant which can be calculated when the B values for two different vibrational states can be found. For carbon monoxide r_eq = 113.0 pm.[8]

Nitric oxide, NO, is a special case as the molecule is paramagnetic, with one unpaired electron. Coupling of the electron spin angular momentum with the molecular vibration causes lambda-doubling[note 5] with calculated harmonic frequencies of 1904.03 and 1903.68 cm⁻¹. Rotational levels are also split.[9]

Homonuclear diatomic molecules

The quantum mechanics for homonuclear diatomic molecules such as dinitrogen, N₂, and fluorine, F₂, is qualitatively the same as for heteronuclear diatomic molecules, but the selection rules governing transitions are different. Since the electric dipole moment of the homonuclear diatomics is zero, the fundamental vibrational transition is electric-dipole-forbidden and the molecules are infrared inactive.[10] However, a weak quadrupole-allowed spectrum of N₂ can be observed when using long path-lengths both in the laboratory and in the atmosphere.[11] The spectra of these molecules can be observed by Raman spectroscopy because the molecular vibration is Raman-allowed.

Dioxygen is a special case as the molecule is paramagnetic so magnetic-dipole-allowed transitions can be observed in the infrared.[11] The unit electron spin has three spatial orientations with respect to the molecular rotational angular momentum vector, N,[note 6] so that each rotational level is split into three states with total angular momentum (molecular rotation plus electron spin) ${\displaystyle \mathrm {J\hbar } \,}$, J = N + 1, N, and N - 1, each J state of this so-called p-type triplet arising from a different orientation of the spin with respect to the rotational motion of the molecule.[12] Selection rules for magnetic dipole transitions allow transitions between successive members of the triplet (ΔJ = ±1) so that for each value of the rotational angular momentum quantum number N there are two allowed transitions. The ¹⁶O nucleus has zero nuclear spin angular momentum, so that symmetry considerations demand that N may only have odd values.[13][14]

Raman spectra of diatomic molecules

The selection rule is

${\displaystyle \Delta J=0,\pm 2}$

so that the spectrum has an O-branch (∆J = −2), a Q-branch (∆J = 0) and an S-branch (∆J=+2). In the approximation that B′′ = B′ = B the wavenumbers are given by

${\displaystyle {\bar {\nu }}(S(J))=\omega _{0}+4BJ+6B=\omega _{0}+6B,\quad \omega _{0}+10B,\quad \omega _{0}+14B,\quad ...}$

${\displaystyle {\bar {\nu }}(O(J))=\omega _{0}-4BJ+2B=\omega _{0}-6B,\quad \omega _{0}-10B,\quad \omega _{0}-14B,\quad ...}$

since the S-branch starts at J=0 and the O-branch at J=2. So, to a first approximation, the separation between S(0) and O(2) is 12B and the separation between adjacent lines in both O- and S- branches is 4B. The most obvious effect of the fact that B′′ ≠ B′ is that the Q-branch has a series of closely spaced side lines on the low-frequency side due to transitions in which ΔJ=0 for J=1,2 etc.[15] Useful difference formulae, neglecting centrifugal distortion are as follows.[16]

${\displaystyle \Delta _{4}^{\prime \prime }F(J)={\bar {\nu }}[S(J-2)]-{\bar {\nu }}[O(J+2)]=4B^{\prime \prime }(2J+1)}$

${\displaystyle \Delta _{4}^{\prime }F(J)={\bar {\nu }}[S(J)]-{\bar {\nu }}[O(J)]=4B^{\prime }(2J+1)}$

Molecular oxygen is a special case as the molecule is paramagnetic, with two unpaired electrons.[17]

For homonuclear diatomics, nuclear spin statistical weights lead to alternating line intensities between even-${\displaystyle J^{\prime \prime }}$ and odd-${\displaystyle J^{\prime \prime }}$ levels. For nuclear spin I = 1/2 as in ¹H₂ and ¹⁹F₂ the intensity alternation is 1:3. For ²H₂ and ¹⁴N₂, I=1 and the statistical weights are 6 and 3 so that the even-${\displaystyle J^{\prime \prime }}$ levels are twice as intense. For ¹⁶O₂ (I=0) all transitions with even values of ${\displaystyle J^{\prime \prime }}$ are forbidden.[16]

