Sigma & Pi Bonds Simulation | Chemical Bonding

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Sigma & Pi Bonds Visualization

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Sigma (σ) Overlap

Pi (π) Overlap

Concept Quiz

Valence Bond Theory: $\sigma$ and $\pi$ bonds

Covalent bonds are formed by the overlap of atomic orbitals.

• Sigma ($\sigma$) Bond: Formed by the head-on (axial) overlap of orbitals. The electron density is concentrated along the internuclear axis. It allows free rotation.
• Pi ($\pi$) Bond: Formed by the sideways (lateral) overlap of unhybridized p-orbitals. The electron density is above and below the internuclear axis. It restricts rotation.

Single Bond = 1 $\sigma$
Double Bond = 1 $\sigma$ + 1 $\pi$
Triple Bond = 1 $\sigma$ + 2 $\pi$

Molecule Selection

Select Molecule Methane (CH₄) - Single Bonds Ethane (C₂H₆) - Single Bond Ethene (C₂H₄) - Double Bond Ethyne (C₂H₂) - Triple Bond

Show Atoms & Skeleton Show Sigma (σ) Bonds Show Pi (π) Bonds

Molecular Properties

Molecule Methane

C Hybridization sp³

Geometry Tetrahedral

Bond Angle 109.5°

Bond Accounting

Sigma ($\sigma$) Bonds 4

Pi ($\pi$) Bonds 0

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