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Despite the fact than fluorine is more e...

Despite the fact than fluorine is more electronegative than iodine, yet `HF` is less acidic as compared to `HI` . Explain.

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Fluorine atom is much smaller in size than iodine, hence `H-F` bond length is less than `H-I` and the bond dissociation energy of `H-F` is very high as compared to `H-I`. As a result, `H-I` bond breaks more readily than `H-F` and `HI` is a stronger acid than `HF`.
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Fluorine is more electronegative than chlorine. Is the statement true ?

(i) Hydrogen fluoride is a weaker acid than hydrogen chloride in aqueous solution. Or Which is a stronger acid in aqueous solution, HF or HCI ? (ii) In aqueous solution, HI is a stronger acid than HCI ? (iii) F atom is more electronegative than I atom, yet HF has lower acid strength than HI. Explain.

Knowledge Check

  • Fluorine is more reactive than chlorine because

    A
    fluorine has lower bond energy
    B
    fluorine has a greater ionisation potential
    C
    the covalent bond in fluorine molecule is weaker
    D
    fluorine has no available d-orbitals.

  • Fluorine is more electronegative than nitrogen the best explanation is that

    A
    the avlence electron in F are on an average a little closer to the nucleus than in N
    B
    the charge of a F nucleus is +9 while that on N nucleus is +7
    C
    The valence electrons in F and N are in different shells and thus their energy are greatly different
    D
    electronegativity increase from left to right in each of the period

  • Fluorine is more electronegativity than nitrogen. The best explanation is that:

    A
    the valency electrons in F are on the average, a little farther to the nucleus than in N
    B
    the charge on a F nucleus is `+9`, while that on N nucleus is `+7`
    C
    the nitrogen has half filled valence shell electron configuration, `ns^(2)np^(3)` where as fluorine has partially filled electron configuration `ns^(2)np^(5)`
    D
    the electronegativity decreases from top to bottom in each of the group as the effect nuclear charge remains constant.

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    CHF_(3) is less acidic than CHCl_(3) . Explain.

    Account for the following observations : (i) AlCl_(3) is a lewis acid. (ii) Though fluorine is more electronegative than chlorine yet BF_(3) is a weaker Lewis acid than BCl_(3) . (iii) PbO_(2) is stronger oxidising agent than SnO_(2) . (iv) The +1 oxidation state of thallium is more stable than its +3 state.

    Fluorine is more electronegative than chlorine but p-fluorobenzoic acid is a weaker acid than p-chlorobenzoic acid. Explain.

    Assertion: Although fluorine is more electronegative than chlorine, yet p-flurobenzoic acid is a weaker acid than p-chlorobenzoic acid. Reason: Due to matching sizes of 2p-orbitals of F and carbon, F has a stronger +R-effect than Cl.

    Statement-1 : Fluorine is more electronegative than chlorine. Statement-2 : Fluorine is smaller in size than chlorine.

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