Which of the following best describes an atomic emission spectrum?

• A. A spectrum showing dark lines on a bright background, resulting from absorption of specific wavelengths.
• B. A series of discrete lines of color produced when atoms emit light at specific wavelengths.
• C. A continuous band of colors with no gaps, produced by a heated solid.
• D. A single color of light emitted by an atom.

Answer: (B)

Verified step by step guidance

1. Understand that an atomic emission spectrum is related to the light emitted by atoms when their electrons transition from higher energy levels to lower energy levels.
2. Recall that when electrons in an atom drop to lower energy states, they emit photons of specific energies, which correspond to specific wavelengths of light.
3. Recognize that these emitted wavelengths appear as discrete lines of color, each line corresponding to a particular electronic transition within the atom.
4. Contrast this with an absorption spectrum, which shows dark lines on a bright background due to absorption of specific wavelengths, and a continuous spectrum, which shows a full range of colors without gaps.
5. Conclude that the atomic emission spectrum is best described as a series of discrete lines of color produced when atoms emit light at specific wavelengths.