Polyatomic linear molecules

Spectrum of bending mode in ^14N^14N^16O simulated with Spectralcalc.[6] The weak superimposed spectrum is due to species containing ^15N at natural abundance of 0.3%

Spectrum of a perpendicular band from acetylene, C2H2, simulated with Spectralcalc[6] showing 1,3 intensity alternation in both P- and R- branches. See also Hollas p157

Spectrum of the asymmetric stretching (parallel) band of carbon dioxide, ^12C^16O2 simulated with Spectralcalc.[6] The weak superimposed spectrum is due to absorption of the first vibrationally excited level (0 1^1 0), which due to its low energy is populated at room temperature

These molecules fall into two classes, according to symmetry: centrosymmetric molecules with point group D_∞h, such as carbon dioxide, CO₂, and ethyne or acetylene, HCCH; and non-centrosymmetric molecules with point group C_∞v such as hydrogen cyanide, HCN, and nitrous oxide, NNO. Centrosymmetric linear molecules have a dipole moment of zero, so do not show a pure rotation spectrum in the infrared or microwave regions. On the other hand, in certain vibrational excited states the molecules do have a dipole moment so that a ro-vibrational spectrum can be observed in the infrared.

The spectra of these molecules are classified according to the direction of the dipole moment change vector. When the vibration induces a dipole moment change pointing along the molecular axis the term parallel is applied, with the symbol ${\displaystyle \parallel }$. When the vibration induces a dipole moment pointing perpendicular to the molecular axis the term perpendicular is applied, with the symbol ${\displaystyle \perp }$. In both cases the P- and R- branch wavenumbers follow the same trend as in diatomic molecules. The two classes differ in the selection rules that apply to ro-vibrational transitions.[18] For parallel transitions the selection rule is the same as for diatomic molecules, namely, the transition corresponding to the Q-branch is forbidden. An example is the C-H stretching mode of hydrogen cyanide.[19]

For a perpendicular vibration the transition ΔJ=0 is allowed. This means that the transition is allowed for the molecule with the same rotational quantum number in the ground and excited vibrational state, for all the populated rotational states. This makes for an intense, relatively broad, Q-branch consisting of overlapping lines due to each rotational state. The N-N-O bending mode of nitrous oxide, at ca. 590 cm⁻¹ is an example.[6]

The spectra of centrosymmetric molecules exhibit alternating line intensities due to quantum state symmetry effects, since rotation of the molecule by 180° about a 2-fold rotation axis is equivalent to exchanging identical nuclei. In carbon dioxide, the oxygen atoms of the predominant isotopic species ¹²C¹⁶O₂ have spin zero and are bosons, so that the total wavefunction must be symmetric when the two ¹⁶O nuclei are exchanged. The nuclear spin factor is always symmetric for two spin-zero nuclei, so that the rotational factor must also be symmetric which is true only for even-J levels. The odd-J rotational levels cannot exist and the allowed vibrational bands consist of only absorption lines from even-J initial levels. The separation between adjacent lines in the P- and R- branches is close to 4B rather than 2B as alternate lines are missing.[20] For acetylene the hydrogens of ¹H¹²C¹²C¹H have spin ½ and are fermions, so the total wavefunction is antisymmetric when two ¹H nuclei are exchanged. As is true for ortho and para hydrogen the nuclear spin function of the two hydrogens has three symmetric ortho states and one antisymmetric para states. For the three ortho states, the rotational wave function must be antisymmetric corresponding to odd J, and for the one para state it is symmetric corresponding to even J. The population of the odd J levels are therefore three times higher than the even J levels, and alternate line intensities are in the ratio 3:1.[21][22]

Spherical top molecules

Upper: low-resolution infrared spectrum of asymmetric stretching band of methane (CH₄); lower: PGOPHER[23] simulated line spectrum, ignoring Coriolis coupling

These molecules have equal moments of inertia about any axis, and belong to the point groups T_d (tetrahedral AX₄) and O_h (octahedral AX₆). Molecules with these symmetries have a dipole moment of zero, so do not have a pure rotation spectrum in the infrared or microwave regions.[24]

