Why is lead oxide a strong oxidising agent?

PbO2, PbO, SnO2 and SnO. Lead(IV)oxide, (PbO2) is a stronger oxidizing agent than either tin(II)oxide or tin(IV) oxide because it has a higher tendency to be reduced, which means to gain electrons. This makes the 2+ ion of lead (in which only the two 5p electrons are given up) more stable than the 4+ ion.

Is Pb a strong oxidising agent?

Pb4+ compounds are stronger oxidizing agents than Sn4+ compounds. and. STATEMENT-2: The higher oxidation states for the group 14 elements are more stable for the heavier members of the group due to inert pair effect.

Why is PbO2 an oxidizing agent?

Pb has an oxidation state of +4 in PbO2, but Pb+2 is more stable, due to which pb+4 has an innate ability to get converted into Pb+2, thus being able to oxidise others in the reactions.

In which oxidation state of Pb is powerful oxidizing agent?

Due to higher stability of Pb2+, Pb4+ will readily undergo reduction to form Pb2+. Thus, Pb4+ act as a strong oxidising agent.

Which is stronger oxidising agent co2 or PbO2?

As Oxidising agent oxidises other species and itself undergoes reduction therefore, Pb in PbO2 (i.e. +4 Oxidation state ) acts as a strong oxidising agent. …

Why is PbO2 a stronger oxidizing agent than SnO2?

In PbO2 and SnO2, both lead and tin are present in +4-oxidation state. But due to stronger inert pair effect, Pb2+ ions is more stable than Sn2+ ions . Thus, PbO2 acts a stronger oxidising agent than SnO2.

Why PB 4 is a strong oxidising agent?

In p-block elements (14th group here) the lower oxidation state becomes more stable on going down the group due to inert pair effect. This makes Pb+4 a stronger oxidising agent.

Which is stronger oxidizing agent between co2 and PbO2?

As Oxidising agent oxidises other species and itself undergoes reduction therefore, Pb in PbO2 (i.e. +4 Oxidation state ) acts as a strong oxidising agent.

Why SnCl2 is a strong reducing agent?

● SnCl2 acts as reducing agent because – -SnCl2 readily reacts with other compounds & get converted to stable SnCl4. -During the reaction, SnCl2 gets oxidised while other compound is reduced. -Thus, SnCl2 is a good reducing agent.

Why bi5 is stronger oxidising agent than sb5?

Complete answer: (i) Bi has +5 oxidation state and it is a stronger oxidizing agent than Sb because Bi gains electrons from the reducing agent very much faster than the Sb and becomes stable from +5 oxidation state to +3 oxidation state.

Is lead oxidizing or reducing agent?

Hydrogen peroxide is the oxidizing agent and lead(II) sulfite is the reducing agent.

Which is the strongest oxidising agent between CO2 and PbO2?

If you ask between CO2 (Carbon Dioxide) and PbO2 (Lead Oxide ) ,the strongest oxidising agent is PbO2 because Lead is loosely bonded to Oxygen as compared to the Carbon bonding with Oxygen. PbO2 notPB?O2 Why are you asking?? Which bond is most covalent? CO, KF, CH, OH

What is the difference between PbO2 and lead dioxide?

Lead dioxide is the more powerful oxidising agent, as lead is more stable in its +2 oxidation state. PbO2 is such a strong oxidant in fact that it’ll oxidise HCl to chlorine gas. [ 1]

Why does lead dioxide act as a strong oxidizing agent?

That is why lead dioxide undergoes reduction and oxidises other substances because we know that removal of oxygen is an example of reduction .That is why it acts as a strong oxidizing agent . Are acids oxidising agents or reducing agents?

What is the oxidation number of electrons in Pb and CO2?

Due to inert pair effect, pb is able to form only +2 oxidation state.But Carbon can form +4 oxidation state. Therefore in co2 four bonds =>4 electrons aready involved un bondig. But in pb it can only have 2 electrons in bonding due to +2 oxidation state.