Ch 27 HW (Part 2)
The Hydrogen Spectrum
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Part B
What is the wavelength of the line corresponding to n=5 in the Balmer series?
Express your answer in nanometers to three significant figures.
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Part C
What is the smallest wavelength λmin in the Balmer's series?
Express your answer in nanometers to three significant figures.
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Part D
What is the largest wavelength λmax in the Balmer series?
Express your answer in nanometers to three significant figures.
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Part E
What is the smallest value of n for which the wavelength of a Balmer series line is smaller than 400nm, which is the lower limit for wavelengths in the visible spectrum?
Enter your answer as an integer.
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Encouraged by the success of Balmer's formula, other scientists extended the formula by simply changing the 22 term to 12 or 32, or more generally to m2, and verified the existence of the corresponding wavelengths in the hydrogen spectrum. The resulting formula contains two integer quantities, m and n, and it is given by
1λ=R(1m2−1n2),
where R is again the Rydberg constant. For m=2, you can easily verify that the formula gives the Balmer series. For m=1,3,4,5, the formula gives other sets of lines, or series, each one named after its discoverer. Note that for each value of m, n=m+1,m+2,m+3,....
Part F
If m=1, in what range are the wavelengths calculated from the generalized formula shown above?
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If , in what range are the wavelengths calculated from the generalized formula shown above?
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Part G
If m=3, in what range are wavelengths calculated from the generalized formula shown above?
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If , in what range are wavelengths calculated from the generalized formula shown above?
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The Hydrogen Spectrum When a low-pressure gas of hydrogen atoms is placed in a tube
and a large voltage is applied to the end of the tube, the atoms
will emit electromagnetic radiation and visible light can be
observed. If this light passes through a diffraction grating, the
resulting spectrum appears as a pattern of four isolated, sharp
parallel lines, called spectral lines. Each spectral line
corresponds to one specific wavelength that is present in the light
emitted by the source. Such a discrete spectrum is referred to as a
line spectrum. |
The first quantitative description of the hydrogen
spectrum was given by Johann Balmer, a Swiss school teacher, in
1885. By trial and error, he found that the correct wavelength
λ of each line observed in the hydrogen spectrum was given
by
1λ=R(122−1n2), where R is a constant, later called the Rydberg constant, and n may have the integer values 3, 4, 5, .... If λ is in meters, the numerical value of the Rydberg constant (determined from measurements of wavelengths) is R = 1.097×107 m−1 . Balmer knew only the four lines in the visible spectrum of hydrogen. Thus, the original formula was written for a limited set of values of n. However, as more techniques to detect other regions of the spectrum were developed, it became clear that Balmer's formula was valid for all values of n. The entire series of spectral lines predicted by Balmer's formula is now referred to as the Balmer series.Part A What is the wavelength of the line corresponding to n=4 in the Balmer series? Express your answer in nanometers to three significant figures.
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λ(n) = | ||||
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λmin = | ||||
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λmax = | ||||
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n = | ||||
microwave (1 to 10−4m) | ||||
infrared (10−3 to 7×10−7m) | ||||
visible (7×10−7 to 4×10−7m) | ||||
ultraviolet (4×10−7 to 10−8m) | ||||
X rays (10−8 to 10−13m) | ||||
microwave (1 to 10−4m) | ||||
infrared (10−3 to 7×10−7m) | ||||
visible (7×10−7 to 4×10−7m) | ||||
ultraviolet (4×10−7 to 10−8m) | ||||
X rays (10−8 to 10−13m) | ||||
Ch 27 HW (Part 2) The Hydrogen Spectrum « previous 5 of 19 next » SubmitMy...
this kinda of a long question, but all parts are connected. so, please explain ! The first quantitative description of the hydrogen spectrum was given by Johann Balmer, a Swiss school teacher, in 1885. By trial and error, he found that the correct wavelength ? of each line observed in the hydrogen spectrum was given by 1?=R(122?1n2), where R is a constant, later called the Rydberg constant, and n may have the integer values 3, 4, 5, .... If ?...
4 Item 4 Learning Goal: To calculate the wavelengths of the lines in the hydrogen emission spectrum Atoms give off light when heated or otherwise excited! The light emitted by excited atoms consists of only a few wavelengths, rather than a full rainbow of colors. When this light is passed through a prism, the result is a series of discrete lines separated by blank areas. The visible lines in the series of the hydrogen spectrum are caused by emission of...
The hydrogen spectrum shows 4 lines in the region visible spectral (this series is called the Balmer series: Hα (red): λ= 656.3 nm, Hβ (blue-green): λ = 481.1 nm, Hγ (purple): λ = 434.1 nm, and Hλ (purple): λ = 410.2 nm). Another series in the hydrogen spectrum is the Lyman series. Determine the wavelength of the second line of the Lyman series in m and nm (give two digits after the decimal point).
Problem 8: Consider the Balmer series of spectral lines in the hydrogen atom. Part (a) What is the smallest-wavelength line, in nanometers, in the Balmer series? Numeric : A numeric value is expected and not an expression. Amin Part (b) Which part of the electromagnetic spectrum is this photon? MultipleChoice: 1) Gamma ray 2) Infrared 3) X-ray 4) Visible 5) Ultraviolet
+ The Rydberg Equation An astrophysicist working at an observatory is interested in finding clouds of hydrogen in the galaxy. Usually hydrogen is detected by looking for the Balmer series of spectral lines in the visible spectrum. Unfortunately, the instrument that detects hydrogen emission spectra at this particular observatory is not working very well and only detects spectra in the infrared region of electromagnetic radiation. Therefore the astrophysicist decides to check for hydrogen by looking at the Paschen series, which...
Electronically excited hydrogen emits in the visible part of the spectrum in a series of lines known as the Balmer series. Each of these transitions terminates in the n=2 level of hydrogen. What is the energy and wavelength and upper state quantum number for the first four of these transitions starting with the longest wavelength emission?
Use the following information to answer the next question. The following diagram represents the emission lines that are produced for the Balmer Series of hydrogen. Each line is produced as an electron makes a transition from a higher Bohr energy level to n-2. Balmer Series Spectral Line Wavelengths IT I 300 nm 400 nm 500 nm 600 mm 700 nm 8. The regions of the electromagnetic spectrum into which the lines of the Balmer Series of hydrogen are classified are...
.019 1. When Johann Balmer found his famous series for hydrogen in wavelengths in the visible and near ultraviolet regions from series lie in that region. On the basis of the entries in Table 11.3 and me diagram, what common characteristic do the lines in the Balmer sein Print Preview ous series for hydrogen in 1886, he was limited experimentally to car ultraviolet regions from 250 nm to 700 nm, so all the lines in his entries in Table 11.3...
- White light spectrum – a. How does the spectrum of white light differ from the spectrum of hydrogen, neon and sodium? b. What color corresponds to 5.7 x 10-7 meters? _____________________________ - Hydrogen Emission Spectrum – There are several lines with colors and 3 lines which are white. The white lines are in the infrared region and not visible. a. Which line in the visible spectrum has the longest wavelength and lowest energy? ______________________ b. Figure 6.1 in the lab manual represents the Balmer...
please answer all 5, thanks:) attributed to stray light or impurities in the discharge lube.) Data Analysis 1. Using the scale position reading for the hydroxen snectrum and the equation generated from your calibration curve, calculate the wavelengths (in A) for each of the four lines in the hydrogen spectrum. Compare these calculated values with the reported values. Look up the four lines that are visible in the atomic spectrum of hydrogen (Be sure to provide a reference or URL)....