Final answer:
Titanium in TiO₂ has an oxidation number of +4, and oxygen has an oxidation number of -2. These oxidation states are consistent with the overall neutral charge of the compound and the crystal lattice structure as observed in the coordination numbers of titanium (IV) ions and oxide anions.
Step-by-step explanation:
Oxidation Numbers in Titanium Dioxide (TiO₂)
Assigning the correct oxidation numbers to each type of atom in a chemical compound is crucial for understanding the compound's properties and behavior. In the case of TiO₂, Titanium (IV) oxide, we can determine the oxidation numbers of titanium and oxygen based on a few fundamental rules of oxidation states.
Oxygen generally has an oxidation number of -2, except in peroxides and superoxides. Since TiO₂ is not a peroxide or superoxide, we assign oxygen an oxidation number of -2. Titanium's oxidation number can be calculated based on the fact that the total charge of the compound must equal zero, as it is a neutral compound.
If we designate the oxidation number of titanium as x and the charge of oxygen as -2, we can set up the following equation based on TiO₂:
x + 2(-2) = 0
Solving for x gives us:
x = +4
This means that each titanium atom in TiO₂ has an oxidation number of
+4
. With two oxygen atoms each at an oxidation number of -2, the oxidation states balance each other resulting in a neutral molecule.
The coordination number of a titanium (IV) cation is 6, while the coordination number of the oxide anion is 3. This coordination illustrates the ratio of titanium to oxygen atoms in the crystal lattice, supporting the TiO₂ formula unit.