Lewis Structure Generator

Instant Lewis Dot Structures, geometry analysis, and formal charge calculations. Enter a molecule to visualize its electron configuration.

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Supports: Chemical elements (e.g., Ca, Fe, Br), functional groups (e.g., Ph, Me, Et), parentheses/brackets, and common names (e.g., water, ammonia).

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Result: Water (H₂O)

Molecular Properties

Valence Electrons 8

Net Charge 0

Central Atom Oxygen

Molar Mass 18.015 g/mol

Geometry

Bent (V-shaped)

Bond Angle 104.5°

Hybridization sp³

Element Composition

Mass Percentage

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Common Examples

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About Our Lewis Structure Generator

This app was designed to help chemistry students, educators, and researchers visualize molecular bonding instantly, by clarifying the gap between abstract chemical formulas and actual electron configurations (intuitive and visual).

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Advanced Input Support

Handles complex notation including functional groups, expanded octets, and common names.

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High-Quality Diagrams

Instantly generates clean, professional diagrams for all your reports.

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What is a Lewis Structure?

A Lewis Structure is an efficient graphical representation of the valence electrons in molecules and polyatomic ions. It is a single line for a single bond (a shared pair or a double bond), a double line is a split line or a triple bond (a pair of dots next to atom next to an unpaired electron) radical).

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Bonding Pairs: A single line for a single bond, double line for double bonds, and a triple line for triple bonds.

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Lone Pairs: Pairs of dots located on an atom not involved in bonding (non-bonding valence electrons).

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Radical Dots: A single dot next to the atom indicates (single electron or radical).

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Step-by-Step Guide (Example: CO₂)

Count Valence Electrons

Calculate total valence electrons. Carbon (Group 14) has 4, Oxygen (Group 16) has 6. Total = 4 + (2×6) = 16 e⁻.

Determine Central Atom

Carbon is less electronegative than Oxygen, so it's central: O-C-O

Draw Single Bonds

Connect each oxygen to carbon with a single bond: 2 bonds × 2 e⁻ = 4 e⁻ used. Remaining = 12 e⁻.

Add Lone Pairs to Outer Atoms

Place remaining electrons on oxygen to satisfy their octet. Each needs 6 more e⁻ (3 lone pairs).

Check Central Atom Octet

Carbon has only 4 e⁻ (needs 8). Form double bonds: O=C=O

Verify Final Structure

Check that all atoms satisfy the octet rule and calculate formal charges.

check_circle All octets complete

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Frequently Asked Questions

Why do some atoms expand their octet? expand_more

Elements in period 3+ can use d-orbitals, allowing more than 8 electrons (e.g., PCl₅ has 10).

What is Formal Charge? expand_more

A theoretical charge calculated by: FC = V - (L + B/2), where V = valence electrons, L = lone pairs, B = bonding electrons.

How do I use the Lewis Structure Generator? expand_more

Enter your chemical formula and click "Generate". The tool accepts standard notation, ions, and functional groups.

Does this tool support charged ions? expand_more

Yes! Input ions using notation like SO4 2- or NH4 +.

What molecules are supported? expand_more

We support a vast range from simple diatomic gases to complex organic compounds, including acids, salts, hydrocarbons, and expanded octets.

Can I see resonance structures? expand_more

Currently shows the most stable resonance contributor based on formal charge minimization.

Is the VSEPR theory applied here? expand_more

Yes, molecular geometry and bond angles are calculated using VSEPR theory.

What does "Hybridization" mean? expand_more

Mixing of atomic orbitals to form new hybrid orbitals (e.g., sp³ in tetrahedral CH₄, sp² in trigonal planar BF₃).

Is this tool free for students? expand_more

Absolutely! This is a free educational resource for students and teachers.