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All molecules with polar bonds have dipo...

All molecules with polar bonds have dipole moment.

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The correct Answer is:
F
The resultant of individual bond dipoles may or may not be non-zero.
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Assertion : All diatomic molecules with polar bond have dipole moment. Reason : Dipole moment is a vector quantity.

Assertion : All diatomic molecules with polar bond have dipole moment. Reason : Dipole moment is a vector quantity.

Statement 1 : All molecules with polar bonds may not have dipole moments Statement 2 : Dipole moment is a vectot quantity and bond dipoles may cancel out.

Which of the following molecules will have polar bonds but zero dipole moment?

Which of the following molecules will have polar bonds but zero dipole moment ?

The molecule (s) that will have dipole moment is/are:

Which of the following molecules does not have net dipole moment?

The molecule which does not exhibit net dipole moment is

The measure of net molecular polarity is a quantity called dipole moment which is defined as the magnitude of the charge Q at either end of the molecular dipole times the distance 'r' between the charge : mu=Qxxr Molecular polarities give rise to some of the forces that occur between molecules.Such forces are termed as intermolecular forces.These molecular forces are of several different types including dipole-dipole forces, London dispersion forces, hydrogen bonds and ion-dipole forces (operate between ions and molecules).These intermolecular forces are electrical in origin and results from the mutual attraction of unlike charges or the mutual repulsion of like charges. A formal positive charge on the central atom affect the size of orbitals.A formal positive charge on central atom will pull in all electrons towards the nucleus and this will leads to the contraction in size of orbitals. Which of the following molecule does not have dipole moment ?

Polar covalent molecules exhibit dipole moment. Dipole moment is equal to the product of charge separation , q and the bond length d for the bond. Unit of dipole moment is debye. One debye is equal to 10^(-18) esu cm. Dipole moments is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule 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 moment helps to predict the geometry of a molecules. Dipole moment values can be distinguish between cis- and trans- isomers, ortho, meta and pare-forms of a substance, etc. Q. Which is a polar molecule?

VMC MODULES ENGLISH-CHEMICAL BONDING-I & II-JEE Advanced (Archive)
  1. The dipole moment of KCI is 3.36 xx 10^(-29)Cm The interatomic distanc...

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  2. The two types of bonds pressent in B(2)H(6) are covalent and .

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  3. All molecules with polar bonds have dipole moment.

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  4. Explain the difference in the nature of bonding in LiF and LiI .

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  5. Among the following species identify the isostructural pairs NH(3), NO...

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  6. Which of the following molecules is planar ? .

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  7. The number and type of bonds between two carbon atoms in C(2) are:

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  8. Fill in the blanks by chossing the appropriate word/words from those g...

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  9. Among N(2)O,SO(2),I(3)^(o+) and I(3)^(Theta) the linear species are an...

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  10. Which one of the following compounds has sp^(2) hybridisation ? .

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  11. Among KO(2) , AlO(2)^(+) , BaO(2) and NO(2)^(+) unpaired electron is p...

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  12. CN^(Theta) and N(2) are isoelectronic But in contrast to CN^(Theta),N(...

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  13. Which contains both polar and non-polar bonds ? .

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  14. Assertion (A) : LiCl is predominantly a covalent compound. Reason (R...

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  15. Statement I: The electronic structure of O(3) is : Statement II...

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  16. Explain the non-linear shape of H(2)S and non-planar shape of PCl(3) u...

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  17. Using the VSEPR theory, identify the type of hybridization and draw th...

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  18. The geometry and the type of hybrid orbital present about the central ...

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  19. In compounds of type ECl(3), where E=B,P. As or Bi, the angles Cl-E-Cl...

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  20. The corrrect order of C-O bond length among CO, CO3^(2-), CO2 is

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