Coordinate Bond
Visualize how one atom supplies both electrons to form a bond. Explore NH₄⁺ formation, CO's triple bond, and metal complexes with interactive orbital animations.
About this simulation
- What
- An interactive Chemistry simulation of Coordinate Bond.
- Who
- Designed for AP, IB, and A‑Level Chemistry students.
- How
- Runs in any modern browser — drag, adjust, and explore in real time.
Updated 2026-04-08
Key Concepts
Lone Pair Donation
A coordinate bond forms when one atom (the donor / Lewis base) provides both electrons in the shared pair to another atom (the acceptor / Lewis acid) with an empty orbital.
Identical Once Formed
After formation, a coordinate bond is indistinguishable from an ordinary covalent bond — same bond length, same bond energy, same geometry.
Metal Complexes
Ligands (like H₂O or NH₃) donate lone pairs into empty d orbitals of transition metal ions, forming coordination compounds with characteristic colors.
Understanding Coordinate Bonds
A Coordinate Bond (also called a dative covalent bond) is a type of covalent bond where both electrons in the shared pair come from the same atom. The donor atom has a lone pair, and the acceptor atom has an empty orbital.
This mechanism is fundamental to understanding ammonium ion (NH₄⁺) formation, the unusual strength of the carbon monoxide (CO) triple bond, and the colorful world of transition metal complexes.
Our interactive visualizer lets you watch the lone pair donation in real time, toggle orbital overlaps on and off, and build metal complexes by swapping different ligands.