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Chapter 16: Problem 2

Give reasons for the following: (a) Fluorine exhibits only (-I) oxidation state while the other halogens can show higher oxidation states. (b) HF has the highest boiling point while lowest acidic strength among the halogen acids. (c) \(\mathrm{F}_{2}\) is the strongest oxidising agent.

Short Answer

Expert verified
Fluorine always exhibits -1 oxidation state due to its highest electronegativity and no available d-orbitals. HF's high boiling point and lowest acidic strength amongst halogen acids can be attributed to its high polarity and strong bond . F2 is the strongest oxidizing agent due its extremely high electronegativity, small size and the stability it gains after reduction to F-.

Step by step solution

01

Explanation of Fluorine Oxidation State

Fluorine is the most electronegative element in the periodic table. Thus, it always attracts electron to gain a stable electronic configuration of the nearest noble gas, and forms a \( \mathrm{-1} \) oxidation state. It does not have d-orbitals to expand its covalency beyond one, so it cannot show a positive oxidation state. Hence, Fluorine exhibits only a -1 oxidation state, while other halogens, which have empty d-orbitals, can exhibit positive oxidation states.
02

Explanation of HF Boiling Point and Acidic Strength

HF has the highest boiling point among halogen acids due to the high polarity of the bond and the presence of strong hydrogen bonds. The acidic strength of a hydrogen halide is determined by the ease with which it can lose a proton (H+). In comparison to other hydrogen halides, HF is least willing to donate a proton due to its strong H − F bond, resulting in its least acidic strength.
03

Explanation of F2 as the Strongest Oxidising Agent

F2 is the strongest oxidizing agent because of its extremely high electronegativity and small size, which contributes to a strong desire to gain electrons. Also, when F2 is reduced to F-, it forms an exceptionally stable ion. The ability for elements and compounds to attract and accept electrons is what makes them potent oxidation agents. Thus, F2, having the strongest ability to attract electrons, is the strongest oxidizing agent.

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Most popular questions from this chapter

Discuss the special properties of HF in brief.

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