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A polar bond is a covalent bond in which there is a separation of charge between one end and the other - in other words in which one end is slightly positive and the other slightly negative. In the diagram, " " (read as "delta") means "slightly" - so + means "slightly positive". At the same time, the A end (rather short of electrons) becomes slightly positive. That means that the B end of the bond has more than its fair share of electron density and so becomes slightly negative. What happens if B is slightly more electronegative than A?ī will attract the electron pair rather more than A does. This sort of bond could be thought of as being a "pure" covalent bond - where the electrons are shared evenly between the two atoms. The electrons are actually in a molecular orbital, and are moving around all the time within that orbital. Note: It's important to realise that this is an average picture. You will find this sort of bond in, for example, H 2 or Cl 2 molecules. To get a bond like this, A and B would usually have to be the same atom. If the atoms are equally electronegative, both have the same tendency to attract the bonding pair of electrons, and so it will be found on average half way between the two atoms. Each atom may be forming other bonds as well as the one shown - but these are irrelevant to the argument. What happens if two atoms of equal electronegativity bond together?Ĭonsider a bond between two atoms, A and B. Fluorine (the most electronegative element) is assigned a value of 4.0, and values range down to caesium and francium which are the least electronegative at 0.7. The Pauling scale is the most commonly used. If you are interested in electronegativity in an organic chemistry context, you will find a link at the bottom of this page.Įlectronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. It looks at the way that electronegativity differences affect bond type and explains what is meant by polar bonds and polar molecules.
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This page explains what electronegativity is, and how and why it varies around the Periodic Table.