O=-2
Pb=x
x+(-2)*2=0
x+4-=0
-4+4=0
Pb4-
No, Pb is not a transition metal and it has 2 oxidation states
The symbol for the plumbic ion, which is the cation of lead with a +4 oxidation state, is Pb⁴⁺. Lead can also exist in a +2 oxidation state, represented as Pb²⁺, but the term "plumbic" specifically refers to the +4 state.
Lead dioxide can be produced from lead carbonate by heating the lead carbonate in the presence of oxygen to convert it to lead oxide, then further heating the lead oxide in the presence of oxygen to convert it to lead dioxide. This process involves two steps of thermal decomposition and oxidation to yield lead dioxide.
86.62(8)%The molar masses of the constituent elements must be known.M(Pb) = 2.072(1) x 102 gmol-1M(O) = 1.59994(3) x 10 gmol-1From these and their respective molar ratios in the compound, the total molar mass of the compound must be calculated.M(PbO2) = M(Pb) + 2M(O)M(PbO2) = (2.072 x 10 gmol-1 + 2(1.59994 gmol-1)) x 10M(PbO2) = 2.392(1) x 102 gmol-1From the molar mass of the element in question and its ratio, and the compound, their total masses present in one mole of compound must be calculated.m = nMm(Pb) = 1 mol x 2.072 x 102 gmol-1m(Pb) = 2.072(1) x 102 gm(PbO2) = 1 mol x 2.392(1) x 102 g (always 1 mole)m(PbO2) = 2.392(1) x 102 gFrom these, the percentage of the element in question present in the compound can be calculated.m(Pb) x 100%/m(PbO2) = 2.072 g x 100%/2.392 gm(Pb) x 100%/m(PbO2) = 86.62(8)%
Plumbate and plumbite are two different chemical species of lead compounds. Plumbate refers to a compound in which lead is in its higher oxidation state of +4, typically in the form of PbO2. Plumbite, on the other hand, refers to a compound in which lead is in its lower oxidation state of +2, typically in the form of Pb(OH)2 or PbO. The key distinction lies in the oxidation state of lead within the compound.
O is 2- and there are two of them so Pb would have to be 4+
The oxidation number for Pb in PbO2 is +4. Oxygen in compounds is typically -2, so with two oxygens, the total oxidation number contributed by oxygen is -4. This means that the oxidation number of Pb must be +4 to balance the charges.
The ionic chemical formula of lead(IV) oxide is: (Pb)4+ + 2 O-.
An ionic bond.
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.
The composition of PbO and PbO2 is explained by the different oxidation states of lead. In PbO, lead is in the +2 oxidation state, while in PbO2, lead is in the +4 oxidation state. This difference in oxidation states leads to the formation of the two different oxides with distinct properties.
To balance the chemical equation Pb + PbO2 + H2SO4 → H2O + PbSO4, start by balancing the Pb atoms on the left side by adding a coefficient of 2 in front of Pb on the left side. Then balance the SO4 atoms by adding a coefficient of 4 in front of H2SO4. The balanced equation is 2Pb + PbO2 + 4H2SO4 → 2H2O + 2PbSO4.
Pb3O4 contains oxygen in the 2- oxidation state. and lead in the 2+ and 4+ oxidation states.
No, Pb is not a transition metal and it has 2 oxidation states
Possible valences of plutonium are: +2,3,4,5,6.
The formula for plumbous oxide is PbO.
Assuming the 2 oxidation state of lead. Pb + 2HNO3 --> Pb(NO3)2 + H2