Hydrogen Bonding MCQ Quiz in मल्याळम - Objective Question with Answer for Hydrogen Bonding - സൗജന്യ PDF ഡൗൺലോഡ് ചെയ്യുക
Last updated on Apr 11, 2025
Latest Hydrogen Bonding MCQ Objective Questions
Top Hydrogen Bonding MCQ Objective Questions
Hydrogen Bonding Question 1:
NH3 has a much higher boiling point than PH3 because
Answer (Detailed Solution Below)
Hydrogen Bonding Question 1 Detailed Solution
Concept:
Hydrogen bonding:
- It is the electrostatic attraction between hydrogen atoms bonded to small, strongly electronegative atoms (N, O, and F).
- The bonding occurs through the lone pair of electrons on the electronegative atoms.
- Example: HF, H2O, etc.
2 Types of Hydrogen bonding:- Intermolecular and Intramolecular H-bonding.
- Intermolecular: Hydrogen bond formed between 2 molecules.
- Intramolecular: Hydrogen bond formed between two different atoms of the same molecule.
- Intermolecular Hydrogen bonding is stronger than van der waals' forces.
The essential requirement of Hydrogen bonding:
1. An H atom must be directly bonded to a highly electronegative atom.
2. Lone pair of electrons must be present on the electronegative atom.
Factors affecting Hydrogen bonding:
1. Association
Due to intermolecular H-bonding, carboxylic acid exists as dimers even in the vapor state.
2. Higher Boiling and Melting point
- Compounds having H-bonding requires larger energy to separate the molecules before they can melt or boil.
- So, the compounds containing H-bonds have high melting and boiling points.
3. Physical state
Explanation:
The difference in characteristics between NH3 and PH3 is given below:-
NH3 | PH3 |
Polar molecule | Non-polar molecule |
Have a large electronegativity difference between N and H. Eg:- N=3.01 and H=2.2 |
Have no electronegativity difference between P and H. Eg:- P=2.19 and H=2.2 |
Can form hydrogen bonding with the neighboring NH3 molecules. |
Doesn't form hydrogen bonding. |
The stronger hydrogen bonding makes it difficult to break the bonds between N and H atoms. |
Have weak dispersion force.
|
Have a higher boiling and melting point. |
Have low boiling and melting point. |
- Due to the lesser electronegativity of PH3 molecules, they cannot form H-bonding.
- PH3 can H-bond with water only but not with itself.
- Although PH3 is larger than NH3 with greater dispersion forces, NH3 has a higher polar N--H bond which gives rise to H-bonding.
- Since the strength of the H-bond is greater than the dispersion forces, the boiling point of NH3 is greater.
The hydrogen bonding in NH3 is shown below:
Hence, NH3 has a much higher boiling point than PH3 because NH3 forms hydrogen bond.
Hydrogen Bonding Question 2:
In which of the following substances will hydrogen bond be strongest?
Answer (Detailed Solution Below)
Hydrogen Bonding Question 2 Detailed Solution
Concept:
Hydrogen bonding:
- Hydrogen bonding is a special type of interaction that occurs between a hydrogen atom bonded covalently to an electronegative atom and another highly electronegative atom in the vicinity of this hydrogen.
- It is a special type of dipole-dipole interaction.
- Although H-bond is very weak but compounds having H-bond have high melting and boiling point.
There are two types of H-bonding -
- Intermolecular H-bonding
- Intramolecular H-bonding
→ Only small size and highly electronegative atoms are capable of forming H-bond with Hydrogen.
Explanation:
The hydrogen bond is a special type of bond between a hydrogen atom bonded covalently to an electronegative atom and another highly electronegative atom in the vicinity of this hydrogen.
→ Condition for H-Bonding :
Only small size and highly electronegative atoms are capable of forming H-bond with Hydrogen.
∴ only F, O, and N are such atoms that can make an H-bond with the hydrogen of other molecules.
In the given compounds HCl, H2O, HI, and H2S only H2O can form H-bond because Cl, S, and I are large size atoms and cannot form H-bond.
∴ Only H2O will form H-bond
- Intermolecular H-bonding is there in the water.
- Each H2O can make four H-bonds. Two with O-atom and two with H-atom.
- Each H2O molecule is tetrahedrally linked to the four other H2O molecules.
Conclusion:
Therefore, H-bonding will be strongest in H2O.
Hence, the correct answer is option 2.
Hydrogen Bonding Question 3:
In which of the following substances will hydrogen bond be strongest?
Answer (Detailed Solution Below)
Hydrogen Bonding Question 3 Detailed Solution
Concept:
Hydrogen bonding:
- Hydrogen bonding is a special type of interaction that occurs between a hydrogen atom bonded covalently to an electronegative atom and another highly electronegative atom in the vicinity of this hydrogen.
- It is a special type of dipole-dipole interaction.
