This simulator shows how atomic s and p orbitals mathematically combine into sp3, sp2, and sp hybrid orbitals, and how that mixing produces the tetrahedral, trigonal-planar, and linear geometries seen in real molecules like methane, ethylene, and acetylene.
Select a hybridization type to watch the atomic orbitals merge into hybrid orbitals in real time, then rotate the resulting molecule to inspect the bond angles and any leftover unhybridized p orbitals forming pi bonds.
Toggle between sp3, sp2, and sp hybridization modes and rotate the 3D molecule view to examine bond angles and pi-bond orientation from any angle.
The tetrahedral bond angle of roughly 109.5 degrees found throughout sp3 chemistry is the exact angle that maximizes the distance between four points arranged around a central point in three dimensions.
This simulator shows how atomic s and p orbitals mathematically combine into sp3, sp2, and sp hybrid orbitals, and how that mixing produces the tetrahedral, trigonal-planar, and linear geometries seen in real molecules like methane, ethylene, and acetylene.
This simulator shows how atomic s and p orbitals mathematically combine into sp3, sp2, and sp hybrid orbitals, and how that mixing produces the tetrahedral, trigonal-planar, and linear geometries seen in real molecules like methane, ethylene, and acetylene.
Select a hybridization type to watch the atomic orbitals merge into hybrid orbitals in real time, then rotate the resulting molecule to inspect the bond angles and any leftover unhybridized p orbitals forming pi bonds.
The tetrahedral bond angle of roughly 109.5 degrees found throughout sp3 chemistry is the exact angle that maximizes the distance between four points arranged around a central point in three dimensions.