Rotational spectroscopy is concerned with the measurement of the energies of transitions between quantized rotational states of molecules in the gas phase. The spectra of polar molecules can be measured in absorption or emission by microwave spectroscopy or by far infrared spectroscopy. The rotational spectra of non-polar molecules cannot be observed by those methods, but can be observed and measured by Raman spectroscopy. Rotational spectroscopy is sometimes referred to as pure rotational spectroscopy to distinguish it from rotational-vibrational spectroscopy where changes in rotational energy occur together with changes in vibrational energy, and also from ro-vibronic spectroscopy (or just vibronic spectroscopy) where rotational, vibrational and electronic energy changes occur simultaneously.
For rotational spectroscopy, molecules are classified according to symmetry into spherical top, linear and symmetric top; analytical expressions can be derived for the rotational energy terms of these molecules. Analytical expressions cannot be derived for the fourth category, asymmetric top, but spectra can be fitted using numerical methods. The rotational energies are derived theoretically by considering the molecules to be rigid rotors and then applying extra terms to account for centrifugal distortion, fine structure, hyperfine structure and Coriolis coupling. Fitting the spectra to the theoretical expressions gives numerical values of the angular moments of inertia from which very precise values of molecular bond lengths and angles can be derived in favorable cases. In the presence of an electrostatic field there is Stark splitting which allows molecular electric dipole moments to be determined.
Rotational spectroscopy has primarily been used to investigate fundamental aspects of molecular physics. It is a uniquely precise tool for the determination of molecular structure in gas phase molecules. It can be used to establish barriers to internal rotation such as that associated with the rotation of the CH3 group relative to the C6H4Cl group in chlorotoluene (C7H7Cl). When fine or hyperfine structure can be observed, the technique also provides information on the electronic structures of molecules. Much of current understanding of the nature of weak molecular interactions such as van der Waals, hydrogen and halogen bonds has been established through rotational spectroscopy. In connection with radio astronomy, the technique has a key role in exploration of the chemical composition of the interstellar medium. Microwave transitions are measured in the laboratory and matched to emissions from the interstellar medium using a radio telescope. NH3 was the first stable polyatomic molecule to be identified in the interstellar medium. Current projects in astrochemistry involve both laboratory microwave spectroscopy and observations made using modern radiotelescopes such as the Atacama Large Millimetre Array (ALMA). Unlike NMR, Infrared and UV-Visible spectroscopies, microwave spectroscopy has not yet found widespread application in analytical chemistry; the measurement of chlorine monoxide is important for atmospheric chemistry.
A molecule in the gas phase is free to rotate relative to a set of mutually orthogonal axes of fixed orientation in space, centered on the center of mass of the molecule. Free rotation is not possible for molecules in liquid or solid phases due to the presence of intermolecular forces. Rotation about each unique axis is associated with a set of quantized energy levels dependent on the moment of inertia about that axis and a quantum number. Thus, for linear molecules the energy levels are described by a single moment of inertia and a single quantum number, J. For symmetric tops there are two moments of inertia and two rotational quantum numbers to consider. Analysis of spectroscopic data with the expressions detailed below results in quantitative determination of the value(s) of the moment(s) of inertia. From these precise values of the molecular structure and dimensions may be obtained.
For a linear molecule, analysis of the rotational spectrum provides values for the rotational constant and the moment of inertia of the molecule, and, knowing the atomic masses, can be used to determine the bond length directly. For diatomic molecules this process is straightforward. For linear molecules with more than two atoms it is necessary to measure the spectra of two or more isotopologues, such as 16O12C32S and 16O12C34S. This allows a set of simultaneous equations to be set up and solved for the bond lengths).[notes 2] It should be noted that a bond length obtained in this way is slightly different from the equilibrium bond length. This is because there is zero-point energy in the vibrational ground state, to which the rotational states refer, whereas the equilibrium bond length is at the minimum in the potential energy curve. The relation between the rotational constants is given by
where ν is a vibrational quantum number and α is a vibration-rotation interaction constant which can be calculated if the B values for two different vibrational states can be found.
