Table of Contents
What makes an oxidant strong?
Atoms, ions, and molecules that have an unusually large affinity for electrons tend to be good oxidizing agents. These compounds are strong oxidizing agents because elements become more electronegative as the oxidation states of their atoms increase.
How do you tell what the strongest oxidizing agent is?
The higher the electronegativity the greater the pull an oxidizing agent has for electrons. The higher the pull for electrons the stronger the oxidizing agent. So the element with the highest electronegativity is the strongest oxidizing agent.
Is P more oxidising than SB?
The stability of + 5 oxidation state decreases and that of + 3 state increases (due to invert pair effect) down the group….The p-Block Elements.
| Properties | White Phosphorus | Red phosphorus |
|---|---|---|
| 3. Density | 1.84 g cm-3 | 2.1 gcm3 |
| 4. Ignition | 307 K | 543 K |
| temperature | ||
| 5. Stability | Less stable at ordi- | More stable at ordi – |
Which chlorine species is a stronger oxidant?
Chlorine dioxide is also a strong oxidant and disinfectant more effective than free chlorine at basic pH. Ct values for chlorine dioxide are less than 1 mg-min l−1 for most vegetative bacteria and viruses (Table 3).
What is meant by oxidant?
noun, plural: oxidants. (1) Any substance that has the ability to oxidize other substance. (2) A molecule or atom capable of accepting electrons during a redox reaction. Supplement. An oxidant is a substance that accepts or receives electron from another substance, hence, is consequently reduced.
Is I2 an oxidizing agent?
Consequently, you can say that iodine, I2 , is acting as an oxidizng agent because it is oxidizing the thiosulfate anion to the tetrathionate anion, S4O2−6 . Notice that the oxidation number of iodine goes from 0 on the reactants’ side to −1 on the products’ side.
Why is be stronger oxidant than Sb?
Bismuth (Bi) in the pentavalent state can easily accept two electrons and gets reduced to trivalent bismath. Therefore , it acts as a strong oxidising agent .
Which is a stronger reducing agent SbH3 or BiH3 and why?
BiH3 is a stronger reducing agent than SbH3 since Sb-H bond has smaller bond length as compared to bond length of Bi-H bond.
Is I2 a strong oxidizing agent?
This indicates that chlorine is a more powerful oxidizing agent than either bromine or iodine. Similarly, bromine is a more powerful oxidizing agent than iodine. Bromine can remove electrons from iodide ions, producing iodine; iodine cannot reclaim those electrons from the resulting bromide ions.
Can I2 oxidise BR?
A red solution of iodine is formed (see the note above) until the bromine is in excess. Then you get a dark grey precipitate. Iodine won’t oxidise any of the other halide ions (unless you happened to have some extremely radioactive and amazingly rare astatide ions – astatine is at the bottom of this Group).
Is lithium a good oxidizing agent?
Since oxidation and reduction are symmetric processes, always occurring together, there is always an oxidizing agent and a reducing agent in the reaction. Lithium, having the largest negative value of electrode potential, is the strongest reducing agent.
Why does Bi(V) act as a stronger oxidant than Sb(V)?
Both Sb and Bi are same group elements and as we go down the group then due to inert pair effect there will be increase in +3 oxidation state. Hence, Bi being the last element easily gains two electrons and reduces to +3 oxidation state from +5. Therefore, Bi (V) acts as a stronger oxidant than Sb (V).
What is the difference between Bi(V) and Sb(V)?
Bi (V) means Bi has lost 5 electrons and it is in a +5 oxidation state. Bi (V) is a stronger oxidizing agent than Sb (V) means that it will pick electrons from a reducing agent (electron donor) much faster than Sb (V) to go from a unstable +5 to a more stable +3 oxidation state.
Why is Bibi+5 a stronger oxidising agent than bi?
Bi+5 is a stronger oxidising agent. As bismuth is the last member of 15th group it has the largest size. Due to inert pair effect, Bi+5 rarely exists and Bi mostly exist in +3 Oxidation State, due to which Bi acts as an Oxidising agent so that it can reduce to it’s lower oxidation state.
Why SB is an oxidising agent while bismuth is not?
See what the community says and unlock a badge. inert pair effect of bismuth is more prominent than sb so its +3 oxidation state is more stable +5.So bismuth will take up 2 electrons and changeinto bismuth and bi is an oxidising agent. In case of sb reduction from +5 to +3 will not occur easily.