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A diatomic molecule has a dipole moment ...

A diatomic molecule has a dipole moment 1.2D. If the internuclear distance is `1A^@`, what is the fraction of charge exists on each atom?

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The correct Answer is:
0.25
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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?

The dipole moment of HX molecule is 1.92 D and bond distance is 1.2 A'. What is the percentage ionic character of HX ?

A: Water molecule has zero dipole moment R: In water molecule dipole moment of the two O-H bonds cancel each other.

In a planar tetraatomic molecule, AB_(3) , A is at the centroid of the equilateral triangle formed by the atoms, B. If the A-B bond distance is 1Å , what is the distance between the centres of any two B atoms?

If a molecule MX_(3) has zero dipole moment the sigma bonding orbitals used by (atomic numer lt 21 ) are

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?

If the bond length and dipole moment of a diatomic molecule are 1.25 A^(@) and 1.0 D respectively, what is the percent ionic character of the bond ?

AAKASH SERIES-CHEMICAL BONDING-SUBJECTIVE EXERCISE -3 (Very Short answer questions)
  1. What types of bonds are present in NH4 CI? Write its structure.

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  2. Define hydrogen bond. Is it weaker or stronger than vander Waals force...

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  3. Give reasons for the higher bioling point of H2 O than HF and NH3

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  4. Why o - Nitrophenol is more volatile than p - Nitrophenol.

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  5. Why HCI cannot form hydrogen bond.

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  6. Water is a liquid at room temperature, but not hydrogen sulphide. Why?

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  7. What are the types of bonds present in H3 O^+ and NH(4)^(+)?

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  8. Write any two properties of compounds with dative bond.

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  9. What is bond length? Discuss different factors influencing bond length...

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  10. Distinguish between bond enthalpy and dissociation enthalpy.

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  11. Compare carbon -carbon bond lengths and bond energies by taking ethane...

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  12. What isbond angel? What are the different aspects influence bond angle...

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  13. What are non-polar and polar covalent bonds? Give examples.

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  14. What is dipolemoment? How is it calculated?

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  15. Write the SI unit of dipolement.

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  16. BF3 is non-polar but NH3 is polar. Why?

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  17. Write two applications of dipolemoment.

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  18. cis-1,2-Dehloroethene is polar, but tans-1. 2-dichloroethane is non ...

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

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  20. Dipole moment of HCl is 1.03D. Bond length is 1.27A^@. Calculate the p...

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