How do you open the closed circle?
Romeo and Juliet were two of the great lovers of all time. Their embrace allowed no other person to be a part of it – they only wanted to be with each other. It took outside intervention (parents are like that!) to get them away from one another. Paired electrons are similar to the lovers. They do not bond covalently until they are unpaired. Then they can become a part of a larger chemical structure.
Hybrid Orbitals – sp and sp2
A beryllium hydride (BeH2) molecule is predicted to be linear by VSEPR. The beryllium atom contains all paired electrons and so must also undergo hybridization. One of the 2s electrons is first promoted to the empty 2px orbital (see Figure below).
Now the hybridization takes place only with the occupied orbitals and the result is a pair of sp hybrid orbitals. The two remaining p orbitals (py and pz) do not hybridize and remain unoccupied (see Figure below).
The geometry of the sp hybrid orbitals is linear, with the lobes of the orbitals pointing in opposite directions along one axis, arbitrarily defined as the x-axis (see Figure below). Each can bond with a 1s orbital from a hydrogen atom to form the linear BeH2 molecule.
Other molecules whose electron domain geometry is linear and for whom hybridization is necessary also form sp hybrid orbitals. Examples include CO2 and C2H2, which will be discussed in further detail later.
Boron trifluoride (BF3) is predicted to have a trigonal planar geometry by VSEPR. First a paired 2s electron is promoted to the empty 2py orbital (see Figure below).
This is followed by hybridization of the three occupied orbitals to form a set of three sp2 hybrids, leaving the 2pz orbital unhybridized (see Figure below).
The geometry of the sp2 hybrid orbitals is trigonal planar, with the lobes of the orbitals pointing towards the corners of a triangle (see Figure below). The angle between any two of the hybrid orbital lobes is 120°. Each can bond with a 2p orbital from a fluorine atom to form the trigonal planar BF3 molecule.
Other molecules with a trigonal planar electron domain geometry form sp2 hybrid orbitals. Ozone (O3) is an example of a molecule whose electron domain geometry is trigonal planar, though the presence of a lone pair on the central oxygen makes the molecular geometry bent. The hybridization of the central O atom of ozone is sp2.
- Paired electrons can be hybridized and then participate in covalent bonding.
Use the link below to answer the following questions. Only read the boron section.
- How many unpaired electrons are in the ground state of boron?
- Where does the boron get three unpaired electrons for bonding to form BCl3?
- What is the geometry of the BCl3?
- Does the ground state beryllium atom contain any unpaired electrons?
- Why does one 2s electron in Be get promoted to a 2p orbital?
- What is the geometry of the two sp orbitals?