Final answer:
An emission spectrum shows colorful lines corresponding to wavelengths emitted by energized atoms, while an absorption spectrum displays dark lines where wavelengths are absorbed by atoms. These spectra are unique to each element and have spectral lines that match in both types of spectra, providing a type of elemental 'fingerprint'.
Step-by-step explanation:
Difference Between Emission and Absorption Spectrum
The primary difference between an emission spectrum and an absorption spectrum lies in the way each spectrum is produced and the appearance of the spectral lines. The emission spectrum is characterized by colorful lines against a dark background. These lines represent specific wavelengths that are emitted by atoms or molecules when they transition from a higher to a lower energy state. In contrast, an absorption spectrum features dark lines against the backdrop of a continuous spectrum. These dark lines, also known as Fraunhofer lines, correspond to wavelengths that are absorbed as atoms or molecules transition to higher energy states. Both spectra are unique to each chemical element and reveal precise information regarding the elemental composition of a substance.
Each element's characteristic pattern of spectral lines is essentially its 'fingerprints' in both emission and absorption spectra. This means that, for any given element, the positions of the spectral lines in the emission spectrum are exactly the same as those in its absorption spectrum, signifying that the atoms can absorb and emit radiation at specific, characteristic wavelengths.