It is a bit long, please be patient to finish the whole question, THX!~
According to what I have learnt, atoms will donate/accept electrons to form ions, and thus, attain the electronic structures of Group 0 elements.
This enables atoms to form compounds, which is of a lower energy level, and become more stable (things about
圖片參考:http://imgcld.yimg.com/8/n/HA00656648/o/701107140006213873428440.jpg
).
So, I feel a bit puzzled :
For the the atoms of the same element of transition metals/lanthanide/actinides, of course, have the same electronic diagram,
but when they lose electron(s) to form cation, their electronic structures should same as that of Group 0 elements.
Which means that, they can only lose a specific number of electrons to form ions.
However, the truth is that, they can form more than one type of ion, take Molybdenum(atomic number = 42; [Kr] 4d5 5s1) as an example, it can form the following compounds:
MoCl2, MoCl3, MoCl4, MoCl5 and MoCl6
So, since metal and non-metal forms ionic compounds. Then, the compounds above should classified as ionic compounds.
As ion of chlorine is Cl-, so , the cation will be Mo(2+), Mo(3+), Mo(4+), Mo(5+) and Mo(6+) respectively.
And here comes my problem, isn't an ion have a electronic structure of Group 0 element? How can the Mo atom loss 2~6 electrons in different compounds and still attain an electronic structure of Group 0 element.
Is this about oxidation states, octet rule, 18-electron rule, orbitals, ligand field theory, energy level or else?
Can anyone explain these to me? THX a lot a lot!!!
If I have any mistakes/misconceptions, please point them out!!!
THX!!!
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