![]() When there is no main center atom, we label the geometry based on what central atom we choose. ![]() When we label a molecule's geometry, we base it on the center atom's geometry. Sp2/double-bond hybridized orbitals have the trigonal planar geometry. Next, double-bond/sp 2 hybridized orbitals form the trigonal planar geometry: The bottom three orbitals are all on one plane, with the top orbital sticking upward. In a tetrahedral, the bond lengths and bond angles are all the same. Sp3/single-bond hybridized orbitals form the tetrahedral geometry. Electrons repel each other, so each geometry maximizes the distance between orbitals.įirst up are single-bond/sp 3 hybridized orbitals, which have the tetrahedral geometry: Sp 3, sp and sp 2 Hybridization and bond anglesĮach type of hybridization has its own geometry. Lastly, let's look at triple-bond hybridization (sp-hybridization). The π-bond is shown as a dotted line since the electrons in the bond are in the p-orbitals, not the sp 2 orbitals as shown. The carbon p-orbitals overlap to form the second bond in the carbon-carbon double bond (π-bond). Like before, the carbon hybridized orbitals (here sp 2 orbitals) overlap with hydrogen's s-orbital to form single bonds. The unhybridized carbon p-orbitals overlap to form the other bond in the carbon-carbon double bond (π-bond). Also, the 2sp 2 orbitals are lower in energy than the 2p orbital, since the energy level is an average of the s and p energy levels.Ĭarbon's sp2 orbitals overlap with hydrogen's s-orbital and the other carbon's sp2 orbital to form single (σ) bonds. Π-bonds can only be formed with orbitals of "p" energy or higher, so it is left untouched. The 2p-orbital is left unhybridized to form the C=C π-bond. Let's look at an example with C 2H 6 (ethane): Carbon hybridizes 1 2s orbital and 2 2p orbitals to form 3 sp2 orbitals, leaving one 2p orbital unhybridized. The sp 2 hybrid orbitals form 3 equal σ-bonds and the unhybridized p-orbitals forms the π-bond. Sp 2 hybridization ( double- bond hybridization) involves the "mixing" of 1 s- and 2 p-orbitals into 3 sp 2 orbitals. However, this theory doesn't perfectly explain all types of bonds, which is why the hybridization theory was created. When orbitals directly overlap, that is called a σ-bond and a sideways overlap is a π-bond. It states that two orbitals, each with one electron, overlap to form a bond. There are two theories that describe how bonds are made and what they look like.
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