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The former relates qualitatively to uneven share of charge density between two bonded atoms. The latter is a quantitative measure of this.
Explanation:
Bond dipole relates to separation of electronic charge betweeen two atoms bonded together. If they are identical then there is no separation of charge - the electron cloud is "evenly shared" between the two atoms. In such a case there is no dipole. If, however, one atoms is very electronegative, and the other one isn't, then the electronegative atom tends to "pull" electron cloud density towards itself, accumulating a partial negative charge, and the other atom receives an unevenly low share of electron density, and a partial positive charge. This bond is then said to have a bond dipole.
Classic examples of bond dipoles are those containing the most electronegative elements, oxygen, nitrogen and halogens (H-Cl, the -OH group, -NH group).
Dipole moment is the product of the separation of the ends of a dipole and the size of the partial charges. The units are "coulomb-metre" but because bond dipole moments are generally small, they are generally measured in debye units (D). 1 debye relates to an electron and a proton separated by 0.208 Angstroms. Alternatively 1 coulomb metre is 2.9979 ×
10
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CintiaSalazar

Taking into account their definitions, the relationship between the bond dipoles and molecule dipole is that the polarity is characteristic of each bond and is due to the difference of  electronegativity between the bonded atoms, while the sum of all the polarities of the bonds in the molecule results in the polarity of the molecule.

The polarity of a chemical bond occurs when there is an asymmetric distribution of the electron cloud of the bond around the two atoms that form said bond. This happens when both atoms have different electronegativity. In other words, the polarity is characteristic of each bond and is due to the difference in electronegativity between the bonded atoms.

On the other hand, to determine the polarity of the molecules, you must take into account the difference in electronegativity of the bonds and the geometry, to determine if the dipole moments cancel out or not due to the geometric arrangement of the bonds.

Finally, the relationship between the bond dipoles and molecule dipole is that the polarity is characteristic of each bond and is due to the difference of  electronegativity between the bonded atoms, while the sum of all the polarities of the bonds in the molecule results in the polarity of the molecule.

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