I2 and CCl4 are symmetrical molecule, their dipole moment is zero, while ICl, PCl3 And POCl3 will exhibit dipole moment.
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I2 and CCl4 are symmetrical molecule, their dipole moment is zero, while ICl, PCl3 And POCl3 will exhibit dipole moment.
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CH4, CF4 (both tetrahedral), and CO2 (linear) are symmetrical molecules. Their dipole moment is zero. Since fluorine is more electronegative than oxygen, the dipole moment of CH3F is higher that of CH3OH. Thus, among CH3OH, CH4 CO2 and CH3F, CH3F has the largest dipole moment.
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Both NH3 and NF3 have sp3 hybridization and trigonal pyramidal shape.
Fluorine has
more electronegative than nitrogen but NH3 has more dipole moment
than NF3. In NH3, Nitrogen is
more electronegative than Hydrogen. So Nitrogen pulls the electrons from Hydrogen
towards itself and so, the direction of moment due to the N-H bonds is in the
same direction as that of the lone pair of electrons on Nitrogen. Hence here
additive effect appears while in case of NF3, Fluorine is more
electronegative than Nitrogen. So fluorine pulls electrons from nitrogen
towards itself so that direction of
moment due to N-F bonds is in the opposite direction as the lone pair of
electron on nitrogen atom. Hence it is clear dipole moment of NH3 is
more than NF3.
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Both NH3 and
NF3 have sp3 hybridization and trigonal pyramidal shape.
Fluorine has more electronegative than nitrogen but NH3 has more dipole moment than NF3. In NH3, Nitrogen is more electronegative than Hydrogen. So Nitrogen pulls the electrons from Hydrogen towards itself and so, the direction of moment due to the N-H bonds is in the same direction as that of the lone pair of electrons on Nitrogen. Hence here additive effect appears while in case of NF3, Fluorine is more electronegative than Nitrogen. So fluorine pulls electrons from nitrogen towards itself so that direction of moment due to N-F bonds is in the opposite direction as the lone pair of electron on nitrogen atom. Hence it is clear dipole moment of NH3 is more than NF3.
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Both
Fluorine has
more electronegative than nitrogen but NH3 has more dipole moment
than NF3. In NH3, Nitrogen is
more electronegative than Hydrogen. So Nitrogen pulls the electrons from Hydrogen
towards itself and so, the direction of moment due to the N-H bonds is in the
same direction as that of the lone pair of electrons on Nitrogen. Hence here
additive effect appears while in case of NF3, Fluorine is more
electronegative than Nitrogen. So fluorine pulls electrons from nitrogen
towards itself so that direction of
moment due to N-F bonds is in the opposite direction as the lone pair of
electron on nitrogen atom. Hence it is clear dipole moment of NH3 is
more than NF3.
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Both
Fluorine has more electronegative than nitrogen but NH3 has more dipole moment than NF3. In NH3, Nitrogen is more electronegative than Hydrogen. So Nitrogen pulls the electrons from Hydrogen towards itself and so, the direction of moment due to the N-H bonds is in the same direction as that of the lone pair of electrons on Nitrogen. Hence here additive effect appears while in case of NF3, Fluorine is more electronegative than Nitrogen. So fluorine pulls electrons from nitrogen towards itself so that direction of moment due to N-F bonds is in the opposite direction as the lone pair of electron on nitrogen atom. Hence it is clear dipole moment of NH3 is more than NF3.
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Let’s draw the structure of both two compounds and then analyses it.
In both H2O and F2O the structure is quite the
same. In H2O as O is more electronegative
than hydrogen so the resultant bond dipole is towards O, which means both the
lone pair and bond pair dipole are acting in the same direction and dipole
moment of H2O is high. In case of F2O the bond dipole is acting towards fluorine, so in F2O the lone pair and bond pair dipole are acting in opposition
resulting in a low dipole.
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Both CCl4 & CHCl3 have tetrahedral structure but CCl4 is symmetrical while CHCl3 is non-symmetrical.
Due to the symmetric.al structure of CCl4 the resultant of bond dipoles comes out to be zero. But in case of CHCl3 it is not possible as the presence of hydrogen introduces some dissymmetry.
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The structure of CO2is this is a highly symmetrical structure with a plane of symmetry passing through the carbon. The bond dipole of C–O is directed towards oxygen as it is the negative end. Here two equal dipoles acting in opposite direction cancel each other and therefore the dipole moment is zero.
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Since C-Cl bond is longer than C-F bond, thus it is compensates the lower electronegativity factor of chlorine. Hence dipole moment of chloromethane is more than fluoromethane.
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