Advertisements
Advertisements
Question
Give reasons: SO2 is reducing while TeO2 is an oxidising agent.
Solution
In case of sulphur, because of the presence of empty d-orbital, it can expand its oxidation state from the + 4 to the +6 oxidation state. Hence, it acts as a reducing agent.
Te is a heavy element and so because of the inert pair effect, the lower oxidation state is more stable. Hence, it acts as an oxidising agent.
APPEARS IN
RELATED QUESTIONS
Account for the following: Oxygen shows catenation behavior less than sulphur.
a. Explain the trends in the following properties with reference to group 16:
1 Atomic radii and ionic radii
2 Density
3 ionisation enthalpy
4 Electronegativity
b. In the electolysis of AgNO3 solution 0.7g of Ag is deposited after a certain period of time. Calulate the quantity of electricity required in coulomb. (Molar mass of Ag is 107.9g mol-1)
List the important sources of sulphur.
Why does NH3 form hydrogen bond but PH3 does not?
Knowing the electron gain enthalpy values for O → O− and O → O2− as −141 and 702 kJ mol−1 respectively, how can you account for the formation of a large number of oxides having O2− species and not O−? (Hint: Consider lattice energy factor in the formation of compounds).
Why are halogens strong oxidising agents?
The boiling points of hydrides of group 16 are in the order:
In forming (i) \[\ce{N2 -> N^{+}2}\] and (ii) \[\ce{O2 -> O^{+}2}\]; the electrons respectively are removed from:
The correct order of ΔiHs among the following elements is
Which of the following compound is a peroxide?
