Arsenic hexafluoride Lewis Structure

Arsenic hexafluoride Lewis Structure: AsF₆ Lewis Structure, octahedral Geometry, sp3d2 Hybridization & Polarity

Arsenic hexafluoride Key Facts

The Arsenic hexafluoride Lewis structure is As–F single bond, As–F single bond, As–F single bond, As–F single bond, As–F single bond and As–F single bond; the central As has 6 electron domains (0 lone pairs), giving a octahedral electron-domain arrangement and a octahedral molecular geometry with a 90° bond angle. As is best described as sp3d2-hybridized, and Arsenic hexafluoride is nonpolar because the bond dipoles cancel by molecular symmetry.

Figure 1: Lewis Structure of Arsenic hexafluoride (AsF₆)

Chemical Formula	AsF6
CAS Number	17435-33-5
Total Valence Electrons	47
Lewis Structure	As–F single bond, As–F single bond, As–F single bond, As–F single bond, As–F single bond and As–F single bond
Electron-Domain Geometry	octahedral
Molecular Geometry	octahedral
Hybridization Model	sp3d2 (central As)
Bond Angle	90°
Polarity	Nonpolar molecule

PubChem and NIST list Arsenic hexafluoride as AsF ₆ with CAS 17435-33-5; molecular weight ≈ None g/mol. View CAS 17435-33-5 dictionary details on Guidechem →

Applications of Arsenic hexafluoride (CAS 17435-33-5)

Arsenic hexafluoride is encountered as a reagent, intermediate or specialty chemical in inorganic, organometallic and materials synthesis. Confirm grade, purity and supplier documentation (SDS) before specifying for a process.

Step 1 - Valence Electrons & Central Atom

To draw the Arsenic hexafluoride Lewis structure we first count the total valence electrons. AsF₆ contains 5 (As) + 6×7 (F); the net charge of 0 gives a total of 47 valence electrons to place.

The central atom is As. 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 As 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: As–F single bond, As–F single bond, As–F single bond, As–F single bond, As–F single bond and As–F single bond; no lone pairs on As.

Counting bonding and nonbonding electrons around As 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 As arrange to minimize mutual repulsion, giving an octahedral electron-domain geometry.

Because 0 of these domains are lone pair(s) — and lone pairs repel more strongly than bonding pairs — the observed molecular geometry is octahedral; the As 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, As uses sp3d2 hybrid orbitals to form the 6 equivalent electron-domain directions (6 bonding + 0 lone pair).

Is Arsenic hexafluoride Polar or Nonpolar?

Arsenic hexafluoride is nonpolar. Although individual As–terminal bonds are polar when the atoms differ in electronegativity, the octahedral 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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