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The larger the difference in electronegativities of bonded atoms the larger the dipole.
What has a net dipole moment. Dipole moments tell us about the charge separation in a molecule. While it may seem counterintuitive molecules may possess dipole moments yet entire molecules may still maintain no net dipole moment. In tetra-atomic boron trihydride BH3 the dipole moment is zero but that of ammonia NH3 is 149D.
The condition when a molecule has net dipole moment equal to zero. We expect the concentration of negative charge to be on the oxygen the more electronegative atom and positive charge on the two hydrogens. 1 μ Q r.
Oxygen has a stronger pull on the electron in the bond betweem S and O the result is a dipole moment which can be seem more easily using vectors. If there are two. Dipole moment μ is the measure of net molecular polarity which is the magnitude of the charge Q at either end of the molecular dipole times the distance r between the charges.
Using the equation above the dipole moment is calculated to be 185 D by multiplying the distance between the oxygen and hydrogen atoms by the charge difference between them and then finding the components of each that point in the direction of the net dipole moment the angle of the molecule is 1045. As the molecule is linear both the bond dipoles cancel each other out ie. However for b as both vectors are pointing in the same direction it has a net dipole charge.
It depends on the geometry of molecule. As the 3 bonds are in a single plane dipole moments cancel each other with net dipole moment equal to zero. They have equal and opposite dipole moment which gives them net zero dipole moment.
The net dipole moment is the vector sum of the dipole moments of the individual bonds in a molecule. Net dipole moment is simply sum of all dipole moments in molecule. Hence it possesses a net dipole moment.
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