I’m super excited to teach you the lewis structure of PF5 in just 5 simple steps.
Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of PF5 molecule.
So, if you are ready to go with these 5 simple steps, then let’s dive right into it!
Lewis structure of PF5 contains five single bonds between the Phosphorus (P) atom and each Fluorine (F) atom. The Phosphorus atom (P) is at the center and it is surrounded by 5 Fluorine atoms (F). The Phosphorus atom does not have a lone pair while all the 5 Fluorine atoms have 3 lone pairs.
Let’s draw and understand this lewis dot structure step by step.
(Note: Take a pen and paper with you and try to draw this lewis structure along with me. I am sure you will definitely learn how to draw lewis structure of PF5).
5 Steps to Draw the Lewis Structure of PF5
Step #1: Calculate the total number of valence electrons
Here, the given molecule is PF5 (Phosphorus pentafluoride). In order to draw the lewis structure of PF5, first of all you have to find the total number of valence electrons present in the PF5 molecule.
(Valence electrons are the number of electrons present in the outermost shell of an atom).
So, let’s calculate this first.
Calculation of valence electrons in PF5
- For Phosphorus:
Phosphorus is a group 15 element on the periodic table.
Hence, the valence electrons present in phosphorus is 5 (see below image).
- For Fluorine:
Fluorine is a group 17 element on the periodic table.
Hence, the valence electrons present in fluorine is 7 (see below image).
Hence in a PF5 molecule,
Valence electrons given by Phosphorus (P) atom = 5
Valence electrons given by each Fluorine (F) atom = 7
So, total number of Valence electrons in PF5 molecule = 5 + 7(5) = 40
Step #2: Select the center atom
While selecting the atom, always put the least electronegative atom at the center.
(Remember: Fluorine is the most electronegative element on the periodic table and the electronegativity decreases as we move right to left in the periodic table as well as top to bottom in the periodic table).
Here in the PF5 molecule, if we compare the phosphorus atom (P) and Fluorine atom (F), then the phosphorus is less electronegative than fluorine.
So, phosphorus should be placed in the center and the remaining 5 fluorine atoms will surround it.
Step #3: Put two electrons between the atoms to represent a chemical bond
Now in the above sketch of PF5 molecule, put the two electrons (i.e electron pair) between each phosphorus atom and fluorine atom to represent a chemical bond between them.
These pairs of electrons present between the Phosphorus (P) and Fluorine (F) atoms form a chemical bond, which bonds the phosphorus and fluorine atoms with each other in a PF5 molecule.
Step #4: Complete the octet (or duplet) on outside atoms. If the valence electrons are left, then put the valence electrons pair on the central atom
Don’t worry, I’ll explain!
In the Lewis structure of PF5, the outer atoms are fluorine atoms.
So now, you have to complete the octet on these fluorine atoms (because fluorine requires 8 electrons to have a complete outer shell).
Now, you can see in the above image that all the fluorine atoms form an octet.
Also, all the 40 valence electrons of PF5 molecule (as calculated in step #1) are used in the above structure. So there are no remaining electron pairs.
Hence there is no change in the above sketch of PF5.
Let’s move to the next step.
Step #5: Final step – Check the stability of lewis structure by calculating the formal charge on each atom
Now, you have come to the final step and here you have to check the formal charge on phosphorus atom (P) as well as each fluorine atom (F).
For that, you need to remember the formula of formal charge;
Formal charge = Valence electrons – Nonbonding electrons – (Bonding electrons)/2
- For Phosphorus:
Valence electrons = 5 (as it is in group 15)
Nonbonding electrons = 0
Bonding electrons = 10
- For Fluorine:
Valence electron = 7 (as it is in group 17)
Nonbonding electrons = 6
Bonding electrons = 2
|Formal charge||=||Valence electrons||–||Nonbonding electrons||–||(Bonding electrons)/2|
So you can see above that the formal charges on phosphorus as well as fluorine are “zero”.
Hence, there will not be any change in the above structure and the above lewis structure of PF5 is the final stable structure only.
Each electron pair (:) in the lewis dot structure of PF5 represents the single bond ( | ). So the above lewis dot structure of PF5 can also be represented as shown below.