For other molecules, if the spectra can be resolved and individual transitions assigned both bond lengths and bond angles can be deduced. When this is not possible, as with most asymmetric tops, all that can be done is to fit the spectra to three moments of inertia calculated from an assumed molecular structure. By varying the molecular structure the fit can be improved, giving a qualitative estimate of the structure. Isotopic substitution is invaluable when using this approach to the determination of molecular structure.
Classification of molecular rotors
In quantum mechanics the free rotation of a molecule is quantized, so that the rotational energy and the angular momentum can take only certain fixed values, which are related simply to the moment of inertia, , of the molecule. For any molecule, there are three moments of inertia: , and about three mutually orthogonal axes A, B, and C with the origin at the center of mass of the system. The general convention, used in this article, is to define the axes such that , with axis corresponding to the smallest moment of inertia. Some authors, however, define the axis as the molecular rotation axis of highest order.
The particular pattern of energy levels (and, hence, of transitions in the rotational spectrum) for a molecule is determined by its symmetry. A convenient way to look at the molecules is to divide them into four different classes, based on the symmetry of their structure. These are
- Spherical tops (spherical rotors) All three moments of inertia are equal to each other: . Examples of spherical tops include phosphorus tetramer (P4), carbon tetrachloride (CCl4) and other tetrahalides, methane (CH4), silane, (SiH4), sulfur hexafluoride (SF6) and other hexahalides. The molecules all belong to the cubic point groups Td or Oh.
- Linear molecules. For a linear molecule the moments of inertia are related by . For most purposes, can be taken to be zero. Examples of linear molecules include dioxygen, O2, dinitrogen, N2, carbon monoxide, CO, hydroxy radical, OH, carbon dioxide, CO2, hydrogen cyanide, HCN, carbonyl sulfide, OCS, acetylene (ethyne, HC≡CH) and dihaloethynes. These molecules belong to the point groups C∞v or D∞h
- Symmetric tops (symmetric rotors) A symmetric top is a molecule in which two moments of inertia are the same, or . By definition a symmetric top must have a 3-fold or higher order rotation axis. As a matter of convenience, spectroscopists divide molecules into two classes of symmetric tops, Oblate symmetric tops (saucer or disc shaped) with and Prolate symmetric tops (rugby football, or cigar shaped) with . The spectra look rather different, and are instantly recognizable. Examples of symmetric tops include
- As a detailed example, ammonia has a moment of inertia IC = 4.4128 × 10−47 kg m2 about the 3-fold rotation axis, and moments IA = IB = 2.8059 × 10−47 kg m2 about any axis perpendicular to the C3 axis. Since the unique moment of inertia is larger than the other two, the molecule is an oblate symmetric top.
- Asymmetric tops (asymmetric rotors) The three moments of inertia have different values. Examples of small molecules that are asymmetric tops include water, H2O and nitrogen dioxide, NO2 whose symmetry axis of highest order is a 2-fold rotation axis. Most large molecules are asymmetric tops.
Transitions between rotational states can be observed in molecules with a permanent electric dipole moment.[notes 3] A consequence of this rule is that no microwave spectrum can be observed for centrosymmetric linear molecules such as N2 (dinitrogen) or HCCH (ethyne), which are non-polar. Tetrahedral molecules such as CH4 (methane), which have both a zero dipole moment and isotropic polarizability, would not have a pure rotation spectrum but for the effect of centrifugal distortion; when the molecule rotates about a 3-fold symmetry axis a small dipole moment is created, allowing a weak rotation spectrum to be observed by microwave spectroscopy.
With symmetric tops, the selection rule for electric-dipole-allowed pure rotation transitions is ΔK=0, ΔJ = ±1. Moreover the quantum number K is limited to have values between and including +J to -J.
