Describe how the Bohr model of the atom explains emission line spectra. - Leaving Cert Physics - Question 1 - 2022

The Bohr model of the atom introduces the concept of quantized energy levels for electrons. In this model, electrons orbit the nucleus at specific distances corresponding to distinct energy levels. When an electron transitions from a higher energy level to a lower one, it emits energy in the form of light.

This emitted light has a frequency that can be determined using the formula:

u$$ where: - $E$ is the energy difference between the two levels, - $h$ is Planck's constant, and - $\nu$ is the frequency of the emitted photon. The energy difference between the levels can also be expressed as: $$E = E_1 - E_2$$ This results in the emission of light with a particular wavelength, related by the equation: $$\lambda = \frac{c}{\nu}$$ where: - $\lambda$ is the wavelength of the emitted light, and - $c$ is the speed of light. Thus, the transition of an electron falling from one energy level to another results in the emission of light at specific frequencies, leading to the characteristic line spectra observed in elements.