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Draw Lewis structures for: Molecules, ions, chemical compounds, organic molecules, inorganic compounds, Lewis dot diagrams with electron pairs, bonding electrons, and lone pairs.
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Result: Water (H₂O)
Molecular Properties
Geometry
Element Composition
Mass Percentage
Common Examples
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Stop wasting hours drawing Lewis structures by hand. Our tool saves you time, eliminates errors, and helps you understand chemistry faster—so you can spend more time mastering concepts and less time struggling with diagrams.
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Generate accurate structures in seconds instead of struggling for minutes on each molecule.
Boost Your Grades
Get perfect diagrams every time and understand complex molecules faster with clear visualizations.
Learn Faster
Visual learning helps you grasp molecular geometry and bonding concepts that seem confusing in textbooks.
Zero Mistakes
Avoid common errors in electron counting, formal charges, and bond placement with our validated algorithm.
What is a Lewis Dot 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).
Bonding Pairs: A single line for a single bond, double line for double bonds, and a triple line for triple bonds.
Lone Pairs: Pairs of dots located on an atom not involved in bonding (non-bonding valence electrons).
Radical Dots: A single dot next to the atom indicates (single electron or radical).
How to Draw Lewis Structures: Step-by-Step Guide
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.
Frequently Asked Questions
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