For Raman spectra the general rule is that the molecular polarizability must be anisotropic, which means that it is not the same in all directions. Polarizability is a 3-dimensional tensor that can be represented as an ellipsoid. The polarizability ellipsoid of spherical top molecules is in fact spherical so those molecules show no rotational Raman spectrum. For all other molecules both Stokes and anti-Stokes lines[notes 4] can be observed and they have similar intensities due to the fact than many rotational states are thermally populated. The selection rule for linear molecules is ΔJ = 0, ±2. The reason for the value of 2 is that the ellipsoid must rotate twice during a transition. The selection rule for symmetric top molecules is
- ΔK = 0
- If K=0, then ΔJ = ±2
- If K ≠ 0, then ΔJ = 0, ±1, ±2
Transitions with ΔJ = +1 are said to belong the an R series, whereas transitions with ΔJ = +2 belong to an S series.
The units used for rotational constants depend on the type of measurement. With infrared spectra, the unit of measurement is usually wavenumbers per cm, written as cm−1 and shown with the symbol . Wavenumbers per cm is literally the number of waves in one centimeter, or the reciprocal of wavelength in cm. On the other hand, microwave spectra are usually measured in Gigahertz. The relationship between the two units is derived from the expression
As 1 GHz = 109 hz, the numerical conversion can be expressed as
Effect of vibration on rotation
The population of vibrationally excited states follows a Boltzmann distribution, so low frequency vibrational states are appreciably populated even at room temperatures. As the moment of inertia is higher when a vibration is excited, the rotational constants, B decrease. Consequently, the rotation frequencies in each vibration state are different from each other. This can give rise to "satellite" lines in the rotational spectrum. An example is provided by cyanodiacetylene, H-C≡C−C≡C-C≡N,
Further, there is a fictitious force, Coriolis coupling, between the vibrational motion of the nuclei in the rotating (non-inertial) frame. However, as long as the vibrational quantum number does not change (i.e., the molecule is in only one state of vibration), the effect of vibration on rotation is not important, because the time for vibration is much shorter than the time required for rotation. The Coriolis coupling is often negligible, too, if one is interested in low vibrational and rotational quantum numbers only.
Effect of rotation on vibrational spectra
Historically, the theory of rotational energy levels was developed to account for observations of vibration-rotation spectra of gases in infrared spectroscopy, which was used before microwave spectroscopy had become practical. To a first approximation the energy of rotation is added to, or subtracted from the energy of vibration. The vibration-rotation wavenumbers of transitions for a harmonic oscillator with rigid rotor are given by
In reality, this expression has to be modified for the effects of anharmonicity of the vibrations, for centrifugal distortion and for Coriolis coupling. The plus sign implies simultaneous excitation of both vibration and rotation, giving the so-called R branch in the spectrum, whereas with the minus sign a quantum of rotational energy is lost while a quantum of vibrational energy is gained, giving the P branch. The pure vibration, ΔJ=0, gives rise to the Q branch of the spectrum. Because of the thermal population of the rotational states the P branch is slightly less intense than the R branch.
Rotational constants obtained from infrared measurements are in good accord with those obtained by microwave spectroscopy while the latter usually offers greater precision.
Structure of rotational spectra
Spherical top molecules have no net dipole moment. A pure rotational spectrum cannot be observed by absorption or emission spectrocopy because there is no permanent dipole moment whose rotation can be accelerated by the electric field of an incident photon. Also the polarizability is isotropic, so that pure rotational transitions cannot be observed by Raman spectroscopy either. Nevertheless, rotational constants can be obtained by ro-vibrational spectroscopy. This occurs when a molecule is polar in the vibrationally excited state. For example, the molecule methane is a symmetric top but the asymmetric C-H stretching band shows rotational fine structure in the infrared spectrum, illustrated in rovibrational coupling. This spectrum is also interesting because it shows clear evidence of Coriolis coupling in the asymmetric structure of the band.
