Chapter 2: Problem 7

Explain how Bohr's model of the atom accounts for spectra.

Short Answer

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Answer: In Bohr's model of the atom, electrons can only occupy specific discrete energy levels. When electrons transition between these energy levels, they either absorb or emit a photon with a specific wavelength corresponding to the energy difference between the levels. Since there are only specific wavelengths that can be absorbed or emitted during energy level transitions, this results in discrete atomic spectra with well-defined lines rather than continuous spectra. Each element has a unique pattern of lines in their spectra due to specific energy level transitions, which can be used to identify the element.

Step by step solution

Introduce Bohr's Model of the Atom

Bohr's model of the atom is based on the idea that electrons in atoms can only occupy certain discrete energy levels. In this model, electrons orbit the nucleus at specific distances, and each orbit corresponds to a specific energy level. When an electron jumps between energy levels, it either absorbs or emits light with a specific wavelength corresponding to the energy difference.

Describe Energy Levels and Transitions

According to Bohr's model, the energy levels in an atom are quantized, meaning that they are discrete and not continuous. An electron can only exist in these specific energy levels and nowhere in between. When an electron changes energy levels, it undergoes a transition, either absorbing or emitting a photon with an energy equal to the difference between the initial and final energy levels. The energy of a photon is related to its wavelength by the simple equation: E = h * c / λ, where E is the energy, h is the Planck constant, c is the speed of light, and λ is the wavelength.

Connect Energy Level Transitions to Spectra

When an electron jumps to a higher energy level, it absorbs a photon with a wavelength corresponding to the energy difference between the levels. This absorbed wavelength is removed from white light passing through the atom, resulting in an absorption spectrum with dark lines at the absorbed wavelengths. Conversely, when an electron transitions to a lower energy level, it emits a photon with a wavelength corresponding to the energy difference. The emitted wavelengths combine to form an emission spectrum, which consists of bright lines at the emitted wavelengths.

Explain Discrete Spectra

Since energy levels in an atom are quantized, there are only specific wavelengths that can be absorbed or emitted during energy level transitions. This results in discrete atomic spectra with well-defined lines rather than continuous spectra. For each element, the specific energy level transitions result in a unique pattern of lines in their spectra, which can then be used to identify the element.

Relate the Concept to Real-Life Observations

The discrete spectra resulting from Bohr's atomic model have been observed in various real-life experiments like flame tests and hydrogen spectrum analysis. In a flame test, a metal salt is heated in a flame, and the color of the flame corresponds to the specific wavelengths emitted by electrons in the metal ions transitioning between energy levels in the atom. Similarly, the Balmer series of hydrogen's atomic spectrum consists of specific lines corresponding to electron transitions in the hydrogen atom, further validating the concept of quantized energy levels and Bohr's model of the atom.

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Explain how Bohr's model of the atom accounts for spectra.

Short Answer

Step by step solution

Introduce Bohr's Model of the Atom

Describe Energy Levels and Transitions

Connect Energy Level Transitions to Spectra

Explain Discrete Spectra

Relate the Concept to Real-Life Observations

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