ok so this is what ive got:
An electrically excited hydrogen atom has its electron in a 5f subshell. the electron drops down to the 3d subshell, releasing a photon in the process.
Give n and l quantum numbers for both subshells, and give the range of possible m1 quantum numbers.
wha tis the wavelength of light emitted by this process?
the hydrogen atom now has a single electron in the 3d subsell. what is the energy (in kj/mol) required to remove this atom?
if you could point me in the right direction i'd be grateful. is this something i have to use the rydberg equation for?
the n numbers are 5, and 3, which are just the numbers in front of your shells. the l quantum numbers are always 0 to n-1, so
where n=5, l= 0 to 5-1, or 0,1,2,3,4
where n=3 l= 0 to 3-1 or 0,1,2
the m
l are -l to +l
so we have
l=1, -1, 0, 1
l=2, -2;-1,0,1,-1
l=3, -3, -2, -1, 0,1, 2, 3
l=4 and so on
l=5 and so on
remember that you have to make these "big" charts under both n=3, and n=5,
You should also know that the "n" numbers denote the energy, the l numbers denote the shape, and the m
l numbers denote the orientation i.e. along the x,y,z axis.
If you don't understand some of this stuff, don't fret, this is a basic introduction into quantum theory and alot of people have difficulties with it. Just don't make it to complicating, it really isn't.