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Chapter 5: Problem 21

Why do different elements display different patterns of lines in their spectra?

Short Answer

Expert verified
Different elements display different patterns of spectral lines because of their unique atomic structure. Each element has a unique arrangement of electrons in energy levels, leading to specific patterns of energy absorption and emission, which in turn create distinct spectra.

Step by step solution

01

Understand the Atomic Structure

Each element is made up of atoms. These atoms have a nucleus, composed of protons and neutrons, with electrons circling around it in defined energy levels or shells. The energy levels of the electrons in an atom are distinct, and specific to each element.
02

The Role of Energy Levels (Bohr's Theory)

Niels Bohr's theory explains that an electron in an atom can jump from a lower energy level to a higher energy level when energy is absorbed. When the electron returns to its original energy level, energy is emitted. This emission or absorption of energy is observed as light.
03

Light Emission and Spectra

Light is emitted when an electron drops from a higher energy level to a lower one. The energy difference between the two levels determines the energy, and hence the wavelength or color, of the emitted light. This gives rise to spectral lines.
04

Different Elements, Different Spectra

Each element has a unique number of electrons, and a unique arrangement of energy levels. As a result, each element has a unique pattern of spectral lines. This difference in atomic structure leads to different patterns of lines in their spectra.

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Most popular questions from this chapter

(a) Can a hydrogen atom in the ground state absorb an \(\mathrm{H}\)-alpha \(\left(\mathrm{H}_{\alpha}\right)\) photon? Explain why or why not. (b) Can a hydrogen atom in the \(n=2\) state absorb a Lyman-alpha \(\left(\mathrm{L}_{a}\right)\) photon? Explain why or why not.

Obtain a glass prism (or a diffraction grating, which is probably more readily available and is discussed in the next chapter) and look through it at various light sources, such as an ordinary incandescent light, a neon sign, and a mercury vapor street lamp. Do not look at the sun! Looking directly at the Sun causes permanent eye damage or blindness. Do you have any trouble seeing spectra? What do you have to do to see a spectrum? Describe the differences in the spectra of the various light sources you observed.

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What is meant by the frequency of light? How is frequency related to wavelength?

The equation that relates the frequency, wavelength, and speed of a light wave, \(v=c / \lambda\), can be rewritten as \(c=v \lambda . \mathrm{A}\) friend who has studied mathematics but not much astronomy or physics might look at this equation and say: "This equation tells me that the higher the frequency \(v\), the greater the wave speed \(c\). Since visible light has a higher frequency than radio waves, this means that visible light goes faster than radio waves." How would you respond to your friend?
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