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Chapter 16: Problem 1

Discuss the special properties of HF in brief.

Short Answer

Expert verified
Hydrogen Fluoride (HF) is a polar molecule and exhibits significant hydrogen bonding due to a highly electronegative fluorine atom. It has a high boiling point thanks to these strong intermolecular forces. HF is highly soluble in water forming hydrogen bonds with water molecules and it acts as a weak acid in solution due to limited ionization.

Step by step solution

01

Discuss Polarity of HF

HF, Hydrogen Fluoride, is a polar molecule. Polarity exists due to a difference in electronegativity; the fluorine atom is more electronegative than the hydrogen atom. Consequently, it pulls the electron pair in the bond closer to itself, leading to a polarity, resulting in a positive pole at the hydrogen end and a negative pole at the fluorine end of the molecule.
02

Discuss Hydrogen Bonding in HF

HF exhibits strong hydrogen bonding due to the presence of a highly electronegative fluorine atom and a hydrogen atom. The highly negative fluorine atom of one molecule and the positive hydrogen atom from a different HF molecule form a strong intermolecular hydrogen bond.
03

Discuss Boiling Point of HF

The boiling point of HF is higher compared to molecules of similar size. This can be attributed to strong hydrogen bonding in HF. The strong intermolecular forces need more energy to break down, leading to a high boiling point.
04

Discuss Solubility of HF

HF is highly soluble in water because it forms hydrogen bonds with water molecules. The negative end of the HF molecule is drawn to the positive hydrogen of the water molecule, resulting in a strong intermolecular force of attraction, i.e., hydrogen bonding.
05

Discuss HF as a Weak Acid

HF is considered a weak acid when dissolved in water. Although it does ionize to produce H+ (proton) and F- (fluoride ion), it doesn't completely ionize because the intermolecular hydrogen bonding holds the HF molecules together, limiting its ionization.

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Most popular questions from this chapter

Account for the following: (a) HF is not stored in glass bottles. (b) \(\mathrm{SiF}_{4}\) reacts with \(\mathrm{HF}\) to give \(\mathrm{H}_{2} \mathrm{SiF}_{6}\) (c) Electrolysis of aqueous HF does not give \(F_{2}\) at anode (d) Fluorine does not form any oxyacid except HOF. (e) \(\mathrm{I}_{2}\) is insoluble in \(\mathrm{H}_{2} \mathrm{O}\) but dissolves in aqueous solution of \(\mathrm{KI}\).

Discuss the electropositive character of iodine with the help of suitable examples.

Discuss the structures of the following compounds. (a) \(\mathrm{IF}_{5}\) (b) \(\mathrm{IO}_{4}^{-}\) (c) \(\mathrm{ClO}_{3}^{-}\) (d) \(\mathrm{Cl}_{2} \mathrm{O}\) (e) \(\mathrm{I}_{2} \mathrm{O}_{5}\) (f) \(\mathrm{IF}_{7}\)

What are pseudohalogens and what are their important characteristics?

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.
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