Critical Radius Ratio. This diagram is for coordination number six: 4 anions in the plane shown, 1 above the plane and 1 below. The stability limit is at rC/rA = 0.414

In condensed matter physics and inorganic chemistry the cation-anion radius ratio is the ratio of the ionic radius of the cation to the ionic radius of the anion in a cation-anion compound. This is simply given by ${\displaystyle r_{C}/r_{A}}$.

According to Pauling's rules for crystal structures, the allowed size of the cation for a given structure is determined by the critical radius ratio.[1] If the cation is too small, then it will attract the anions into each other and they will collide hence the compound will be unstable due to anion-anion repulsion; this occurs when the radius ratio drops below 0.155.

At the stability limit the cation is touching all the anions and the anions are just touching at their edges (radius ratio = 0.155). Beyond this stability limit (radius ratio < 0.155) the compound may be stable.

The table below gives the relation between radius ratio and coordination number, which may be obtained from a simple geometrical proof.[2]

Radius Ratio Coordination number Type of void Example
< 0.155 2 Linear
0.155 - 0.225 3 Triangular Planar B2CO3[citation needed]
0.225 - 0.414 4 Tetrahedral ZnS, CuCl
0.414 - 0.732 6 Octahedral NaCl, MgO
0.732 - 1.000 8 Cubic CsCl, NH4Br