I need to know how the octet rule, electron configuration sublevels and orbitals all go together.
I'm pretty sure that the octet rule states that atoms will move around and bond to become like the nearest noble gas.also that the outside orbital is what determines how many electrons it needs to "gain" to become like the nearest noble gas. so in electron configuration the numbers are S-2,P-6,D-10,F-14 i think those are just sublevels so then how does that tie in with regular orbitals and if thats true then why are the noble gases atomic number:2, 10,18,36,54, 86.i just don't understand how they all work together.
So as you can see I'm just really confused about all of this so if you could help it would be greatly appeiciated!
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The octet rule is actually a simple chemistry term, a rule of thumb, stating that atoms would tend to combine together so that they would have eight electrons each on their valence shell, which would give them the same electronic configuration as a noble gas, meaning have eight outermost electron shells, becoming stable.
Main energy levels and numbered 1 (which is the lowest energy level), 2 and 3 and so much on, and these levels are further split into sub-levels. The number of sub-levels in each main energy level actually equals to the number of the main energy level. But for what reason, these sub-levels were given unhelpful alphabets like s, p, d and f, which stand for sharp, principle, diffuse and fundamental. Each sub-levels further consists of many orbitals, which are usually odd number, and each orbital can consist of only 2 electrons.
For sub-level s, it consists of 1 orbital and have two electrons. For sub-level p, it consists of 3 orbitals and have six electrons. For sub-level d, it consits of 5 orbitals and have 10 electrons. For sub-level f, it consists of 7 orbitals and have 14 electrons.
Also there is another easy way to calculate the number of electrons that can be held in a given energy level, which is by using this formula- 2n^2.
Hope it helps to clear your doubt with electrons!
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