I need help with the orbital notation and electron configuration for the following atom or ion. Im not very good at them.
Calcium
Arsenic
Fluride,F1-
Mg2+
Ca = 20
1s2 2s2 2p6 3s2 3p6 4s2
F^- = 10
1s2 2s2 2p6
These are filled this way.
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d
7s 7p
8s
Start at the top with an arrow pointed down and to the left like this / with the tip of the arrow at the bottom. Draw that arrow diagonally through the orbitals I have written above. If done correctly, it will go through 1s, the next arrow will go through 2s, the next arrow will go through 2p and 3s, the next arrow will go through 3p and 4s, the next arrow will go through 3d, etc in that order. That will tell you the order of filling. The correct order will be given for the first 38 elements except for Cr and Cu (elements 24 and 29). Cr and Cu have one more 3d and 1 less 4s than the scheme will predict. I will leave As and Mg^+2 for you. But you can go to web elements to check your answers.
Is that the electron configuration or the orbital notation above?
Its the electron configuration.
What do you not understand about the orbital notation?
Nothing...=/
We need to do better than that. I'm sure you understand something about it. I can go through the definitions.
n can be any whole number above zero; i.e., 1,2,3, 4, etc.
l (that's as in "ell") can be any whole number beginning with 0 with additional values of 1, 2, 3, etc but it can be no larger than n-1.
ml = values beginning with -l with whole values up to +l. Later I will call this just m.
ms = two values. One is +1/2 and the other is -1/2. Later I will call this just s.
Therefore, for n=1,
l = 0
m = 0
s = 1/2 for one electron and -1/2 for the other.
for n = 2,
l = 0 or 1
m = 0 and -1, 0, +1
s = +/- 1/2 for each of the 4 m values (to make 8 in the n=2 shell).
Anything about this you want to ask?
Can you give me an example for the orbital notation for another element not listed above?...
I am having a problem understanding your problem. Do you want the orbital notation for all of the electrons, for the valence electrons, for a specific electron, or do you really want the term symbol.
For boron, 5B, the electron configuration is
1s2 2s2 2p1.
Electrons in the n = 1 shell. It's easier to write m for ml and s for ms. (In fact that was the notation when I was in school.)
n=1 (the two 1s electrons)
l=0
m=0
s = +1/2 for 1 electron; -1/2 for the other.
n=2 (the two 2s electrons)
l = 0
m = 0
s = +1/2 for 1 electron; -1/2 for the other.
n=2 (the 1 2p electron)
l = 1
m = -1
s = 1/2
If this doesn't address the question you have, then please be specific about what you don't understand. Otherwise, I'm groping in the dark.