Advertisements
Advertisements
प्रश्न
Give reasons: SO2 is reducing while TeO2 is an oxidising agent.
Advertisements
उत्तर
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
संबंधित प्रश्न
Account for the following: Oxygen shows catenation behavior less than sulphur.
Give reasons for the following : H2Te is the strongest reducing agent amongst all the hydrides of Group 16 elements.
Give reasons for the following : Oxygen has less electron gain enthalpy with negative sign than sulphur.
Arrange the following in the order of the property indicated against set :
H2O, H2S, H2Se, H2Te − increasing acidic character.
Explain the following properties of group 16 elements :
1) Electro negativity
2) Melting and boiling points
3) Metallic character
4) Allotropy
Strong reducing behaviour of \[\ce{H3PO2}\] is due to ______.
Write a balanced chemical equation for the reaction showing catalytic oxidation of NH3 by atmospheric oxygen.
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
What is the basicity of \[\ce{H3PO4}\]?
