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Chapter 23: Problem 12

What are the differences between an emission spectrum and an absorption spectrum?

Short Answer

Expert verified
Emission spectrum has bright lines on dark background; absorption spectrum has dark lines on bright background.

Step by step solution

01

Understand the Emission Spectrum

An emission spectrum results when atoms or molecules release energy in the form of light. When an electron in an atom jumps from a higher energy level to a lower one, it emits light at specific wavelengths. The emission spectrum consists of bright lines or bands on a dark background.
02

Understand the Absorption Spectrum

An absorption spectrum occurs when atoms or molecules absorb light energy and cause electrons to jump from lower to higher energy levels. This spectrum shows dark lines or bands where wavelengths have been absorbed on a continuous bright background.
03

Compare Both Spectra

Compare the appearance: the emission spectrum shows bright lines on a dark background, while the absorption spectrum displays dark lines on a bright background. Compare the process: the emission spectrum results from electrons falling to lower energy levels, and the absorption spectrum results from electrons jumping to higher energy levels.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

emission spectrum
The emission spectrum is a unique set of wavelengths of light emitted by atoms or molecules. When an atom's electron transitions from a higher energy level to a lower energy level, it releases energy in the form of light. This light corresponds to specific wavelengths, which form the emission spectrum. You will observe bright lines or bands against a dark background. These lines are like fingerprints for different elements, each having a distinct emission spectrum. For instance, when you see bright red lines in the spectrum, you might be observing hydrogen emissions.
absorption spectrum
The absorption spectrum is created when atoms or molecules absorb certain wavelengths of light, causing electrons to jump from a lower energy level to a higher energy level. This results in a spectrum with dark lines or bands. These dark lines occur precisely at the wavelengths where light has been absorbed. The rest of the spectrum is a continuous bright background. You can think of the dark lines as 'missing pieces' where light has been taken up by the atoms. This spectrum can help identify substances based on which wavelengths of light they absorb, such as in identifying gases in stars.
energy levels in atoms
Atoms have discrete energy levels where electrons can reside. Imagine the levels like rungs on a ladder. An electron can jump between these levels by absorbing or releasing energy. When an electron absorbs energy, it moves to a higher energy level. When it releases energy, it falls to a lower level. The amount of energy absorbed or released corresponds to specific wavelengths of light. This is fundamentally what creates either emission or absorption spectra. Think of each jump corresponds to a unique color or wavelength of light.
wavelengths of light
Wavelengths of light are the different distances between the peaks of light waves. Light can have long or short wavelengths, which we perceive as different colors. For example, red light has longer wavelengths, while blue light has shorter wavelengths. In both emission and absorption spectra, specific wavelengths are released or absorbed by atoms. The precise wavelengths involved tell us a lot about the elements or compounds present. Each element absorbs or emits light at characteristic wavelengths, which can be measured to identify substances.

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