- Although H-bond is very weak but compounds having H-bond have high melting and boiling point.
There are two types of H-bonding -
- Intermolecular H-bonding
- Intramolecular H-bonding
→ Only small size and highly electronegative atoms are capable of forming H-bond with Hydrogen.
Explanation:
The hydrogen bond is a special type of bond between a hydrogen atom bonded covalently to an electronegative atom and another highly electronegative atom in the vicinity of this hydrogen.
→ Condition for H-Bonding :
Only small size and highly electronegative atoms are capable of forming H-bond with Hydrogen.
∴ only F, O, and N are such atoms that can make an H-bond with the hydrogen of other molecules.
In the given compounds HCl, H2O, HI, and H2S only H2O can form H-bond because Cl, S, and I are large size atoms and cannot form H-bond.
∴ Only H2O will form H-bond
- Intermolecular H-bonding is there in the water.
- Each H2O can make four H-bonds. Two with O-atom and two with H-atom.
- Each H2O molecule is tetrahedrally linked to the four other H2O molecules.
Conclusion:
Therefore, H-bonding will be strongest in H2O.
Hence, the correct answer is option 2.
Hydrogen Bonding Question 4:
Given below are two statements :
Statement 1: o-Nitrophenol is steam volatile due to intramolecular hydrogen bonding.
Statement II: o-Nitrophenol has high melting due to hydrogen bonding.
In the light of the above statements, choose the most appropriate answer from the options given below :
Answer (Detailed Solution Below)
Hydrogen Bonding Question 4 Detailed Solution
Concept:
Intermolecular hydrogen bonding:
- This type of bonding mainly occurs between two or more same or different molecules when they combine to form a dimer or polymer respectively and leads to a phenomenon known as an association.
- Such a type of hydrogen bonding increases the boiling point of the compound and also its solubility in water.
Intramolecular hydrogen bonding:
- This type of bonding occurs within two atoms of the same molecule and leads to a phenomenon known as chelation.
- This type of hydrogen bonding frequently occurs in organic compounds and results in the cyclization (six or five-membered ring) of the molecule.
Explanation:
- o-nitrophenol has intramolecular hydrogen bonding so it is more volatile.
- So, the statement I is true.
- The lowest melting point of o-isomer is due to intramolecular hydrogen bonding whereas meta and para isomers possess intermolecular hydrogen bonding and thus, they have higher melting points.
- Thus statement II is false.
Correct Answer: (3)
Hydrogen Bonding Question 5:
NH3 has a much higher boiling point than PH3 because
Answer (Detailed Solution Below)
Hydrogen Bonding Question 5 Detailed Solution
Concept:
Hydrogen bonding:
- It is the electrostatic attraction between hydrogen atoms bonded to small, strongly electronegative atoms (N, O, and F).
- The bonding occurs through the lone pair of electrons on the electronegative atoms.
- Example: HF, H2O, etc.
2 Types of Hydrogen bonding:- Intermolecular and Intramolecular H-bonding.
- Intermolecular: Hydrogen bond formed between 2 molecules.
- Intramolecular: Hydrogen bond formed between two different atoms of the same molecule.
- Intermolecular Hydrogen bonding is stronger than van der waals' forces.
The essential requirement of Hydrogen bonding:
1. An H atom must be directly bonded to a highly electronegative atom.
2. Lone pair of electrons must be present on the electronegative atom.
Factors affecting Hydrogen bonding:
1. Association
Due to intermolecular H-bonding, carboxylic acid exists as dimers even in the vapor state.
2. Higher Boiling and Melting point
- Compounds having H-bonding requires larger energy to separate the molecules before they can melt or boil.
- So, the compounds containing H-bonds have high melting and boiling points.
3. Physical state
Explanation:
The difference in characteristics between NH3 and PH3 is given below:-
NH3 | PH3 |
Polar molecule | Non-polar molecule |
Have a large electronegativity difference between N and H. Eg:- N=3.01 and H=2.2 |
Have no electronegativity difference between P and H. Eg:- P=2.19 and H=2.2 |
Can form hydrogen bonding with the neighboring NH3 molecules. |
Doesn't form hydrogen bonding. |
The stronger hydrogen bonding makes it difficult to break the bonds between N and H atoms. |
Have weak dispersion force.
|
Have a higher boiling and melting point. |
Have low boiling and melting point. |
- Due to the lesser electronegativity of PH3 molecules, they cannot form H-bonding.
- PH3 can H-bond with water only but not with itself.
- Although PH3 is larger than NH3 with greater dispersion forces, NH3 has a higher polar N--H bond which gives rise to H-bonding.
- Since the strength of the H-bond is greater than the dispersion forces, the boiling point of NH3 is greater.
The hydrogen bonding in NH3 is shown below:
Hence, NH3 has a much higher boiling point than PH3 because NH3 forms hydrogen bond.