Home
Class 12
CHEMISTRY
It is a common observation that many com...

It is a common observation that many compounds containing hydrogen attached to highly electronegative elements such as oxygen, nitrogen, or fluorine, often exhibit unexpected properties, such as relatively high melting points, boiling points, viscosity, solubility in water etc Such an unexpected behaviour can be explained on the basis of hydrogen bonding. When a hydrogen atom is attached to a highly electronegative element of small size such as F. N, 0. etc. the electronegative atoms strongly attracts the shared pair of electrons towards it self. As a result, the hydrogen atom becomes slightly positive and the electronegative element becomes slightly negative when two molecules of such a substance say HF come close to each other, the negatively charged fluorine atom of one molecule attracts the positively charged hydrogen atom of the other molecule. A hydrogen atom, thus links to highly electronegative atoms, one by a strong covalent bond and the other by weak electrostatic attraction as shown ahead `overset(delta+)H-overset(delta-)F....overset(delta+)H-overset(delta-)F`, the dotted line represents a hydrogen bond.
`NH_3` has much higher boiling point than `PH_3` because

A

`NH_3` has larger molecular mass

B

`NH_3` undergoes umbrella mass

C

`NH_3` forms hydrogen bond

D

`NH_3` contains ionic bonds whereas `PH_3` contain covalent bonds

Text Solution

Verified by Experts

The correct Answer is:
C
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    DINESH PUBLICATION|Exercise Matrix Match|4 Videos

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    DINESH PUBLICATION|Exercise Integer|4 Videos

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    DINESH PUBLICATION|Exercise REVISION|279 Videos

  • CARBOXYLIC ACIDS

    DINESH PUBLICATION|Exercise BRAIN STORMING MULTIPLE CHOICE QUESTIONS (MCQS)|13 Videos

  • CHEMICAL KINETICS

    DINESH PUBLICATION|Exercise Additional Numerical Problems For Practice|16 Videos

Similar Questions

Explore conceptually related problems

It is a common observation that many compounds containing hydrogen attached to highly electronegative elements such as oxygen, nitrogen, or fluorine, often exhibit unexpected properties, such as relatively high melting points, boiling points, viscosity, solubility in water etc Such an unexpected behaviour can be explained on the basis of hydrogen bonding. When a hydrogen atom is attached to a highly electronegative element of small size such as F. N, 0. etc. the electronegative atoms strongly attracts the shared pair of electrons towards it self. As a result, the hydrogen atom becomes slightly positive and the electronegative element becomes slightly negative when two molecules of such a substance say HF come close to each other, the negatively charged fluorine atom of one molecule attracts the positively charged hydrogen atom of the other molecule. A hydrogen atom, thus links to highly electronegative atoms, one by a strong covalent bond and the other by weak electrostatic attraction as shown ahead overset(delta+)H-overset(delta-)F....overset(delta+)H-overset(delta-)F , the dotted line represents a hydrogen bond. The molecular containing hydrogen bond is

It is a common observation that many compounds containing hydrogen attached to highly electronegative elements such as oxygen, nitrogen, or fluorine, often exhibit unexpected properties, such as relatively high melting points, boiling points, viscosity, solubility in water etc Such an unexpected behaviour can be explained on the basis of hydrogen bonding. When a hydrogen atom is attached to a highly electronegative element of small size such as F. N, 0. etc. the electronegative atoms strongly attracts the shared pair of electrons towards it self. As a result, the hydrogen atom becomes slightly positive and the electronegative element becomes slightly negative when two molecules of such a substance say HF come close to each other, the negatively charged fluorine atom of one molecule attracts the positively charged hydrogen atom of the other molecule. A hydrogen atom, thus links to highly electronegative atoms, one by a strong covalent bond and the other by weak electrostatic attraction as shown ahead overset(delta+)H-overset(delta-)F....overset(delta+)H-overset(delta-)F , the dotted line represents a hydrogen bond. Hydrogen bond is strongest in

It is a common observation that many compounds containing hydrogen attached to highly electronegative elements such as oxygen, nitrogen, or fluorine, often exhibit unexpected properties, such as relatively high melting points, boiling points, viscosity, solubility in water etc Such an unexpected behaviour can be explained on the basis of hydrogen bonding. When a hydrogen atom is attached to a highly electronegative element of small size such as F. N, 0. etc. the electronegative atoms strongly attracts the shared pair of electrons towards it self. As a result, the hydrogen atom becomes slightly positive and the electronegative element becomes slightly negative when two molecules of such a substance say HF come close to each other, the negatively charged fluorine atom of one molecule attracts the positively charged hydrogen atom of the other molecule. A hydrogen atom, thus links to highly electronegative atoms, one by a strong covalent bond and the other by weak electrostatic attraction as shown ahead overset(delta+)H-overset(delta-)F....overset(delta+)H-overset(delta-)F , the dotted line represents a hydrogen bond. Hydrogen bonding is maximum in

