Answered By . Reason. Thus, it becomes easy to lose H + ion. Hydrobromic acid. I-Iodide. HBr. This causes the increase in acidic strength down the group. HF is a weak acid, but very dangerous (you may hear it etches glass, that’s because the SiF bond is the strongest bond) HCl and the rest of them (HBr, HI) are all “strong acids” but HI is the strongest (see pKa’s below) Due to poor orbital overlap (Iodine is much larger than H, and therefore the electrons are not very well shared, which imparts an extremely ionic character to the molecule) HX à H + + X- ; (where X – = F –, Cl –, Br –, I –) The above order of acidic character can be explained in terms of strength of H-X bonds, which is in the order H-I< H-Br < H-Cl < H-F.
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… Down the group the electronegativity decreases and the size increases. answr.
HI. Acid Strength and Bond Strength Binary acids are certain molecular compounds in which hydrogen is combined with a second nonmetallic element; these acids include HF, HCl, HBr, and HI. HCl, HBr, and HI are all strong acids, whereas HF is a weak acid. Assertion: The acidic strength of halogen acids varies in the order HF > HCl > HBr > HI Reason: The bond dissociation enthalpy of halogen acids decreases in the order HF > HCl > HBr > HI (A) Both assertion and reason are correct statements, and reason is the correct explanation of the assertion. The acid strength increases as the experimental pKa values decrease in the following order: toppr. Answer . Upvote(2) How satisfied are you with the answer? 1.0 * 10 9. HF < HCl < HBr < HI. HF HCl HBr HI. HF; HCl; HBr; HI Arrange the above acids in terms of strength. Hydroiodic acid. All the halogen acids ionise to give H + ion and halide ion, x-. 1.3 * 10 6. Br-Bromide.
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… Down the group the electronegativity decreases and the size increases. answr.
HI. Acid Strength and Bond Strength Binary acids are certain molecular compounds in which hydrogen is combined with a second nonmetallic element; these acids include HF, HCl, HBr, and HI. HCl, HBr, and HI are all strong acids, whereas HF is a weak acid. Assertion: The acidic strength of halogen acids varies in the order HF > HCl > HBr > HI Reason: The bond dissociation enthalpy of halogen acids decreases in the order HF > HCl > HBr > HI (A) Both assertion and reason are correct statements, and reason is the correct explanation of the assertion. The acid strength increases as the experimental pKa values decrease in the following order: toppr. Answer . Upvote(2) How satisfied are you with the answer? 1.0 * 10 9. HF < HCl < HBr < HI. HF HCl HBr HI. HF; HCl; HBr; HI Arrange the above acids in terms of strength. Hydroiodic acid. All the halogen acids ionise to give H + ion and halide ion, x-. 1.3 * 10 6. Br-Bromide.