The purpose for this experiment is to observe the emission of spectra from several atoms including hydrogen and helium. Measuring the wavelengths of these emitted spectra will allow us to calculate energies of emitted photons. It is important to note that we will be using the Bohr model of the atom to denote the orbit numbers from which electrons in the sample are relaxing from in hydrogen. This will be important for the conclusions that we will make based upon the calculations using the data collected in the lab. Spectroscopy is the study of how matter and electromagnetic radiation interact with one another. In this experiment, we are observing and recording the emission of photons with wavelengths on the visible light spectrum. To understand
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It is also a large part of spectroscopy to relate a wave’s wavelength (ʎ), frequency (υ), and energy (E). Unlike our calculations described in the previous paragraph, these relations are true of any electromagnetic radiation, and therefore the release of any photons from a sample of any excited atom. To determine the frequencies of energy associated with all of our observed spectra, the following frequency equation can be used: υ= c/λ
C=Speed of light (3.00×〖10〗^8)
We can also determine the energy for the emitted photon using the wavelength or the frequency. In this experiment I chose to calculate the energy after I had calculated the frequency.
E=hc/λ or E=hυ
C=Speed of light (3.00×〖10〗^8) h=Plank^' s Constant …show more content…
It is also an important part of the study of chemistry as it helps us study the nature and properties of matter in its smallest and most basic forms.
The purpose of this experiment was to use spectroscopy to observe and record the visible emission spectra of hydrogen and other samples to determine certain properties of these spectra. In this experiment recorded the spectra of several element samples and found several properties of these spectra using fundamental equations in spectroscopy. I calculated with some degree of certainty the orbital levels from which the electrons moved in hydrogen and came to conclusions about the changes in energy of other
It is also a large part of spectroscopy to relate a wave’s wavelength (ʎ), frequency (υ), and energy (E). Unlike our calculations described in the previous paragraph, these relations are true of any electromagnetic radiation, and therefore the release of any photons from a sample of any excited atom. To determine the frequencies of energy associated with all of our observed spectra, the following frequency equation can be used: υ= c/λ
C=Speed of light (3.00×〖10〗^8)
We can also determine the energy for the emitted photon using the wavelength or the frequency. In this experiment I chose to calculate the energy after I had calculated the frequency.
E=hc/λ or E=hυ
C=Speed of light (3.00×〖10〗^8) h=Plank^' s Constant …show more content…
It is also an important part of the study of chemistry as it helps us study the nature and properties of matter in its smallest and most basic forms.
The purpose of this experiment was to use spectroscopy to observe and record the visible emission spectra of hydrogen and other samples to determine certain properties of these spectra. In this experiment recorded the spectra of several element samples and found several properties of these spectra using fundamental equations in spectroscopy. I calculated with some degree of certainty the orbital levels from which the electrons moved in hydrogen and came to conclusions about the changes in energy of other