What is the oxidation state of the metal in the complex [FeCl2(H2O)4]*?

To determine the oxidation state of the metal in the complex [FeCl2(H2O)4]*, we start by evaluating the charges of the ligands and the overall charge of the complex. Water (H2O) is a neutral ligand and contributes 0 charge. Chloride ions (Cl-) are negatively charged ligands and each contributes a -1 charge.

In this complex, there are two chloride ions, so their total contribution to the charge is -2. Let’s denote the oxidation state of iron (Fe) as x. The total charge of the complex needs to equal the overall charge of the complex, which is neutral in this case as there is no charge indicated in the asterisk.

Setting up the equation for the overall charge:

x + (2 × -1) + (4 × 0) = 0

x - 2 = 0

Solving for x gives:

x = 2

Thus, the oxidation state of iron in the complex [FeCl2(H2O)4]* is +2. This means that the answer indicating the oxidation state of the metal is appropriate with the value of 2. This oxidation state is commonly encountered in many iron complexes, illustrating a common oxidation