The purpose of this spectroscopy experiment was to determine if the spectra matched the electronic transitions that occur in the hydrogen atom among several other atoms. We used the Bohr model of atomic structure to determine the orbit numbers that correspond with the spectrum emitted by the hydrogen atom. The Bohr model states that electrons will never be found in between states, but rather completely in one state or the other. We used this model to determine the initial n value at which the electron started at prior to dropping down to n = 2.
An emission spectra, as it suggests, is when a substance emits radiation due to being heated or chemically affected. When viewing an emission spectra, there will be a group of colored lines separated by black spaces. Where the lines are, is where photons …show more content…
An absorption spectra is seen as a continuous band of colors with black lines within. The black lines are where the photons are being absorbed by the electrons.
A continuous spectrum is when all of the wavelengths are present in a given area. An example of this would be the rainbow. The rainbow doesn’t have any breaks in color, it is continuous. Both emission spectrums and absorption spectrums are examples of line spectrums. This is because when you view the spectrum, there are only a few lines on it, therefore meaning only a few wavelengths.
To determine the wavelength of each color emitted, we used the spectrometer and read the wavelengths that corresponded with each color line we observed. This data is located on the data sheets within the lab manual. To determine the energy level (n), one must use the formula E = -RH (1/nf2 – 1/ni2) where E = hc/. The energy emitted by the hydrogen atom compared to the other atoms tested, was very similar. All of the atoms tested had emitted energy between approximately 3.0x10-19J and 5.0x10-19 J.
Calculations and
An emission spectra, as it suggests, is when a substance emits radiation due to being heated or chemically affected. When viewing an emission spectra, there will be a group of colored lines separated by black spaces. Where the lines are, is where photons …show more content…
An absorption spectra is seen as a continuous band of colors with black lines within. The black lines are where the photons are being absorbed by the electrons.
A continuous spectrum is when all of the wavelengths are present in a given area. An example of this would be the rainbow. The rainbow doesn’t have any breaks in color, it is continuous. Both emission spectrums and absorption spectrums are examples of line spectrums. This is because when you view the spectrum, there are only a few lines on it, therefore meaning only a few wavelengths.
To determine the wavelength of each color emitted, we used the spectrometer and read the wavelengths that corresponded with each color line we observed. This data is located on the data sheets within the lab manual. To determine the energy level (n), one must use the formula E = -RH (1/nf2 – 1/ni2) where E = hc/. The energy emitted by the hydrogen atom compared to the other atoms tested, was very similar. All of the atoms tested had emitted energy between approximately 3.0x10-19J and 5.0x10-19 J.
Calculations and