Answer :
To determine the formula for manganese (IV) oxide, we need to consider the typical oxidation states of the elements involved.
1. Identify the oxidation state of manganese (IV):
- Manganese (IV) indicates that manganese has an oxidation state of +4.
2. Identify the oxidation state of oxygen:
- Oxygen typically has an oxidation state of -2.
3. Combine the ions in a way that the total charge is neutral:
- Let’s denote manganese as [tex]\( \text{Mn}^{4+} \)[/tex]
- Let’s denote oxygen as [tex]\( \text{O}^{2-} \)[/tex]
4. Balance the charges:
- Since manganese has a charge of +4 and oxygen has a charge of -2, we need two oxygen atoms to balance the charge of one manganese atom.
- Therefore, one manganese (IV) ion combines with two oxygen ions to form a neutral compound.
5. Write the formula:
- Since one manganese ion combines with two oxygen ions, the formula for manganese (IV) oxide is [tex]\( \text{MnO}_2 \)[/tex].
Hence, the correct chemical formula for manganese (IV) oxide is:
[tex]\[ \boxed{\text{MnO}_2} \][/tex]
1. Identify the oxidation state of manganese (IV):
- Manganese (IV) indicates that manganese has an oxidation state of +4.
2. Identify the oxidation state of oxygen:
- Oxygen typically has an oxidation state of -2.
3. Combine the ions in a way that the total charge is neutral:
- Let’s denote manganese as [tex]\( \text{Mn}^{4+} \)[/tex]
- Let’s denote oxygen as [tex]\( \text{O}^{2-} \)[/tex]
4. Balance the charges:
- Since manganese has a charge of +4 and oxygen has a charge of -2, we need two oxygen atoms to balance the charge of one manganese atom.
- Therefore, one manganese (IV) ion combines with two oxygen ions to form a neutral compound.
5. Write the formula:
- Since one manganese ion combines with two oxygen ions, the formula for manganese (IV) oxide is [tex]\( \text{MnO}_2 \)[/tex].
Hence, the correct chemical formula for manganese (IV) oxide is:
[tex]\[ \boxed{\text{MnO}_2} \][/tex]
