Chapter 26. Rydberg formula for the spectral lines of hydrogen (26-14)

Question

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{"title":"Wavelength of an absorption or emission line in the spectrum of atomic hydrogen","description":"Correct!","type":"correct","color":"#99CCFF","code":"[{\"shape\":\"poly\",\"coords\":\"82,133\"},{\"shape\":\"rect\",\"coords\":\"10,16,12,16\"},{\"shape\":\"poly\",\"coords\":\"144,22\"},{\"shape\":\"rect\",\"coords\":\"5,55,29,91\"}]"} {"title":"n and m are integers: n can be 1, 2, 3, 4, ... and m can be any integer greater than n.","description":"Incorrect","type":"incorrect","color":"#ffff00","code":"[{\"shape\":\"rect\",\"coords\":\"162,61,184,88\"},{\"shape\":\"rect\",\"coords\":\"243,64,276,88\"}]"} {"title":"Rydberg constant = 1.09737 × 10 sup 7 m sup −1","description":"Incorrect","type":"incorrect","color":"#00ff00","code":"[{\"shape\":\"rect\",\"coords\":\"86,22,113,62\"}]"}

Question

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{"title":"Wavelength of an absorption or emission line in the spectrum of atomic hydrogen","description":"Wrong","type":"incorrect","color":"#99CCFF","code":"[{\"shape\":\"poly\",\"coords\":\"82,133\"},{\"shape\":\"rect\",\"coords\":\"10,16,12,16\"},{\"shape\":\"poly\",\"coords\":\"144,22\"},{\"shape\":\"rect\",\"coords\":\"5,55,29,91\"}]"} {"title":"n and m are integers: n can be 1, 2, 3, 4, ... and m can be any integer greater than n.","description":"Correct!","type":"correct","color":"#ffff00","code":"[{\"shape\":\"rect\",\"coords\":\"162,61,184,88\"},{\"shape\":\"rect\",\"coords\":\"243,64,276,88\"}]"} {"title":"Rydberg constant = 1.09737 × 10 sup 7 m sup −1","description":"Incorrect","type":"incorrect","color":"#00ff00","code":"[{\"shape\":\"rect\",\"coords\":\"86,22,113,62\"}]"}

Question

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{"title":"Wavelength of an absorption or emission line in the spectrum of atomic hydrogen","description":"Wrong","type":"incorrect","color":"#99CCFF","code":"[{\"shape\":\"poly\",\"coords\":\"82,133\"},{\"shape\":\"rect\",\"coords\":\"10,16,12,16\"},{\"shape\":\"poly\",\"coords\":\"144,22\"},{\"shape\":\"rect\",\"coords\":\"5,55,29,91\"}]"} {"title":"n and m are integers: n can be 1, 2, 3, 4, ... and m can be any integer greater than n.","description":"Wrong","type":"incorrect","color":"#ffff00","code":"[{\"shape\":\"rect\",\"coords\":\"162,61,184,88\"},{\"shape\":\"rect\",\"coords\":\"243,64,276,88\"}]"} {"title":"Rydberg constant = 1.09737 × 10 sup 7 m sup −1","description":"Correct!","type":"correct","color":"#00ff00","code":"[{\"shape\":\"rect\",\"coords\":\"86,22,113,62\"}]"}

Review

The value of the constant \(R_{\mathrm{H}}\) in Equation 26-14, called the Rydberg constant, is chosen to match the experimental data. To four significant figures, \(R_{\mathrm{H}} = 1.097 \times 10^7\ \mathrm{m}^{-1}\) As an example, the hydrogen absorption and emission lines shown in Figure 26-12 all correspond to \(n =2\) in Equation 26-14. The series of wavelengths for which \(n =2\) are called the Balmer series.