Tetrahedral molecules such as methane, CH₄, have infrared-active stretching and bending vibrations, belonging to the T₂ (sometimes written as F₂) representation.[note 7] These vibrations are triply degenerate and the rotational energy levels have three components separated by the Coriolis interaction.[25] The rotational term values are given, to a first order approximation, by[26]

${\displaystyle F^{+}=B_{\nu }J(J+1)+2B_{\nu }\zeta _{r}(J+1)}$

${\displaystyle F^{0}=B_{\nu }J(J+1)}$

${\displaystyle F^{-}=B_{\nu }J(J+1)-2B_{\nu }\zeta _{r}(J+1)}$

where ${\displaystyle \zeta _{r}}$ is a constant for Coriolis coupling. The selection rule for a fundamental vibration is

${\displaystyle \Delta J=0,\pm 1}$

Thus, the spectrum is very much like the spectrum from a perpendicular vibration of a linear molecule, with a strong Q-branch composed of many transitions in which the rotational quantum number is the same in the vibrational ground and excited states, ${\displaystyle J^{\prime }=J^{\prime \prime }=1,2...}$ The effect of Coriolis coupling is clearly visible in the C-H stretching vibration of methane, though detailed study has shown that the first-order formula for Coriolis coupling, given above, is not adequate for methane.[27][28][29]

Symmetric top molecules

These molecules have a unique principal rotation axis of order 3 or higher. There are two distinct moments of inertia and therefore two rotational constants. For rotation about any axis perpendicular to the unique axis, the moment of inertia is ${\displaystyle I_{\perp }}$ and the rotational constant is ${\displaystyle B={h \over {8\pi ^{2}cI_{\perp }}}}$, as for linear molecules. For rotation about the unique axis, however, the moment of inertia is ${\displaystyle I_{\parallel }}$ and the rotational constant is ${\displaystyle A={h \over {8\pi ^{2}cI_{\parallel }}}}$. Examples include ammonia, NH₃ and methyl chloride, CH₃Cl (both of molecular symmetry described by point group C_3v), boron trifluoride, BF₃ and phosphorus pentachloride, PCl₅ (both of point group D_3h), and benzene, C₆H₆ (point group D_6h).

For symmetric rotors a quantum number J is associated with the total angular momentum of the molecule. For a given value of J, there is a 2J+1- fold degeneracy with the quantum number, M taking the values +J ...0 ... -J. The third quantum number, K is associated with rotation about the principal rotation axis of the molecule. As with linear molecules, transitions are classified as parallel, ${\displaystyle \parallel }$ or perpendicular,${\displaystyle \perp }$, in this case according to the direction of the dipole moment change with respect to the principal rotation axis. A third category involves certain overtones and combination bands which share the properties of both parallel and perpendicular transitions. The selection rules are

${\displaystyle \parallel }$ If K ≠ 0, then ΔJ = 0, ±1 and ΔK = 0

If K = 0, then ΔJ = ±1 and ΔK = 0

${\displaystyle \perp }$ ΔJ = 0, ±1 and ΔK = ±1

The fact that the selection rules are different is the justification for the classification and it means that the spectra have a different appearance which can often be immediately recognized. An expression for the calculated wavenumbers of the P- and R- branches may be given as[30]

${\displaystyle {\bar {\nu }}={\bar {\nu }}_{0}+(B^{\prime }+B^{\prime \prime })m+(B^{\prime }-B^{\prime \prime }-D_{J}^{\prime }+D_{J}^{\prime \prime })m^{2}}$

${\displaystyle -2(D_{J}^{\prime }+D_{J}^{\prime \prime })m^{3}-(D_{J}^{\prime }-D_{J}^{\prime \prime })m^{4}}$

${\displaystyle +\left\{\left[(A^{\prime }-B^{\prime })-(A^{\prime \prime }-B^{\prime \prime })\right]-\left[D_{JK}^{\prime }+D_{JK}^{\prime \prime }\right]m-\left[D_{JK}^{\prime }-D_{JK}^{\prime \prime }\right]m^{2}\right\}K^{2}-(D_{K}^{\prime }-D_{K}^{\prime \prime })K^{4}}$

in which m = J+1 for the R-branch and -J for the P-branch. The three centrifugal distortion constants ${\displaystyle D_{J},D_{JK}}$, and ${\displaystyle D_{K}}$ are needed to fit the term values of each level.[1] The wavenumbers of the sub-structure corresponding to each band are given by

