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Lewis Structure Bf3

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Last Updated: 15 November 2020

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Three cases can be constructed that do not follow the Octet Rule, and as such, they are known as exceptions to the Octet Rule. Following the Octet Rule for Lewis Dot structure leads to the most accurate depictions of stable molecular and atomic structures and because of this, we always want to use the Octet Rule when drawing Lewis Dot Structures. However, it is hard to imagine that one rule could be followed by all molecules. There is always exception, and in this case, three exceptions. The Octet Rule is violated in these three scenarios: when there are odd number of Valence electrons when there are too few Valence electrons When there are too many Valence electrons, there are actually very few stable molecules with odd numbers of electrons that exist, since that unpaired electron is willing to react with other unpaired electrons. Most odd electron species are highly reactive, which we call Free Radicals. Because of their instability, Free Radicals Bond to atoms in which they can take electrons from in order to become stable, making them very chemically reactive. Radicals are found as both reactants and products, but generally react to form more stable molecules as soon as they can. To emphasize the existence of unpaired electron, Radicals are denoted with Dot in front of their chemical symbol as with {matheq}{\cdot}OH{endmatheq} hydroxyl radical. The example of radical you may be familiar with already is gaseous chlorine atom, denote {matheq}{\cdot}Cl{endmatheq} interestingly, molecules with an odd number of Valence electrons will always be paramagnetic. Example 2: {matheq}SO_4^{-2}{endmatheq} ion sulfate ion, SO 4-2. Is ion that prefers expand Octet structure. Strict adherence to Octet Rule forms following Lewis structure: if we look at formal charges on this molecule, we can see that all of the oxygen atoms have seven electrons around them. This is one more electron than the number of Valence electrons then they would have normally, and as such, each of the oxygen atoms in this structure has a formal charge of-1. Sulfur has four electrons around it in this structure, which is two electrons fewer than the number of Valence electrons it would have normally, and as such it carries a formal charge of + 2. If instead we make structure for sulfate ion with expanded Octet, it would look like this: looking at formal charges for this structure, sulfur ion has six electrons around it. This is the same amount as the number of Valence electrons it would have naturally. This leaves sulfur with a formal charge of zero. Two oxygens that have double bonds to sulfur have six electrons each around them. This is the same amount of electrons as the number of Valence electrons that oxygen atoms have on their own, and as such, both of these oxygen atoms have a formal charge of zero.

* Please keep in mind that all text is machine-generated, we do not bear any responsibility, and you should always get advice from professionals before taking any actions.

* Please keep in mind that all text is machine-generated, we do not bear any responsibility, and you should always get advice from professionals before taking any actions

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* Please keep in mind that all text is machine-generated, we do not bear any responsibility, and you should always get advice from professionals before taking any actions.

* Please keep in mind that all text is machine-generated, we do not bear any responsibility, and you should always get advice from professionals before taking any actions

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