Answer : The Lewis-dot structure of [tex]Cl_3PO[/tex] is shown below.
Explanation :
Lewis-dot structure : It shows the bonding between the atoms of a molecule and it also shows the unpaired electrons present in the molecule.
In the Lewis-dot structure the valance electrons are shown by 'dot'.
The given molecule is, [tex]Cl_3PO[/tex]
As we know that chlorine has '7' valence electrons, phosphorous has '5' valence electrons and oxygen has '6' valence electrons.
Therefore, the total number of valence electrons in [tex]Cl_3PO[/tex] = 3(7) + 5 + 6 = 32
According to Lewis-dot structure, there are 10 number of bonding electrons and 22 number of non-bonding electrons.
Now we have to determine the formal charge for each atom.
Formula for formal charge :
[tex]\text{Formal charge}=\text{Valence electrons}-\text{Non-bonding electrons}-\frac{\text{Bonding electrons}}{2}[/tex]
[tex]\text{Formal charge on O}=6-4-\frac{4}{2}=0[/tex]
[tex]\text{Formal charge on P}=5-0-\frac{10}{2}=0[/tex]
[tex]\text{Formal charge on }Cl_1=7-6-\frac{2}{2}=0[/tex]
[tex]\text{Formal charge on }Cl_2=7-6-\frac{2}{2}=0[/tex]
[tex]\text{Formal charge on }Cl_2=7-6-\frac{2}{2}=0[/tex]
Hence, the Lewis-dot structure of [tex]Cl_3PO[/tex] is shown below.
