# Introduction for Module 11 – Light and the Bohr Model

Textbook: Open Stax Chemistry 2e

Suggested Reading: Chapter 6.1-6.2

Learning Objectives:

- Use appropriate equations to calculate related light-wave properties such as frequency, wavelength, and energy
- Describe the particle nature of light
- Distinguish between line and continuous emission spectra
- Describe the Bohr model of the hydrogen atom

Captions and Attributions:

- The photoelectric effect demonstrated the particle-like nature of light. Figure 6.11 Photons with low frequencies do not have enough energy by Open Stax is licensed under CC BY 4.0.
- The principle quantum number increases as we "go out" from the nucleus. While these are not the only energy levels, it is an important step in realizing that energy levels are quantized within the atom and can only have specific predetermined values. Figure 6.19, Different shells are numbered by principal quantum numbers by Open Stax is licensed under CC BY 4.0.
- Emission Spectrum for Hydrogen shows the energies between electron orbitals, and is always the same for Hydrogen. Figure 6.13, Compare the two types of emission spectra by Open Stax is licensed under CC BY 4.0.
- The electromagnetic spectrum goes well beyond visible light and is directly related to energy. Figure 6.3, Portions of the electromagnetic spectrum by Open Stax is licensed under CC BY 4.0.