Hydrogen bonding is maximum in ethanol.

Explanation:

What is hydrogen bonding?

Hydrogen bonding is a special type of intermolecular force that occurs between molecules containing hydrogen atoms bonded to highly electronegative elements such as oxygen, nitrogen, or fluorine. It is a strong dipole-dipole interaction that results in the formation of a partially positive hydrogen atom and a partially negative atom.

Factors affecting hydrogen bonding:

There are several factors that influence the strength of hydrogen bonding, including:

1. Electronegativity difference: The greater the electronegativity difference between hydrogen and the atom it is bonded to, the stronger the hydrogen bonding.

2. Size of the atom: Smaller atoms with higher electronegativity can form stronger hydrogen bonds.

3. Number of hydrogen bonding sites: The more hydrogen atoms bonded to electronegative atoms, the more hydrogen bonding sites are available.

4. Molecular shape: The presence of hydrogen bonding sites in a linear or planar arrangement increases the strength of hydrogen bonding.

Comparison of the given compounds:

a) Ethanol: Ethanol (CH3CH2OH) contains an -OH group, which can form hydrogen bonds. The electronegative oxygen atom attracts the hydrogen atom, resulting in the formation of strong hydrogen bonds between ethanol molecules.

b) Ethyl chloride: Ethyl chloride (CH3CH2Cl) does not contain any hydrogen bonding sites. The chlorine atom is not electronegative enough to form strong hydrogen bonds.

c) Diethyl ether: Diethyl ether (CH3CH2OCH2CH3) contains an oxygen atom, but it does not have any hydrogen bonding sites. The oxygen atom is not bonded to a hydrogen atom.

d) Triethylamine: Triethylamine (N(C2H5)3) does not contain any hydrogen bonding sites. Although it contains a nitrogen atom, it is not bonded to a hydrogen atom.

Conclusion:

Among the given compounds, ethanol has the maximum hydrogen bonding because it contains an -OH group, which can form strong hydrogen bonds. The other compounds do not have hydrogen bonding sites or have less electronegative atoms, resulting in weaker or no hydrogen bonding.