Question

The comparatively high boiling point of HF is due to :
A. High reactivity of fluorine
B. Small size of hydrogen atom
C. Formation of hydrogen bonds
D. High IE of fluorine

Answer 1

Intermolecular bonding is the compound property of a particle to join to another atom. There are a few sorts of synthetic bonds like Covalent bonds, Ionic bonds, Hydrogen bonds, Metallic bonds, and Van der Waals cooperation.

Complete step by step solution:
a. The intermolecular bonding for $HF$ is van der Waals, though for , $HCl$ the intermolecular holding is hydrogen. Since the van der Waals bond is more grounded than hydrogen, HF will have a higher bubbling temperature.
b. The intermolecular holding for $HF$ is covalent, though for, $HCl$ the intermolecular holding is hydrogen. Since the covalent bond is more grounded than van der Waals, HF will have a higher bubbling temperature.
c. The intermolecular holding for $HF$ is hydrogen, though for $HCl$ the intermolecular holding is van der Waals. Since the hydrogen bond is more grounded than van der Waals, $HF$ will have a higher bubbling temperature.
d. The nuclear number for $Cl$ is more noteworthy than for $F$ ,so $HF$ will have a higher bubbling temperature.

The little size of the particle is significant in making the impact of the core more noteworthy. Henceforth fluorine has a high electron fondness (for the main electron to be included). Just chlorine has a higher electron fondness.

**So, this question has multiple correct answers A,B,C

Note: **
Fluorine is the most electronegative element because it has 5 electrons in it's 2P shell. The optimal electron configuration of the 2P orbital contains 6 electrons, so since Fluorine is so close to ideal electron configuration, the electrons are held very tightly to the nucleus.