Which of the following substances exhibits strong hydrogen...

Which of the following substances exhibits strong hydrogen bonding in the liquid and solid states?
(a) $\mathrm{H}_{2} \mathrm{~S}$;
(b) $\mathrm{NH}_{3}$
(c) $\mathrm{SiH}_{4}$
(d) $\mathrm{HF}$;
(e) HCl.

Key Concepts

Molecular Polarity

Molecular polarity describes the uneven distribution of electron density in a molecule, leading to a dipole moment. Polar molecules, especially those with hydrogen atoms bonded to highly electronegative atoms, are capable of forming hydrogen bonds, which greatly influence their physical behavior in both liquid and solid states.

Intermolecular Forces

Intermolecular forces are the attractions between molecules that determine many physical properties, including state of matter and phase behavior. Among these forces, hydrogen bonding is one of the strongest, and its presence can lead to significantly higher boiling and melting points compared to substances where only weaker interactions like dipole-dipole interactions or dispersion forces are present.

Electronegativity

Electronegativity refers to the ability of an atom to attract electrons towards itself in a chemical bond. When hydrogen is bonded to a highly electronegative atom, the resulting bond becomes highly polarized, which is a requisite condition for effective hydrogen bonding between molecules.

Hydrogen Bonding

Hydrogen bonding is a strong type of intermolecular force that occurs when a hydrogen atom covalently bonded to a highly electronegative atom (typically nitrogen, oxygen, or fluorine) interacts with a lone pair on another electronegative atom in a nearby molecule. This interaction significantly impacts the physical properties of substances, such as their boiling and melting points.

Transcript

Please give Ace some feedback