![]() ![]() And that's because all of the noble gasses have full outer shells. They're very content, they don't wanna messĪround with anyone else. They're known as the noble gasses because they're very unreactive, We have around this octet rule are the group 18 elements right over here, also known as the noble gasses. Only has two electrons, is very, very, very stable. Octet rule is the first shell, where it is full with two electrons. For our second, third, fourth,įifth, and on and on shells, you're full when you have eight electrons. So just to remind ourselves, what does it mean to haveĪ full, full outer shell? Well, in general, people To having a full outer shell, either by losing electrons Video, I'm gonna focus most on the extremes of the periodic table, the groups at the left and the right, because those are the closest Similar valence electrons will have similar reactivities, ![]() Remember, valence electronsĪre the reactive electrons, the ones that might Have similar properties is, in most cases, they have the same number of valence electrons. The elements in a given column might have very different atomic numbers, they all have similar properties. When we talk about a group, we're just talking about a column. And in particular, we're going to focus on groups of the periodic table of elements. I hope you have completely understood all the above steps.įor more practice and better understanding, you can try other lewis structures listed below.- In this video, we're gonna gain even more appreciation for why the periodic table By doing so, you will get the following lewis structure of SiF4. In the above lewis dot structure of SiF4, you can also represent each bonding electron pair (:) as a single bond (|). This indicates that the above lewis structure of SiF4 is stable and there is no further change in the above structure of SiF4. You can see the number of bonding electrons and nonbonding electrons for each atom of SiF4 molecule in the image given below.įor Silicon (Si) atom: Valence electrons = 4 (because silicon is in group 14) Bonding electrons = 8 Nonbonding electrons = 0įor Fluorine (F) atom: Valence electron = 7 (because fluorine is in group 17) Bonding electrons = 2 Nonbonding electrons = 6 Formal chargeįrom 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. 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.įor calculating the formal charge, you have to use the following formula įormal charge = Valence electrons – (Bonding electrons)/2 – Nonbonding electrons The stability of lewis structure can be checked by using a concept of formal charge. ![]() Now you have come to the final step in which you have to check the stability of lewis structure of SiF4. Step 6: Check the stability of lewis structure Total valence electrons in SiF4 molecule = valence electrons given by 1 silicon atom + valence electrons given by 4 fluorine atoms = 4 + 7(4) = 32. You can see the 7 valence electrons present in the fluorine atom as shown in the above image. Hence the valence electron present in fluorine is 7. → Valence electrons given by fluorine atom:įluorine is group 17 element on the periodic table. You can see the 4 valence electrons present in the silicon atom as shown in the above image. Hence the valence electrons present in silicon is 4. Silicon is a group 14 element on the periodic table. → Valence electrons given by silicon atom: Here, I’ll tell you how you can easily find the valence electrons of silicon as well as fluorine using a periodic table. (Valence electrons are the electrons that are present in the outermost orbit of any atom.) 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. Steps of drawing SiF4 lewis structure Step 1: Find the total valence electrons in SiF4 molecule ![]()
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