Hydrogen Bonding MCQ Quiz in मल्याळम - Objective Question with Answer for Hydrogen Bonding - സൗജന്യ PDF ഡൗൺലോഡ് ചെയ്യുക

Last updated on Apr 11, 2025

നേടുക Hydrogen Bonding ഉത്തരങ്ങളും വിശദമായ പരിഹാരങ്ങളുമുള്ള മൾട്ടിപ്പിൾ ചോയ്സ് ചോദ്യങ്ങൾ (MCQ ക്വിസ്). ഇവ സൗജന്യമായി ഡൗൺലോഡ് ചെയ്യുക Hydrogen Bonding MCQ ക്വിസ് പിഡിഎഫ്, ബാങ്കിംഗ്, എസ്എസ്‌സി, റെയിൽവേ, യുപിഎസ്‌സി, സ്റ്റേറ്റ് പിഎസ്‌സി തുടങ്ങിയ നിങ്ങളുടെ വരാനിരിക്കുന്ന പരീക്ഷകൾക്കായി തയ്യാറെടുക്കുക

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

  1. NH3 has a largest molecular weight
  2. NHundergoes umbrella inversion
  3. NHforms hydrogen bond
  4. NHcontains ionic whereas PH3 contains covalent bonds
  5. None of the above/More than one of the above.

Answer (Detailed Solution Below)

Option 3 : NHforms hydrogen bond

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 NHforms hydrogen bond.

Hydrogen Bonding Question 2:

In which of the following substances will hydrogen bond be strongest?

  1. HCl
  2. H2O
  3. HI
  4. H2S
  5. Not Attempted

Answer (Detailed Solution Below)

Option 2 : H2O

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 -

  1. Intermolecular H-bonding
  2. 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?

  1. HCl
  2. H2O
  3. HI
  4. More than one of the above
  5. None of the above

Answer (Detailed Solution Below)

Option 2 : H2O

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 -

  1. Intermolecular H-bonding
  2. 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 :

  1.  Both Statement I and Statement II are true
  2. Both Statement I and Statement II are false
  3. Statement I is true but Statement Il is false
  4. Statement I is false but Statement II is true
  5. Not Attempted

Answer (Detailed Solution Below)

Option 3 : Statement I is true but Statement Il is false

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

  1. NH3 has a largest molecular weight
  2. NHundergoes umbrella inversion
  3. NHforms hydrogen bond
  4. NHcontains ionic whereas PH3 contains covalent bonds
  5. Not Attempted

Answer (Detailed Solution Below)

Option 3 : NHforms hydrogen bond

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 NHforms hydrogen bond.

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