Continuous Emission Monitoring. James A. Jahnke

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      (4‐1)

      where c is the velocity of light, 3.0 × 10⁸ m/s.

      Literature describing continuous monitoring instruments often specifies the wavelength to characterize the spectral region used in the analytical method. Different units are often used for wavelength in different regions of the electromagnetic spectrum although the nanometer (nm) = 10⁻⁹ m has become the standard unit. Another unit, the Angstrom, Å = 10⁻¹⁰ m, has been used historically in the ultraviolet region. In the infrared region, both the μm = 10⁻⁶ m (also called 1 “micron”) and the wavenumber are commonly used by spectroscopists. The wavenumber is expressed as

      (4‐2)

      Note that the units of are given in terms of the number of wavelengths per centimeter, called reciprocal centimeters or wavenumbers. The wavenumber is essentially a measure of frequency, differing from v by the constant factor of the velocity of light. The wavenumber is calculated by calculating the reciprocal of the wavelength expressed in μm and multiply by 10⁴ to obtain wavenumbers in units of cm⁻¹.

The wavelength of light used in CEM instrumentation ranges from 200 nm in the ultraviolet to 20 000 nm in the infrared. Figure 4‐2 shows the regions of the electromagnetic spectrum and the wavelength bands where molecules interact with light energy. Instruments are designed to measure the effects of these interactions.

      The infrared spectral region is particularly important for the measurement of gaseous pollutants, and many instruments have been designed to operate in the infrared region. The infrared region is separated into the near infrared (NIR), mid infrared (MIR), and far infrared. Although an ISO standard does exist (ISO 2015), the boundaries of these regions are not universally agreed upon; there exists some ambiguity as to where the mid infrared ends and the far infrared begins, depending upon the usage by instrument manufacturers, spectroscopists, astronomers, or others.

      Absorption of Light by Molecules

Light carries energy. Light has the properties of waves, but in some of its interactions with matter it behaves as if it were composed of discrete packets of energy called photons. In a beam of light having frequency v, each of these photons carries energy defined by the Planck‐Einstein relation of Equation 4‐3.

(4‐3)

      where h is Planck's constant and has a numerical value of 6.62 × 10⁻²⁷ erg‐s. Clearly, the energy of a photon is dependent upon the frequency or wavelength of the light. Light (photons) of short wavelengths (such as in the ultraviolet) will carry more energy than light (photons) of longer wavelengths (such as in the infrared). Photons of different energies will have different effects. From a practical sense, sitting on the beach too long in bright sunlight can cause a severe sunburn. On the other hand, sitting under an infrared heat lamp will soothe sore muscles without causing sunburn. The effects of UV radiation are extremely severe under the Antarctic ozone hole, but less severe where the stratospheric ozone layer reduces the number of photons per unit time reaching Earth's surface. Light of different wavelengths (photons of different energies) will have a variety of effects on molecules. In a monitoring instrument, the manufacturer determines the best way to use these effects to make gas concentration measurements.

Molecules are made up of atoms and molecular electrons that are arranged in very specific patterns, which undergo unique and complex motions. If light of a given wavelength should resonate with one of these motions, it will have a high probability of being absorbed by a molecule. The light essentially alters the molecular energy, causing the molecule to act differently than it was acting before the light was absorbed.