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1.2: Component 2 - Matter

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    A typical molecule will have thousands of possible energy levels involving rotational, vibrational and electronic excitations and combinations thereof. However, relatively few transitions between these states will be allowed. Rules restricting transitions between states are call Selection Rules. They all have a basis in symmetry of the molecules. Thus, Group theory is a powerful tool to develop selection rules, and thus, to interpret the observed spectra.

    From undergraduate quantum mechanics, you are familiar with the solutions to the time-independent Schrödinger Equation

    \[H^{(0)} \psi_n(\vec{r}) = E_n \psi_n(\vec{r})\]

    or in bra/ket notation

    \[\hat{H}^{(0)} | n \rangle = E_n | n \rangle\]

    which can be solved exactly for many systems, such as the harmonic oscillator, the rotating diatomic (rigid) molecule, and the H-atom and numerically for the rest. The wavefunctions, \(\{| n \rangle\}\), are called stationary states with energies \(\{E_n\}\). These are solutions to the time-independent Schrödinger equation.

    If \(\hat{H}\) is absolutely independent of time, then a molecule describes by a particular ψn will stay in that state forever. There will no possibility for transitions between different ψn, which is the essence of spectroscopy. Transitions between stationary states can only happen in the presence of a time-dependent Hamiltonian. This is provided by the oscillating electric and magnetic fields of the radiation. So the total Hamiltonian is now

    \[H_{tot} = H^{(0)} + H^{(1)}(t)\]

    where \(H^{(1)}(t)\) us the time-dependent Hamiltonian that describes the interaction with the electromagnetic radiation.

    Electric Dipole Coupling

    Ultraviolet and visible radiation interacts with matter which causes electronic transitions (promotion of electrons from the ground state to a high energy state). The ultraviolet region falls in the range between 190-380 nm, the visible region falls between 380-750 nm. For the interaction of the oscillating electric field, \(\vec{E}(t)\) of monochromatic radiation of frequency, \(\nu\), with the electrons of the molecules,

    \[H^{(1)}(t) = \vec{E} \cdot \vec{\mu} \cos (\pi \nu t) \label{eq1}\]

    where \(\vec{E}\) is the amplitude of the oscillating electric field vector and \(\vec{\mu}\) is the electric dipole moment of the molecule and \(\nu\) is the frequency of the radiation. The electric dipole moment is a summation of all charges in the species.

    \[ \vec{\mu} = -e \sum_i \vec{R}_i\]

    \(\vec{E}\) is polarized in a plane to the direction of propagation. Generally, light is depolarized meaning that polarization is uniformly distributed in the XY place for Z direction. Laser radiation, in contrast, is often plane polarized, with a simple polarization in the XY plane or at some angle.

    For Reference

    The energy of 285 nm photons is \(6.97\times 10^{-19} J\) and for one mole of photon \(419.7 \, kJ/mol\).

    The mean wavelength in visible is 565 nm. The energy of 565 nm photons is \(3.52 \times 10^{-19} J\) and for one mole of photon \(211.7 \,kJ/mol\).

    If the radiation is not strong, then \(H^{(1)}(t) \ll H^{(0)}\) and the change introduced by H(1)(t) can be treated as a perturbation, e.g., 1st order transition theory. We will not go through the steps here, which are covered in many standard textbooks in Quantum Mechanics.

    From such approaches, we get an expression for the transition probability is often called “Fermi’s Golden Rule

    \[W_{i \rightarrow f}=\left(\frac{4 \pi}{h}\right)\left|H_{f i}^{(1)}\right|^{2} \rho(\Delta E)\]

    where

    • \(i\) and \(f\) label the initial and final states in the transition
    • \(W_{i \rightarrow f}\) is the probability per unit time that a transition occurs.
    • \(ρ_N(ΔE)\) is the density of final states and
    • \(ΔE=abs(E_f-E_i)\) in dimensions of energy-1. This important part of is \(W_{i \rightarrow f}\) is \(H_{f i}^{(1)}\)

    \[ H_{f i}^{(1)} = \langle f | H^{(1)} | i \rangle \label{eq10}\]

    For example, for the electric dipole-induced transition (Equation \ref{eq1}), the coupling element is

    \[ H_{f i}^{(1)} = \vec{E} \cdot \langle f | \vec{\mu} | i \rangle \label{eq11}\]

    other transitions (e.g., electric quadrupole-induced transition, magnetic dipole-induced transitions, etc) will have different expressions.

    If this matrix element of the perturbed Hamiltonian is non-zero, then transitions CAN be induced from \(| i \rangle\) to \(| f \rangle \). The importance of symmetry is that the integrals (Equation \ref{eq10} or \ref{eq11}) can often be shown to be ZERO, using group theory arguments. We will be getting to this later. Transitions can be assigned because we know that some for them cannot occur or can only occur with some probability with a weak absorption from the applied radiation (within 1st order perturbation theory).

    Separation of Eigenstates

    Born-Oppenheimer approximation: energy separated into three types rotational levels superimposed on vibrational levels and vibrational levels superimposed on electronic levels.

    \[ ΔE = Δ_{Eelectronic} + ΔE_{vibration} + ΔE_{rotation}\]

    And there is a strong separation of magnitude in these energies (Figure \(\PageIndex{1}\)):

    \[ΔE_{electronic} > ΔE_{vibration} > ΔE_{rotation}\]

    Molecular_energy_levels_en.svg
    Figure \(\PageIndex{1}\): A diagram representing singlet energy-levels in a molecule to help explain the concept of electronic, rotational and vibrational energy-levels to my students. (CC BY-SA 3.0; Lvzon via Wikipedia)

    The energy levels (eigenstates) can be rated in the following order electronic > vibrational > rotational. Each of these transitions differ by an order of magnitude. Rotational transitions occur at lower energies (longer wavelengths) and this energy is insufficient and cannot cause vibrational and electronic transitions, but vibrational (near infra-red) and electronic transitions (ultraviolet region of the electromagnetic spectrum) require higher energies. The diagram below illustrates possible transitions that occur.

    • transitions represents pure rotational changes (far infrared).
    • transitions rotational-vibrational (rovibrational) transitions;
    • transitions are rotational-vibrational-electronic transitions (visible and ultraviolet) \(S_o\) is electronic ground state and \(S_1\) and \(S_2\) are electronic excited states.

    For a transition to be spectroscopically observed

    1. There must exist a coupling mechanism (via \(H^{(1)|}\)) between initial and final eigenstates
    2. The initial eigenstate (\(| i \rangle \)) must be populated (e.g., d0 d-d electronic transition). Since most spectroscopies involve molecules/systems that are thermally populated, then the Boltzmann distribution is required \[p_{i}=\frac{e^{-E_{i / k T}}}{Q}\] with \[Q=\sum_{i}^{\infty} e^{-E_{i} / k T}\] (assuming non-degenerate eigenstates)
    3. The final eigenstate (\(| f \rangle \)) must be unpopulated (e.g., d10 d-d electronic transitions)
    Note

    At room temperature (\(kT=200\, cm^{-1}\)), most electronic transitions occur from \(v=0\), but not from \(J=0\) eigenstate. So potentially multiple excitation transitions typically coexist.


    1.2: Component 2 - Matter is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts.

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