The ionic radius of Na$$^+$$ ions is 1.02 angstrom. The ionic radii (in $$\mathring{A}$$) of Mg$$^{2+}$$ and Al$$^{3+}$$, respectively, are:

Na$$^+$$, Mg$$^{2+}$$, and Al$$^{3+}$$ are isoelectronic species (all have 10 electrons), but they differ in nuclear charge. Na has 11 protons, Mg has 12, and Al has 13. As the nuclear charge increases for the same number of electrons, the ionic radius decreases because the electrons are pulled more tightly toward the nucleus.

The ionic radius of Na$$^+$$ is given as $$1.02$$ angstrom. Since Mg$$^{2+}$$ has a higher nuclear charge, its radius is smaller, and Al$$^{3+}$$ with an even higher charge is smaller still. The standard ionic radii are approximately: Mg$$^{2+} = 0.72$$ angstrom and Al$$^{3+} = 0.54$$ angstrom.

The answer is $$\boxed{0.72 \text{ and } 0.54}$$.