${\displaystyle {\bar {\nu }}={\bar {\nu }}_{sub}+(B^{\prime }-B^{\prime \prime })J(J+1)-(D_{J}^{\prime }-D_{J}^{\prime \prime })J^{2}(J+1)^{2}-(D_{JK}^{\prime }-D_{JK}^{\prime \prime })J(J+1)K^{2}}$

${\displaystyle {\bar {\nu }}_{sub}}$ represents the Q-branch of the sub-structure, whose position is given by

${\displaystyle {\bar {\nu }}_{sub}={\bar {\nu }}_{0}+\left[(A^{\prime }-B^{\prime })-(A^{\prime \prime }-B^{\prime \prime })\right]K^{2}-(D_{K}^{\prime }-D_{K}^{\prime \prime })K^{4}}$.

Spectrum of the C-Cl stretching band in CH3Cl (parallel band) simulated with Spectralcalc.[6]

Part of the spectrum of the asymmetric H-C-H bending vibration in CH3Cl (perpendicular band), simulated with Spectralcalc[6]

Parallel bands

The C-Cl stretching vibration of methyl chloride, CH₃Cl, gives a parallel band since the dipole moment change is aligned with the 3-fold rotation axis. The line spectrum shows the sub-structure of this band rather clearly;[6] in reality, very high resolution spectroscopy would be needed to resolve the fine structure fully. Allen and Cross show parts of the spectrum of CH₃D and give a detailed description of the numerical analysis of the experimental data.[31][32]

Perpendicular bands

The selection rule for perpendicular bands give rise to more transitions than with parallel bands. A band can be viewed as a series of sub-structures, each with P, Q and R branches. The Q-branches are separated by approximately 2(A′-B′). The asymmetric HCH bending vibration of methyl chloride is typical. It shows a series of intense Q-branches with weak rotational fine structure.[6] Analysis of the spectra is made more complicated by the fact that the ground-state vibration is bound, by symmetry, to be a degenerate vibration, which means that Coriolis coupling also affects the spectrum.[33]

Hybrid bands

Overtones of a degenerate fundamental vibration have components of more than one symmetry type. For example, the first overtone of a vibration belonging to the E representation in a molecule like ammonia, NH₃, will have components belonging to A₁ and E representations. A transition to the A₁ component will give a parallel band and a transition to the E component will give perpendicular bands; the result is a hybrid band.[34]

Inversion in ammonia

Spectrum of central region of the symmetric bending vibration in ammonia simulated with Spectralcalc,[6] illustrating inversion doubling.

Nitrogen inversion in ammonia

For ammonia, NH₃, the symmetric bending vibration is observed as two branches near 930 cm⁻¹ and 965 cm⁻¹. This so-called inversion doubling arises because the symmetric bending vibration is actually a large-amplitude motion known as inversion, in which the nitrogen atom passes through the plane of the three hydrogen atoms, similar to the inversion of an umbrella. The potential energy curve for such a vibration has a double minimum for the two pyramidal geometries, so that the vibrational energy levels occur in pairs which correspond to combinations of the vibrational states in the two potential minima. The two v = 1 states combine to form a symmetric state (1⁺) at 932.5 cm⁻¹ above the ground (0⁺) state and an antisymmetric state (1⁻) at 968.3 cm⁻¹.[35]

The vibrational ground state (v = 0) is also doubled although the energy difference is much smaller, and the transition between the two levels can be measured directly in the microwave region, at ca. 24 Ghz (0.8 cm⁻¹).[36][37] This transition is historically significant and was used in the ammonia MASER, the fore-runner of the LASER.[38]

Asymmetric top molecules

Absorption spectrum (attenuation coefficient vs. wavelength) of liquid water (red) [39] atmospheric water vapor (green) [40][41] and ice (blue line) [42][43] between 667 nm and 200 μm.[44] The plot for vapor is a transformation of data Synthetic spectrum for gas mixture "Pure H₂O" (296K, 1 atm) retrieved from Hitran on the Web Information System.[45]

Asymmetric top molecules have at most one or more 2-fold rotation axes. There are three unequal moments of inertia about three mutually perpendicular principal axes. The spectra are very complex. The transition wavenumbers cannot be expressed in terms of an analytical formula but can be calculated using numerical methods.

The water molecule is an important example of this class of molecule, particularly because of the presence of water vapor in the atmosphere. The low-resolution spectrum shown in green illustrates the complexity of the spectrum. At wavelengths greater than 10 μm (or wavenumbers less than 1000 cm⁻¹) the absorption is due to pure rotation. The band around 6.3 μm (1590 cm⁻¹) is due to the HOH bending vibration; the considerable breadth of this band is due to the presence of extensive rotational fine structure. High-resolution spectra of this band are shown in Allen and Cross, p 221.[46] The symmetric and asymmetric stretching vibrations are close to each other, so the rotational fine structures of these bands overlap. The bands at shorter wavelength are overtones and combination bands, all of which show rotational fine structure. Medium resolution spectra of the bands around 1600 cm⁻¹ and 3700 cm⁻¹ are shown in Banwell and McCash, p91.

Ro-vibrational bands of asymmetric top molecules are classed as A-, B- or C- type for transitions in which the dipole moment change is along the axis of smallest moment of inertia to the highest.[47]

Experimental methods

Ro-vibrational spectra are usually measured at high spectral resolution. In the past, this was achieved by using an echelle grating as the spectral dispersion element in a grating spectrometer.[9] This is a type of diffraction grating optimized to use higher diffraction orders.[48] Today at all resolutions the preferred method is FTIR. The primary reason for this is that infrared detectors are inherently noisy, and FTIR detects summed signals at multiple wavelengths simultaneously achieving a higher signal to noise by virtue of Fellgett's advantage for multiplexed methods. The resolving power of an FTIR spectrometer depends on the maximum retardation of the moving mirror. For example, to achieve a resolution of 0.1 cm⁻¹, the moving mirror must have a maximum displacement of 10 cm from its position at zero path difference. Connes measured the vibration-rotation spectrum of Venusian CO₂ at this resolution.[49] A spectrometer with 0.001 cm⁻¹ resolution is now available commercially. The throughput advantage of FTIR is important for high-resolution spectroscopy as the monochromator in a dispersive instrument with the same resolution would have very narrow entrance and exit slits.

When measuring the spectra of gases it is relatively easy to obtain very long path-lengths by using a multiple reflection cell.[50] This is important because it allows the pressure to be reduced so as to minimize pressure broadening of the spectral lines, which may degrade resolution. Path lengths up to 20m are commercially available.

Notes

1. Traditionally, infrared spectra are shown with the wavenumber scale decreasing from left to right, corresponding to increasing wavelength. More modern texts may show the wavenumber scale increasing from left to right. The P-branch is always at lower wavenumbers than the Q-branch.
2. Observed spectra of the fundamental band (shown here) and the first overtone band (for double excitation near 2 × 2140 cm⁻¹) can be seen in Banwell and McCash, p 67
3. Term value is directly related to energy by ${\displaystyle E=hcG(v)}$
4. Transitions with ∆v≠1 are called overtones. They are forbidden in the harmonic approximation but can be observed as weak bands because of anharmonicity.
5. Another example of lambda-doubling is found in the energy levels of the hydroxyl radical.
6. Some texts use the symbol K for this quantum number
7. The term representation is used in group theory to classify the effect of symmetry operations on, in this case, a molecular vibration. The symbols for the representations are to be found in the first column of the character table that applies to the particular molecular symmetry.

Appendix

The method of combination differences uses differences of wavenumbers in the P- and R- branches to obtain data that depend only on rotational constants in the vibrational ground or excited state. For the excited state

${\displaystyle \Delta _{2}^{\prime }F(J)^{observed}={\bar {\nu }}[R(J)]-{\bar {\nu }}[P(J)]}$

This function can be fitted, using the method of least-squares to data for carbon monoxide, from Harris and Bertolucci.[51] The data calculated with the formula

${\displaystyle \Delta _{2}^{\prime }F(J)^{calculated}=2B^{\prime \prime }\left(2J+1\right)}$

in which centrifugal distortion is ignored, are shown in the columns labelled with (1). This formula implies that the data should lie on a straight line with slope 2B′′ and intercept zero. At first sight the data appear to conform to this model, with a root mean square residual of 0.21 cm⁻¹. However, when centrifugal distortion is included, using the formula

${\displaystyle \Delta _{2}^{\prime }F(J)^{calculated}=(2B^{\prime \prime }-3D^{\prime \prime })\left(2J+1\right)-D^{\prime \prime }\left(2J+1\right)^{3}}$

the least-squares fit is improved markedly, with ms residual decreasing to 0.000086 cm⁻¹. The calculated data are shown in the columns labelled with (2).

