( Cl 2 > Br 2 > I 2) I-is a better reducing agent than Br-. 2 I - (aq) …
All of the halogens have equal strength as reducing agents. A oxidizing agent is a chemical substance that has the ability to subtract electrons from another substance (reducing agent) that donates or loses them. Cl2. Methods of Preparing the Halogens from their Halides The halogens can be made by reacting a solution of the halide ion with any substance that is a stronger oxidizing agent. Fluorine oxidises water to oxygen and so it is impossible to do simple solution reactions with it. X 2 must be a stronger oxidizing agent than Y 2, and Y must be a stronger reducing agent than X in order for the reactions to occur. It is also known as an oxidizing agent to that element or compound that passes electronegative atoms to another substance. This indicates that chlorine is a more powerful oxidizing agent than either bromine or iodine. Halogens have high electronegativity and electron affinity. Bromide is oxidized to bromine in the process, as in the half-equation below: \[ 2Br^- \rightarrow Br_2 + 2e^-\] Bromide reduces sulfuric acid to sulfur dioxide gas, decreasing the oxidation state of sulfur from +6 to +4. Fluorine is the strongest oxidising agent because:-1) Low enthalpy of dissociation of F-F bond (158.8/KJ mol-1) due to its small size Fluorine's hydration energy is very high hence better the oxidizing power. For example, among Na, Cr, Cu + and Cl −, Na is the strongest reducing agent and Cl − is the weakest one. Chlorine has the ability to take electrons from both bromide ions and iodide ions. In each case, a halogen higher in the Group can oxidise the ions of one lower down.
As the reduction potential decrease down the group,the oxidizing power decrease down the group the order of the oxidizing power will be as under F2 > Cl2> Br2> I2 The half-equation for this transition is as follows: From the previous page, the more reactive halogen will displace the ions of a less reactive halogen from its solution.
Fluorine is said to be the strongest elemental oxidizing agent due to …
H 2 SO 4 because HBr and HI being stronger reducing agents, reduces the oxidizing acid (i.e.conc. For example, chlorine can oxidise the bromide ions (in, for example, potassium bromide solution) to … Halogen oxidizing power Fluorine is the strongest oxidizing agent because fluorine atoms are the smallest halogen atoms, and so accept electrons most easily. upper left, lower right upper right, lower left lower left, upper right … 8. Br2. They have greater tendency to accept electrons or easily reduced, therefore they are strong oxidizing agent. 2) High hydration enthalpy of F- ( 515/KJ mol-1 ). Br 2 is a stronger oxidizing agent than I 2. Iodine, for example, can be made by reacting the iodide ion with either bromine or chlorine. Ans: HBr and HI cannot be prepared in the same way as HCl by using conc. (I-> Br-> Cl-) I2. This is a redox reaction with the halogen acting as an oxidising agent and the halide ion as a reducing agent. Cl 2 is a stronger oxidizing agent than Br 2. This is because the strength of oxidizing agent increases down the group. F2. This implies that they have the ability to easily attract electrons towards their respective nuclei. Which is the strongest oxidizing agent Lead Silver or Copper? Bromine and iodine cannot reclaim those electrons from the chloride ions formed. Similarly, the iodide anion, I −, is the strongest reducing agent among the stable halogens, being the most easily oxidised back to diatomic I 2. 2HBr + H 2 SO 4 → SO 2 + 2H 2 O + Br 2. Chlorine oxidises iodide ions to iodine and is itself reduced to chloride ions:
(From wps.prenhall.com) The species at the top left have the greatest "potential" to be reduced, so they are the strongest oxidizing agents. Bromide is a strong enough reducing agent to reduce sulfuric acid. The weakest oxidizing agent is Iodine. > Here's a typical table of standard reduction potentials.
The trend in reducing power of the halide ions is opposite to the trend in oxidising power of the halogen … This is a redox reaction with the halogen acting as an oxidising agent and the halide ion as a reducing agent. (Astatine goes further, being indeed unstable as At − and readily oxidised to At 0 or At +, although the existence of At 2 is not settled.) Br - is a better reducing agent than Cl-. Down group 7, as the halogen atoms get larger, they accept electrons less easily, and the oxidizing power becomes weaker.
Chlorine, bromine and iodine.
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