# Is pyrite (FeS₂) an ionic or a covalent compound?

I have searched all over the web and found a lot of diverse explanations, but none of them are concluding exactly whether $\ce{FeS2}$ (solid - pyrite) is a covalent or an ionic compound.

From electronegativity, it should be covalent as the $\Delta\chi=0.7$ which is less than $1.5$ and thus said to make covalent bonds and therefore be a covalent compound.

From the definition of ionic bonds, which are bonds between a metal and a non-metal element (whereas covalent bonds are bonds between non-metal elements), it should be an ionic compound.

Does someone know which of those is 'true', or better, if there is another, more detailed explanation?

You seem to have fallen into the trap of thinking that ionic and covalent bonds are fundamentally different. They are not - they are just two ends of a spectrum, which has an arbitrary division somewhere in the middle into an ionic and covalent regime. This is explained in the answers to this question.

In the case of pyrite we have a relatively hard cation, with a small ionic radius and charge of +2, and a rather large anion, with a charge of -2. Therefore there will be a significant degree of covalent character in the Fe-S bonds due to the polarising effect of the cation on the anion. This is confirmed by experimental results and theoretical calculations which suggest that the charge on Fe is about +2/3 and the charge on S is about -1/3. This is significantly less than the expected charges of +2 and -1 from a purely ionic model and so indicates that there is significant sharing of electrons. This is supported by measurements and calculations of the electron density, which show significant electron density between the atoms.

Your definition of ionic bonding is incorrect as non-metallic polyatomic cations (e.g ammonium) form ionic compounds. Ionic bonding is the electrostatic attraction of cations and anions forming a regular giant lattice. Transition metal compounds do not have simple close packing ionic lattices as they prefer coordination compounds due to the energies of d-orbitals. Here is the pyrite structure:

Note that the iron has octahedral geometry and sulfur has tetrahedral. These are the most common geometries in coordination chemistry.

• but couldn't you simplify Iron(II) Sulfide(or pyrite) to Fe^2+ ions and S^2- ions ionically bonded like how you can simplify Iron(III) Oxide into Fe^3+ ions and O^2- ions in ionic bonds? – Caters Aug 14 '14 at 17:12