Answer: The CORRECT option is 1 ,2 and 3. Therefore all of the above.
Step-by-step explanation:
Hybrid orbitals results when atoms are bound together in a molecule, the wave functions combine to produce new mathematical descriptions that have different shapes. The wave functions combine through a process called hybridisation. The following are characteristics of hybrid orbitals
- The number of atomic orbitals combined is always equals to the number of hybrid orbitals formed. This is in accordance with the bonding theory which states that atomic orbitals can mix together or hybridise to become hybrid orbitals that are equal in energy.
- When atomic orbitals are hybridized, the s orbital and at least one p orbital are always hybridized. The p orbital electrons would form stronger (higher energy bonds) than the s orbital electrons. This leads to formation of different geometrical structures such as linear electron pair in sp hybridisation, trigonal electron - pair in sp² hybridisation.
- To create tetrahedral structures, the s orbital and all three p orbitals must be hybridized. This is so as the 2s orbitals and all three of the 2p orbitals( px, Py and pz) hybridize to form four sp³orbital which are oriented at a bond angle of 109.5° from each other. This arrangement gives the tetrahedral geometrical shape.