In an sp^3 hybridization, color(red)"one" s orbital is mixed with color(red)"three" p orbitals to form color(red)"four" sp^3 hybridized orbitals. Each of these hybridized orbitals have 25% s character and 75% p character (calculated according to the proportion of s:p mixing). These sp^3 hybridized orbitals are oriented with bond angle of 109.5 degrees to minimize electron repulsion, in a tetrahedral geometry. An example of sp^3 hybridization can be seen in the carbons in ethane.
In an sp^2 hybridization, color(red)"one" s orbital is mixed with color(red)"two" p orbitals to form color(red)"three" sp^2 hybridized orbitals. Each of these hybridized orbitals have 33% s character and 67% p character. These sp^2 hybridized orbitals are oriented with bond angle of 120 degrees, in a trigonal planar (triangular) geometry. The remaining p orbital is unchanged and perpendicular to the plane of the hybridized orbitals. An example of sp^2 hybridization can be seen in the carbons in ethene.
In an sp hybridization, color(red)"one" s orbital is mixed with color(red)"one" p orbitals to form color(red)"two" sp hybridized orbitals. Each of these hybridized orbitals have 50% s character and 50% p character. These sp hybridized orbitals are oriented with bond angle of 180 degrees, in a linear geometry. The remaining two p orbitals are unchanged, and perpendicular to each other and the plane of the hybridized orbitals. An example of sp hybridization can be seen in the carbons in ethyne.
The mixing of orbitals can be seen here:
![Hybridization - Wikimedia Commons]()
Hybridization - Wikimedia Commons
Orientation of the hybridized orbitals in respective geometries:
![Formation and geometry of hybridized orbitals]()
Formation and geometry of hybridized orbitals
