Three of the known wavelengths of the emission spectrum of helium are 402.6 nm, 447.1 nm and 587.5 nm.If n1 = 2, calculate n2 for these three lines.  Convert from nanometers to meterswhy do these results indicate the electron behavior of atoms of elements with more than one electron is not well described by the Rydberg equation if Bohr's picture of the atom is correct?

Question
Asked Nov 14, 2019
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Three of the known wavelengths of the emission spectrum of helium are 402.6 nm, 447.1 nm and 587.5 nm.

If n1 = 2, calculate n2 for these three lines.  Convert from nanometers to meters

why do these results indicate the electron behavior of atoms of elements with more than one electron is not well described by the Rydberg equation if Bohr's picture of the atom is correct?

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Expert Answer

Step 1

Electromagnetic spectrum involves different radiations from the lowest to the highest frequency values. Some common radiations which are part of electromagnetic radiations are infrared radiation, visible light, ultraviolet radiation, X-rays, and gamma rays.

Step 2

 Convert nm to m

1 m = 109 nm

m
- 402.6 x10 m
100 nm
402.6 nm x
Im
-447.1 x10 m
447.1 nm x
10°nm
m
= 587.5 x10 m
587.5 nm x
10°nm
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m - 402.6 x10 m 100 nm 402.6 nm x Im -447.1 x10 m 447.1 nm x 10°nm m = 587.5 x10 m 587.5 nm x 10°nm

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Step 3

The wavelength of radiation of transition can be calcu...

1
=RgxZ2
H
2
n,
2
RHRydberg constant = 1.097 x 107 m1)
n1 and n2 energy levels (n2 >n)
Z atomic number
help_outline

Image Transcriptionclose

1 =RgxZ2 H 2 n, 2 RHRydberg constant = 1.097 x 107 m1) n1 and n2 energy levels (n2 >n) Z atomic number

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