Where does the electron come from to make a scandium +1 ion?
From which orbital and which shell would the electron be taken to form a scandium +1 ion?
I thought at first the 4s, but then you have one half-full shell and only one electron in the 3d. So, would it come out of the 3d instead?
Answer:
Deborah,
You're right, it comes out of the 3d. The rule about the transition metals of taking from the 4s subshell first is really only valid for columns 5 and up, since this is usually enough electrons to make things like half full or totally full subshells a mute point. Sorry I didn't mention that in my previous answer.
It's true that in this spot in the periodic table, the 4s subshell will have a SLIGHTLY higher energy than the 3d, which is why you normally take from the 4s. But, since Sc has only 3 valence electrons, you can acheive a completely full subshell (the 4s) and a completely empty subshell (the 3d) by simply removing the 3d electron. Completely full or completely empty subshells are given priority if you are close to making them, and then AFTER that are half full subshells.
Dear Deborah,
With these transition elements all the outer electron energies are very similar. Hence the multiple valencies.
The electron comes from the highest energy band which is influenced by the Sc surroundings such as the presence of polar solvents and other molecules.
The electron structure is:
K 2
L 2 6
M 2 6 1
N 2
It is most likely to come from the singleton in the M orbital as being unpaired (spin) it will have a higher energy than the others; and the energy levels of the M and N bands are extremely close together.
With more aggresive electrophilic atoms like Cl the 3d and 4s electrons are stripped giving a trivalent ion.
Best of luck. RufusCat
CopyLeft:RufusCat
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I thought at first the 4s, but then you have one half-full shell and only one electron in the 3d. So, would it come out of the 3d instead?
Answer:
Deborah,
You're right, it comes out of the 3d. The rule about the transition metals of taking from the 4s subshell first is really only valid for columns 5 and up, since this is usually enough electrons to make things like half full or totally full subshells a mute point. Sorry I didn't mention that in my previous answer.
It's true that in this spot in the periodic table, the 4s subshell will have a SLIGHTLY higher energy than the 3d, which is why you normally take from the 4s. But, since Sc has only 3 valence electrons, you can acheive a completely full subshell (the 4s) and a completely empty subshell (the 3d) by simply removing the 3d electron. Completely full or completely empty subshells are given priority if you are close to making them, and then AFTER that are half full subshells.
Dear Deborah,
With these transition elements all the outer electron energies are very similar. Hence the multiple valencies.
The electron comes from the highest energy band which is influenced by the Sc surroundings such as the presence of polar solvents and other molecules.
The electron structure is:
K 2
L 2 6
M 2 6 1
N 2
It is most likely to come from the singleton in the M orbital as being unpaired (spin) it will have a higher energy than the others; and the energy levels of the M and N bands are extremely close together.
With more aggresive electrophilic atoms like Cl the 3d and 4s electrons are stripped giving a trivalent ion.
Best of luck. RufusCat
CopyLeft:RufusCat
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