Which of the two will have dipole moment?
`"cis or trans "-C_(2)H_(2)Cl(2)`

Which one of the following has the highest dipole moment? (i) CH_(2)Cl_(2) , (ii) CHCl_(3) , (iii) C Cl_(4)

Which of the following molecules will have zero dipole moment: SiCl_(4), H_(2)O, CO_(2), BF_(3), NH_(3) ?

Sketch the bond moments and resultant dipole moments in cis and trans forms of C_(2)H_(2)Cl_(2)

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 of the following statement is correct regarding C_(2)H_(2)F_(2) molecule?

Which of the following molecule (s) have dipole moment (I) Trans -pent -2-me (II) cis-hex -3-ene (III) 2,2-Dimethy1 propane (IV) 2,2,3,3 tetramethy1 butane .