It is a common observation that many compounds containing hydrogen attached to highly electronegative elements such as oxygen, nitrogen, or fluorine, often exhibit unexpected properties, such as relatively high melting points, boiling points, viscosity, solubility in water etc Such an unexpected behaviour can be explained on the basis of hydrogen bonding. When a hydrogen atom is attached to a highly electronegative element of small size such as F. N, 0. etc. the electronegative atoms strongly attracts the shared pair of electrons towards it self. As a result, the hydrogen atom becomes slightly positive and the electronegative element becomes slightly negative when two molecules of such a substance say HF come close to each other, the negatively charged fluorine atom of one molecule attracts the positively charged hydrogen atom of the other molecule. A hydrogen atom, thus links to highly electronegative atoms, one by a strong covalent bond and the other by weak electrostatic attraction as shown ahead overset(delta+)H-overset(delta-)F....overset(delta+)H-overset(delta-)F , the dotted line represents a hydrogen bond. Hydrgen bonding is not present in

It is a common observation that many compounds containing hydrogen attached to highly electronegative elements such as oxygen, nitrogen, or fluorine, often exhibit unexpected properties, such as relatively high melting points, boiling points, viscosity, solubility in water etc Such an unexpected behaviour can be explained on the basis of hydrogen bonding. When a hydrogen atom is attached to a highly electronegative element of small size such as F. N, 0. etc. the electronegative atoms strongly attracts the shared pair of electrons towards it self. As a result, the hydrogen atom becomes slightly positive and the electronegative element becomes slightly negative when two molecules of such a substance say HF come close to each other, the negatively charged fluorine atom of one molecule attracts the positively charged hydrogen atom of the other molecule. A hydrogen atom, thus links to highly electronegative atoms, one by a strong covalent bond and the other by weak electrostatic attraction as shown ahead overset(delta+)H-overset(delta-)F....overset(delta+)H-overset(delta-)F , the dotted line represents a hydrogen bond. The boiling point of p-nitrophenol is higher than that of o-nitrophenol because

It is a common observation that many compounds containing hydrogen attached to highly electronegative elements such as oxygen, nitrogen, or fluorine, often exhibit unexpected properties, such as relatively high melting points, boiling points, viscosity, solubility in water etc Such an unexpected behaviour can be explained on the basis of hydrogen bonding. When a hydrogen atom is attached to a highly electronegative element of small size such as F. N, 0. etc. the electronegative atoms strongly attracts the shared pair of electrons towards it self. As a result, the hydrogen atom becomes slightly positive and the electronegative element becomes slightly negative when two molecules of such a substance say HF come close to each other, the negatively charged fluorine atom of one molecule attracts the positively charged hydrogen atom of the other molecule. A hydrogen atom, thus links to highly electronegative atoms, one by a strong covalent bond and the other by weak electrostatic attraction as shown ahead overset(delta+)H-overset(delta-)F....overset(delta+)H-overset(delta-)F , the dotted line represents a hydrogen bond. High density of water as compared to ice is due to

The second most highly electronegative elements in the periodic table is

In which compound hydrogen is electronegative-

Knowledge Check

  • It is a common observation that many compounds containing hydrogen attached to highly electronegative elements such as oxygen, nitrogen, or fluorine, often exhibit unexpected properties, such as relatively high melting points, boiling points, viscosity, solubility in water etc Such an unexpected behaviour can be explained on the basis of hydrogen bonding. When a hydrogen atom is attached to a highly electronegative element of small size such as F. N, 0. etc. the electronegative atoms strongly attracts the shared pair of electrons towards it self. As a result, the hydrogen atom becomes slightly positive and the electronegative element becomes slightly negative when two molecules of such a substance say HF come close to each other, the negatively charged fluorine atom of one molecule attracts the positively charged hydrogen atom of the other molecule. A hydrogen atom, thus links to highly electronegative atoms, one by a strong covalent bond and the other by weak electrostatic attraction as shown ahead overset(delta+)H-overset(delta-)F....overset(delta+)H-overset(delta-)F , the dotted line represents a hydrogen bond. The molecular containing hydrogen bond is

