Hypobromite ion Lewis Structure

Hypobromite ion Lewis Structure: BrO^- Lewis Structure, linear (diatomic) Geometry, sp3 Hybridization & Polarity

Hypobromite ion Key Facts

The Hypobromite ion Lewis structure is a linear diatomic with a polar bond between its two atoms; because the two atoms differ in electronegativity, Hypobromite ion is polar.

Figure 1: Lewis Structure of Hypobromite ion (BrO^-)

Chemical Formula	BrO^-
CAS Number	15316-62-8
Net Charge	-1
Total Valence Electrons	14
Lewis Structure	linear diatomic molecule with one single bond and a lone pair on each atom
Electron-Domain Geometry	linear
Molecular Geometry	linear (diatomic)
Hybridization Model	sp3
Bond Angle	180°
Polarity	Polar molecule

PubChem (CID 5460626) and NIST list Hypobromite ion as BrO ^- with CAS 15316-62-8; molecular weight ≈ 95.90 g/mol. View CAS 15316-62-8 dictionary details on Guidechem →

Applications of Hypobromite ion (CAS 15316-62-8)

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

Ion Source / Counterion Supplied as salts and solutions; specify hydration, counter-cation and concentration.

Analytical & Electrochemical Used in titrations, plating baths and ionic-strength control where the ion is the active species.

Synthesis Reagent A controlled source of O in precipitation, complexation and redox procedures.

Procurement Note "Hypobromite ion" is supplied in multiple commercial grades and package sizes. Specify purity, grade, moisture/impurity limits, package (cylinder, drum or bulk) and intended process, and use CAS 15316-62-8 as the primary identifier when screening suppliers; always confirm regional availability and safety documentation (SDS).

Step 1 - Valence Electrons & Central Atom

To draw the Hypobromite ion Lewis structure we first count the total valence electrons. BrO^- contains 7 (Br) + 6 (O) − 1 (net anion); the net charge of -1 gives a total of 14 valence electrons to place.

The central atom is O. 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).

Valence-electron count

Total valence electrons = 7 (Br) + 6 (O) − 1 (net anion) = 14 electrons.

Step 2 - Lewis Structure & Electron Distribution

Place O 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: linear diatomic molecule with one single bond and a lone pair on each atom.

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

O–Br

O: 3 lone pairs, 1 bonding domain

1 bonding domains + 3 lone pairs = 4 electron domains

Octet & Diradical Note In a simple Lewis drawing each atom of this homonuclear diatomic carries lone pairs; species such as O₂ are more accurately described by molecular-orbital theory (paramagnetism arises from unpaired electrons in π* orbitals).

Step 3 - VSEPR Theory & Geometry

VSEPR theory states that the 4 electron domains around O arrange to minimize mutual repulsion, giving an linear electron-domain geometry.

Because 3 of these domains are lone pair(s) — and lone pairs repel more strongly than bonding pairs — the observed molecular geometry is linear (diatomic); the O bond angle is set to 180° rather than the ideal value for the electron-domain geometry.

Repulsion hierarchy

A useful VSEPR approximation is: lone pair–lone pair repulsion > lone pair–bonding pair repulsion > bonding pair–bonding pair repulsion. With 3 lone pair(s) on O, the lone-pair domains occupy positions that minimize overall repulsion while pushing the bonding domains (and therefore the bonded atoms) closer together.

Hybridization & Formal Charge

In the conventional localized-bond model, O uses sp3 hybrid orbitals to form the 4 equivalent electron-domain directions (1 bonding + 3 lone pair).

Formal-charge check

Formal charge on central O = V − N − ½B = 6 − 6 − ½×2 = -1. The nonzero formal charge is distributed by resonance / charge separation; the drawn structure is the lowest-energy contributor.

Modeling Note Modeling Note: sp3 is a compact model for the 4 electron-domain directions around O; full quantum-chemical treatments use molecular orbitals.

Is Hypobromite ion Polar or Nonpolar?

Hypobromite ion is polar. The linear (diatomic) shape prevents cancellation of the bond dipoles. The bond dipoles do not cancel, leaving a net molecular dipole, which strongly influences solvation behavior and intermolecular interactions.

Expert Quote — Structural Chemistry Perspective

The decisive structural fact is not simply that the individual bonds are polar; it is whether molecular symmetry allows their vector sum to vanish. In Hypobromite ion the linear (diatomic) arrangement prevents cancellation, so a permanent dipole remains.

Interpretation consistent with standard VSEPR / molecular-geometry references.

This polarity profile underpins its behavior as a solvent, reactant or process intermediate; when sourcing, specify grade and container compatibility.

Structural Comparison Table

Species	Formula	Central Atom	Electron Domains	Molecular Geometry	Polarity
Hypobromite ion	BrO^-	O	4	linear (diatomic)	Polar
Water	H₂O	O	4	bent	Polar
Hydrogen peroxide	H₂O₂	O	4	bent	Polar
Ozone	O₃	O	3	bent	Polar
Hydronium	H₃O	O	4	trigonal pyramidal	Polar
Hypochlorite	ClO	O	4	linear (diatomic)	Polar

Practice question Starting from the 14 valence electrons of BrO^-, draw the Lewis structure and confirm the central O atom is sp3-hybridized with linear (diatomic) geometry. What happens to the bond angle if one terminal atom is replaced by a more electronegative substituent?

Looking for industrial bulk or specified-grade supplies of Hypobromite ion (CAS 15316-62-8)? Browse Supplier on Guidechem →

FAQs

Is BrO^- polar or nonpolar?

Hypobromite ion is polar. Its linear (diatomic) geometry (and/or unequal terminal atoms) stops the bond dipoles from cancelling.

What is the Lewis structure of Hypobromite ion?

linear diatomic molecule with one single bond and a lone pair on each atom. It uses all 14 valence electrons and the preferred structure carries a formal charge of -1 on the central atom.

What is the bond angle in Hypobromite ion?

The O angle is about 180°. Lone-pair repulsion compresses the angle from the ideal linear value.

What is the hybridization of O in Hypobromite ion?

The conventional model is sp3. Hypobromite ion has 4 electron domains around the central O.

What is the CAS number of Hypobromite ion?

The CAS number is 15316-62-8. PubChem (CID 5460626) and NIST identify this with BrO^-; use it to locate suppliers and database records.

References

PubChem CID 5460626, Hypobromite ion. Molecular formula, CAS number, molecular weight and chemical identity.
NIST Chemistry WebBook, SRD 69, Hypobromite ion. Formula, CAS Registry Number and thermochemical / spectroscopic data.
IUPAC Gold Book. Definitions for "lone pair", "VSEPR", "hybridization" and "formal charge".
Atkins, P. & de Paula, J., Physical Chemistry. VSEPR, molecular geometry and dipole moments.
Guidechem supplier & dictionary records. Commercial sourcing and CAS-linked property pages for Hypobromite ion (CAS 15316-62-8).

Technical scope: Lewis structures, VSEPR and hybridization are model-based descriptions for chemical communication and structure prediction; actual molecular electronic structure is more accurately represented by molecular-orbital and quantum-chemical methods. Commercial grades vary substantially by supplier and intended use; CAS 15316-62-8 identifies the substance, not a universal purity specification.

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Hypobromite ion Lewis Structure

Hypobromite ion Lewis Structure