A level chemistry - ligands, d-block elements and complexes

[yiuscott]

Homework Statement

Draw out the electron configuration of [Fe(H2O)6]3+

The Attempt at a Solution

I did the work, but i am not sure if its correct:

Is the following electron configuration correct for this complex?

[Fe(H2O)6]3+:
[Ar]
4s [ i L ]
3d [ i L l i L l i L l i L l i L ]
The i represents the electrons from the Fe, the L represents the electrons form the H2O.

Thank You.

 

[Invictious]

Seems correct from first glance.

As far as I can deduce, this should be an octahedral complex, so if you want to work out the structure by drawing a Lewis diagram, you should be able to double check.

 

[Blueshift5]

I would like to clarify that the electron configuration for [Fe(H2O)6]3+ is not entirely correct. It should be written as [Ar] 3d5 4s0, indicating that there are 5 electrons in the 3d orbital and 0 electrons in the 4s orbital. The H2O ligands do not contribute any electrons to the complex, they only act as neutral ligands. It is important to remember that the d-block elements, such as Fe, have their highest energy electrons in the d-orbital rather than the s-orbital. Additionally, the +3 charge of the complex indicates that 3 electrons have been removed from the neutral [Fe(H2O)6] complex.