Wavelength, emission spectrum, electron transitions

In summary, the question is asking for the wavelength, in nanometers, of the line in the emission spectrum of He+ ion produced by a transition from n=3 to n=1. The Rydberg equation was used to calculate the wavelength, but it is important to note that the Rydberg constant for He+ is different than for Hydrogen due to the difference in charge. The correct answer is 25.6nm.
  • #1
FsLiu
21
0

Homework Statement



Determine the wavelength (in nm, to one decimal place) of the line in the emission spectrum of the He+ ion produced by a transition from n = 3 to n = 1.

Homework Equations


I used the Rydberg equation for this, although I'm not sure it is the correct one to use.
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The Attempt at a Solution


Plugging in n1=1 and n2=3, I get an answer of 102.6nm. A search on wikipedia for the Lyman series also shows that transition from n=3 to n=1 is 102.6nm.

The solution given, however, is 25.6nm. Obviously I am not understanding the question. Help would be appreciated.
 
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  • #2
The Rydberg constant will be different for He+ than for hydrogen because He+ has more protons in its nucleus.
 
  • #3
The equation you used is for Hydrogen. The He ion has a charge of +2, so the Rydberg constant is modified. Go back and look up the equation for how this Rydberg constant is derived.
 

FAQ: Wavelength, emission spectrum, electron transitions

1. What is a wavelength?

Wavelength is the distance between two consecutive peaks or troughs of a wave, such as an electromagnetic wave or a sound wave. It is commonly measured in meters, and shorter wavelengths correspond to higher frequencies.

2. What is an emission spectrum?

An emission spectrum is a display of the wavelengths of light emitted by a substance when it is excited by energy, typically in the form of heat or electricity. Each element has a unique emission spectrum, making it a useful tool for identifying unknown substances.

3. How do electron transitions relate to emission spectra?

Electron transitions refer to the movement of electrons from one energy level to another within an atom. When an electron transitions to a lower energy level, it emits a photon of light with a specific wavelength, which contributes to the emission spectrum of the atom.

4. Can emission spectra be used to determine the composition of a substance?

Yes, emission spectra can be used to identify the elements present in a substance. Each element has a unique emission spectrum, so by analyzing the wavelengths of light emitted, scientists can determine the composition of the substance.

5. How is the visible light spectrum related to electron transitions?

The visible light spectrum is a range of wavelengths of light that can be detected by the human eye. This spectrum corresponds to the energy levels involved in electron transitions within atoms. When an electron transitions between these levels, it emits a photon of light with a specific wavelength, which can fall within the visible light spectrum.

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