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Write the significance/applications of dipole moment. |
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Answer» Solution :In determining the POLARITY of bond As `mu = a xx d` obviously greater the magnitude of dipole moment the polarity of bond will be more. For one polar bond A - B TYPE molecule. H - F `gt H - Cl gt H - Br gt H - I and " if" mu = 0 ` then `mu= 1.78` D, HCL `mu` = 1.07 , H - Br = 13.79 D, H- I = 0.38 D molecule is non polar. e.g. `O_(2), N_(2), F_(2),Cl_(2), Br_(2), Z_(1), H_(1) ` etc. `BeF_(2) , CO_(2), BeCl_(2)` forsuch molecule `mu` = 0 so they are linear do, but `H_(2)`O. `SO_(2) mu ne 0` So they must have angular shapeSimilarly `BF_(3), CH_(4), "CCl"_(4)` non polar but `NF_(3),NH_(3), CH_(3)Cl` are polar so their shape can be determine. In CALCULATION of ionic or covalent characters : Ionic character`prop` Difference of electronegativity. ln HI, HBr, HCl, HF ionic character increase by using felon rules ionic character can be calculated. To distinguish between cis & trans isomers for cis isomers `mu ne 0` for trans isomer `mu = 0 `. To distinguish between ortho, META and para isomers for paraisomers `mu` = 0 and dipole moment of ortho is greater than meta. |
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