Understanding Bohr Theory (Wavelengths for Electron States)

In summary, the conversation discusses the use of Bohr Theory in calculating orbit radius and wavelength for an electron. It is mentioned that the orbit radius is equal to n^2 times a constant, and the wavelength for an electron with l=0 is equal to 2∏r. However, there is confusion about whether n should be squared or not when calculating the orbital radius. The source provided shows that n is not squared in the equation.
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Ok, I am having some trouble with the maths regarding Bohr Theory. I understand that the orbit radius is
r=n^2xa0
where a0=0.0529

and that the wavelength for an electron with l=0 (circular orbit), is
λ=2∏r

so for n=1, λ=6.28a0.

So, following the same maths, for n=2, I get λ=2x∏x2^2=8∏a0.

However, according to http://hyperphysics.phy-astr.gsu.edu/hbase/bohr.html#c5, The answer is 4∏a0, which means that n is not squared.

Can anyone please explain whether or not n is squared to work out the orbital radius?
 
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FAQ: Understanding Bohr Theory (Wavelengths for Electron States)

1. What is Bohr Theory and why is it important?

Bohr Theory is a model proposed by Danish physicist Niels Bohr to explain the atomic structure and behavior of electrons. It is important because it revolutionized our understanding of the atom and laid the foundation for modern quantum mechanics.

2. How does Bohr Theory explain the wavelengths of electron states?

Bohr Theory states that electrons orbit the nucleus in specific energy levels, each with a different energy and distance from the nucleus. When an electron jumps from a higher energy level to a lower one, it emits a photon of light with a specific wavelength corresponding to the energy difference between the levels.

3. Can Bohr Theory accurately predict the wavelengths of all electron states?

No, Bohr Theory is a simplified model and does not accurately predict the wavelengths of all electron states. It only works for atoms with one electron, such as hydrogen, and does not take into account the effects of electron-electron interactions.

4. How does the concept of quantization play a role in Bohr Theory?

Quantization, or the idea that energy is not continuous but exists in discrete packets, is a fundamental aspect of Bohr Theory. It explains why electrons can only exist in specific energy levels and why they cannot exist between levels.

5. What are the limitations of Bohr Theory?

Bohr Theory has several limitations, including its inability to accurately predict the wavelengths of more complex atoms and its failure to fully explain the behavior of electrons. It also does not account for the wave-like nature of electrons, which is better understood through quantum mechanics.

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