All of the factors that we have discussed for Bronsted acidity, or the ability of a compound to provide a proton to its surroundings, have an effect on basicity as well.  In other words, factors like nuclear charge / electron affinity influence how strongly a compound will attract or bind a proton.

In summary:

• the higher the electron affinity or core charge of an atom, the less likely it is to donate its electrons to a proton.

• the greater the delocalization of electrons that could potentially donate to a proton, the less able they are to donate.

• the greater the electron-withdrawing effects in another part of a molecule, the less likely the electrons on a particular atom are to donate.

These factors are generally complementary to the effects on acidity.  A factor that makes a Bronsted acid more acidic usually makes the corresponding conjugate base less basic.

However, sometimes things can be more subtle. 

• the higher the polarizability of an atom (i.e. the larger an atom), the more easily it can donate to a Lewis acid (its electrons are not held very tightly because they are far from the nucleus, and so they can be donated easily).

• except:  a larger atom cannot donate easily to a proton.  In this specific case, the Lewis acid (the proton) is too small to get good covalent overlap with the Lewis base, so it can't form a very strong bond