CURRICULUM | SCIENCE | TECHNOLOGY | ENGINEERING | MATH
“Sometimes it is the people no one can imagine anything of, who do the things no one can imagine.” - Alan Turing
SPECTROSCOPY PRACTICE
UNDERSTANDING THE EMISSION SPECTRUM
EMISSION SPECTRA EXPLAINED
SIMULATION FOR THOSE AT HOME
FOR YOUR NOTEBOOK:
Notes for Spectroscopy
When it comes to getting the spectra of different elements, Visible light spectrum is continuous (You see all of ROYGBIV); light emission is discontinuous and focuses on specific bands of the visible light spectrum depending on the element
An electron of an atom starts at a low energy level. We excite the entire atom with electricity and it can't handle that excess energy. The electron jumps to a higher energy level (orbital), and releases a photon of light.
By changing the amount of a substance we have, it will affect the brightness of the emission lines.
Each element in the periodic table has its own unique emission lines.
Atoms tend to be in a lower energy state (ground state)
To do this they must get rid of some energy
When an atom gets rid of the energy they emit a wave of light with that exact energy
Spectrometers allow us to see this change in energy in the form of light emission
EMISSION SPECTRA ID LAB
Below is a link to the Emission Spectra Lab. In class, we are going to give electricity to specific elements. You will use a spectrometer to find the emission bands to determine what element you are looking at. In your assessment, feel free to use the Periodic Table Emission Spectra chart to determine what elements we are describing.