Bright Line Spectrum - Mr. Fischer
Bright Line
Spectrum Lab
Purpose: To identify elements using bright line spectra and to calculate the frequency (ν) for those elements.
Background: Light is composed of different wavelengths and frequencies. These wavelengths represent different colors. The frequency and wavelength are related by the formula ν = c/λ, where ν is the frequency, c is the speed of light, and λ is the wavelength. Each element will emit a specific series of lines. This information has been translated to astrometry to determine which elements are present in stars.
Materials: Gas Tubes
Polarizing Glasses
Spectrum Chart
Electric Source
Procedure: 1. Look at the tubes with glasses on.
2. Draw the colors you see in your lab book next to the element’s name.
3. Compare your drawing to the spectrum chart to find the wavelength.
4. Calculate the frequency (ν) for wavelength. ν = c/λ
λ= wavelength
c= 3.00 x 108 m/sec
Data:
Hg: H2:
N2: Ar:
He: Ne:
Analysis:
Find the Wavelength for :
Hg first pink line:
H first orange line:
Ca first yellow line:
Sr first purple line:
The frequencies for the wavelengths were:
Hg
H
Ca
Sr
What are the electron configurations for:
Ti
Co
N
Al
What are the quantum numbers for:
Ti
Co
N
Al
Conclusion:
What properties of an electron allow us to see different color?
Why were there large spaces of black or absence of color?
For an electron to move to a higher energy level it must energy.
For an electron to move to a lower energy level it must energy.
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