To determine the correct chemical name of the compound represented by the formula [tex]$Ni_2O_3$[/tex], we need to analyze the oxidation states of the elements in the compound.
1. Identify the elements and their common oxidation states:
- Nickel (Ni) can exhibit different oxidation states, commonly +2 and +3.
- Oxygen (O) almost always has an oxidation state of -2.
2. Determine the total oxidation state for the given formula:
- The formula [tex]$Ni_2O_3$[/tex] indicates that there are two nickel atoms and three oxygen atoms in the compound.
3. Calculate the total oxidation state of the oxygen atoms:
- Each oxygen atom has an oxidation state of -2.
- Therefore, for three oxygen atoms: [tex]$3 \times (-2) = -6$[/tex].
4. Balance the total oxidation state:
- In a neutral compound, the sum of the oxidation states of all atoms must be zero.
- Let the oxidation state of Ni be [tex]\( x \)[/tex]. For two Ni atoms, the total oxidation state of nickel will be [tex]\( 2x \)[/tex].
- Form the equation: [tex]\( 2x + (-6) = 0 \)[/tex].
5. Solve for the oxidation state of Nickel:
- [tex]\( 2x - 6 = 0 \)[/tex]
- [tex]\( 2x = 6 \)[/tex]
- [tex]\( x = 3 \)[/tex]
6. Determine the name based on the oxidation state:
- The oxidation state for Ni in this compound is +3.
- Therefore, the chemical name for the compound is nickel(III) oxide.
The correct answer is:
C. nickel(III) oxide
