Why would a HCl molecule have a dipole moment?

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The HCl molecule exhibits a dipole moment due to the difference in electronegativity between hydrogen and chlorine, with chlorine being more electronegative. This results in a partial negative charge on chlorine and a partial positive charge on hydrogen. The dipole moment arises because these charges do not cancel out; instead, they create a vector that points from the positive to the negative charge. The discussion emphasizes the importance of understanding electronegativity values, specifically referencing Pauling's scale. Therefore, the dipole moment is a consequence of the unequal distribution of electron density in the HCl molecule.
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If we have a HCl molecule, then we know that the electronegativity of hydrogen is greater than that of chlorine. So in an electric field, the chlorine will be partially negative and the hydrogen will be partially positive: H: \delta + Cl: \delta -. Then why would this have a dipole moment? Wouldn't the charges cancel each other out?

Thanks :smile:
 
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Look up the definition of dipole moment. It's self-explanatory.
 
And HYDROGEN HAS A SMALLER ELECTRONEGATIVITY THAN CHLORINE...Check a complete periodic table which gives electronegativity & electropositivity (i would follow Pauling's numbers).

Daniel.
 

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