Iodine tetrachloride ion Lewis Structure

Iodine tetrachloride ion Lewis Structure: ICl₄ Lewis Structure, square planar Geometry, sp3d2 Hybridization & Polarity

Iodine tetrachloride ion Key Facts

The Iodine tetrachloride ion Lewis structure is I–Cl single bond, I–Cl single bond, I–Cl single bond and I–Cl single bond; the central I has 6 electron domains (2 lone pairs), giving a octahedral electron-domain arrangement and a square planar molecular geometry with a 90° bond angle. I is best described as sp3d2-hybridized, and Iodine tetrachloride ion is nonpolar because the bond dipoles cancel by molecular symmetry.

Figure 1: Lewis Structure of Iodine tetrachloride ion (ICl₄)

Chemical Formula	ICl4
CAS Number	16330-00-2
Net Charge	-1
Total Valence Electrons	36
Lewis Structure	I–Cl single bond, I–Cl single bond, I–Cl single bond and I–Cl single bond
Electron-Domain Geometry	octahedral
Molecular Geometry	square planar
Hybridization Model	sp3d2 (central I)
Bond Angle	90°
Polarity	Nonpolar molecule

PubChem and NIST list Iodine tetrachloride ion as ICl ₄ with CAS 16330-00-2; molecular weight ≈ 268.7 g/mol. View CAS 16330-00-2 dictionary details on Guidechem →

Applications of Iodine tetrachloride ion (CAS 16330-00-2)

In aqueous and process chemistry, ICl₄ exists as the anion Iodine tetrachloride ion ion. It is encountered as a counterion and a controlled source of I in salts, buffers, electrochemistry and analytical protocols, and as a reactant in syntheses that require a defined equivalent of I-containing material.

Step 1 - Valence Electrons & Central Atom

To draw the Iodine tetrachloride ion Lewis structure we first count the total valence electrons. ICl₄ contains 7 (I) + 4×7 (Cl) − 1 (net anion); the net charge of -1 gives a total of 36 valence electrons to place.

The central atom is I. It is the least electronegative atom capable of forming multiple bonds and is surrounded by the more electronegative terminal atom(s); hydrogen, when present, always occupies a terminal position. Electronegativity considerations place the electron density toward the terminal atom(s).

Step 2 - Lewis Structure & Electron Distribution

Place I at the center and connect each surrounding atom with a single bond, complete octets on the terminal atoms, and place any remaining electrons on the central atom. The resulting electron distribution is: I–Cl single bond, I–Cl single bond, I–Cl single bond and I–Cl single bond; 2 lone pairs on I.

Counting bonding and nonbonding electrons around I therefore satisfies the octet/expanded-octet requirement for the drawn structure.

Step 3 - VSEPR Theory & Geometry

VSEPR theory states that the 6 electron domains around I arrange to minimize mutual repulsion, giving an octahedral electron-domain geometry.

Because 2 of these domains are lone pair(s) — and lone pairs repel more strongly than bonding pairs — the observed molecular geometry is square planar; the I bond angle is set to 90° rather than the ideal value for the electron-domain geometry.

Hybridization & Formal Charge

In the conventional localized-bond model, I uses sp3d2 hybrid orbitals to form the 6 equivalent electron-domain directions (4 bonding + 2 lone pair).

Is Iodine tetrachloride ion Polar or Nonpolar?

Iodine tetrachloride ion is nonpolar. Although individual I–terminal bonds are polar when the atoms differ in electronegativity, the square planar geometry makes their vector sum zero, so there is no net molecular dipole.

Its nonpolar character governs solvation and intermolecular behavior; specify grade and handling when sourcing.

Structural Comparison Table

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