Plot of the differences R(J)-P(J) as a function of 2J+1 taken from observed data for the fundamental vibration of carbon monoxide[51]

Wavenumbers /cm⁻¹ for the fundamental ro-vibrational band of carbon monoxide

J	2J+1	${\displaystyle \Delta _{2}^{\prime }F(J)}$	Calculated (1)	Residual (1)	Calculated (2)	Residual (2)
1	3	11.4298	11.3877	0.0421	11.4298	−0.000040
2	5	19.0493	18.9795	0.0698	19.0492	0.000055
3	7	26.6680	26.5713	0.0967	26.6679	0.000083
4	9	34.2856	34.1631	0.1225	34.2856	0.000037
5	11	41.9020	41.7549	0.1471	41.9019	0.000111
6	13	49.5167	49.3467	0.1700	49.5166	0.000097
7	15	57.1295	56.9385	0.1910	57.1294	0.000089
8	17	64.7401	64.5303	0.2098	64.7400	0.000081
9	19	72.3482	72.1221	0.2261	72.3481	0.000064
10	21	79.9536	79.7139	0.2397	79.9535	0.000133
11	23	87.5558	87.3057	0.2501	87.5557	0.000080
12	25	95.1547	94.8975	0.2572	95.1546	0.000100
13	27	102.7498	102.4893	0.2605	102.7498	−0.000016
14	29	110.3411	110.0811	0.2600	110.3411	0.000026
15	31	117.9280	117.6729	0.2551	117.9281	−0.000080
16	33	125.5105	125.2647	0.2458	125.5105	−0.000041
17	35	133.0882	132.8565	0.2317	133.0882	0.000035
18	37	140.6607	140.4483	0.2124	140.6607	0.000043
19	39	148.2277	148.0401	0.1876	148.2277	−0.000026
20	41	155.7890	155.6319	0.1571	155.7891	−0.000077
21	43	163.3443	163.2237	0.1206	163.3444	−0.000117
22	45	170.8934	170.8155	0.0779	170.8935	−0.000053
23	47	178.4358	178.4073	0.0285	178.4359	−0.000093
24	49	185.9713	185.9991	−0.0278	185.9714	−0.000142
25	51	193.4997	193.5909	−0.0912	193.4998	−0.000107
26	53	201.0206	201.1827	−0.1621	201.0207	−0.000097
27	55	208.5338	208.7745	−0.2407	208.5338	−0.000016
28	57	216.0389	216.3663	−0.3274	216.0389	0.000028
20	59	223.5357	223.9581	−0.4224	223.5356	0.000128
30	61	231.0238	231.5499	−0.5261	231.0236	0.000178

