So you have seen the above image by now, right?
Let me explain the above image in short.
BeF2 lewis structure has a Beryllium atom (Be) at the center which is surrounded by two Fluorine atoms (F). There are 2 single bonds between the Beryllium atom (Be) and each Fluorine atom (F). There are 3 lone pairs on both the Fluorine atoms (F).
If you haven’t understood anything from the above image of BeF2 (beryllium difluoride) lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of BeF2.
So let’s move to the steps of drawing the lewis structure of BeF2.
Steps of drawing BeF2 lewis structure
Step 1: Find the total valence electrons in BeF2 molecule
In order to find the total valence electrons in a BeF2 (beryllium difluoride) molecule, first of all you should know the valence electrons present in beryllium 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 beryllium as well as fluorine using a periodic table.
Total valence electrons in BeF2 molecule
→ Valence electrons given by beryllium atom:
You can see the 2 valence electrons present in the beryllium 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 BeF2 molecule = valence electrons given by 1 beryllium atom + valence electrons given by 2 fluorine atoms = 2 + 7(2) = 16.
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 BeF2 (beryllium difluoride) and it contains beryllium atom (Be) and fluorine atoms (F).
You can see the electronegativity values of beryllium atom (Be) and fluorine atom (F) in the above periodic table.
If we compare the electronegativity values of beryllium (Be) and fluorine (F) then the beryllium atom is less electronegative.
So here the beryllium atom (Be) 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 BeF2 molecule, you have to put the electron pairs between the beryllium atom (Be) and fluorine atoms (F).
This indicates that the beryllium (Be) and fluorine (F) are chemically bonded with each other in a BeF2 molecule.
Step 4: Make the outer atoms stable
Now in this step, you have to check the stability of the outer atoms.
Here in the sketch of BeF2 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 BeF2 molecule.
The BeF2 molecule has a total 16 valence electrons and all these valence electrons are used in the above sketch of BeF2.
Hence there are no remaining electron pairs to be kept on the central atom.
So now let’s proceed to the next step.
Step 5: Check the stability of the central atom
In this step, you have to check whether the central beryllium atom (Be) is stable or not.
Now beryllium requires only 4 electrons to become stable. The s-orbitals of beryllium get completely filled by these 4 electrons.
You can see from the above picture that the beryllium atom has 4 electrons and hence it is stable.
Now let’s proceed to the final step to check whether the lewis structure of BeF2 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 BeF2.
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 beryllium (Be) atom as well as fluorine (F) atoms present in the BeF2 molecule.
For calculating the formal charge, you have to use the following formula;
Formal charge = Valence electrons – (Bonding electrons)/2 – Nonbonding electrons
For Beryllium (Be) atom:
Valence electrons = 2 (because beryllium is in group 2)
Bonding electrons = 4
Nonbonding electrons = 0
For Fluorine (F) atom:
Valence electron = 7 (because fluorine is in group 17)
Bonding electrons = 2
Nonbonding electrons = 6
From the above calculations of formal charge, you can see that the beryllium (Be) atom as well as fluorine (F) atom has a “zero” formal charge.
This indicates that the above lewis structure of BeF2 is stable and there is no further change in the above structure of BeF2.
In the above lewis dot structure of BeF2, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of BeF2.
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:
|N2H2 lewis structure
|CH3Cl lewis structure
|HBr lewis structure
|N2H4 lewis structure
|CH3NH2 lewis structure
|SiO2 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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