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Polarity
4.2.8 - Predict whether or not a molecule is polar from its molecular shape and bond polarities
Electronegativity
The ability of an atom in a molecule to attract electrons to itself
You can measure how polar a molecule is based on the difference in the electronegativities of the
constituent elements.
Based on its relative position on the periodic table, you can estimate the electronegativity of an
element. The arrows below show increasing electronegativity.
For example, if we look at OH:
We can see that oxygen has the higher electronegativity. Although it is one period lower, it is 15
groups to the right, which means that it is higher. So, as a molecule, OH would look like this:
OH is therefore a polar molecule. Since electrons actually exist in a probability cloud, it would
appear more like this:
When looking at molecules with more atoms, it is possible for the dipoles to be cancelled out
In the majority of cases, any molecule that is completely symmetrical will have cancelled dipoles.
This means that CH4, and many others, are non-polar molecules, even though the constituent
elements have different electronegativities.
Remember that the diatomic molecules (C2, H2, I2, N2, F2, O2, Br2) are also non-polar, since they are
symmetrical. This explains why they exist as gases.
Be careful to make sure that a molecule is really symmetrical. HCN, for example, is linear, but is polar
because it has different elements, with different electronegativities, on either side. CO2, on the other
hand, is non-polar, because the same element is found on each side.
Ionic bonds form when the electronegativity of one atom is so strong that it completely removes the
electron(s) from the other one altogether.
Each element has an assigned numerical value for their electronegativity. Therefore, we can
calculate the difference between the electronegativities of two elements, and hence its degree of
polarity.
The types of bonds are classified into the difference in electronegativity.
Difference in Electronegativity Bond Type
0.0 – 0.4 Non-polar covalent 0.5 – 2.0 Polar covalent > 2.0 Ionic
For example, the difference between C and O is 1. Therefore, a CO molecule would be polar
covalent. Be careful when calculating this to ensure that the dipoles do not cancel.
As we can see, the highest possible difference occurs between Cs and F – I would love to see that
reaction!!