A. HF
B. HBr
C. HC
D. HI
¨ The reducing power of a compound is a measure of its ability to donate electrons and reduce other compounds. In general, compounds with weaker bonds and more negative oxidation states tend to be better reducing agents.
¨ Hydrogen halides, such as HF, HBr, HCl, and HI, are all acidic compounds that can act as reducing agents under certain conditions. Of these, HF is the weakest reducing agent, as it has the strongest bond and the least negative oxidation state.
¨ In HF, the bond between hydrogen and fluorine is a polar covalent bond, with the fluorine atom having a higher electronegativity than the hydrogen atom. This makes the bond more difficult to break and reduces the ability of HF to donate electrons and act as a reducing agent.
¨ In contrast, HI is the strongest reducing agent among the hydrogen halides, as it has the weakest bond and the most negative oxidation state. The bond between hydrogen and iodine is relatively weak due to the large size of the iodine atom, and iodine has a greater tendency to gain electrons and become reduced.
Submitted by :- Jamil Ahmed