I have a couple question I with atomic physics

[demolition35]

Homework Statement

According to Maxwells laws of electromagnetism:
If an electron spirals into the nucleus:
1. what would happen to the electron’s orbital frequency?
2. what would happen to the frequency of the emitted radiation? and
3. what kind of spectrum would be produced—a continuous or line spectrum? Explain.

2. Homework Equations are:

Angular frequency =

(f is also written with the symbol of speed, v)

Circular motion = [PLAIN]https://upload.wikimedia.org/math/9/d/1/9d1cb34656f4ed9ce94952c445bcaa90.png[/B] 3. The attempt at a solution
I am not sure if these answers are correct but:

1. The electrons orbital frequency would increase because the orbit gets smaller and smaller as the relationship between the frequency and the radius is inversely proportional.
2. The frequency of the emitted frequency will also decrease because according to Maxwell's law of electromagnetism the orbital frequency of a electron will match up with the frequency of the emitted radiation.
3. If an electron spirals into the nucleus, a line spectrum would be produced. This is due to the fact that electron energy is quantized and it needs to release a set amount of energy in order to go down to the previous energy level.

 

[SteamKing]

Homework Equations

are:

Angular frequency =

(f is also written with the symbol of speed, v)[/B]

What appears to be 'v' to you is actually lower case Greek letter 'nu' ( $\nu$ ), which is often used in atomic physics to indicate frequency.

The Planck relation $E = h\nu$ is usually written this way.

 

[demolition35]

Thank you for you help SteamKing

 

[J Hann]

You have a bit of a conflict between your reasoning for (a) and (c).
In (c) you say that the emitted energy is quantized, but if this is the case then
the electron reaches a point where it cannot fall into the nucleus because
it cannot obtain the energy to emit the photon.
Also, if the electron is "spiraling" what does that imply about the emitted radiation?