How are emission line spectra produced?
As stated by Kirchhoff.
How are emission line spectra produced?
At an atomic level
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Sources of continuous, emission, and absorption spectra |
Kirchhoff's Laws
Thus, emission spectra are produced by thin gases in which the atoms do not experience many collisions (because of the low density). The emission lines correspond to photons of discrete energies that are emitted when excited atomic states in the gas make transitions back to lower-lying levels.
A continuum spectrum results when the gas pressures are higher, so that lines are broadened by collisions between the atoms until they are smeared into a continuum. We may view a continuum spectrum as an emission spectrum in which the lines overlap with each other and can no longer be distinguished as individual emission lines. BLACKBODY IS AN EXAMPLE OF CONTINUUM EMISSION (energy at all frequencies).
An absorption spectrum occurs when light passes through a cold, dilute gas and atoms in the gas absorb at characteristic frequencies; since the re-emitted light is unlikely to be emitted in the same direction as the absorbed photon, this gives rise to dark lines (absence of light) in the spectrum.
How are emission line spectra produced? As stated by Kirchhoff. How are emission line spectra produced?...
How are the lines in atomic emission spectra produced? Group of answer choices electrons absorb a specific amount of energy and become excited electrons release a specific amount of energy, moving to a higher energy state electrons release a specific amount of energy, moving to a lower energy state electrons absorb a specific amount of energy, moving to a lower energy state
The characteristic flame test colors of metal ions are due to atomic emission spectra. Discuss the relationship between the absorption and emission of light and the factors responsible for flame test colors. Include quantization of electron energy level and planck's law in your answer
Emission line spectra for various elements are shown in Table 1
and Table 2 shows the wavelengths for various colors. Remember, E =
h*c/?, where E is energy, h = 6.626*10-34 J*s, c =
3.00*108 m/s, ? is the wavelength, and 1 m =
109 nm.
Table 1. Emission Line Spectra of Various Elements
Element
Emission Lines (nm)
H
410.2, 434.1, 486.1, 656.3
He
447.1, 492.1, 501.5, 587.5
Hg
404.7, 435.8, 546.1, 577.0
Na
588.9, 589.5
Mg
487.8, 502.5, 574.1,...
Laboratory questions: Atomic Emission Spectra This sheet has to be returned with your lab report and placed at the annex section A one electron excited ion (not hydrogen) absorbs a green photon: 2 - 542 nm. The electron, initially at the Bohr energy level n=8, moves to the level n = 14 after the photon absorption. Identify this ion (hint: find the Z value).
You obtain spectra for two galaxies and measure the observed wavelength of a hydrogen emission line that has a rest wavelength of 656.3 nm. Here are your results: Galaxy 1: Observed wavelength of hydrogen line is 672.9 nm Galaxy 2: Observed wavelength of hydrogen line is 692.6 nm (a) Calculate the redshift, z, for each of the two galaxies. (b) What is each one’s recessional velocity (in km/s)? (c) Which of these galaxies is farther away from you? (d) How...
QUESTION 96 Consider the four X-ray emission spectra shown here. Which was produced at the highest operating KVp? # of X-Ray Photons A 0 10 20 30 40 50 60 70 80 90 100 110 X-Ray Photon Energy (keV)
How would the absorption and emission spectra of a powdered 1:1 GaP and GaAs physical mixture differ from the spectra that would be seen for a GaP0.5As0.5 solid solution?
I was having trouble with some lab question on atomic emission
spectra.
Also answer the following questions about your observations: Are the lines present in the hydrogen spectrum the same lines predicted by the Bohr model the atom? Which lines, if any, are missing? Why might there be lines missing? Compare the spectral lines from your unknown substance to the other spectra you observed. Based on these comparisons, what is the identity of the unknown substance? Are there any general...
The emission line used for zinc determinations in atomic emissionspectroscopy is 214 nm. If there are 6.00×1010atoms of zinc emitting light in the instrument flame at any giveninstant, what energy (in joules) must the flame continuously supplyto achieve this level of emission? (Answer must be inJoules)
a. Compare the following absorption spectra for an unknown element to the emission spectra for known elements. UNKNOWN ABSORPTION SPECTRA 19 wavelength, A (nm) KNOWN EMISSSION SPECTRA (Na) Sodium (H) Hydrogen (Ca) Calelum (Mg) Magnesium (Ne) Neon b) Identify the unknown element Question 20 (3 points) b. Which type of electromagnetic waves do these lines emit? Format BI U Question 21 (4 points) U 152 282 2p6 352 3p6 4s2 3010 4p6 552 4d10 5p6 4f14 5d10 Question 22 (7...