The structure of ICl₄ is

The structure of ICl₄⁻ (tetraiodide anion) can be understood by examining its electron configuration and applying the Valence Shell Electron Pair Repulsion (VSEPR) theory.

Electron Configuration and VSEPR Theory:

• Central Atom: Iodine (I)
• Valence Electrons: Iodine has 7 valence electrons, and each chlorine (Cl) atom contributes 7 valence electrons. The negative charge on the ion adds one more electron, totaling 7 + (4 × 7) + 1 = 32 valence electrons.
• Electron Pairs: These 32 electrons form 16 pairs. Four pairs are bonding pairs between iodine and chlorine atoms, and the remaining 12 pairs are lone pairs on the iodine atom.
• Electron Geometry: According to VSEPR theory, the electron pairs around the central atom arrange themselves to minimize repulsion. With 16 electron pairs, the geometry is octahedral.
• Molecular Geometry: The four bonding pairs occupy the equatorial positions of the octahedron, while the two lone pairs occupy the axial positions. This arrangement results in a square planar molecular geometry for ICl₄⁻.

Summary:

The ICl₄⁻ ion has a square planar structure due to the arrangement of bonding and lone electron pairs around the central iodine atom.

For a visual explanation, you might find the following video helpful: