Bond order counts shared electron pairs: single, double, or triple.order 1 · length 154 pm · energy 347 kJ/mol

Single · Double · Triple Bonds

Shared pairs, sigma and pi orbitals, strength, length, and geometry

Workspace

Molecular bond laboratory

Model controls

Selected bond

Molecule family

Atomic separation154 pm

Model rotation0°

Electron density100%

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Molecular sound effects

Visual experiments

Live bond evidence

Bond order1

Bond length154 pm

Bond energy347 kJ/mol

Components1σ

Relationships

Bond order = shared electron pairs

Single: σ · Double: σ + π · Triple: σ + 2π

Higher order → shorter, usually stronger bond

A single bond contains one shared pair in one sigma bond.

Object focus

Tap an atom, sigma cloud, pi cloud, bond station, or molecule.

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Chapters

Learning objectives

Identify single, double, and triple covalent bonds.
Count shared electron pairs and bond order.
Separate sigma and pi orbital overlap.
Relate bond order to length, strength, geometry, and rotation.
Compare ethane, ethene, ethyne, H₂, O₂, and N₂.

Key relationships

Single: one shared pair and one sigma bond.

Double: two shared pairs, one sigma plus one pi.

Triple: three shared pairs, one sigma plus two pi.

Carbon trend: 154 → 134 → 120 pm as order rises.

Suggested experiments

Rotate each bond and inspect orbital overlap.
Reduce separation to compare electron density.
Switch between carbon and diatomic examples.
Compare length and energy indicators.

Questions for exploration

Why does a double bond restrict rotation?
Why is a triple-bonded carbon arrangement linear?
Why are three drawn lines not three rigid sticks?

Seven-question bond-order check

Answer all seven questions.

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