An ionic bond.
Lead dioxide (PbO2) is typically a dark brown or black color.
PbO2 is lead(IV) oxide.
Lead Dioxide or Lead IV Oxide
PbO2 is a stronger oxidizing agent compared to PbO because PbO2 has a higher oxidation state of +4 for lead, allowing it to accept more electrons during a redox reaction. This makes PbO2 more likely to cause other substances to be oxidized.
2PbS + 3O2 ----> 2PbO + 2SO2
The product for the reaction between PbO2 and O2 is PbO2.
The traditional name for PbO2 is lead dioxide.
PbO2 is lead(IV) oxide.
Lead dioxide (PbO2) is typically a dark brown or black color.
Lead Dioxide or Lead IV Oxide
PbO2 is a stronger oxidizing agent compared to PbO because PbO2 has a higher oxidation state of +4 for lead, allowing it to accept more electrons during a redox reaction. This makes PbO2 more likely to cause other substances to be oxidized.
2PbS + 3O2 ----> 2PbO + 2SO2
The formula for plumbous oxide is PbO.
The chemical equation 2 PbO2 → 2 PbO + O2 represents a decomposition reaction. In this reaction, lead(IV) oxide (PbO2) breaks down into lead(II) oxide (PbO) and oxygen gas (O2). Decomposition reactions typically involve a single compound breaking down into two or more products.
The balanced chemical equation for the given reaction is: PbO2 + PbO -> 2PbO + O2 Coefficients: 1 PbO2, 1 PbO, 2 PbO, 1 O2.
The ionic chemical formula of lead(IV) oxide is: (Pb)4+ + 2 O-.
PbO2 is an ionic compound composed of lead (Pb) and oxide ions (O2-) bound together by ionic bonds.