Question

Spectroscopy, or the study of how light interacts with matter, is an extremely powerful tool scientists use to identify unknown substances. One branch of spectroscopy is the measurement of the interactions between gases and visible light. Sending a very high voltage through a gas adds energy to the system causing some of the electrons to enter a more unstable, or excited state. To return to the stable state, the electron emits some of that energy in the form of light. Using the fact that electrons can only exist in certain energy "shelves, we can predict what wavelengths of light, or colors, are emitted when we add energy to the system. The following equation shows the energy levels for a hydrogen atom with only one electron (when dealing with multiple electrons and protons the math becomes far more complex and is outside the scope of this activity) 1 = RH(-) Where: is the wavelength of light Rh is the Rydberg Constant for a Hydrogen atom, 1.0974 . 109/m ng is the final energy level ni is the starting energy level (ny and ng are always integers: 1,2,3...) 1. Using the formula above, what is the energy emitted between the 2nd and 18 energy levels? 121.5 nm 102.5 nm

Answer 1

Pago n=1 - PH 1 가 LI पि 4. A 8 X 10934X104 141.5m