Can anyone tell me how to calculate the known orbital wavelengths of the
Bohr Hydrogen atom whe [N1] = 9.12x10^-8 m, [N2] = 3.65x10^-7 m, etc.
using the de Broglie wavelength equation of current Quantum Mechanics
whe

wavelength of moving particle = Plank's constant / mass x orbital
velocity.

Thanks in advance.

Jeff

Jeff Lee wrote:

Can anyone tell me how to calculate the known orbital wavelengths

What do you mean by "orbital wavelengths"?


of the Bohr Hydrogen atom whe [N1] = 9.12x10^-8 m, [N2] = 3.65x10^-7
m, etc.

What are [N1] and [N2]?


using the de Broglie wavelength equation of current Quantum
Mechanics whe

wavelength of moving particle = Plank's constant / mass x orbital
velocity.

There is no such thing as "orbital velocity". Electrons don't move
on "orbits" in the atom. Or do you mean something like the square
root of the expectation value of velocity squared? (in other words,
the standard deviation of velocity, because the expectation value
for the velocity itself is zero).


Bye,
Bjoern

Don't post in HTML. It makes a mess of replying in-line.
The Bohr model of the hydrogen atom died a death about seventy or eighty years ago.
Learn to understand the solution to the Schrodinger equation for the Hydrogen atom instead.

Franz Heymann

"Jeff Lee" wrote in message ...
Can anyone tell me how to calculate the known orbital wavelengths of the Bohr Hydrogen atom whe [N1] = 9.12x10^-8 m, [N2] = 3.65x10^-7 m, etc. using the de Broglie wavelength equation of current Quantum Mechanics whe
wavelength of moving particle = Plank's constant / mass x orbital velocity.

Thanks in advance.

Jeff

In article , Jeff Lee wrote:
-=-=-=-=-=-

Can anyone tell me how to calculate the known orbital wavelengths of the
Bohr Hydrogen atom whe [N1] = 9.12x10^-8 m, [N2] = 3.65x10^-7 m, etc.
using the de Broglie wavelength equation of current Quantum Mechanics
whe

wavelength of moving particle = Plank's constant / mass x orbital
velocity.

Thanks in advance.

As has been said, the Bohr atom is an historical footnote and the
electrons in an atom don't really have a velocity. But it's a perfectly
good question in the context of Bohr's model of the atom.

If the atom were treated as a classical system, the orbit of the electron
would be determined the same way as the orbit of a planet about the Sun.
Assume a circular orbit, and

F = ma = mv^2/r = -kqQ/r^2

for some nuclear charge Q, electron charge q, electron mass m, assuming
the mass of the nucleus is much greater than the mass of the electron and
it's a hydrogen-like atom -- one electron, regardless of nuclear charge.
And not really ignoring the problem of radiation, since that's what Bohr
was trying to overcome.

Bohr added the quantization of angular momentum, L=nh. Or n*hbar,
something like that. L is angular momentum, L=mvr. That constrains the
velocities of the electron, hence constrains the orbits. Bohr
hypothesized there would be no radiation for those angular momenta.

Determining a wavelength involves some simple algebra to find v_n, or the
velocity for a particular orbit n, then plug it into Planck's relation,
which you've given. The other way is to assume one complete wavelength
wraps around the electron's orbit, the find r_n, and the wavelength is
equal to the circumference.
--
"When the fool walks through the street, in his lack of understanding he
calls everything foolish." -- Ecclesiastes 10:3, New American Bible

Bjoern Feuerbacher wrote:

Jeff Lee wrote:

Can anyone tell me how to calculate the known orbital wavelengths

What do you mean by "orbital wavelengths"?

of the Bohr Hydrogen atom whe [N1] = 9.12x10^-8 m, [N2] = 3.65x10^-7
m, etc.

What are [N1] and [N2]?

using the de Broglie wavelength equation of current Quantum
Mechanics whe

wavelength of moving particle = Plank's constant / mass x orbital
velocity.

