![]() The electronic configuration of the Phosphorus atom in excited state is 1s2 2s2 2p6 3s2 3px1 3py1 3pz1. When it is in an excited state, one of the electrons in the s-orbital moves to the d-orbital and the valence electrons of p orbitals get unpaired to move to the higher orbitals. Phosphorus’s electronic configuration in its ground state is 1s2 2s2 2p6 3s2 3p2 as the total number of valence electrons is 5. Here three Chlorine atoms are bonded with Phosphorus atom, which means that there formation of hybrid orbitals that accommodate these shared electrons. Hence the electron geometry of Phosphorus Trichloride is tetrahedral.PCl3 HybridizationThe hybridization of PCl3 can be determined once we know the Lewis dot structure of this molecule. This pair of electrons is the nonbonding pair of electrons for this molecule.PCl3 Electron GeometryWhen you look at the Lewis Structure of the molecule, you can see that electrons’ arrangement is in a tetrahedral geometry. However, Phosphorus is left with two valence electrons that do not participate in forming any bond. Chlorine atom shares one valence electron of Phosphorus to complete its octet.Now if you look at the molecule, every Chlorine atom has a complete octet as it has eight valence electrons in its outer shell. To show bonds between Phosphorus and Chlorine atoms, draw a straight line to show the bond formation.Each bond uses up two valence electrons which means we have used a total of six valence electrons. So, Phosphorus atoms will take the central position as it is less electronegative than the Chlorine atom.Place Phosphorus in the centre and all the other chlorine atoms around it. In contrast, the ones that do not participate in bond formation are called lone pair of nonbonding pair of electrons.Here we will first place the atoms along with its individual valence electrons to understand the bond formation. ![]() The Lewis Structure for any molecule helps to know the arrangement of valence electrons in the molecule, bond formation and the number of bonding as well as nonbonding pairs of electrons.The electrons that participate in forming bonds are called bonding pairs of electrons. To calculate the total number of valence electrons of this molecule, we will add up the valence electrons of both Phosphorus and Chlorine atoms.Phosphorus has five valence electrons.Chlorine has seven valence electrons, but as there are three atoms of Chlorine, we will multiply this number by 3.Total number of valence electrons of PCl3: Valence electrons of Phosphorus + Valence electrons of Chlorine= 5 + 7*3= 26Phosphorus Trichloride (PCl3) has a total of 26 valence electrons.PCl3 Lewis StructureNow that we know the total number of valence electrons for Phosphorus Trichloride, we will start drawing the Lewis Dot Structure for this molecule. In this blog post, we will go through the total number of valence electrons, Lewis dot structure, shape and more.ContentsPCl3 Valence ElectronsPCl3 Lewis StructurePCl3 Electron GeometryPCl3 HybridizationPCl3 Molecular GeometryPCl3 Bond AnglePCl3 ShapeIs PCl3 polar or nonpolar? PCl3 Valence ElectronsOne needs to know the total number of valence electrons for a molecule to construct the Lewis Dot Structure. ![]() To understand any molecule’s chemical and physical properties, it is essential to know the Lewis structure and its molecular geometry.
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