    A
    HI
    B
    `CuSO_4 . 5H_2O`
    C
    HF
    D
    All of these

  • It is a common observation that many compounds containing hydrogen attached to highly electronegative elements such as oxygen, nitrogen, or fluorine, often exhibit unexpected properties, such as relatively high melting points, boiling points, viscosity, solubility in water etc Such an unexpected behaviour can be explained on the basis of hydrogen bonding. When a hydrogen atom is attached to a highly electronegative element of small size such as F. N, 0. etc. the electronegative atoms strongly attracts the shared pair of electrons towards it self. As a result, the hydrogen atom becomes slightly positive and the electronegative element becomes slightly negative when two molecules of such a substance say HF come close to each other, the negatively charged fluorine atom of one molecule attracts the positively charged hydrogen atom of the other molecule. A hydrogen atom, thus links to highly electronegative atoms, one by a strong covalent bond and the other by weak electrostatic attraction as shown ahead overset(delta+)H-overset(delta-)F....overset(delta+)H-overset(delta-)F , the dotted line represents a hydrogen bond. Hydrogen bond is strongest in

    A
    F-HO
    B
    F-HF
    C
    O-HS
    D
    O-HN

  • It is a common observation that many compounds containing hydrogen attached to highly electronegative elements such as oxygen, nitrogen, or fluorine, often exhibit unexpected properties, such as relatively high melting points, boiling points, viscosity, solubility in water etc Such an unexpected behaviour can be explained on the basis of hydrogen bonding. When a hydrogen atom is attached to a highly electronegative element of small size such as F. N, 0. etc. the electronegative atoms strongly attracts the shared pair of electrons towards it self. As a result, the hydrogen atom becomes slightly positive and the electronegative element becomes slightly negative when two molecules of such a substance say HF come close to each other, the negatively charged fluorine atom of one molecule attracts the positively charged hydrogen atom of the other molecule. A hydrogen atom, thus links to highly electronegative atoms, one by a strong covalent bond and the other by weak electrostatic attraction as shown ahead overset(delta+)H-overset(delta-)F....overset(delta+)H-overset(delta-)F , the dotted line represents a hydrogen bond. Hydrogen bonding is maximum in

    A
    ethyl chloride
    B
    triethylamine
    C
    ethanol
    D
    diethyl ether.
    • DINESH PUBLICATION-CHEMICAL BONDING AND MOLECULAR STRUCTURE-Comprehension M.C.Q
    1. It is a common observation that many compounds containing hydrogen att...

      Text Solution

      |

    2. It is a common observation that many compounds containing hydrogen att...

      Text Solution

      |

    3. It is a common observation that many compounds containing hydrogen att...

      Text Solution

      |

    4. It is a common observation that many compounds containing hydrogen att...

      Text Solution

      |

    5. It is a common observation that many compounds containing hydrogen att...

      Text Solution

      |

    6. It is a common observation that many compounds containing hydrogen att...

      Text Solution

      |

    7. It is a common observation that many compounds containing hydrogen att...

      Text Solution

      |

    8. It is a common observation that many compounds containing hydrogen att...

      Text Solution

      |

    9. It is a common observation that many compounds containing hydrogen att...

      Text Solution

      |

    10. Atomic orbitals of bonded atoms combine to form molecular orbitals. Th...

      Text Solution

      |

    11. Atomic orbitals of bonded atoms combine to form molecular orbitals. Th...

      Text Solution

      |

    12. Atomic orbitals of bonded atoms combine to form molecular orbitals. Th...

      Text Solution

      |

    13. Atomic orbitals of bonded atoms combine to form molecular orbitals. Th...

      Text Solution

      |

    14. Atomic orbitals of bonded atoms combine to form molecular orbitals. Th...

      Text Solution

      |

    15. Atomic orbitals of bonded atoms combine to form molecular orbitals. Th...

      Text Solution

      |

    16. Atomic orbitals of bonded atoms combine to form molecular orbitals. Th...

      Text Solution

      |

    17. A polar covalent bond with positive and negative charge centres at its...

      Text Solution

      |

    18. A polar covalent bond with positive and negative charge centres at its...

      Text Solution

      |

    19. A polar covalent bond with positive and negative charge centres at its...

      Text Solution

      |

    20. A polar covalent bond with positive and negative charge centres at its...

      Text Solution

      |