one reason for transition metal to form complexes is that it has some vacant d-orbitals
but i wonder how this can really help the formation of complexes
as in a complex, electrons are donated by ligands to stabilize the positive charge of metal cation
there is just no need to promote...
Plz comment on my way of thinking:
Fe2+ is more stable than Fe3+ in aqueous solution because of the more -ve hydration energy of Fe2+
so in what situation will Fe3+ be more stable than Fe2+??
In terms of electronic structure, Fe3+ is more stable than Fe2+ because it has a half filled d-orbital which gives extra stability.
i.e. Fe3+ : [Ar]3d5
Fe2+ : [Ar]3d6
But the standard electrode potential of the following reaction is 0.77V,
Fe3+(aq) + e- => Fe2+(aq)
which means...
well the web says the +ve charge should spread over the whole of the complex, so that means in no way can i know the charge on a specific atom?
also, how can i know when the charge will spread over and when it won't? just like the example quoted from the website, the positive charge will just...
does an atom necessarily becomes +1 charged after forming a dative covalent bond with another atom?
just like something I learned in organic chem:
C6H5-H2N:+ H+ ------> C6H5-H2N+→H
the positive charge of H+ is transferred to the N atom as N forms a dative covalent bond with it...