Advertisements
Advertisements
Question
Account for the following observations:
PbO2 is a stronger oxidising agent than SnO2
Solution
PbO2, lead is in +2 oxidation state and can be reduced to its most stable oxidation state of +2. Hence PbO2 can be further exidised or act as a strong oxidising agent. and in SnO, Sn is and +2 oxidation state and can extend its oxidation state up to +4. Thus, SnO can be used as a reducing agent.
APPEARS IN
RELATED QUESTIONS
How would you explain the lower atomic radius of Ga as compared to Al?
Write a balanced equation for B2H6 + NH3 → ?
Ionisation enthalpy (∆iH1kJ mol–1) for the elements of Group 13 follows the order.
A compound X, of boron reacts with NH3 on heating to give another compound Y which is called inorganic benzene. The compound X can be prepared by treating BF3 with Lithium aluminium hydride. The compounds X and Y are represented by the formulas.
Explain the following:
Boron does not exist as B3+ ion.
Explain the following:
PbX2 is more stable than PbX4.
Explain the following:
Tl (NO3)3 acts as an oxidising agent.
Account for the following observations:
Though fluorine is more electronegative than chlorine yet BF3 is a weaker Lewis acid than BCl3
Three pairs of compounds are given below. Identify that compound in each of the pairs which has group 13 element in more stable oxidation state. Give reason for your choice. State the nature of bonding also.
InCl3, InCl
BCl3 exists as monomer whereas AlCl3 is dimerised through halogen bridging. Give reason. Explain the structure of the dimer of AlCl3 also.
