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BCl3 Lewis Structure Explained: Step-by-Step Guide to Nitrogen Trichloride Bonding

May 26,2026

Boron trichloride(BCl3) is a colorless gas with a pungent odor. Fumes irritate the eyes and mucous membranes. Corrosive to metals and tissue and is toxic. Under prolonged exposure to fire or intense heat, the containers may rupture violently and rocket.

Use

Boron trichloride is used in manufacturing Boron, as a catalyst, and in semiconductors.

Health hazard

Boron trichloride is a strong irritant to tissue. Fumes are corrosive and highly toxic. Boron affects the central nervous system causing depression of circulation as well as shock and coma. May cause severe burns to skin. May result in marked fluid and electrolyte loss and shock.

Steps of draw the Lewis structure for BCl3

Boron trichloride

Step 1. Count the total number of valence electrons

Boron (B) has 3 valence electrons.

Chlorine (Cl) has 7 valence electrons, but there are three Chlorine atoms, so total valence electrons from Chlorine are 21.

Adding these together, we get a total of 24 valence electrons.

Step 2. Draw the skeleton structure of the molecule

Boron (B) is the least electronegative atom, so it is the central atom.

Draw a single bond (represented by a line) between Boron and each Chlorine atom.

Step 3. Distribute the remaining electrons as lone pairs

Start by completing the octet of the outer atoms (Chlorine in this case).

Any remaining electrons after the octets of the outer atoms are complete should be placed on the central atom.

Step 4. Check stability

All atomic forms have 0 charge, the structure is stable;

No extra electrons, no double/triple bonds needed.

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  • What is Boron trichloride used for? Nov 15, 2024

    Boron trichloride (chemical formula: BCl3) is an inorganic compound commonly used in dry etching and chemical vapor deposition (CVD) processes in semiconductor manufacturing.

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