Yeah, I know... pons asinorum Polar covalent bonding/dipole moment: If mu=Qr, where Q is the charge and r is the separation of charges, does it follow that as bond length increases that the dipole moment (mu) would increase in magnitude for the same charge? I do not understand this... If separation of charge refers to the slight neg. and slight pos. charge on say, an H and a Cl, respectively, then the more tightly bonded the molecule, the lower the "r" would be. It seems counter intuitive... Suppose you have HCl and you want the dipole moment, aren't you contemplating the amount of charge incurred on H or Cl atom multiplied by the bond length? That is to say, H polarizes and Cl polarizes, then a polar covalent bond is formed.