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chem: fix and clarify formal charges

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eggy 2020-10-08 22:06:38 -04:00
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@ -318,10 +318,10 @@ There may be several correct ways to draw covalent bonds in Lewis structures and
The formal charge of an atom can be calculated using the following equation: The formal charge of an atom can be calculated using the following equation:
$$\text{Formal charge} = \text{# of valence electrons of element} - \text{# of unpaired electrons} - \text{# of covalent bonds}$$ $$\text{Formal charge} = \text{# of valence electrons of element} - \text{# of unpaired electrons} - \text{# of covalent bonds}$$
To find the best structure for a covalently bonded compound, the formal charge of all atoms in that compound should be **minimised**. To find the best structure for a covalently bonded compound, the **absolute value** of the formal charge of all atoms in that compound should be **minimised**. Positively charged atoms will even accept **dative covalent bonds** from other atoms with negative formal charges.
!!! warning !!! warning
Some elements want formal charges of zero so much that they break the octet rule. These elements are $\text{P, S, Cl, Br, I, and Xe}$. To do so, they will accept **dative covalent bonds** from other atoms with opposite formal charges. This brings the formal charges of both atoms closer to zero by one. Some elements want formal charges of zero so much that they break the octet rule. These elements are $\text{P, S, Cl, Br, I, and Xe}$.
### Resonance structures ### Resonance structures