Discussion The objective of this experiment is to apply spectroscopic methods to explore light emitted by different atoms heated in a flame; this is an introduction to the relationship between atomic line spectra and atomic structure. In part 1, we measured each color of light (from violet to yellow) and noticed that the wavelength increased as the spectroscope scale reading increased. The violet and blue lines were close together and so were the green and yellow lines. There was a gap between the violet/blue lines and the green/yellow lines. In plotting wavelength as a function of the spectroscope readings, we observed that the points formed a pretty straight line (indicating a linear relationship). We then took the linear least square fit of the data and used the equation of that line to determine the wavelengths in part 2. In part 2, the lines were spaced similarly to part 1. The violet and blue lines were close together and so were the green and yellow lines. There was a gap between the violet/blue lines and the green/yellow lines. The observed wavelength for blue was more close to its accepted wavelength than were the observed wavelengths for violet, green, and yellow. The % errors for the wavelength of each color were: violet=7.48%, blue=1.12%, green=7.45%, and yellow=11.40%. Most of our ninitial values were off (due to the observed wavelengths being off). They were violet: ninitial=7, blue: ninitial=4, green: ninitial=3, and yellow: ninitial=3. The actual values are violet: ninitial=6, blue: ninitial=5, green: ninitial=4, and yellow: ninitial=3. As such, the
