So you have seen the above image by now, right?
Let me explain the above image in short.
OF2 lewis structure has an Oxygen atom (O) at the center which is surrounded by two Fluorine atoms (F). There are 2 single bonds between the Oxygen atom (O) and each Fluorine atom (F). There are 2 lone pairs on the Oxygen atom (O) and 3 lone pairs on both the Fluorine atoms (F).
If you haven’t understood anything from the above image of OF2 (oxygen difluoride) lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of OF2.
So let’s move to the steps of drawing the lewis structure of OF2.
Steps of drawing OF2 lewis structure
Step 1: Find the total valence electrons in OF2 molecule
In order to find the total valence electrons in OF2 (oxygen difluoride) molecule, first of all you should know the valence electrons present in oxygen atom as well as fluorine atom.
(Valence electrons are the electrons that are present in the outermost orbit of any atom.)
Here, I’ll tell you how you can easily find the valence electrons of oxygen as well as fluorine using a periodic table.
Total valence electrons in OF2 molecule
→ Valence electrons given by oxygen atom:
You can see the 6 valence electrons present in the oxygen atom as shown in the above image.
→ Valence electrons given by fluorine atom:
You can see the 7 valence electrons present in the fluorine atom as shown in the above image.
Total valence electrons in OF2 molecule = valence electrons given by 1 oxygen atom + valence electrons given by 2 fluorine atoms = 6 + 7(2) = 20.
Step 2: Select the central atom
For selecting the center atom, you have to remember that the atom which is less electronegative remains at the center.
Now here the given molecule is OF2 (oxygen difluoride) and it contains oxygen atom (O) and fluorine atoms (F).
You can see the electronegativity values of oxygen atom (O) and fluorine atom (F) in the above periodic table.
If we compare the electronegativity values of oxygen (O) and fluorine (F) then the oxygen atom is less electronegative.
So here the oxygen atom (O) is the center atom and the fluorine atoms (F) are the outside atoms.
Step 3: Connect each atoms by putting an electron pair between them
Now in the OF2 molecule, you have to put the electron pairs between the oxygen atom (O) and fluorine atoms (F).
This indicates that the oxygen (O) and fluorine (F) are chemically bonded with each other in a OF2 molecule.
Step 4: Make the outer atoms stable. Place the remaining valence electrons pair on the central atom.
Now in this step, you have to check the stability of the outer atoms.
Here in the sketch of OF2 molecule, you can see that the outer atoms are fluorine atoms.
These outer fluorine atoms are forming an octet and hence they are stable.
Also, in step 1 we have calculated the total number of valence electrons present in the OF2 molecule.
The OF2 molecule has a total 20 valence electrons and out of these, only 16 valence electrons are used in the above sketch.
So the number of electrons which are left = 20 – 16 = 4.
You have to put these 4 electrons on the central oxygen atom in the above sketch of OF2 molecule.
Now let’s proceed to the next step.
Step 5: Check the octet on the central atom
In this step, you have to check whether the central oxygen atom (O) is stable or not.
In order to check the stability of the central oxygen (O) atom, we have to check whether it is forming an octet or not.
You can see from the above picture that the oxygen atom is forming an octet. That means it has 8 electrons.
And hence the central oxygen atom is stable.
Now let’s proceed to the final step to check whether the lewis structure of OF2 is stable or not.
Step 6: Check the stability of lewis structure
Now you have come to the final step in which you have to check the stability of lewis structure of OF2.
The stability of lewis structure can be checked by using a concept of formal charge.
In short, now you have to find the formal charge on oxygen (O) atom as well as fluorine (F) atoms present in the OF2 molecule.
For calculating the formal charge, you have to use the following formula;
Formal charge = Valence electrons – (Bonding electrons)/2 – Nonbonding electrons
For Oxygen (O) atom:
Valence electrons = 6 (because oxygen is in group 16)
Bonding electrons = 4
Nonbonding electrons = 4
For Fluorine (F) atom:
Valence electron = 7 (because fluorine is in group 17)
Bonding electrons = 2
Nonbonding electrons = 6
This indicates that the above lewis structure of OF2 is stable and there is no further change in the above structure of OF2.
In the above lewis dot structure of OF2, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of OF2.
I hope you have completely understood all the above steps.
For more practice and better understanding, you can try other lewis structures listed below.
Try (or at least See) these lewis structures for better understanding:
|NF3 lewis structure
|CCl4 lewis structure
|CS2 lewis structure
|SF6 lewis structure
|PH3 lewis structure
|NO lewis structure
Jay is an educator and has helped more than 100,000 students in their studies by providing simple and easy explanations on different science-related topics. He is a founder of Pediabay and is passionate about helping students through his easily digestible explanations.
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