4.Make a prediction using your model. If an electron were to emit a photon and move from the n=3 level to the n=1 level, what wavelength of light would it emit? (Hint: use the Ryberg equation) Would this be a bigger energy What would be the energy change for this transition? change or a smaller energy change that the transition from the n=3 to the n=2 transition? Would you be able to see this energy change (will it be visible light?) What part of the electromagnetic spectrum should you look in to find these photons, the ultraviolet or the infrared?

Introduction

It is mathematically possible to determine the wavelength of light using the Rydberg formula. A shift in an electron's energy occurs when it moves from one atomic orbit to another. The photon of light is formed when the electron transitions from a high-energy orbit to a state with lower energy.

There is a unique spectral fingerprint for each element. An element that is in the gaseous state will emit light when heated. Bright lines of distinct colors can be seen when this light travels through a prism. Each component differs somewhat from the others. The study of spectroscopy began with this finding.

Swedish scientist Johannes Rydberg discovered the mathematical connection between one element's spectral line and the next. He found that the wavenumbers of succeeding lines had an integer relationship. This formula was developed by combining his discoveries with Bohr's atomic model.

                                                        $\frac{1}{\lambda }=R{Z}^2(\frac{1}{{final level}^2}-\frac{1}{{initial level}^2})$

where  R is Rydberg’s constant 

Z is The atomic number of the atom

n is the integer number where n₂>n₁.

$\lambda$ is the wavelength