Naked Science Forum

Non Life Sciences => Chemistry => Topic started by: Richard777 on 21/02/2019 20:20:31

Title: Can an electron have two orbital directions?
Post by: Richard777 on 21/02/2019 20:20:31

The quantum numbers are associated with physical properties of an electron.
Four quantum numbers (n, l, m_L, m_s) are well defined in the literature;

n is associated with electron distance from the nucleus
l is associated with angular momentum
m_L is magnetic moment associated with angular momentum
m_s is magnetic moment associated with spin; m_s = ±½  (spin up, spin down)

The magnitude of angular momentum (L_L) is quantized by the rule; L_L = ђsqr.root[l(l +1)]
Where;   ђ is the reduced Plank constant

There is also a fifth quantum number (s) representing the “spin momentum” of an electron; s = ½
The fifth quantum number is usually omitted, because it is constant for all leptons (including electrons).
The magnitude of spin momentum (L_S) is quantized by the rule; L_S = ђsqr.root[s(s+1)]
The magnetic moment of spin (m_s) permits two “directions of spin motion” (spin up, spin down).

It is reasonable to assume two possible “directions of orbital motion” (say; orbit clockwise, orbit ccw).
Assume a “magnetic moment of orbit” (m_n) permits two “directions of orbital motion”; m_n = ±½
   m_n = +½ represents “clockwise orbit”
   m_n = -½ represents “counter-clockwise orbit”

If “orbital direction” is included, the quantum numbers of an electron may be represented as a “quantum matrix”;

n   l   s
m_n   m_L   m_s

The quantum number for orbital magnetic moment (m_n) may be responsible for the groupings and periods of the Janet Periodic Table (Left Step Periodic Table).

Title: Re: Can an electron have two orbital directions?
Post by: chiralSPO on 21/02/2019 20:46:55

m_l is the closest thing to an "orbit direction"

ie if l = 0 then there is no need to describe a direction
if l = 1 then m_l can be +1 or –1 or 0 (representing each of the axes that the spin could be about)
if l = 2 then m_l can be +2 or +1 or –1 or –2 or 0 (representing each of the pairs axes that the spin could be about) (this one is more of a stretch)

there is no reasonable interpretation of an m_n

Title: Re: Can an electron have two orbital directions?
Post by: Fannie838 on 22/02/2020 06:52:47

Quote from: chiralSPO on 21/02/2019 20:46:55

m_l is the closest thing to an "orbit direction"

ie if l = 0 then there is no need to describe a direction
if l = 1 then m_l can be +1 or –1 or 0 (representing each of the axes that the spin could be about)
if l = 2 then m_l can be +2 or +1 or –1 or –2 or 0 (representing each of the pairs axes that the spin could be about) (this one is more of a stretch)

there is no reasonable interpretation of an m_n

I have not cleared this orbit direction yet.

Title: Re: Can an electron have two orbital directions?
Post by: Colin2B on 22/02/2020 08:31:36

Quote from: Fannie838 on 22/02/2020 06:52:47

I have not cleared this orbit direction yet.

Can you explain what you mean please?

Title: Re: Can an electron have two orbital directions?
Post by: Fannie838 on 23/02/2020 04:47:11

By far I know, an electron has orbital direction but when it comes to two orbital directions I say no because the signs must be opposite to each other and hence they cancel the power in an electron which is definitely wrong. So an electron can never have two orbital directions opposing to each other. By the way your researched is far better than my lines because you have given related examples with it which is good to make it understand to others so thanks for it.