Please answer 4 questions, it would be great if they are handwritten in order to see the graphs better:) The observations are at the bottom, they were from a spectroscope.
1. Using the emission spectrum results for helium, create a helium calibration graph for your spectrum as seen in the figure below.
2. Use your calibration graph to determine the correct wavelength for the individual bands.
3. Draw the emission line spectra for the hydrogen, fluorescent, and incandescent light sources.
4. Examine your spectrum for hydrogen. Using your knowledge of energy levels and the formulas provided below, calculate which electron transitions cause the lines in the visible spectrum (i.e. Balmer Series). Show your work.
Discussion:
1. Using the emission spectrum results for helium, create a Helium Calibration graph for your spectroscope as seen in the figure below. [5 marks; 1]
Helium Calibration Graph
$5 65 7.5
Wavelength for the individual bands. [5 marks; 1]
Draw the emission line spectra for the hydrogen, fluorescent, and incandescent light sources. [6 marks; 1]
Examine your spectrum for hydrogen. Using your knowledge of energy levels and the formulas provided below, calculate which electron transitions cause the lines in the visible spectrum (i.e. Balmer Series). Show your work. [5 marks; 1]
Useful equation NB: You may not need to use these relationships.
Equation 1: Energy of the first energy level Energy of subsequent energy levels Ers = 13.6 eV
ΔE = hc/λ
E = hv
E = Ei - Ef
c = 3.00 x 10^8 m/s, h = 6.63 x 10^-34, 4.14 x 10^-15 eVs, 1.602 x 10^-19 = 1eV
Equation 2: Rydberg Equation
R = 109678 cm
Fluorescent: violet - 435, green - 535, red - 605, orange - 575
Hydrogen Light: green - 475, red - 645