Molecular vibration Totally Explained

Everything about Molecular Vibration totally explained

A molecular vibration occurs when atoms in a molecule are in periodic motion while the molecule as a whole has constant translational and rotational motion. The frequency of the periodic motion is known as a vibration frequency. A nonlinear molecule with n atoms has 3n−6 normal modes of vibration, whereas a linear molecule has 3n−5 normal modes of vibration as rotation about its molecular axis can't be observed. A diatomic molecule thus has one normal mode of vibration. The normal modes of vibration of polyatomic molecules are independent of each other, each involving simultaneous vibrations of different parts of the molecule.
   A molecular vibration is excited when the molecule absorbs a quantum of energy, E, corresponding to the vibration's frequency, ν, according to the well-known relation E=hν, where h is Planck's constant. A fundamental vibration is excited when one such quantum of energy is absorbed by the molecule in its ground state. When two quanta are absorbed the first overtone is excited, and so on to higher overtones. To a first approximation, the motion in a normal vibration can be described as a kind of simple harmonic motion. In this approximation, the vibrational energy is a quadratic function (parabola) with respect to the atomic displacements and the first overtone would have twice the frequency of the fundamental. In reality, vibrations are anharmonic and the first overtone has a frequency that's slightly lower than twice that of the fundamental. Excitation of the higher overtones involves progressively less and less additional energy and eventually leads to dissociation of the molecule, as the potential energy of the molecule is more like a Morse potential.
   The vibrational states of a molecule can be probed in a variety of ways. The most direct way is through infrared spectroscopy, as vibrational transitions typically require an amount of energy that corresponds to the infrared region of the spectrum. Raman spectroscopy, which typically uses visible light, can also be used to measure vibration frequencies directly.
   Vibrational excitation can occur in conjunction with electronic excitation (vibronic transition), giving vibrational fine structure to electronic transitions, particularly with molecules in the gas state.
   Simultaneous excitation of a vibration and rotations gives rise to vibration-rotation spectra.

Vibrational coordinates

The coordinate of a normal vibration is a combination of changes in the positions of atoms in the molecule. When the vibration is excited the coordinate changes sinusoidally with a frequency ν, the frequency of the vibration.

Internal coordinates

Internal coordinates are of the following types, illustrated with reference to the planar molecule ethylene,

Stretching: a change in the length of a bond, such as C-H or C-C
Bending: a change in the angle between two bonds, such as the HCH angle in a methylene group
Rocking: a change in angle between a group of atoms, such as a methylene group and the rest of the molecule.
Wagging: a change in angle between the plane of a group of atoms, such as a methylene group and a plane through the rest of the molecule,
Twisting: a change in the angle between the planes of two groups of atoms, such as a change in the angle between the two methylene groups.
Out-of-plane: Not present in ethene, but an example is in BF₃ when the boron atom moves in and out of the plane of the three fluorine atoms.

In a rocking, wagging or twisting coordinate the angles and bond lengths within the groups involved don't change. Rocking may be distinguished from wagging by the fact that the atoms in the group stay in the same plane.
In ethene there are 12 internal coordinates: 4 C-H stretching, 1 C-C stretching, 2 H-C-H bending, 2 CH₂ rocking, 2 CH₂ wagging, 1 twisting. Note that the H-C-C angles can't be used as internal coordinates as the angles at each carbon atom can't all increase at the same time.
See infrared spectroscopy for some animated illustrations of internal coordinates.

Symmetry-adapted coordinates

Symmetry-adapted coordinates may be created by applying a projection operator to a set of internal coordinates. The projection operator is constructed with the aid of the character table of the molecular point group. For example, the four(un-normalised) C-H stretching coordinates of the molecule ethene are given by ť Q_s1 = q₁ + q₂ + q₃ + q₄

   Q_s2 = q₁ + q₂ - q₃ - q₄ ť Q_s3 = q₁ - q₂ + q₃ - q₄

   Q_s4 = q₁ - q₂ - q₃ + q₄ where q₁ - q₄ are the internal coordinates for stretching of each of the four C-H bonds.
   Illustrations of symmetry-adapted coordinates for most small molecules can be found in Nakamoto.

Normal coordinates

A normal coordinate, Q, may sometimes be constructed directly as a symmetry-adapted coordinate. This is possible when the normal coordinate belongs uniquely to a particular irreducible representation of the molecular point group. For example, the symmetry-adapted coordinates for bond-stretching of the linear carbon dioxide molecule, O=C=O are both normal coordinates:

symmetric stretching: the sum of the two C-O stretching coordinates; the two C-O bond lengths change by the same amount and the carbon atom is stationary. Q = q₁ + q₂

asymmetric stretching: the difference of the two C-O stretching coordinates; one C-O bond length increases while the other decreases. Q = q₁ - q₂ When two or more normal coordinates belong to the same irreducible representation of the molecular point group (colloquially, have the same symmetry) there's "mixing" and the coefficients of the combination can't be determined a priori. For example, in the linear molecule hydrogen cyanide, HCN, The two stretching vibrations are

principally C-H stretching with a little C-N stretching; Q₁ = q₁ + a q₂ (a << 1)

principally C-N stretching with a little C-H stretching; Q₂ = b q₁ + q₂ (b << 1) The coefficients a and b are found by performing a full normal coordinate analysis by means of the Wilson GF method.

Newtonian mechanics

Perhaps surprisingly, molecular vibrations can be treated using Newtonian mechanics, to calculate the correct vibration frequencies. The basic assumption is that each vibration can be treated as though it corresponds to a spring. In the harmonic approximation the spring obeys Hooke's law: the force required to extend the spring is proportional to the extension. The proportionality constant is known as a force constant, f. The anharmonic oscillator is considered elsewhere. ť

mathrm !

,

where n is a quantum number that can take values of 0, 1, 2 ... The difference in energy when n changes by 1 are therefore equal to the energy derived using classical mechanics. See quantum harmonic oscillator for graphs of the first 5 wave functions. Knowing the wave functions, certain selection rules can be formulated. For example, for a harmonic oscillator transitions are allowed only when the quantum number n changes by one, ť

Delta n = pm 1

but this doesn't apply to an anharmonic oscillator; the observation of overtones is only possible because vibrations are anharmonic. Another consequence of anharmonicity is that transitions such as between states n=2 and n=1 have slightly less energy than transitions between the ground state and first excited state. Such a transition gives rise to a hot band.

Intensities

In an infrared spectrum the intensity of an absorption band is proportional to the devative of the molecular dipole moment with respect to the normal coordinate. The intensity of Raman bands depends on polarizability. See also transition dipole moment.

Further Information

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