Metals reveal their true colors
On November the 8th, we explored atomic orbitals and energy levels. We began with a review of the particle-wave duality of photons, and then watched a 5 minute TED talk on the history of the structure of the atom and orbitals. We then analyzed the derivation of Bohr’s model and Rydberg’s prediction for energy transformations using this model of excitation and emission of photons from one orbital to the next. Once we arrived at the Rydberg formula, we used the formula to predict the wavelength of light that would be emitted by an excited sodium atom. The theoretical value was then tested in our experiment, which were found to be very close. The experiment was done by taking small amounts of various metal compounds and burning them, while analyzing their specific emission spectral lines through spectroscopes.
The students then came to conclusions as to why certain colors formed and what multiple spectral lines showed.
On November the 1st, we went over the basics of what an atom is and basic particles (protons, neutrons, electrons, photons). We discussed the particle-wave duality of particles, especially photons. We also went over the periodic table and some basic principles of atomic orbitals, which we will further discuss next week in greater detail.
The experiment we conducted was to explore transition metals and how they can rearrange their d orbitals, leading to various colors.