Table of Contents
Why does SO2 acts as oxidising and reducing agent?
In SO2 the oxidation state of sulphur is +4, it can lose its two more electron to attain +6 oxidation state. Since it has a capability to lose and gain electron therefore it acts as oxidizing as well as reducing agents.
Is TeO2 reducing agent?
Down the group, stability of +4 oxidation state decreases due to inner pair effect. Thus, Te in $Te{O_2}$ will not attain higher oxidation state and hence, will not be a reducing agent.
Why does reducing character decreases from SO2 to TeO2?
As the size of group 16 elements increases down the group, the element–oxygen bond strength decreases from SO2 to TeO2. Therefore, the bond dissociation enthalpy decreases. Hence, due to increase in the tendency to release oxygen, the oxidising tendency increases and, consequently, the reducing character decreases.
Why is Sulphur dioxide a reducing agent?
The reducing nature of sulfur dioxide is due to the evolution of nascent hydrogen. The oxidising nature appears when it reacts with strong oxidising agents.
Is SO2 oxidizing agent or reducing agent?
Featuring sulfur in the +4 oxidation state, sulfur dioxide is a reducing agent.
Why does SO2 act as a bleaching agent?
Bleaching property of chlorine is due to oxidation whereas the bleaching property of sulphur dioxide is due to reduction. Chlorine reacts with water and produces nascent oxygen. Sulphur dioxide acts as a temporary bleaching agent and removes oxygen by reduction as mentioned in the above reaction.
Is SO2 a reducing or oxidizing agent?
Reactions. Featuring sulfur in the +4 oxidation state, sulfur dioxide is a reducing agent.
How is TeO2 an oxidising agent?
But in TeO2. Te is heaver element. electrons are reluctant to take part in bond formation due to poor shielding of d- and f-orbitals thus lower oxidation states (+2, -2) becomes more stable( inert pair effect) and hence TeO2 is oxidising agent.
Why does reducing character increase down the group?
The reducing character increases down the group because ionisation energy decreases as we move down the group from O to Po.
Why is fluorine stronger oxidizing agent than chlorine?
As the electronegativity increases the oxidising power of halogen increases. Fluorine is the most electronegative element in the periodic table. Despite having low electron gain enthalpy it is the stronger oxidising agent than chlorine because of the high hydration energy and low bond dissociation energy.
Is sulphur a reducing agent or oxidising agent?
Sulfur is called the oxidizing agent. The zinc causes the sulfur to gain electrons and become reduced and so the zinc is called the reducing agent. The oxidizing agent is a substance that causes oxidation by accepting electrons. The reducing agent is a substance that causes reduction by losing electrons.
Is so2 a strong oxidising agent?
However, it can also act as an oxidizing agent.
Is TeO2 a reducing agent or an oxidising agent?
it is an reducing agent because it reduces others and oxidise itself. In TeO2 Te have +4 oxidation state and Te can’t go to +6 because in Te lower oxidation state is more stable due to inert pair effect so it go to higher to lower oxidation state so it reduces itself so it is oxidising agent.
Why is sulphur used as a reducing agent in SO2?
Give reasons: SO 2 is reducing while TeO 2 is an oxidising agent. 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.
Is SO2 an oxidizer or a reducer?
SO2 CAN BE either an oxidizer or reducer because it is in an intermediate oxidation state [+4] of the oxidation states sulfur can attain [-2 to +6]. This is a property of any ion or molecule in an intermediate oxidation state. In some cases the substance can oxidize and reduce itself in a reaction called disproportionation.
What is the difference between SO2 and TeO2?
Give reasons: (i) SO2 is reducing while TeO2 is an oxidising agent. (ii) Nitrogen does not form pentahalide. (iii) ICl is more reactive than I2 .