Sodium hydroxide Lewis Structure

Sodium hydroxide Lewis Structure: HNaO Lewis Structure, see text Geometry, sp3 Hybridization & Polarity

Sodium hydroxide Key Facts

The Sodium hydroxide Lewis structure is O–H single bond; the central O has 4 electron domains (3 lone pairs), giving a tetrahedral electron-domain arrangement and a see text molecular geometry with a — bond angle. O is best described as sp3-hybridized, and Sodium hydroxide is polar because the see text shape (and/or unequal terminal atoms) prevents cancellation of the bond dipoles.

Figure 1: Lewis Structure of Sodium hydroxide (HNaO)

Chemical Formula	HNaO
CAS Number	1310-73-2
Total Valence Electrons	8
Lewis Structure	O–H single bond
Electron-Domain Geometry	tetrahedral
Molecular Geometry	see text
Hybridization Model	sp3 (central O)
Bond Angle	—
Polarity	Polar molecule

PubChem (CID 14798) and NIST list Sodium hydroxide as HNaO with CAS 1310-73-2; molecular weight ≈ 39.997 g/mol. View CAS 1310-73-2 dictionary details on Guidechem →

Applications of Sodium hydroxide (CAS 1310-73-2)

Sodium hydroxide 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.

Reagent / Intermediate Used in synthesis and formulation where the substance's reactivity is required.

Specialty Chemical Specified by grade for the intended process or research use.

Sourcing Verify purity, package and regional availability via the CAS identifier.

Procurement Note "Sodium hydroxide" 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 1310-73-2 as the primary identifier when screening suppliers; always confirm regional availability and safety documentation (SDS).

Step 1 - Valence Electrons & Central Atom

To draw the Sodium hydroxide Lewis structure we first count the total valence electrons. HNaO contains 1 (H) + 1 (Na) + 6 (O); the net charge of 0 gives a total of 8 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 = 1 (H) + 1 (Na) + 6 (O) = 8 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: O–H single bond; 3 lone pairs on O.

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

O–H

O: 3 lone pairs, 1 bonding domain

1 bonding domains + 3 lone pairs = 4 electron domains

Octet Rule: Why O Has Eight Electrons O forms 1 bond(s) and retains 6 nonbonding electron(s), reaching an octet. No expanded octet is required for this second-row (or octet-satisfying) central atom.

Step 3 - VSEPR Theory & Geometry

VSEPR theory states that the 4 electron domains around O arrange to minimize mutual repulsion, giving an tetrahedral 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 see text; the O bond angle is set to — 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 = 0. The preferred Lewis structure carries zero formal charge on the central atom (and on the terminals), so it is the dominant 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 Sodium hydroxide Polar or Nonpolar?

Sodium hydroxide is polar. The see text 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 Sodium hydroxide the see text 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
Sodium hydroxide	HNaO	O	4	see text	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 8 valence electrons of HNaO, draw the Lewis structure and confirm the central O atom is sp3-hybridized with see text 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 Sodium hydroxide (CAS 1310-73-2)? Browse Supplier on Guidechem →

FAQs

Is HNaO polar or nonpolar?

Sodium hydroxide is polar. Its see text geometry (and/or unequal terminal atoms) stops the bond dipoles from cancelling.

What is the Lewis structure of Sodium hydroxide?

O–H single bond; 3 lone pairs on O. It uses all 8 valence electrons and the preferred structure carries zero formal charge on the central atom.

What is the bond angle in Sodium hydroxide?

The O angle is about —. Lone-pair repulsion compresses the angle from the ideal tetrahedral value.

What is the hybridization of O in Sodium hydroxide?

The conventional model is sp3. Sodium hydroxide has 4 electron domains around the central O.

What is the CAS number of Sodium hydroxide?

The CAS number is 1310-73-2. PubChem (CID 14798) and NIST identify this with HNaO; use it to locate suppliers and database records.

References

PubChem CID 14798, Sodium hydroxide. Molecular formula, CAS number, molecular weight and chemical identity.
NIST Chemistry WebBook, SRD 69, Sodium hydroxide. 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 Sodium hydroxide (CAS 1310-73-2).

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 1310-73-2 identifies the substance, not a universal purity specification.

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Sodium hydroxide Lewis Structure