Cyanide radical Lewis Structure

Cyanide radical Lewis Structure: CN⁺ Lewis Structure, linear (diatomic) Geometry, sp Hybridization & Polarity

Cyanide radical Key Facts

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

Figure 1: Lewis Structure of Cyanide radical (CN⁺)

Chemical Formula	CN⁺
CAS Number	2074-87-5
Net Charge	+1
Total Valence Electrons	8
Lewis Structure	linear diatomic molecule with one triple bond
Electron-Domain Geometry	linear
Molecular Geometry	linear (diatomic)
Hybridization Model	sp
Bond Angle	180°
Polarity	Polar molecule

PubChem (CID 5460614) and NIST list Cyanide radical as CN ⁺ with CAS 2074-87-5; molecular weight ≈ 26.017 g/mol. View CAS 2074-87-5 dictionary details on Guidechem →

Applications of Cyanide radical (CAS 2074-87-5)

In aqueous and process chemistry, CN⁺ exists as the cation Cyanide radical ion. It is encountered as a counterion and a controlled source of C in salts, buffers, electrochemistry and analytical protocols, and as a reactant in syntheses that require a defined equivalent of C-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 C in precipitation, complexation and redox procedures.

Procurement Note "Cyanide radical" 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 2074-87-5 as the primary identifier when screening suppliers; always confirm regional availability and safety documentation (SDS).

Step 1 - Valence Electrons & Central Atom

To draw the Cyanide radical Lewis structure we first count the total valence electrons. CN⁺ contains 4 (C) + 5 (N) + 1 (net cation); the net charge of +1 gives a total of 8 valence electrons to place.

The central atom is C. 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 = 4 (C) + 5 (N) + 1 (net cation) = 8 electrons.

Step 2 - Lewis Structure & Electron Distribution

Place C 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 triple bond.

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

C–N

C: 0 lone pairs, 1 bonding domain

1 bonding domains + 0 lone pairs = 1 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 1 electron domains around C arrange to minimize mutual repulsion, giving an linear 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 linear (diatomic); the C 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 0 lone pair(s) on C, 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, C uses sp hybrid orbitals to form the 1 equivalent electron-domain directions (1 bonding + 0 lone pair).

Formal-charge check

Formal charge on central C = V − N − ½B = 4 − 0 − ½×6 = 1. The nonzero formal charge is distributed by resonance / charge separation; the drawn structure is the lowest-energy contributor.

Modeling Note Modeling Note: sp is a compact model for the 1 electron-domain directions around C; full quantum-chemical treatments use molecular orbitals.

Is Cyanide radical Polar or Nonpolar?

Cyanide radical 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 Cyanide radical 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
Cyanide radical	CN⁺	C	1	linear (diatomic)	Polar
Carbon dioxide	CO₂	C	2	linear	Nonpolar
Carbon monoxide	CO	C	2	linear (diatomic)	Polar
Carbon disulfide	CS₂	C	2	linear	Nonpolar
Methane	CH₄	C	4	tetrahedral	Nonpolar
Ethane	C₂H₆	C	4	tetrahedral	Nonpolar

Practice question Starting from the 8 valence electrons of CN⁺, draw the Lewis structure and confirm the central C atom is sp-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 Cyanide radical (CAS 2074-87-5)? Browse Supplier on Guidechem →

FAQs

Is CN⁺ polar or nonpolar?

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

What is the Lewis structure of Cyanide radical?

linear diatomic molecule with one triple bond. It uses all 8 valence electrons and the preferred structure carries a formal charge of 1 on the central atom.

What is the bond angle in Cyanide radical?

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

What is the hybridization of C in Cyanide radical?

The conventional model is sp. Cyanide radical has 1 electron domains around the central C.

What is the CAS number of Cyanide radical?

The CAS number is 2074-87-5. PubChem (CID 5460614) and NIST identify this with CN⁺; use it to locate suppliers and database records.

References

PubChem CID 5460614, Cyanide radical. Molecular formula, CAS number, molecular weight and chemical identity.
NIST Chemistry WebBook, SRD 69, Cyanide radical. 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 Cyanide radical (CAS 2074-87-5).

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 2074-87-5 identifies the substance, not a universal purity specification.

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Cyanide radical Lewis Structure

Cyanide radical Lewis Structure