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Give the Oxidation state for each metal species.
Fe—> Fe(CO)5—>Fe(CO)4I2
Oxidation state, also known as oxidation numbers. This is the charge present on the metal, assuming that all the bonds made by the metal with the ligands are in the form of ionic.
General guidance
A metal’s oxidation state is always positive. You can calculate the oxidation state for a transitional metal by using the oxidation conditions of other elements in the compound.
Transition metals can have different oxidation states.
The number of electrons that were lost or gained by an element during the formation of a compound is called the oxidation state. It can be either positive, negative, or 0.
Step-by-step
Step 1 from 3
(1)
Fe’s oxidation state in Fe is 0. This is because the metal is in its elemental form.
The oxidation state for Fe in Fe is 0.
Hint for next step
All atoms have 0.0 oxidation states in their elemental forms. If all atoms are the same, then electronegativity for all atoms will be equal. The oxidation state therefore is 0.
Find out the oxidation status of Fe using the charge of CO.
Step 2 from 3
(2)
Let the Fe oxidation state be x.
The Fe(CO)5 is the overall charge of the molecule.
x + 5(0) = 0
x = 0
The charge for Fe in fe(CO)5 is therefore justified.
The Fe charge in Fe(CO)5
Hint for next step
CO, a neutral molecule has a charge 0. Substitute it for CO and set the overall charge to 0 in order to calculate the Fe oxidation state.
Find out the oxidation status of Fe using the charge of CO.
Step 3 from 3
(3)
Let Fe(C0)4I2 show the oxidation state for Fe
The Fe(C0)4I2 molecule’s overall charge
x + 4(0) +2 (\u22121) = 0
x = +2
The charge for Fe in Fe(C0)4I2 is +2.
The Fe charge in Fe(C0)4I2 +2
Explanation
CO is a neutral molecule and has a charge 0. The oxidation status of I is -1. These two values can be substituted to calculate the Fe oxidation state.
Answer
The oxidation state for Fe in Fe is 0.
The Fe charge in Fe(CO)5 is 0.
The Fe charge in Fe(C0)4I2 is +2