The rigid rotor is a good starting point from which to construct a model of a rotating molecule. It is assumed that component atoms are point masses connected by rigid bonds. A linear molecule lies on a single axis and each atom moves on the surface of a sphere around the centre of mass. The two degrees of rotational freedom correspond to the spherical coordinates θ and φ which describe the direction of the molecular axis, and the quantum state is determined by two quantum numbers J and M. J defines the magnitude of the rotational angular momentum, and M its component about an axis fixed in space, such as an external electric or magnetic field. In the absence of external fields, the energy depends only on J. Under the rigid rotor model, the rotational energy levels, F(J), of the molecule can be expressed as,
where is the rotational constant of the molecule and is related to the moment of inertia of the molecule. In a linear molecule the moment of inertia about an axis perpendicular to the molecular axis is unique, that is, , so
For a diatomic molecule
where m1 and m2 are the masses of the atoms and d is the distance between them.
Selection rules dictate that during emission or absorption the rotational quantum number has to change by unity; i.e., . Thus, the locations of the lines in a rotational spectrum will be given by
where denotes the lower level and denotes the upper level involved in the transition.
The diagram illustrates rotational transitions that obey the =1 selection rule. The dashed lines show how these transitions map onto features that can be observed experimentally. Adjacent transitions are separated by 2B in the observed spectrum. Frequency or wavenumber units can also be used for the x axis of this plot.
Rotational line intensities
The probability of a transition taking place is the most important factor influencing the intensity of an observed rotational line. This probability is proportional to the population of the initial state involved in the transition. The population of a rotational state depends on two factors. The number of molecules in an excited state with quantum number J, relative to the number of molecules in the ground state, NJ/N0 is given by the Boltzmann distribution as
where k is the Boltzmann constant and T the absolute temperature. This factor decreases as J increases. The second factor is the degeneracy of the rotational state, which is equal to 2J+1. This factor increases as J increases. Combining the two factors
The maximum relative intensity occurs at
The diagram at the right shows an intensity pattern roughly corresponding to the spectrum above it.
When a molecule rotates, the centrifugal force pulls the atoms apart. As a result, the moment of inertia of the molecule increases, thus decreasing the value of , when it is calculated using the expression for the rigid rotor. To account for this a centrifugal distortion correction term is added to the rotational energy levels of the diatomic molecule.
where is the centrifugal distortion constant.
Therefore, the line positions for the rotational mode change to
In consequence, the spacing between lines is not constant, as in the rigid rotor approximation, but decreases with increasing rotational quantum number.
An assumption underlying these expressions is that the molecular vibration follows simple harmonic motion. In the harmonic approximation the centrifugal constant D can be derived as
where k is the vibrational force constant. The relationship between B and D
where : is the harmonic vibration frequency, follows. If anharmonicity is to be taken into account, terms in higher powers of J should be added to the expressions for the energy levels and line positions. A striking example concerns the rotational spectrum of hydrogen fluoride which was fitted to terms up to [J(J+1)]5.
The electric dipole moment of the dioxygen molecule, O2 is zero, but the molecule is paramagnetic with two unpaired electrons so that there are magnetic-dipole allowed transitions which can be observed by microwave spectroscopy. The unit electron spin has three spatial orientations with respect to the given molecular rotational angular momentum vector, K, so that each rotational level is split into three states, J = K + 1, K, and K - 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. The energy difference between successive J terms in any of these triplets is about 2 cm−1 (60 GHz), with the single exception of J = 1←0 difference which is about 4 cm−1. 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 K there are two allowed transitions. The 16O nucleus has zero nuclear spin angular momentum, so that symmetry considerations demand that K have only odd values.
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. In the absence of an external electrical field, the rotational energy of a symmetric top is a function of only J and K and, in the rigid rotor approximation, the energy of each rotational state is given by
where and for a prolate symmetric top molecule or for an oblate molecule.
This gives the transition wavenumbers as
which is the same as in the case of a linear molecule. With a first order correction for centrifugal distortion the transition wavenumbers become
The term in DJK has the effect of removing degeneracy present in the rigid rotor approximation, with different K values.
The quantum number J refers to the total angular momentum, as before. Since there are three independent moments of inertia, there are two other independent quantum numbers to consider, but the term values for an asymmetric rotor cannot be derived in closed form. They are obtained by individual matrix diagonalization for each J value. Formulae are available for molecules whose shape approximates to that of a symmetric top.
