Home
Class 11
CHEMISTRY
The geometry of H(2)S and its dipole mom...

The geometry of `H_(2)S` and its dipole moment are

A

Angular and non-zero

B

Angular and zero

C

Linear and non-zero

D

Linear and zero

Text Solution

Verified by Experts

The correct Answer is:
A
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL BONDING

    AAKASH SERIES|Exercise OBJECTIVE EXERCISE-3|48 Videos

  • CHEMICAL BONDING

    AAKASH SERIES|Exercise EXERCISE ON PASSAGE|16 Videos

  • CHEMICAL BONDING

    AAKASH SERIES|Exercise OBJECTIVE EXERCISE-2A (BOND CHARACTERS)|5 Videos

  • ATOMIC STRUCTURE

    AAKASH SERIES|Exercise OBJECTIVE EXERCISE - 3 (RECENT AIPMT/NEET QUESTIONS)|20 Videos

  • CHEMICAL EQUILIBRIUM

    AAKASH SERIES|Exercise QUESTIONS FOR DESCRIPTIVE ANSWERS|30 Videos

Similar Questions

Explore conceptually related problems

The geometry of H_(3)O^(+) ion is

S.I. unit for dipole moment is

Covalent molecules formed by heteroatoms bound to have some ionic character. The ionic character is due to shifting of the electron pair towards A or B in the molecule AB. Hence, atoms acquire small and equal charge but opposite in sign. Such a bond which has some ionic character is described as polar covalent bond. Polar covalent molecules can exhibit dipole moment. Dipole moment is equal to the product of charge separation, q and the bond length, d for the bond. The unit of dipole moment is Debye. One Debye is equal to 10^(-18) esu cm. Dipole moment is a vector quantity. It has both magnitude and direction. Hence, dipole moment of molecules depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moments help to predict the geometry of the molecules. Dipole moment values can be used to distinguish between cis-and traps-isomers, ortho-, meta-and para-forms of a substance, etc. The percentage of ionic character of a bond can be calculated by the application of the following formula : % " ionic character " = ("Experimental value of dipole moment ")/("Theoretical value of dipole moment ") xx 100 A diatomic molecule has a dipole moment of 1.2 D. If the bond length is 1.0 xx 10^(-8) cm, what fraction of charge does exist on each atom?

Covalent molecules formed by heteroatoms bound to have some ionic character. The ionic character is due to shifting of the electron pair towards A or B in the molecule AB. Hence, atoms acquire small and equal charge but opposite in sign. Such a bond which has some ionic character is described as polar covalent bond. Polar covalent molecules can exhibit dipole moment. Dipole moment is equal to the product of charge separation, q and the bond length, d for the bond. The unit of dipole moment is Debye. One Debye is equal to 10^(-18) esu cm. Dipole moment is a vector quantity. It has both magnitude and direction. Hence, dipole moment of molecules depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moments help to predict the geometry of the molecules. Dipole moment values can be used to distinguish between cis-and traps-isomers, ortho-, meta-and para-forms of a substance, etc. The percentage of ionic character of a bond can be calculated by the application of the following formula : % " ionic character " = ("Experimental value of dipole moment ")/("Theoretical value of dipole moment ") xx 100 Arrange the following compounds in increasing order of dipole moments, toluene (I), o- dichlorobenzene (II), m-dicblorobenzene (III) and p dichlorobenzene (IV) :

Covalent molecules formed by heteroatoms bound to have some ionic character. The ionic character is due to shifting of the electron pair towards A or B in the molecule AB. Hence, atoms acquire small and equal charge but opposite in sign. Such a bond which has some ionic character is described as polar covalent bond. Polar covalent molecules can exhibit dipole moment. Dipole moment is equal to the product of charge separation, q and the bond length, d for the bond. The unit of dipole moment is Debye. One Debye is equal to 10^(-18) esu cm. Dipole moment is a vector quantity. It has both magnitude and direction. Hence, dipole moment of molecules depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moments help to predict the geometry of the molecules. Dipole moment values can be used to distinguish between cis-and traps-isomers, ortho-, meta-and para-forms of a substance, etc. The percentage of ionic character of a bond can be calculated by the application of the following formula : % " ionic character " = ("Experimental value of dipole moment ")/("Theoretical value of dipole moment ") xx 100 The dipole moment of NF_(3) is very much less than that of NH_(3) because :

Covalent molecules formed by heteroatoms bound to have some ionic character. The ionic character is due to shifting of the electron pair towards A or B in the molecule AB. Hence, atoms acquire small and equal charge but opposite in sign. Such a bond which has some ionic character is described as polar covalent bond. Polar covalent molecules can exhibit dipole moment. Dipole moment is equal to the product of charge separation, q and the bond length, d for the bond. The unit of dipole moment is Debye. One Debye is equal to 10^(-18) esu cm. Dipole moment is a vector quantity. It has both magnitude and direction. Hence, dipole moment of molecules depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moments help to predict the geometry of the molecules. Dipole moment values can be used to distinguish between cis-and traps-isomers, ortho-, meta-and para-forms of a substance, etc. The percentage of ionic character of a bond can be calculated by the application of the following formula : % " ionic character " = ("Experimental value of dipole moment ")/("Theoretical value of dipole moment ") xx 100 Which are non-polar molecules?

BeF_2 has zero dipole moment where as H_2 O has a dipole moment because

Identify the correct statements from the following. (1) The dipole moment of CO_(2) and BF_(3) is zero (2) The dipole moment of NF_(3) is higher than the diople moment of NH_(3) (3) The dipole moment of HI is lower than the dipole moment of HCl

No. of compounds having net dipole moment are

AAKASH SERIES-CHEMICAL BONDING-OBJECTIVE EXERCISE-2B
  1. Which of the following will have zero dipole moment?

    Text Solution

    |

  2. The molecules BF3 and NF3 are covalent compounds. But BF3 is non-pol...

    Text Solution

    |

  3. Which of the following has highest dipole moment?

    Text Solution

    |

  4. BeF2 has zero dipole moment where as H2 Ohas a dipole moment because

    Text Solution

    |

  5. Molecule with dipole moment among the following

    Text Solution

    |

  6. Which of the following has highest dipole moment?

    Text Solution

    |

  7. A molecule MX3 has zero dipole moment. The % of's' character in the h...

    Text Solution

    |

  8. A diatomic molecule has a dipole moment 1.2D. If the internuclear dist...

    Text Solution

    |

  9. The C-H bond distance is largest in

    Text Solution

    |

  10. In compounds of type ECl3, where E = B, P, As or Bi, the angles CI-E -...

    Text Solution

    |

  11. The geometry of H(2)S and its dipole moment are

    Text Solution

    |

  12. In O(2), H(2)O(2) and O(3) the correct order of oxygen -oxygen bond le...

    Text Solution

    |

  13. The correct order of bond lengths is

    Text Solution

    |

  14. Bone energy is least in the following

    Text Solution

    |

  15. Which of the following statements is incorrect ?

    Text Solution

    |

  16. Bond length of H2 is 0.074nm, Bond length of Cl2 is 1.98A^@. Bond leng...

    Text Solution

    |

  17. Average C-H energy is 416 KJ.mol^(-1) Which of the following is correc...

    Text Solution

    |

  18. The decreasing order of bond dissociation energies of C-C, C-H and H-H...

    Text Solution

    |

  19. The highest dipolemoment is of

    Text Solution

    |

  20. The correct order of N-O bond length in No, NO(2)^(-) and NO(3)^(-) wi...

    Text Solution

    |