lone pairs
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Re: lone pairs
check the formal charges and also if its a hydrogen, it wouldn't have more than a single bond or if its a halogen (Group 7 elements), they usually like single bonds too, so any extra electrons would go on the central atom.
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Re: lone pairs
Also, check the octet rule to see if the central atom can hold more than 8 e- (whether those be lone pairs and/or bonds).
Re: lone pairs
Do your normal lewis diagram and ensure all electrons are accounted for. If all bound atoms are full it means there is most likely a central atom with an expanded octet.
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Re: lone pairs
Make sure to check the valence electrons and remember that the atom that is more electronegative will hold more electrons.
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Re: lone pairs
You would have to consider the total number of electrons, formal charges, the octet rule, and exceptions to the octet rule to know when to add a lone pair.
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Re: lone pairs
AnayaArnold_3L wrote:Do lone pairs automatically make a molecule nonpolar?
Yes, lone pairs disrupt symmetry, which makes molecules polar.
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