Final answer:
Continuous spectrum displays all wavelengths of light, absorption spectrum shows dark lines where light is absorbed by gas atoms, and emission spectrum exhibits bright lines at specific wavelengths emitted by excited gas atoms. These spectral patterns are crucial for identifying elemental composition.
Step-by-step explanation:
Compare and Contrast: Continuous Spectrum, Absorption Spectrum, and Emission Spectrum
When comparing the three different types of spectra: continuous spectrum, absorption spectrum, and emission spectrum, key distinctions can be observed. A continuous spectrum is characterized by an uninterrupted range of colors, as seen from a source like an incandescent lightbulb, representing all wavelengths within the light spectrum.
In contrast, an absorption spectrum occurs when a less dense gas absorbs certain wavelengths from a continuous spectrum behind it, creating dark lines, where each missing color corresponds to a specific wavelength absorbed by atoms in the gas. Lastly, an emission spectrum is observed when excited atoms of a cloud of gas emit light at distinct wavelengths, with each element displaying a unique pattern of bright lines.
The study of these spectral lines is fundamental in understanding the composition of various gases and celestial objects. For instance, the line spectra of sodium, hydrogen, calcium, and mercury, consist of discrete wavelengths and can help identify the presence of these elements based on their unique emission or absorption signatures.