Use the following equation to answer the questions below.
4Fe+3O2—> 2 Fe2 O3
explain how this compound forms in terms of electron transfer. how many electrons are transferred from which atoms are they donated and into which atoms are they accepted
In the given equation, 4Fe (Iron) reacts with 3O2 (Oxygen) to form 2Fe2O3 (Iron(III) oxide).
To understand the electron transfer in this reaction, we need to determine the oxidation state of each element involved.
In Fe2O3, the oxidation state of Iron (Fe) is +3, and the oxidation state of Oxygen (O) is -2.
Initially, Iron (Fe) atoms have an oxidation state of 0 because they are in their elemental form. Oxygen (O) atoms also have an oxidation state of 0 because they are in their diatomic elemental form (O2).
During the reaction, Iron (Fe) atoms will lose electrons and will be oxidized from an oxidation state of 0 to +3. Oxygen (O) atoms will gain electrons and will be reduced from an oxidation state of 0 to -2.
4Fe + 3O2 → 2Fe2O3
In this balanced equation, 4 Fe atoms lose a total of 12 electrons (4 Fe x 3 electrons/Fe = 12 electrons) and are oxidized to an oxidation state of +3. These electrons are donated by the Iron atoms.
The 3 O2 molecules gain a total of 12 electrons (3 O2 x 4 electrons/O2 = 12 electrons) and are reduced to an oxidation state of -2. These electrons are accepted by the Oxygen atoms.
Overall, the reaction involves the transfer of 12 electrons from the Iron atoms (donor) to the Oxygen atoms (acceptor) in order to achieve the formation of the compound Fe2O3.