Stability by using charge/radius rule I found a question

Which is more stable among the following?
(a) $\ce{CaCO3}$
(b) $\ce{MgCO3}$

Answer : (a)
Explanation was given as:

$\ce{Mg^2+}$ has smaller radius than $\ce{Ca^2+}$ and thus charge/radius of $\ce{Mg^2+}$ is greater , hence it is less stable.

While when reading about the coordination compound, I found the sentence

Higher the charge of central metal atom ion i.e., greater ionic potential
charge/radius then greater is the stability.

In first case higher the ratio less is the stability.
In second case higher the ratio more is the stability.
Is the difference in the answers in both cases due to a difference in the salts (i.e. simple and  complex salt) or is any one of them wrong?
Please allow me to answer the question in two parts.

Stability of carbonates

We observe this order when we compare the thermal stability of group I-A carbonates: $$\ce{Li2CO3 \lt Na2CO3 \lt K2CO3 \lt Rb2CO3 \lt Cs2CO3}$$

On similar grounds, the thermal stability of group II-A carbonates can be predicted.

This order is in accordance with Fajans' Rules. Here's the table we need to glance at from the Wikipedia page.


  $$\begin{array}{|c|c|} \hline
\mathrm{Ionic} &amp; \text{Covalent}\  \\ \hline
\text{Low positive charge} &amp; \text{High positive charge} \\
\text{Large cation} &amp; \text{Small cation} \\
\text{Small anion} &amp; \text{Large anion} \\ \hline \end{array}$$
  Polarization will be increased by high charge and small size of the cation.


Thus, larger the ratio of charge and radius, higher is the polarization power of the cation, more is the covalent character in the compound and lesser is the ionic character; Ionic compounds are more stable when exposed to heat. A higher ratio will therefore mean lesser stability.

Stability of complex compounds

Thermodynamic stability of complexes, on the other hand, is determined by the Irving–Williams series, according to which general stability sequence of high spin octahedral metal complexes for the replacement of water by other ligands is: 
$$\ce{Mn^2+ &lt; Fe^2+ &lt; Co^2+ &lt; Ni^2+ &lt; Cu^2+ &gt; Zn^2+}$$
Owing to this observation, a lot of theories were formulated to explain this phenomenon. One such theory was that since Crystal Field Theory (CFT) was based on the idea that a purely electrostatic interaction existed between the central metal ion and the ligands, the stability of complexes should be somehow related to the size by charge ratio (otherwise known as the ionic potential) of the central metal atom. [Source]

An interesting thing to note here is that Wikipedia has stated in its article that:


  None of the explanations can satisfactorily explain the success of the Irving–Williams series in predicting the relative stabilities of transition metal complexes.


Thus from manganese till copper, it can be said that higher the ionic potential, more is the stability.