Molecular Electron Sharing Studio
Interactive covalent bonding simulation (H₂, O₂, H₂O, CH₄, C₂H₆, C₆H₆)
Covalent Electron Sharing Simulation
Select or type a molecule to see live electron sharing (Duplet & Octet).
📖 · How Electron Sharing Works Across Molecules
1. H₂ (Hydrogen Gas) · 1 Single Bond
Each Hydrogen atom has 1 valence electron. Two Hydrogens share 1 electron pair (2 e⁻ total), fulfilling the 2 e⁻ duplet rule to attain the stable noble gas configuration of Helium (He).
2. O₂ (Oxygen Gas) · Double Covalent Bond (O=O)
Each Oxygen has 6 valence electrons and requires 2 more. Two Oxygen atoms share 2 pairs of electrons (4 e⁻ total) in a double covalent bond + 2 lone pairs on each atom, fulfilling the 8 e⁻ octet rule.
3. H₂O (Water) · Bent Geometry & Lone Pairs
Oxygen (6 valence e⁻) shares 1 electron pair with each of two Hydrogens (forming 2 single covalent O–H bonds) while retaining 2 non-bonding lone pairs at the top. This produces a bent 104.5° molecular geometry where Oxygen reaches an 8 e⁻ octet and both Hydrogens achieve 2 e⁻ duplets.
4. CH₄ (Methane) · Tetrahedral C–H Bonds
Carbon shares 4 valence electrons with 4 Hydrogens, forming 4 single covalent bonds. Carbon reaches an 8 e⁻ octet and each Hydrogen reaches a 2 e⁻ duplet in an sp³ tetrahedral arrangement.
5. C₂H₆ (Ethane) · Central C–C Single Bond
Two Carbon atoms share a central C–C single bond (2 e⁻) alongside 6 radiating C–H bonds (14 shared e⁻ total). Both Carbons reach stable 8 e⁻ octets.
6. C₆H₆ (Benzene) · Aromatic 6π Resonance Ring
A planar 6-Carbon ring where unhybridized p-orbitals form a delocalized 6π electron cloud, providing exceptional resonance stabilization.
Molecular Structure & Bonding Comparison Table
Summary of electron sharing, shared pairs, lone pairs, and VSEPR geometries across standard organic and inorganic molecules:
| Molecule | Formula | Bond Type | Shared Electrons | Lone Pairs | Molecular Geometry |
|---|---|---|---|---|---|
| Hydrogen Gas | H₂ | Single Covalent (H–H) | 2 e⁻ (1 pair) | 0 | Linear (Duplet) |
| Oxygen Gas | O₂ | Double Covalent (O=O) | 4 e⁻ (2 pairs) | 4 (2 on each O) | Linear (Octet) |
| Water | H₂O | 2 Single Bonds (O–H) | 4 e⁻ (2 pairs) | 2 (on Oxygen) | Bent (104.5°) |
| Methane | CH₄ | 4 Single Bonds (C–H) | 8 e⁻ (4 pairs) | 0 | Tetrahedral (109.5°) |
| Ethane | C₂H₆ | 1 C–C + 6 C–H Bonds | 14 e⁻ (7 pairs) | 0 | Tetrahedral around C |
| Benzene | C₆H₆ | Aromatic Resonance Ring | 30 e⁻ (6π cloud) | 0 | Planar Hexagon (120°) |
Frequently Asked Questions (FAQ)
What is the difference between the Octet Rule and the Duplet Rule?
The Duplet Rule applies to Hydrogen and Helium, which require 2 valence electrons to fill their first (1s) electron shell. The Octet Rule applies to main-group atoms like Carbon, Nitrogen, and Oxygen, which require 8 valence electrons to achieve stable noble gas configurations (like Neon).
Why does Oxygen (O₂) form a double covalent bond?
Each Oxygen atom has 6 valence electrons and needs 2 more to satisfy its octet. By sharing 2 pairs of electrons (4 electrons total), both Oxygen atoms complete their octets, forming a double bond (O=O) plus two lone pairs per atom.
Why is the water molecule (H₂O) bent instead of linear?
Oxygen in water has 4 electron domains: 2 bonding pairs with Hydrogen and 2 unbonded lone pairs. According to VSEPR theory, lone pair-lone pair repulsion pushes the O-H bonds into a bent shape with a bond angle of approximately 104.5 degrees.
What is aromatic resonance in Benzene (C₆H₆)?
In Benzene, 6 Carbon atoms form a planar ring where unhybridized p-orbitals overlap continuously, forming a delocalized 6π electron cloud. This resonance stabilization distributes bond lengths equally, making Benzene far more stable than typical alkenes.
How does Methane (CH₄) achieve a stable tetrahedral geometry?
Carbon undergoes sp³ hybridization, arranging its 4 single C-H covalent bonds symmetrically in three dimensions with bond angles of 109.5 degrees to minimize electron repulsion.