The water molecule is an important example of an asymmetric top. It has an intense pure rotation spectrum in the far infrared region, below about 200 cm−1. For this reason far infrared spectrometers have to be freed of atmospheric water vapour either by purging with a dry gas or by evacuation. The spectrum has been analyzed in detail.
When a nucleus has a spin quantum number, I, greater than 1/2 it has a quadrupole moment. In that case, coupling of nuclear spin angular momentum with rotational angular momentum causes splitting of the rotational energy levels. If the quantum number J of a rotational level is greater than I, 2I+1 levels are produced; but if J is less than I, 2J+1 levels result. The effect is known as hyperfine splitting. For example, with 14N (I = 1) in HCN, all levels with J > 0 are split into 3. The energy of the sub-levels are proportional to the nuclear quadrupole moment and a function of F and J. where F = J+I, J+I-1, ..., 0, ... |J-I|. Thus, observation of nuclear quadrupole splitting permits the magnitude of the nuclear quadrupole moment to be determined. This is an alternative method to the use of nuclear quadrupole resonance spectroscopy. The selection rule for rotational transitions becomes
Stark and Zeeman effects
In the presence of a static external electric field the 2J+1 degeneracy of each rotational state is partly removed, an instance of a Stark effect. For example in linear molecules each energy level is split into J+1 components. The extent of splitting depends on the square of the electric field strength and the square of the dipole moment of the molecule. In principle this provides a means to determine the value of the molecular dipole moment with high precision. Examples include carbonyl sulfide, OCS, with μ = 0.71521 ± 0.00020 Debye. However, because the splitting depends on μ2, the orientation of the dipole must be deduced from quantum mechanical considerations.
A similar removal of degeneracy will occur when a paramagnetic molecule is placed in a magnetic field, an instance of the Zeeman effect. Most species which can be observed in the gaseous state are diamagnetic . Exceptions, known as odd molecules, include nitric oxide, NO, nitrogen dioxide, NO2, some chlorine oxides and the hydroxide radical. The Zeeman effect has been observed with dioxygen, O2
Rotational Raman spectroscopy
Molecular rotational transitions can also be observed by Raman spectroscopy. Rotational transitions are Raman-allowed for any molecule with an anisotropic polarizability which includes all molecules except for spherical tops. This means that rotational transitions of molecules with no permanent dipole moment, which cannot be observed in absorption or emission, can be observed, by scattering, in Raman spectroscopy. Very high resolution Raman spectra can be obtained by adapting a Fourier Transform Infrared Spectrometer. An example is the spectrum of 15N2. It shows the effect of nuclear spin, resulting in intensities variation of 3:1 in adjacent lines. A bond length of 109.9985 ± 0.0010 pm was deduced from the data.
Instruments and Methods
The great majority of contemporary spectrometers use a mixture of commercially available and bespoke components which users integrate according to their particular needs. Instruments can be broadly categorised according to their general operating principals. Although rotational transitions can be found across a very broad region of the electromagnetic spectrum, fundamental physical constraints exist on the operational bandwidth of instrument components. It is often impractical and costly to switch to measurements within an entirely different frequency region. The instruments and operating principals described below are generally appropriate to microwave spectroscopy experiments conducted at frequencies between 6 and 24 GHz.
Absorption cells and Stark modulation
A microwave spectrometer can be most simply constructed using a source of microwave radiation, an absorption cell into which sample gas can be introduced and a detector such as a superheterodyne receiver. A spectrum can be obtained by sweeping the frequency of the source while detecting the intensity of transmitted radiation. A simple section of waveguide can serve as an absorption cell. An important variation of the technique in which an alternating current is applied across electrodes within the absorption cell results in a modulation of the frequencies of rotational transitions. This is referred to as Stark modulation and allows the use of phase-sensitive detection methods offering improved sensitivity. Absorption spectroscopy allows the study of samples that are thermodynamically stable at room temperature. The first study of the microwave spectrum of a molecule (NH3) was performed by Cleeton & Williams in 1934. Subsequent experiments exploited powerful sources of microwaves such as the klystron, many of which were developed for radio detection and ranging (RADAR) during the Second World War. The number of experiments in microwave spectroscopy surged immediately after the war. By 1948, Walter Gordy was able to prepare a review of the results contained in approximately 100 research papers. Commercial versions of microwave absorption spectrometer were developed by Hewlett Packard in the 1970s and were once widely used for fundamental research. Most research laboratories now exploit either Balle-Flygare or chirped-pulse Fourier transform microwave (FTMW) spectrometers.
