Dichlorodiazene Lewis Structure

Dichlorodiazene Lewis Structure: Cl₂N₂ Lewis Structure, bent Geometry, sp2 Hybridization & Polarity

Dichlorodiazene Key Facts

The Dichlorodiazene Lewis structure is N–N double bond and N–Cl single bond; the central N has 3 electron domains (1 lone pair), giving a trigonal planar electron-domain arrangement and a bent molecular geometry with a ≈119° bond angle. N is best described as sp2-hybridized, and Dichlorodiazene is polar because the bent shape (and/or unequal terminal atoms) prevents cancellation of the bond dipoles.

Figure 1: Lewis Structure of Dichlorodiazene (Cl₂N₂)

Chemical Formula	Cl₂N₂
CAS Number	590-29-4
Total Valence Electrons	24
Lewis Structure	N–N double bond and N–Cl single bond
Electron-Domain Geometry	trigonal planar
Molecular Geometry	bent
Hybridization Model	sp2 (central N)
Bond Angle	≈119°
Polarity	Polar molecule

PubChem (CID 86062048) and NIST list Dichlorodiazene as Cl ₂N ₂ with CAS 590-29-4; molecular weight ≈ 98.92 g/mol. View CAS 590-29-4 dictionary details on Guidechem →

Applications of Dichlorodiazene (CAS 590-29-4)

Alkenes are polymerization monomers and intermediates: ethylene → polyethylene, propylene → polypropylene, styrene → polystyrene and ABS, butadiene → synthetic rubber. They are also feedstocks for alcohols, oxides and plasticizers.

Polymer Monomer Basis of polyethylene, polypropylene, polystyrene and elastomers.

Intermediate Source of alcohols, epoxides, plasticizers and surfactants.

Process Scale Produced in the largest volumes of any organic commodity class.

Procurement Note "Dichlorodiazene" 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 590-29-4 as the primary identifier when screening suppliers; always confirm regional availability and safety documentation (SDS).

Step 1 - Valence Electrons & Central Atom

To draw the Dichlorodiazene Lewis structure we first count the total valence electrons. Cl₂N₂ contains 2×7 (Cl) + 2×5 (N); the net charge of 0 gives a total of 24 valence electrons to place.

The central atom is N. 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 = 2×7 (Cl) + 2×5 (N) = 24 electrons.

Step 2 - Lewis Structure & Electron Distribution

Place N 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: N–N double bond and N–Cl single bond; one lone pair on N.

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

N=N N–Cl

N: 1 lone pair, 2 bonding domains

2 bonding domains + 1 lone pairs = 3 electron domains

Octet Rule: Why N Has Eight Electrons N forms 2 bond(s) and retains 2 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 3 electron domains around N arrange to minimize mutual repulsion, giving an trigonal planar electron-domain geometry.

Because 1 of these domains are lone pair(s) — and lone pairs repel more strongly than bonding pairs — the observed molecular geometry is bent; the N bond angle is set to ≈119° 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 1 lone pair(s) on N, 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, N uses sp2 hybrid orbitals to form the 3 equivalent electron-domain directions (2 bonding + 1 lone pair).

Formal-charge check

Formal charge on central N = V − N − ½B = 5 − 2 − ½×6 = 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: sp2 is a compact model for the 3 electron-domain directions around N; full quantum-chemical treatments use molecular orbitals.

Is Dichlorodiazene Polar or Nonpolar?

Dichlorodiazene is polar. The bent 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 Dichlorodiazene the bent 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
Dichlorodiazene	Cl₂N₂	N	3	bent	Polar
Ammonia	H₃N	N	4	trigonal pyramidal	Polar
Ammonium	H₄N	N	4	tetrahedral	Nonpolar
Hydrazine	H₄N₂	N	4	trigonal pyramidal	Polar
Nitrogen	N₂	N	2	linear (diatomic)	Nonpolar
Nitric oxide	NO	N	3	linear (diatomic)	Polar

Practice question Starting from the 24 valence electrons of Cl₂N₂, draw the Lewis structure and confirm the central N atom is sp2-hybridized with bent 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 Dichlorodiazene (CAS 590-29-4)? Browse Supplier on Guidechem →

FAQs

Is Cl₂N₂ polar or nonpolar?

Dichlorodiazene is polar. Its bent geometry (and/or unequal terminal atoms) stops the bond dipoles from cancelling.

What is the Lewis structure of Dichlorodiazene?

N–N double bond and N–Cl single bond; one lone pair on N. It uses all 24 valence electrons and the preferred structure carries zero formal charge on the central atom.

What is the bond angle in Dichlorodiazene?

The N angle is about ≈119°. Lone-pair repulsion compresses the angle from the ideal trigonal planar value.

What is the hybridization of N in Dichlorodiazene?

The conventional model is sp2. Dichlorodiazene has 3 electron domains around the central N.

What is the CAS number of Dichlorodiazene?

The CAS number is 590-29-4. PubChem (CID 86062048) and NIST identify this with Cl₂N₂; use it to locate suppliers and database records.

References

PubChem CID 86062048, Dichlorodiazene. Molecular formula, CAS number, molecular weight and chemical identity.
NIST Chemistry WebBook, SRD 69, Dichlorodiazene. 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 Dichlorodiazene (CAS 590-29-4).

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 590-29-4 identifies the substance, not a universal purity specification.

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Dichlorodiazene Lewis Structure