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Can someone explain me what this means? I have never seen this before😱
Thanks!
Thanks!
nice thats pretty good to know...what about the s subshell, since its spherical, the middle is still the nodal plane and you wont find electrons there either??
so it corresponds to the subshell (l), where l=0=s, l=1=p ??? I am having hard time picturing what you are saying.nah, since s orbital is a sphere and there's no gaps like p or d orbitals, so chance of finding an electron within the s orbital is pretty evenly distributed.
There's no node in the s orbital.
For the DAT purposes, I think knowing s = no nodal plane, p = 1 nodal plane, d = 2 nodal planes are good enough.
so it corresponds to the subshell (l), where l=0=s, l=1=p ??? I am having hard time picturing what you are saying.
yes it does.
In general, angular momentum Quantum number = # of nodal planes.
like l=1=p, so ml=-1,0,1 so you will have 3 nodal planes because you have the Px, Py, and Pz???
you have 1 node for each px, py, pz but there are 3 planes where you can have the node. In the x, y, z plane. Imagine the p orbitals being in those 3 different planes, you can only have 1 node per orbital.
so since 2s has l = 0...it has 0 nodal plane?yes it does.
In general, angular momentum Quantum number = # of nodal planes.
so since 2s has l = 0...it has 0 nodal plane?
o i see what you are saying, so if you are looking lets say at a coordinate plane with x,y, z those planes of the p orbital will overlap basically at the origin (0,0,0) correct?? and at that origin you have the nodal plane where the chances of having an electron are zero...
I wish I have a scanner. kk There's no overlap at the node since node means you don't overlap, sort of.
I think you understand that I have said but just saying it wrong.
http://www.chemistry.wustl.edu/~edudev/Orbitals/movie.html
Note how where there's a gap, that's the nodal plane~~