Fourier transform microwave (FTMW) spectroscopy
The theoretical framework underpinning FTMW spectroscopy is analogous to that used to describe FT-NMR spectroscopy. The behaviour of the evolving system is described by optical Bloch equations. First, a short (typically 0-3 microsecond duration) microwave pulse is introduced on resonance with a rotational transition. Those molecules that absorb the energy from this pulse are induced to rotate coherently in phase with the incident radiation. De-activation of the polarisation pulse is followed by microwave emission that accompanies decoherence of the molecular ensemble. This free induction decay occurs on a timescale of 1-100 microseconds depending on instrument settings. Following pioneering work by Dicke and co-workers in the 1950s, the first FTMW spectrometer was constructed by Ekkers and Flygare in 1975.
The Balle-Flygare FTMW spectrometer
Balle, Campbell, Keenan and Flygare demonstrated that the FTMW technique can be applied within a "free space cell" comprising an evacuated chamber containing a Fabry-Perot cavity. This technique allows a sample to be probed only milliseconds after it undergoes rapid cooling to only a few degrees Kelvin in the throat of an expanding gas jet. This was a revolutionary development because (i) cooling molecules to low temperatures concentrates the available population in the lowest rotational energy levels. Coupled with benefits conferred by the use of a Fabry-Perot cavity, this brought a great enhancement in the sensitivity and resolution of spectrometers along with a reduction in the complexity of observed spectra; (ii) it became possible to isolate and study molecules that are very weakly bound because there is insufficient energy available for them to undergo fragmentation or chemical reaction at such low temperatures. William Klemperer was a pioneer in using this instrument for the exploration of weakly bound interactions. While the Fabry-Perot cavity of a Balle-Flygare FTMW spectrometer can typically be tuned into resonance at any frequency between 6 and 18 GHz, the bandwidth of individual measurements is restricted to about 1 MHz. An animation illustrates the operation of this instrument which is currently the most widely used tool for microwave spectroscopy.
The Chirped-Pulse FTMW spectrometer
Noting that digitisers and related electronics technology had significantly progressed since the inception of FTMW spectroscopy, B.H. Pate at the University of Virginia designed a spectrometer which retains many advantages of the Balle-Flygare FT-MW spectrometer while innovating in (i) the use of a high speed (>4 GS/s) arbitrary waveform generator to generate a "chirped" microwave polarisation pulse that sweeps up to 12 GHz in frequency in less than a microsecond and (ii) the use of a high speed (>40 GS/s) oscilloscope to digitise and Fourier transform the molecular free induction decay. The result is an instrument that allows the study of weakly bound molecules but which is able to exploit a measurement bandwidth (12 GHz) that is greatly enhanced compared with the Balle-Flygare FTMW spectrometer. Modified versions of the original CP-FTMW spectrometer have been constructed by a number of groups in the United States, Canada and Europe. The instrument offers a broadband capability that is highly complementary to the high sensitivity and resolution offered by the Balle-Flygare design.
- The spectrum was measured over a couple of hours with the aid of a chirped-pulse Fourier transform microwave spectrometer at the University of Bristol.
- For a symmetric top, the values of the 2 moments of inertia can be used to derive 2 molecular parameters. Values from each additional isotopologue provide the information for one more molecular parameter. For asymmetric tops a single isotopologue provides information for at most 3 molecular parameters.
