2014 Edge Question
"Brett Hall [email protected] [Fabric-of-Reality]" <[email protected]> Tue, 24 Jun 2014 17:43:25 +1000
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Hello,
It takes a while to reorganise one's text book knowledge of quantum=
physics in a way that makes sense in light of the multiverse. I read FoR y=
ears ago many times and I've lost count of the number of times I've read Bo=
I. BoI has a great explanation of what electrons really are as multiversal =
objects. But I'm still confused.
In David's 2014 Edge Question response he=
writes that the following is a misconception: "when an electron in a highe=
r-energy state undergoes a transition to a lower energy level, emitting a p=
hoton, it quantum-jumps from one discrete orbit to another without passing =
through intermediate states".
And he writes a response to this that says: =
"The truth is that the electron in such situations does not have a single e=
nergy, or position, but a range of energies and positions, and the allowed =
range itself can change with time...if an electron in an atom really were a=
t a discrete energy level, and nothing intervened to change that, then it w=
ould never make a transition to any other energy."
This makes sense in ter=
ms of what BoI says but then I do not understand stuff like emission spectr=
a. For example: if there are a range of energies then why is it that the 21=
cm Hydrogen line is *always* 21cm for that particular "transition" rather t=
han a range of wavelengths?
To expand on my misconception:
When an electr=
on changes its (range of?) energies from a higher to a lower state, it emit=
s a photon. But that *photon* has a single energy, doesn't it? An energy gi=
ven precisely by E =3D hf?
The common way of communicating this idea (I am =
thinking typical text books which I know are replete with error in this reg=
ard, clearly) - is that the electron occupies some orbital where it has pot=
ential energy E1 and later it comes to be in orbital of energy E2 and those=
two orbitals differ in energy matched precisely by the energy of the photo=
n emitted (or absorbed, as the case may be).
Now if this matching is so p=
recise, then how is there energy available for the electron to move (and so=
gain kinetic energy) from one orbital to another?
Some misconceptions I a=
m sure I have that will help resolve this:
Electrons in atomic orbitals do=
n't have discrete energies - okay. They have a range of energies. They are =
multiversal objects like an ink-blot spread out in spacetime. But then I do=
n't understand why electrons that move from one orbital to another (say mak=
ing the transition from first excited state to ground state around a hydrog=
en nucleus) *always* result in the production of exactly the same energy ph=
oton (in the case of the H atom ground to first excited state that's exactl=
y a photon of 21cm wavelength - as described here: http://hyperphysics.phy-=
astr.gsu.edu/hbase/hyde.html ).
Any help, because I am confused. Any furth=
er reading I should do might also be useful.
Thankyou!
Brett
>
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<p><div>Hello,</div><div><br></div><div>It takes a while to reorganise one's text book knowledge of quantum physics in a way that makes sense in light of the multiverse. I read FoR years ago many times and I've lost count of the number of times I've read BoI. BoI has a great explanation of what electrons really are as multiversal objects. But I'm still confused.</div><div><br></div><div><span>In David's 2014 Edge Question response he writes that the following is a misconception: "</span><span>when an electron in a higher-energy state undergoes a transition to a lower energy level, emitting a photon, it quantum-jumps from one discrete orbit to another without passing through intermediate states".</span></div><div><span><br></span></div><div><span>And he writes a response to this that
says: "</span><span>The truth is that the electron in such situations does not have a single energy, or position, but a range of energies and positions, and the allowed range itself can change with time...if an electron in an atom really were at a discrete energy level, and nothing intervened to change that, then it would never make a transition to any other energy."</span></div><div><span><br></span></div><div><span>This makes sense in terms of what BoI says but then I do not understand stuff like emission spectra. For example: if there are a range of energies then why is it that the 21cm Hydrogen line is *always* 21cm for that particular "transition" rather than a range of wavelengths?</span></div><div><span><br></span></div><div>To expand on my misconception:</div><div><span><br></spa
n></div><div><span>When an electron changes its (range of?) energies from a higher to a lower state, it emits a photon. But that *photon* has a single energy, doesn't it? An energy given precisely by E = hf?</span></div><div><span>The common way of communicating this idea (I am thinking typical text books which I know are replete with error in this regard, clearly) - is that the electron occupies some orbital where it has potential energy E1 and later it comes to be in orbital of energy E2 and those two orbitals differ in energy matched precisely by the energy of the photon emitted (or absorbed, as the case may be). </span></div><div><span><br></span></div><div><span>Now if this matching is so precise, then how is there energy available for the electron to move (and so gain kinetic
energy) from one orbital to another?</span></div><div><span><br></span></div><div><span>Some misconceptions I am sure I have that will help resolve this:</span></div><div><span><br></span></div><div><span>Electrons in atomic orbitals don't have discrete energies - okay. They have a range of energies. They are multiversal objects like an ink-blot spread out in spacetime. But then I don't understand why electrons that move from one orbital to another (say making the transition from first excited state to ground state around a hydrogen nucleus) *always* result in the production of exactly the same energy photon (in the case of the H atom ground to first excited state that's exactly a photon of 21cm wavelength - as described here: </span><a href="http://hyperphysics.phy-astr.gsu.edu/hba
se/hyde.html">http://hyperphysics.phy-astr.gsu.edu/hbase/hyde.html</a> ).</div><div><br></div><div>Any help, because I am confused. Any further reading I should do might also be useful.</div><div><br></div><div>Thankyou!</div><div><br></div><div>Brett</div><blockquote type="cite"><div><div style="color: #fff;height: 0;"></div>
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