References

1. Hollas p101
2. Hollas p132
3. Atkins and de Paula p458 with diagrams
4. Allen and Cross, p 116
5. Allen and Cross, p113
6. Simulated spectrum created using infrared gas spectra simulator
7. Banwell and McCash, p 70
8. Banwell and McCash, p69
9. Gillette, R. H.; Eyster,Eugene H. (1939). "The Fundamental Rotation-Vibration Band of Nitric Oxide". Phys. Rev. 56 (11): 1113–1119. Bibcode:1939PhRv...56.1113G. doi:10.1103/PhysRev.56.1113.
10. Atkins, Peter; de Paula, Julio (2006). Atkins' Physical Chemistry (8th ed.). New York: W.H.Freeman. p. 454. ISBN 0-7167-8759-8.
11. Goldman, A.; Reid, J.; Rothman, L. S. (1981). "Identification of electric quadrupole O₂ and N₂ lines in the infrared atmospheric absorption spectrum due to the vibration‐rotation fundamentals". Geophysical Research Letters. 8 (1): 77. Bibcode:1981GeoRL...8...77G. doi:10.1029/GL008i001p00077.
12. Hollas p116
13. Strandberg, M. W. P.; Meng, C. Y.; Ingersoll, J. G. (1949). "The Microwave Absorption Spectrum of Oxygen". Phys. Rev. 75 (10): 1524–1528. Bibcode:1949PhRv...75.1524S. doi:10.1103/PhysRev.75.1524.pdf
14. Krupenie, Paul H. (1972). "The Spectrum of Molecular Oxygen" (PDF). J. Phys. Chem. Ref. Data. 1 (2): 423–534. Bibcode:1972JPCRD...1..423K. doi:10.1063/1.3253101. Archived from the original (PDF) on 2016-03-04.
15. Hollas, pp 133–135. The Stokes-side spectrum of carbon monoxide is shown on p134
16. Hollas, p135
17. Fletcher, William H.; Rayside, John S. (1974). "High resolution vibrational Raman spectrum of oxygen". Journal of Raman Spectroscopy. 2 (1): 3–14. Bibcode:1974JRSp....2....3F. doi:10.1002/jrs.1250020102.
18. Straughan and Walker, vol2, p185
19. The spectrum of this vibration mode, centered at ca. 3310 cm⁻¹ is shown in Banwell and McCash, p76, and also in Hollas, p156
20. Straughan and Walker, vol2 p186
21. Hollas p155
22. Straughan and Walker vol2, pp 186−8
23. Western, Colin. "PGOPHER, a program for rotational, vibrational and electronic spectra". pgopher.chm.bris.ac.uk.
24. A very weak spectrum can be observed due to an excited vibrational state being polar. See rotational spectroscopy for more details.
25. Straughan and Walker vol2, p199
26. Allen and Cross, p67
27. Jahn, H. A. (1938). "A New Coriolis Perturbation in the Methane Spectrum. I. Vibrational-Rotational Hamiltonian and Wave Functions". Proceedings of the Royal Society of London. Series A, Mathematical and Physical Sciences. 168 (935): 469–495. Bibcode:1938RSPSA.168..469J. doi:10.1098/rspa.1938.0187. ISSN 0080-4630. JSTOR 97253.
28. Jahn, H. A. (1939). "Coriolis Perturbations in the Methane Spectrum. IV. Four General Types of Coriolis Perturbation". Proceedings of the Royal Society of London. Series A, Mathematical and Physical Sciences. 171 (947): 450–468. Bibcode:1939RSPSA.171..450J. doi:10.1098/rspa.1939.0077. ISSN 0080-4630. JSTOR 97293.
29. Hecht, K.T. (1960). "Vibration-rotation energies of tetrahedral XY₄ molecules: Part II. The fundamental ν3 of CH₄" (PDF). J. Mol. Spectrosc. 5 (1–6): 335, 390. Bibcode:1961JMoSp...5..390H. doi:10.1016/0022-2852(61)90103-5. hdl:2027.42/32396.
30. Allen and Cross, p131
31. Allen and Cross pp 134–148
32. Allen, H.C. Jr.; E.K.Pyler (1959). "Some Vibrational-Rotational Bands of Deuterated Methanes". Journal of Research of the National Bureau of Standards Section A. 63A (2): 145–153. doi:10.6028/jres.063a.007. PMC 5287196. PMID 31216145.
33. Allen and Cross, pp 149–164 has a detailed analysis.
34. Allen and Cross, pp 164–70.
35. Hollas p167 gives 0.79 cm⁻¹ for the 0⁺−0⁻ energy difference, 931.7 cm⁻¹ for 0⁻−1⁺, and 35.8 cm⁻¹ for 1⁺−1⁻.
36. Harris, Daniel, C.; Bertolucci, Michael, D. (1978). Symmetry and Spectroscopy. OUP. pp. 168–170. ISBN 0-19-502001-4.CS1 maint: multiple names: authors list (link)