- Such transitions are called electric dipole-allowed transitions. Other transitions involving quadrupoles, octupoles, hexadecapoles etc. may also be allowed but the spectral intensity is very much smaller, so these transitions are difficult to observe. Magnetic-dipole-allowed transitions can occur in paramagnetic molecules such as dioxygen, O2 and nitric oxide, NO
- In Raman spectroscopy the photon energies for Stokes and anti-Stokes scattering are respectively less than and greater than the incident photon energy. See the energy-level diagram at Raman spectroscopy.
- Gordy, W. (1970). Microwave Molecular Spectra in Technique of Organic Chemistry, Vol. IX, Edited by A. Weissberger. New York: Interscience.
- Nair, K.P.R.; Demaison, J.; Wlodarczak, G.; Merke, I.; (236). "Millimeterwave rotational spectrum and internal rotation in o-chlorotoluene". Journal of Molecular Spectroscopy 237 (2): 137–142. Bibcode:2006JMoSp.237..137N. doi:10.1016/j.jms.2006.03.011.
- Cheung, A.C.; Rank, D.M.; Townes, C.H.; Thornton, D.D. and Welch, W.J. (1968). "Detection of NH3 molecules in the interstellar medium by their microwave emission spectra". Physical Review Letters 21 (25): 1701–1705. Bibcode:1968PhRvL..21.1701C. doi:10.1103/PhysRevLett.21.1701.
- "Astrochemistry in Virginia". Retrieved 2 December 2012.
- Ricaud, P.; Baron, P; de La Noë, J. (2004). "Quality assessment of ground-based microwave measurements of chlorine monoxide, ozone, and nitrogen dioxide from the NDSC radiometer at the Plateau de Bure". Ann. Geophys. 22: 1903–1915. doi:10.5194/angeo-22-1903-2004.
- Banwell and McCash, p99
- Moment of inertia values from P. Atkins and J. de Paula, Physical Chemistry, 8th ed. (W.H. Freeman 2006), p. 445
- Hollas p95
- Hollas, p.104 shows part of the observed rotational spectrum of silane
- Banwell and McCash, p.49
- Hollas p111
- Banwell and McCash, section 4.2, p 105, Pure Rotational Raman Spectra
- Alexander, A.J; Kroto, H.W; Walton, D.R.M. (1967). "The microwave spectrum, substitution structure and dipole moment of cyanobutadiyne". J. Mol. Spectrosc. 62: 175–180. doi:10.1016/0022-2852(76)90347-7. Illustrated in Hollas, p97
- Banwell and McCash, p63
- Banwell and McCash, p40
- Banwell and McCash, p 45.
- Jennings, D.A.; Evenson, K.M; Zink, L.R.;Demuynck, C.;Destombes, J.L.;Lemoine, B;Johns,J.W.C. (April 1987). "High-resolution spectroscopy of HF from 40 to 1100 cm−1: Highly accurate rotational constants". Journal of Molecular Spectroscopy 122 (2): 477–480. doi:10.1016/0022-2852(87)90021-X.pdf
- Strandberg,, M. W. P.; Meng, C. Y.;Ingersoll, J. G. (1949). "The Microwave Absorption Spectrum of Oxygen". Phys.Rev. 75 (10): 1524–1528. doi:10.1103/PhysRev.75.1524.pdf
- Krupenie, Paul H. (1972). "The Spectrum of Molecular Oxygen". J. Phys. Chem. Ref. Data 1, 423 (1972); 1 (2): 423–534. doi:10.1063/1.3253101.
- Hollas, p101
- Hollas, p102, shows the effect on the microwave spectrum of H3SiNCS.
- Hollas, p103
- Hall, Richard T.; Dowling, Jerome M. (1967). "Pure Rotational Spectrum of Water Vapor". J. Chem. Phys. 47 (7): 2454–2461. doi:10.1063/1.1703330. Hall, Richard T.; Dowling, Jerome M. (1971). "Erratum: Pure Rotational Spectrum of Water Vapor". J. Chem. Phys. 54 (11): 4968. doi:10.1063/1.1674785.
