So you have seen the above image by now, right?
Let me explain the above image in short.
SiF4 lewis structure has a Silicon atom (Si) at the center which is surrounded by four Fluorine atoms (F). There are 4 single bonds between the Silicon atom (Si) and each Fluorine atom (F). There are 3 lone pairs on all the four Fluorine atoms (F).
If you haven’t understood anything from the above image of SiF4 lewis structure, then just stick with me and you will get the detailed step by step explanation on drawing a lewis structure of SiF4.
So let’s move to the steps of drawing the lewis structure of SiF4.
Steps of drawing SiF4 lewis structure
Step 1: Find the total valence electrons in SiF4 molecule
In order to find the total valence electrons in a SiF4 molecule, first of all you should know the valence electrons present in silicon 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 silicon as well as fluorine using a periodic table.
Total valence electrons in SiF4 molecule
→ Valence electrons given by silicon atom:
You can see the 4 valence electrons present in the silicon 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 SiF4 molecule = valence electrons given by 1 silicon atom + valence electrons given by 4 fluorine atoms = 4 + 7(4) = 32.
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 SiF4 and it contains silicon atom (Si) and fluorine atoms (F).
You can see the electronegativity values of silicon atom (Si) and fluorine atom (F) in the above periodic table.
If we compare the electronegativity values of silicon (Si) and fluorine (F) then the silicon atom is less electronegative.
So here the silicon atom (Si) 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 SiF4 molecule, you have to put the electron pairs between the silicon atom (Si) and fluorine atoms (F).
This indicates that the silicon (Si) and fluorine (F) are chemically bonded with each other in a SiF4 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 SiF4 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 SiF4 molecule.
The SiF4 molecule has a total 32 valence electrons and all these valence electrons are used in the above sketch of SiF4.
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 octet on the central atom
In this step, you have to check whether the central silicon atom (Si) is stable or not.
In order to check the stability of the central silicon (Si) atom, we have to check whether it is forming an octet or not.
You can see from the above picture that the silicon atom is forming an octet. That means it has 8 electrons.
And hence the central silicon atom is stable.
Now let’s proceed to the final step to check whether the lewis structure of SiF4 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 SiF4.
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 silicon (Si) atom as well as fluorine (F) atoms present in the SiF4 molecule.
For calculating the formal charge, you have to use the following formula;
Formal charge = Valence electrons – (Bonding electrons)/2 – Nonbonding electrons
For Silicon (Si) atom:
Valence electrons = 4 (because silicon is in group 14)
Bonding electrons = 8
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 silicon (Si) atom as well as fluorine (F) atom has a “zero” formal charge.
This indicates that the above lewis structure of SiF4 is stable and there is no further change in the above structure of SiF4.
In the above lewis dot structure of SiF4, you can also represent each bonding electron pair (:) as a single bond (|). By doing so, you will get the following lewis structure of SiF4.
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:
|NH4+ lewis structure
|NH2- lewis structure
|AlCl3 lewis structure
|BeH2 lewis structure
|HNO lewis structure
|NI3 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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