given the reaction fe + o₂ → fe₂(³⁺)o₃(²⁻), what happens to the oxidation states of these elements? fe o
given the reaction fe + o₂ → fe₂(³⁺)o₃(²⁻), what happens to the oxidation states of these elements? fe o
Answer
Explanation:
Step1: Determine initial oxidation state of Fe
In its elemental form, Fe has an oxidation state of 0.
Step2: Determine final oxidation state of Fe
In $Fe_2^{3 +}O_3^{2 -}$, the sub - script of Fe is 2 and the overall charge of the compound is 0. Let the oxidation state of Fe be $x$. Since the oxidation state of O is - 2 and there are 3 O atoms, we have the equation $2x+3\times(-2)=0$. Solving for $x$ gives $x = + 3$. So the oxidation state of Fe changes from 0 to + 3.
Step3: Determine initial oxidation state of O
In $O_2$, oxygen in its elemental form has an oxidation state of 0.
Step4: Determine final oxidation state of O
In $Fe_2^{3 +}O_3^{2 -}$, the oxidation state of O is - 2. So the oxidation state of O changes from 0 to - 2.
Answer:
The oxidation state of Fe changes from 0 to + 3. The oxidation state of O changes from 0 to - 2.