- Simmons, James W.; Anderson, Wallace E.; Gordy,Walter (1950). "Microwave Spectrum and Molecular Constants of Hydrogen Cyanide". Phys. Rev. 77: 77–79. doi:10.1103/PhysRev.77.77.
- Chang, Raymond (1971). Basic Principles of Spectroscopy. McGraw-Hill. p139
- Hollas, p102 gives the equations for diatomic molecules and symmetric tops
- Hollas, p102
- .Burkhalter, James H.; Roy S. Anderson, William V. Smith, and Walter Gordy (1950). "The Fine Structure of the Microwave Absorption Spectrum of Oxygen". Phys. Rev. 79 (4): 651–655. doi:10.1103/PhysRev.79.651.
- Hollas, p113, illustrates the spectrum of 15N2 obtained using 476.5 nm radiation from an argon ion laser.
- Cleeton, C.E.; Williams, N.H. (1934). "Electromagnetic waves of 1.1 cm wave-length and the absorption spectrum of ammonia". Physical Reviews 45 (4): 234–237. Bibcode:1934PhRv...45..234C. doi:10.1103/PhysRev.45.234.
- Gordy, W. (1948). "Microwave spectroscopy". Reviews of Modern Physics 20 (4): 668–717. Bibcode:1948RvMP...20..668G. doi:10.1103/RevModPhys.20.668.
- "June 1971, Hewlett Packard Journal". Retrieved November 2012.
- Schwendemann, R.H. (1978). Ann. Rev. Phys. Chem. 29: 537–558. doi:10.1146/annurev.pc.29.100178.002541.
- Dicke, R.H.; Romer, R.H. (1955). Rev. Sci. Inst. 26 (10): 915–928. doi:10.1063/1.1715156.
- Ekkers, J.; Flygare, W.H. (1976). Rev. Sci. Inst. 47 (4): 448–454. doi:10.1063/1.1134647.
- Balle, T.J.; Campbell, E.J.; Keenan, M.R.; Flygare, W.H. (1980). J. Chem. Phys. 72 (2): 922–932. doi:10.1063/1.439210.
- Jager, W. "Balle-Flygare FTMW spectrometer animation".
- "Web page of B.H. Pate Research Group, Department of Chemistry, University of Virginia.". Retrieved November 2012.
- Brown, G.G.; Dian, B.C.; Douglass, K.O.; Geyer, S.M.; Pate, B.H.; (2006). J. Mol. Spectrosc. 238: 200–212. doi:10.1016/j.jms.2006.05.003.
- Grubbs, G.S.; Dewberry, C.T.; Etchison, K.C.; Kerr, K.E.; Cooke, S.A. (2007). Rev. Sci. Inst. 78 (9): 096106. doi:10.1063/1.2786022.
- Wilcox, D.S.; Hotopp, K.M.; Dian, B.C.; (2011). J. Phys. Chem. A 115 (32): 8895–8905. doi:10.1021/jp2043202.
- 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.). Wiey. ISBN 0471965227.
- Atkins, P.W.; de Paula, J. (2006). Physical Chemistry (8th ed.). Oxford University Press. pp. 431–469. ISBN 0198700725. Chapter (Molecular Spectroscopy), Section (Pure rotation spectra) and page numbers may be differenct in different editions.
- Townes, Charles H.; Schawlow, Arthur L. (1975). Microwave spectroscop. New York: Dover Publications. ISBN 978-0-486-61798-5.
- Kroto, H. W. (2003). Molecular rotation spectr. Mineola, N.Y.: Dover Publications. ISBN 0-486-49540-X.
- Brown, John M.; Carrington, Alan. (2003). Rotational spectroscopy of diatomic molecule. Cambridge ; New York: Cambridge University Press. ISBN 0-521-53078-4.
- McQuarrie, Donald A. (Donald Allan) (2008). Quantum chemistry. Sausalito, Calif.: University Science Books. ISBN 1-891389-50-5.
- infrared gas spectra simulator
- Hyperphysics article on Rotational Spectrum
- A list of microwave spectroscopy research groups around the world