Question

1. type your answer in the box below. what is the relationship between energy, wavelength, and the quantization of energy in the atomic emission spectrum?

Explanation:

The energy of a photon is given by the equation $E = h
u$, where $h$ is Planck's constant and $
u$ is frequency. Since $
u=\frac{c}{\lambda}$ (where $c$ is the speed of light and $\lambda$ is wavelength), we have $E=\frac{hc}{\lambda}$. In the atomic - emission spectrum, energy is quantized. Electrons in an atom can only occupy certain discrete energy levels. When an electron transitions from a higher - energy level to a lower - energy level, it emits a photon with an energy equal to the difference in the energy levels of the two states. The wavelength of the emitted photon is determined by the energy of the photon according to $E=\frac{hc}{\lambda}$. So, the energy of the emitted photon is inversely proportional to its wavelength, and the quantization of energy levels in an atom leads to discrete wavelengths in the atomic emission spectrum.

Answer:

The energy of a photon is inversely proportional to its wavelength ($E=\frac{hc}{\lambda}$), and the quantization of energy levels in an atom results in discrete wavelengths in the atomic emission spectrum.