Compounds showing hydrogen bonding among \[\text{HF,N}{{\text{H}}_{\text{3}}}\text{,}{{\text{H}}_{\text{2}}}\text{S}\] and \[\text{P}{{\text{H}}_{\text{3}}}\] are
A only HF and \[\text{N}{{\text{H}}_{\text{3}}}\] and \[\text{P}{{\text{H}}_{\text{3}}}\]
B only HF and \[\text{N}{{\text{H}}_{\text{3}}}\]
C only \[\text{N}{{\text{H}}_{\text{3}}}\text{,}{{\text{H}}_{\text{2}}}\text{S}\]and \[\text{P}{{\text{H}}_{\text{3}}}\]
D All of four

Question

Compounds showing hydrogen bonding among \[\text{HF,N}{{\text{H}}_{\text{3}}}\text{,}{{\text{H}}_{\text{2}}}\text{S}\] and \[\text{P}{{\text{H}}_{\text{3}}}\] are
A only HF and \[\text{N}{{\text{H}}_{\text{3}}}\] and \[\text{P}{{\text{H}}_{\text{3}}}\]
B only HF and \[\text{N}{{\text{H}}_{\text{3}}}\]
C only \[\text{N}{{\text{H}}_{\text{3}}}\text{,}{{\text{H}}_{\text{2}}}\text{S}\]and \[\text{P}{{\text{H}}_{\text{3}}}\]
D All of four

Vedantu Content Team · Accepted Answer

Hint :  A hydrogen atom that is bound to a highly electronegative atom and another highly electronegative atom that is close by interact with one another to form hydrogen bonds, which are a unique kind of attractive intermolecular interactions. This process is known as hydrogen bonding. Complete Solution: Hydrogen is covalently joined to the more electronegative oxygen atom in water molecules. Therefore, the dipole-dipole interactions between the hydrogen atom of one water molecule and the oxygen atom of another water molecule are what cause hydrogen bonding to form in water molecules.Here, the oxygen nucleus is in close proximity to the bond pair of electrons in the O-H bond (due to the large difference in the electronegativities of oxygen and hydrogen). As a result, the hydrogen atom acquires a partial positive charge while the oxygen atom acquires a partial negative charge. Now, the electrostatic attraction between the hydrogen atom of one water molecule and the oxygen atom of another water molecule allows for the formation of hydrogen bonds.In light of this, hydrogen bonds represent a very distinct type of intermolecular attractive forces that only appear in compounds when hydrogen atoms are bound to strongly electronegative elements. Compared to standard dipole-dipole and dispersion forces, hydrogen bonds are generally much stronger. They are not as strong as actual covalent or ionic connections, though.When hydrogen is joined to an atom that is both strongly electronegative and tiny in radius, a hydrogen bond is created.As a result, electronegativity is a property of an atom's capacity to draw an electron pair. The Pauling scale is the most popular.The hydrogen bond exists in HF. Because of the significant electronegativity difference, there is a persistent dipole. Hydrogen bonds can also form with $$\text{N}{{\text{H}}_{\text{3}}}$$.When any of the three electronegative atoms (N, O, or F) and hydrogen are covalently connected to one another, two molecules create a hydrogen bond. $${{\text{H}}_{\text{2}}}\text{S}$$ and $$\text{P}{{\text{H}}_{\text{3}}}$$do not have hydrogen bonds despite having dipole dipole forces since there is no (N, O, F) in these molecules.  As a result, Option B is the correct answer  Note: When a hydrogen atom is joined to an extremely electronegative atom in a molecule, it draws the shared pair of electrons more and the molecule's one end changes from slightly positive to slightly negative as a result. A weak link between the molecules is created when the positive end of one is drawn to the negative end of the other. The hydrogen bond is the name of this bond.