eiii so this group still dey

prime science lab was gold

now everyone is busy handling diff. stuffs

and ofc today's kids don't like learning 😔👍

🙇
@edsciencelab 📚👨‍🔬

PCl₅ (Phosphorus pentachloride) is a common laboratory compound, most commonly used as a chlorinating agent (chlorine adder) in organic synthesis.

It is also often presented to students as an example of breaking the octet rule (8 electron rule). The octet rule arises due to the fact that, in most cases, for an atom to achive its most stable state, it must have the s²p⁶ configuration.

While this is commonly the case for elements like Carbon or Oxygen, Phosphorus in this molecule doesn't follow the rule. As you can see, since there are 5 chlorine atoms bonded to the Phosphorus atom, it has 10 electrons around it.

In this molecule, the electronic configuration around the Phosphorus atom is a hybridization of the 3s,3p and 3d subshells, creating 5 sp³d hybridized orbitals.

This hybridization occurs by the excitation of an electron in the 3s subshell, up to the 3d subshell.

The hybridization of these orbitals allows Phosphorus to have 5 bonds. In the PCl₅ molecule, these bonds are made with 5 highly electronegetive Chlorine atoms.

They arrange themselves around the Phosphorus atom in the trigonal bipyramidal geometry according to VSEPR theory. This means that the Phosphorus atom is sorrounded on all sides by Chlorine atoms

@edsciencelab 📚👨‍🔬