2013 Blinded By the Light Abstract: In this experiment we were provided a cereal box spectrometer to observe the emission lines of noble gases and hydrogen. Based on the scale readings on the spectrometer and the Balmer-Rydberg formula‚ their wavelengths and percent error were able to be extrapolated. Based on the literature values‚ the cereal box spectrometer proved its value as a decently accurate spectrometer. Introduction: Every element and subsequent atom associated emits light; also know
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through the simulation. • To be determine how to calculate the wavelength of light‚ the work function of the metal‚ or the stopping potential‚ if given the other two. Beginning with the plate made of sodium. Keep all the parameters constant except for the colour (wavelength) of the light and display all the graphs available. 1. Have the light source turned on at very low intensity and battery set to ZERO volts. Vary the wavelength of the light source (from Infra Red to Ultra Violet) until electrons
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Give the color and wavelength value of the five brightest lines in the spectrum. This line spectrum is extending from the color purple meaning that the purple is first to red meaning that the reddest is the last‚ and a lot of other colors in the line spectrum. The wavelengths and the colors of the five brightest lines are the sentences listed below. 1. Color = Purple‚ wavelength which equals 415 nm. 2. Color = Teal‚ wavelength which equals 490 nm. 3. Color = Green‚ wavelength which equals 550 nm
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Hydrogen Objective The purpose of this lab was to calculate an experimental value for the Rydberg constant and then the ionization energy for the hydrogen atom. These values will be obtained by using a prism spectrograph to measure the wavelength value for a section of the visible line spectrum of atomic hydrogen. Theoretical Background When H+ combines with an electron it forms it’s excited state‚ H. This excited atom will release light with a photon of energy as it goes to
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SPECTROPHOTOMETRY Spectrophotometry is the quantitative measurement of the reflection or transmission properties of a material as a function of wavelength It involves with the use of a spectrophotometer. A spectrophotometer is a photometer that can measure intensity as a function of the light source wavelength. A spectrophotometer is commonly used for the measurement of transmittance or reflectance of solutions‚ transparent or opaque solids‚ such as polished glass‚ or gases. Principles
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varies from chemical to chemical. Also‚ the wavelength determines the color that the fireworks have because the colors change in the electromagnetic spectrum. As observed by my data all of the salt’s wavelengths correspond to the specific color that they burned on the electromagnetic spectrum. For example‚ Copper Chloride burned green when placed on the fire. This corresponds to the color green on the electromagnetic spectrum‚ which is around 525nm wavelength. However‚ this energy was not produced by
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spectra and atomic structure. Experimental Procedure Procedure 1: Observation of Line Spectra by Discharge Tubes Six discharge lamps were selected – argon‚ carbon dioxide‚ helium‚ hydrogen‚ iodine‚ mercury‚ and xenon. Using the spectroscopes‚ the wavelengths‚ or the average of them‚ were recorded. It was important to turn on the discharge tubes for only 10 seconds or less at a time with the spectroscope only approximately one inch from the
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the colors‚ and the wavelength values of the observed lines. 2. Describe the line spectrum of the star. Give the color and wavelength value of the five brightest lines in the spectrum. The line spectrum of the star goes from the colors purple to red. ( Purple being first and Red being last.) The five brightest lines were: 1. Color = Purple wavelength = 415 2. Color = Blue/Green wavelength = 490 3. Color = Green wavelength = 550 4. Color = Yellow wavelength = 585
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gaseous element produces bright light of specific wavelengths rather than a continuous spectrum of colors. This phenomenon ultimately lead to the Neils Bohr model of the atom in 1913. Introduction In the middle of the 19th century‚ Robert Bunsen and Gustav Kichoff observed that gases emit spectral lines specific to each element. This made it possible for the composition of these gases to be analyzed by using a spectroscope to identify the wavelengths of the emitted spectral lines. In 1885‚ Johann
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absorption of different wavelengths of light by Chlorophyll Wavelength (nm) Absorbance of light by chlorophyll (Arbitrary units) Diluted Calculation New Reading (Arbitrary units) Violet 430 2.35 50% 2.35 x 2 3.20 Blue 470 1.09 - - 1.09 Blue-Green 492 0.38 - - 0.38 Green 520 0.77 - - 0.77 Yellow-Green 550 0.85 - - 0.85 Yellow 580 1.43 - - 1.43 Orange 600 0.65 - - 0.65 Red 700 0.16 - - 0.16 Absorption and reflection of light: Different substances absorb different wavelengths of light in differing
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