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The dipole moment of BF(3) is zero becau...

The dipole moment of `BF_(3)` is zero because

A

The electronegativity difference between boron and fluorine molecule

B

It is a covalent molecule

C

It is a tetra atomic molecule

D

It is having trigonal planar geometry.

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Verified by Experts

The correct Answer is:
D
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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 The dipole moment of NF_(3) is very much less than that of NH_(3) 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

(A): The dipole moment value of NH_3 is greater than zero (B): In NH_3 bond angle is approximately 104^@

A: SO_(2) molecule has unsymmetrical shape R: The dipole moment of SO_(2) molcule is equal to zero.

The electronegativity difference between N and F is greater than that between N and H yet the dipole moment of NH_(3) (1.5 D) is larger than that of NF_(3) (0.2D) This is because

Dipole moment of CO_(2) is zero and which implies that

Define the dipole moment. Why the BF_3 molecule dipole moment is zero?

Why is dipole moment of CO_(2)' BF_(3), CCl_(4) is zero?

AAKASH SERIES-CHEMICAL BONDING-OBJECTIVE EXERCISE -2(DIPOLE MOMENT )
  1. Dipole moment of H2 X is 1.0 D. If the bond angle is 90^@, the approxi...

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  2. The dipoleoment of HX is 1.2D. If the % ionic character of the bond is...

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  3. Which bond angle theta would result in the maximum dipolemoment for th...

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  4. From the following dipole moment (in Debye) values of methyl halides, ...

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  5. A: Water molecule has zero dipole moment R: In water molecule dipole ...

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  6. The dipole moment of BF(3) is zero because

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  7. If a molecule MX(3) has zero dipole moment the sigma bonding orbitals ...

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  8. Bent molecule having dipole moment among the following

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  9. Which one of the following mu=0

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  10. The difference of electronegativity between X and Y is 2. If X and Y f...

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  11. Arrange in the order of increassing dipole moment I. toluene II. m...

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  12. Whcin bond is most polar?

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  13. The dipoleoment of HX is 1.2D. If the % ionic character of the bond is...

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  14. The following are some statements about dipole moment. i. The dipole...

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  15. Which of the following is more stable

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  16. For which of the following molecule significat mu!=0?

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  17. The table shown lists the bond dissociation energies (E("diss")) for s...

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  18. The number and type of bonds between two carbon atoms in CaC(2) are

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  19. From the following give statements of the order of dipolemoments. (i...

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  20. KF combines with HF to form KHF(2). The compound contains the species

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