37. Spectra are shown in Allen and Cross, pp 172–174
38. Straughan and Walker p124
39. Bertie J. E.; Lan Z. (1996). "Infrared Intensities of Liquids XX: The Intensity of the OH Stretching Band of Liquid Water Revisited, and the Best Current Values of the Optical Constants of H2O(l) at 25°C between 15,000 and 1 cm⁻¹". Applied Spectroscopy. 50 (8): 1047–1057. Bibcode:1996ApSpe..50.1047B. doi:10.1366/0003702963905385. S2CID 97329854. Retrieved 2012-08-08.
40. "Spectroscopy of Atmospheric Gases (spectral databases)". V.E. Zuev Institute of Atmospheric Optics SB RAS. Archived from the original on April 16, 2013. Retrieved August 8, 2012. ... various data sources: HITRAN and GEISA spectral databanks, original data obtained by IAO researchers in collaboration with other scientists, H2O spectra simulated by Partridge and Schwenke etc... ...
41. Aringer B.; Kerschbaum F.; Jørgensen U. G. (2002). "H₂O in stellar atmospheres" (PDF). Astronomy and Astrophysics. EDP Sciences. 395 (3): 915–927. Bibcode:2002A&A...395..915A. doi:10.1051/0004-6361:20021313. Retrieved 2012-08-08.
42. Warren S. G. (1984). "Optical constants of ice from the ultraviolet to the microwave" (PDF). Applied Optics. 23 (8): 1206. Bibcode:1984ApOpt..23.1206W. doi:10.1364/AO.23.001206. PMID 18204705. Retrieved 2012-08-08.
43. Warren S. G.; Brandt R. E. (2008). "Optical constants of ice from the ultraviolet to the microwave: A revised compilation" (PDF). J. Geophys. Res. 113 (D14): D14220. Bibcode:2008JGRD..11314220W. doi:10.1029/2007JD009744. Retrieved 2012-08-08.
44. Wozniak B.; Dera J. (2007). Atmospheric and Oceanographic Sciences Library (PDF). New York: Springer Science+Business Media. LLC. ISBN 978-0-387-30753-4. Retrieved August 4, 2012.
45. "Hitran on the Web Information System". Harvard-Smithsonian Center for Astrophysics (CFA), Cambridge, MA, USA; V.E. Zuev Institute of Atmosperic Optics (IAO), Tomsk, Russia. Retrieved August 11, 2012.
46. Dalby, F.W.; Nielsen, H.H. (1956). "Infrared Spectrum of Water Vapor. Part I—The 6.26μ Region". J. Chem. Phys. 25 (5): 934–940. Bibcode:1956JChPh..25..934D. doi:10.1063/1.1743146.
47. Allen and Cross, chapter 8.
48. Hollas, pp. 38−41. Worked Example 3.1 shows how resolving power is related to diffraction order and line spacing on the grating
49. Connes, J.; Connes, P. (1966). "Near-Infrared Planetary Spectra by Fourier Spectroscopy. I. Instruments and Results". Journal of the Optical Society of America. 56 (7): 896–910. doi:10.1364/JOSA.56.000896.
50. Patricia B. Coleman, ed. (1993). Practical Sampling Techniques for Infrared Analysis. CRC PressINC. ISBN 0-8493-4203-1.
51. Harris, Daniel, C.; Bertolucci, Michael, D. (1978). Symmetry and Spectroscopy. OUP. p. 125. ISBN 0-19-502001-4.CS1 maint: multiple names: authors list (link)

Bibliography

• Allen, H.C.; Cross, P.C. (1963). Molecular vib-rotors; the theory and interpretation of high resolution infra-red spectra. New York: Wiley.
• Atkins, P.W.; de Paula, J. (2006). Physical Chemistry (8th ed.). Oxford University Press. pp. 431–469. ISBN 0198700725. Chapter (Molecular Spectroscopy), Section (Vibration-rotation spectra) and page numbers may be different in different editions.
• Banwell, Colin N.; McCash, Elaine M. (1994). Fundamentals of molecular spectroscopy (4th ed.). McGraw-Hill. p. 40. ISBN 0-07-707976-0.
• Hollas, M.J. (1996). Modern Spectroscopy (3rd ed.). Wiley. ISBN 0471965227.
• Straughan, B.P.; Walker, S. (1976). Spectroscopy. 2 (3rd ed.). Chapman and Hall. pp. 176–204. ISBN 0-470-15032-7.

External links

• infrared gas spectra simulator
• NIST Diatomic Spectral Database
• NIST Triatomic Spectral Database
• NIST Hydrocarbon Spectral Database