The most prominent line in the spectrum of neon is found at...

The most prominent line in the spectrum of neon is found at 865.438 nm. Other lines are located at $837.761 \mathrm{nm}, 878.062 \mathrm{nm}, 878.375 \mathrm{nm},$ and $1885.387 \mathrm{nm}$ (a) In what region of the electromagnetic spectrum are these lines found? (b) Are any of these lines found in the spectrum of neon shown in Figure $7.9 ?$ (c) Which of these lines represents the most energetic light? (d) What is the frequency of the most prominent line? What is the energy of one photon with this wavelength?

The most prominent line in the spectrum of neon is found at 865.438 nm. Other lines are located at $837.761 \mathrm{nm}, 878.062 \mathrm{nm}, 878.375 \mathrm{nm},$ and $1885.387 \mathrm{nm}$
(a) In what region of the electromagnetic spectrum are these lines found?
(b) Are any of these lines found in the spectrum of neon shown in Figure $7.9 ?$
(c) Which of these lines represents the most energetic light?
(d) What is the frequency of the most prominent line? What is the energy of one photon with this wavelength?

Key Concepts

Spectral Line Identification

Spectral lines are the specific wavelengths at which an element emits or absorbs light, and they serve as diagnostic fingerprints for identifying elements. This concept is important for understanding experimental data and determining whether lines observed in one setup (or figure) correspond to those predicted or previously documented for a given element.

Planck’s Equation

Planck’s equation, E = h? or equivalently E = hc/?, provides the mathematical foundation to calculate the energy of a photon from its wavelength or frequency. This concept is fundamental when analyzing spectroscopic emissions and determining both the energy of individual photons and the ordering of spectral lines by their relative energies.

Electromagnetic Spectrum

The electromagnetic spectrum encompasses all types of electromagnetic radiation, classified by wavelength or frequency. In this context, understanding which regions correspond to visible light, infrared, ultraviolet, and so on, is essential to determine where the given wavelengths of light lie. This concept helps in contextualizing the nature of light the atoms emit or absorb.

Infrared Radiation

Infrared radiation refers to electromagnetic waves with wavelengths longer than visible light, typically ranging from about 700 nm to 1 mm. Recognizing that the wavelengths provided (in the range of approximately 837 nm to 1885 nm) fall into the infrared portion is crucial for identifying the energy and technical considerations related to these emissions.

Photon Energy and Frequency Relationship

The energy of any photon is intrinsically linked to its frequency by the relation E = h?, where h is Planck's constant and ? is the frequency. Since frequency and wavelength are related by the speed of light (c = ??), understanding this relationship is key to determining which spectral line is the most energetic, as higher frequency (or shorter wavelength) implies a higher photon energy.

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