In which of the following compounds does oxygen have an oxidation number of +2?
- AOF
2
- BNa
2
O - CNaO
2
- DNaO
3
Solution & Step-by-step Explanation
Fluorine is the most electronegative element in the periodic table and always exhibits an oxidation state of −1 in its compounds.
Let's calculate the oxidation state of oxygen (x) in Oxygen Difluoride (OF
2
):
x+2(Oxidation state of F)=0
x+2(−1)=0
x−2=0⟹x=+2
In almost all other standard metal oxides, peroxides, and superoxides (like Na
2
O or NaO
2
), oxygen has a negative oxidation state (such as −2 or −
2
1
) because metals are less electronegative than oxygen. Therefore, oxygen has an oxidation state of +2 only in OF
2
.
Let's calculate the oxidation state of oxygen (x) in Oxygen Difluoride (OF
2
):
x+2(Oxidation state of F)=0
x+2(−1)=0
x−2=0⟹x=+2
In almost all other standard metal oxides, peroxides, and superoxides (like Na
2
O or NaO
2
), oxygen has a negative oxidation state (such as −2 or −
2
1
) because metals are less electronegative than oxygen. Therefore, oxygen has an oxidation state of +2 only in OF
2
.