There is no such thing as "orbital velocity". Electrons don't move
on "orbits" in the atom. Or do you mean something like the square
root of the expectation value of velocity squared? (in other words,
the standard deviation of velocity, because the expectation value
for the velocity itself is zero).

Bye,
Bjoern


Bjoern,

Since you don't know what [N1] and [N2] are (notations for the electron
orbits) then I can see why you don't know about electron velocity. What does
the electron do when it spins around the atom, I mean how does it move around
the nucleus if it has no velocity?

all the best,

Jeff

Sorry dude, I remember you from before. You weren't worth answering then
and from your reply I can see by your obvious lack of knowledge that
you're really not worth answering now.

all the best,

Jeff


Franz Heymann wrote:

Don't post in HTML. It makes a mess of replying in-line.The Bohr
model of the hydrogen atom died a death about seventy or eighty years
ago.Learn to understand the solution to the Schrodinger equation for
the Hydrogen atom instead. Franz Heymann

"Jeff Lee" wrote in message
anyone tell me how to
calculate the known orbital wavelengths of the Bohr Hydrogen
atom whe [N1] = 9.12x10^-8 m, [N2] = 3.65x10^-7 m, etc.
using the de Broglie wavelength equation of current Quantum
Mechanics whe

wavelength of moving particle = Plank's constant / mass x
orbital velocity.

Thanks in advance.

Jeff

"Gregory L. Hansen" wrote:

In article , Jeff Lee wrote:
-=-=-=-=-=-

Can anyone tell me how to calculate the known orbital wavelengths of the
Bohr Hydrogen atom whe [N1] = 9.12x10^-8 m, [N2] = 3.65x10^-7 m, etc.
using the de Broglie wavelength equation of current Quantum Mechanics
whe

wavelength of moving particle = Plank's constant / mass x orbital
velocity.

Thanks in advance.

As has been said, the Bohr atom is an historical footnote and the
electrons in an atom don't really have a velocity. But it's a perfectly
good question in the context of Bohr's model of the atom.

If the atom were treated as a classical system, the orbit of the electron
would be determined the same way as the orbit of a planet about the Sun.
Assume a circular orbit, and

F = ma = mv^2/r = -kqQ/r^2

for some nuclear charge Q, electron charge q, electron mass m, assuming
the mass of the nucleus is much greater than the mass of the electron and
it's a hydrogen-like atom -- one electron, regardless of nuclear charge.
And not really ignoring the problem of radiation, since that's what Bohr
was trying to overcome.

Bohr added the quantization of angular momentum, L=nh. Or n*hbar,
something like that. L is angular momentum, L=mvr. That constrains the
velocities of the electron, hence constrains the orbits. Bohr
hypothesized there would be no radiation for those angular momenta.

Determining a wavelength involves some simple algebra to find v_n, or the
velocity for a particular orbit n, then plug it into Planck's relation,
which you've given. The other way is to assume one complete wavelength
wraps around the electron's orbit, the find r_n, and the wavelength is
equal to the circumference.
--
"When the fool walks through the street, in his lack of understanding he
calls everything foolish." -- Ecclesiastes 10:3, New American Bible


Gregory,

Thanks for your reply. What if we take the de Broglie wavelength equation:

wavelength of moving particle = Plank's constant / mass x velocity,

instead of using the electron's mass we divide the orbital energy of the [N1]
orbit: 13.6 ev by "c^2", to obtain the "mass loss" from the electron used to form
the orbit to be: 2.42x10^-35 kg.. We now take the orbital velocity of [N1] which
is 2.1885x10^6 m/sec. and plug it into the Fitzgerald Formula, and then multiply
this result by "c" to get a "Photon Spin Velocity" within the particle (electron)
to be: 299,992,017 m/sec. (since according to this way of thinking subatomic
particles (electrons, etc.) are made up of "photon spin" that slows it's rate of
spin at the same rate time dilation occurs, as orbital velocity increases) such
that:

wavelength of moving electron = h / 2.42x10^-35 kg. x 299,992,017 m/sec.

