For no 4 this is the link: https://phet.colorado.edu/en/simulation/legacy/discharge-lamps

https://phet.colorado.edu/en/simulation/legacy/discharge-lamps Open the link Click on the upper tab Multiple Atoms. Click on "Continuous" under Electron Production. Under Options (lower right) click on Spectrometer and Squiggles. The discharge tube contains hydrogen gas with electrons (from the voltage on the tube's electrodes) going through the tube, getting absorbed by the atoms, and then emitting photons. The squiggles on the right show the electrons jumping through energy levels as the atoms get excited, and then emitting photons as the excited electrons drop down to lower levels. The ground state is n = 1, and other levels up to n = 6 are shown. The squiggles show electrons jumping between energy levels as atoms get excited, and then emitting photons as the excited electrons drop down to lower levels. The ground state is n = 1, and levels up to n = 6 are shown. The spectrometer shows the build up of photons, at spectral line locations coming from Bohr's equation. 4.a. Example 27-14 calculated the location of the violet Balmer line at A = 411.1 nm. This was for n = 6 to n' = 2. Calculate the red Balmer line, n = 3 to n' = 2, A = nm. 4.b. Sodium: click on this under the Atom Type pull-down. Sodium has 11 protons, Z= 11. We see a prominent yellow line, and its wavelength A = 589 nm. The squiggles in the energy levels show this occurring for the n' = 2 and n= 1 states. Use sodium's Z, n' and n, to calculate the predicted wavelength for the Bohr model, A = nm. Is this close to 589 nm? Yes/No. 4.c. Conclusion: the Bohr model works well for hydrogen: Yes/No. The Bohr model works well for sodium: Yes/No. Next page Photos: Nothing to turn in, photos of discharge tubes and a diffraction grating "held in front" to show spectral lines