The boiling point of methanol is greater than methyl thiol because
- There is intramolecular hydrogen bonding in methanol and intermolecular hydrogen bonding in methyl thiol
- There is intermolecular hydrogen bonding in methanol and no hydrogen bonding in methyl thiol
- There is no hydrogen bonding in methanol and intermolecular hydrogen bonding in methyl thiol
- There is no hydrogen bonding in methanol and intramolecular hydrogen bonding in methyl thiol.
The Correct Option is B
Solution and Explanation
Top Questions on Hydrogen Bonding
- Consider the following reactions
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Assertion (A) : PH3 has lower boiling point than NH3.
Reason (R) : In liquid state NH3 molecules are associated through vander waal’s forces, but PH3 molecules are associated through hydrogen bonding.
In the light of the above statements.
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For the reaction:
\[ 2A + B \rightarrow 2C + D \]
The following kinetic data were obtained for three different experiments performed at the same temperature:
\[ \begin{array}{|c|c|c|c|} \hline \text{Experiment} & [A]_0 \, (\text{M}) & [B]_0 \, (\text{M}) & \text{Initial rate} \, (\text{M/s}) \\ \hline I & 0.10 & 0.10 & 0.10 \\ II & 0.20 & 0.10 & 0.40 \\ III & 0.20 & 0.20 & 0.40 \\ \hline \end{array} \]
The total order and order in [B] for the reaction are respectively:
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Concepts Used:
Hydrogen Bonding
Hydrogen bonding implies the formation of hydrogen bonds which are an attractive intermolecular force. An example of hydrogen bonding is the bond between the H atom and the O atom in water.
A special type of intermolecular attractive force arises only in the compounds having Hydrogen atoms bonded to an electronegative atom. This force is known as the Hydrogen bond. For instance, in water molecules, the hydrogen atom is bonded to a highly electronegative Oxygen.
The conditions for hydrogen bonding are:
- The molecule must contain a strongly electronegative atom that is bound to the hydrogen atom. The higher the electronegativity, the more polarized is the molecule.
- The electronegative atom must be small. The smaller the size, the greater the electrostatic magnetism.
Effects of Hydrogen Bonding on Elements:
Association: The molecules of carboxylic acids exist as dimer because of the hydrogen bonding. The molecular masses of such compounds are found to be double than those calculated from their simple formula.
Dissociation: In aqueous solution, HF dissociates and gives the difluoride ion instead of fluoride ion. This is due to hydrogen bonding in HF. The molecules of HCl, HBr, HI do not form a hydrogen bond. This explains the non-existence of compounds like KHCl2, KHBr2, KHI2.
Types of Hydrogen bonding
- Intramolecular Hydrogen bonding: When hydrogen bonding takes place between different molecules of the same or different compounds, it is called intermolecular hydrogen bonding.
- Intermolecular hydrogen bonding: The hydrogen bonding which takes place within a molecule itself is called intramolecular hydrogen bonding.
- Symmetrical Hydrogen bonding: The symmetric hydrogen bond is a type of a three-centre four-electron bond.