= 9.12x10^-8 meters = [N1]
wavelength

Now, ain't that one hell of a coincidence? What's even weirder is that it works
for all of the electron orbits of the atom. LOOK OUT academia - BOHR's back!
All comments and opinions appreciated. Thanks.

All the best,

JLee CENTER FOR REALITY PHYSICS

"Jeff Lee" wrote in message
...
Bjoern Feuerbacher wrote:

Jeff Lee wrote:

Can anyone tell me how to calculate the known orbital wavelengths

What do you mean by "orbital wavelengths"?

of the Bohr Hydrogen atom whe [N1] = 9.12x10^-8 m, [N2] =
3.65x10^-7
m, etc.

What are [N1] and [N2]?

using the de Broglie wavelength equation of current Quantum
Mechanics whe

wavelength of moving particle = Plank's constant / mass x orbital
velocity.

There is no such thing as "orbital velocity". Electrons don't move
on "orbits" in the atom. Or do you mean something like the square
root of the expectation value of velocity squared? (in other words,
the standard deviation of velocity, because the expectation value
for the velocity itself is zero).

Bye,
Bjoern


Bjoern,

Since you don't know what [N1] and [N2] are (notations for the electron
orbits) then I can see why you don't know about electron velocity. What
does
the electron do when it spins around the atom, I mean how does it move
around
the nucleus if it has no velocity?

The notation does not occur in any of my texts on atomic physics.
There are no "electron orbits" in a hydrogen atom.
What experimental evidence can you cite to the effect that the electron does
in fact move around the nucleus?
The stationary states of the electron in, for instance, a hydrogen atom, are
eigenstates of energy, but not of velocity.

Franz Heymann

"Jeff Lee" wrote in message ...
Sorry dude, I remember you from before. You weren't worth answering then and from your reply I can see by your obvious lack of knowledge that you're really not worth answering now.

You have also now buggered the attribution marks.
You have neen waffling for so many years now that you could surely have learnt "how" to post, even if you don't know "what" to post.

You won't be hearing from me until you fix your posting style

Franz


Franz Heymann wrote:

Don't post in HTML. It makes a mess of replying in-line.The Bohr model of the hydrogen atom died a death about seventy or eighty years ago.Learn to understand the solution to the Schrodinger equation for the Hydrogen atom instead. Franz Heymann
"Jeff Lee" wrote in message anyone tell me how to calculate the known orbital wavelengths of the Bohr Hydrogen atom whe [N1] = 9.12x10^-8 m, [N2] = 3.65x10^-7 m, etc. using the de Broglie wavelength equation of current Quantum Mechanics whe
wavelength of moving particle = Plank's constant / mass x orbital velocity.

Thanks in advance.

Jeff

If I thought you had the intelligence to understand it I would refer you
to the post I just made to Mr. Hanson where it has been found that it IS
possible to calculate the electron orbital wavelengths with the de
Broglie equation, if you use the right physics. But since you obviously
don't - well, all the best.

Jeff


Franz Heymann wrote:



"Jeff Lee" wrote in message
dude, I remember you
from before. You weren't worth answering then and from your
reply I can see by your obvious lack of knowledge that
you're really not worth answering now. You have also now
buggered the attribution marks.You have neen waffling for so
many years now that you could surely have learnt "how" to
post, even if you don't know "what" to post. You won't be
hearing from me until you fix your posting
style Franz

Franz Heymann wrote:

Don't post in HTML. It makes a mess of replying
in-line.The Bohr model of the hydrogen atom died a death
about seventy or eighty years ago.Learn to understand the
solution to the Schrodinger equation for the Hydrogen atom
instead. Franz Heymann

"Jeff Lee" wrote in message
anyone tell
me how to calculate the known orbital
wavelengths of the Bohr Hydrogen atom whe
[N1] = 9.12x10^-8 m, [N2] = 3.65x10^-7 m, etc.
using the de Broglie wavelength equation of
current Quantum Mechanics whe

wavelength of moving particle = Plank's constant
/ mass x orbital velocity.

Thanks in advance.

Jeff