Why cr6+ is strong oxidizing agent but mo6+ is not?

Answer: (b, c) In d-block elements, for heavier elements, the higher oxidation states are more stable. Hence, Mo(VI) and W(VI) are more stable than Cr (VI). Thats why, Cr (VI) in the form of dichromate is a stronger oxidising agent in acidic medium whereas and are not.

Which one among the following is the strongest oxidising agent ClO4 BrO4 IO4?

Answer: BrO4- is the strongest oxidising agent among ClO4- and IO4-. as the strongest oxidizing agent. The oxidizing agent of a substance is tested for its ability to undergo reduction.

Why Thallium is a good oxidizing agent?

Tl is in +3 oxidation state in TlCl It will act as an oxidising agent, as it can readily gain electrons to change to its more stable oxidation state i.e +1. So, this works as a good oxidising agent.

Why fluorine is the strongest oxidizing agent?

Hence it is the most electronegative element. -So it can easily accept an electron than any other halogen and hence it undergoes reduction and acts as a strong oxidizing agent. -It also has a small size due to which it is nearly impossible for fluorine to donate its electron. Hence it fails to act as a reducing agent.

Is a strong oxidising agent in acidic medium whereas WO3 and MoO3 are not?

In the form of dichromate, Cr (VI) is a strong oxidising agent in acidic medium but Mo (VI) in MoO3 and W (VI) in WO3 are not because. In the form of dichromate, Cr (VI) is a strong oxidising agent in acidic medium but Mo (VI) in MoO3 and W (VI) in WO3 are not because.

Can mno42 act as reducing agent?

MnO2​ can act as an oxidizing agent as well as reducing agent.

Why bro4 is strongest oxidising agent?

It’s because it is easy for bromine to lose electron than chlorine . Making it a better oxidising agent than chlorine.

Which is the strongest oxidising agent and why bro4 or clo4?

Therefore, Br can still accept electrons, which means it can be reduced more easily than the Cl and hence it acts as a strongest oxidizing agent among Cl and Br.

Why is Pb4+ an oxidising agent?

Pb therefore shows stable oxidation state of +2 while Sn shows +4 stable oxidation state. Thus Pb4+ can gain two electrons and become Pb2+ which is the stable form and hence acts as oxididing agent.

Why Tl 3 is a good oxidising agent?

Due ta strong inert pair effect, the +3 oxidation state of Tl is less stable than its +1 oxidation state. Since in Tl(NO3)3 , oxidation state of Tl is +3, therefore, it can easily gain two electrons to form TlNO3 in which the oxidation state of Tl is +1. Consequently, Tl(NO3)3 acts as an oxidising agent.

Why is fluorine a stronger oxidising agent than oxygen?

Why? Considering it has the lowest reduction potential of all elements ( around -2.42 F) in the periodic table, a florine atom can never be oxidised to at positive ion(F+) and hence it is the strongest oxidising agent. It can oxidise oxygen!!

Is fluorine a good oxidizing agent?

Fluorine is such a powerful oxidizing agent that solution reactions are unfeasible. Chlorine has the ability to take electrons from both bromide ions and iodide ions. Similarly, bromine is a more powerful oxidizing agent than iodine.