Question

Name Lab Day circled: Mon. Tues. AM Tues, PM Wed Thurs. Fri. Prelaboratory Exercise for the Atomic Emission and Absorption Experiment The spectroscopes used in our lab are scaled in nanometer units. You will work with three of the four possible Balmer series transitions of Hydrogen whose lines are in the visible region of the electromagnetie spectrum. Electrons absorb energy from n-2 level and depending on how much energy is absorbed, they are excited to different higher energy levels. From the higher energy level, the electrons emit energy which can be seen as light with a certain color depending on how far they fall and thus now much energy is emitted. The Rydberg equation relates the wavelength of light emitted to the difference in energy levels from which the excited electron falls to the level to which the electron falls. Laett-2 Level 5-+2 Level 4-2 Lovel 3-2 Level 2 Energy Absorbed Energy Eimited Rydberg Equation: 1/2 = 1.097 x 107m-(1/n12 - 1/m2) 12 higher energy level in which the excited electron is found n= lower energy level in which the electron is found after emitting light 2 = wavelength of light emitted when an electron falls from na to ni 1. Examine the shortest emission line in the graph above. This is the first emission line or the emission line furthest to the left of the four emission lines. a) What is the energy level for p in this line? b) What is the energy level for nz in this line?

Answer 1

1 The question is based on the Concept of absorption and emission spectra. 17 Shortest emission line from fig.is I n=3 n=2 a) n = lower energy level seis which ē is found after emission 16) M = Higher energy level is. which excited e-is found This energy levels for the emission line was calculated. OVOR