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Lone pairs are pairs of electrons in the valence shell that are not shared with another atom through bonding. The lone pairs in a lewis structure are the pairs of electrons that are drawn as dots around the atom. For example, in NH3, N has one lone pair of electrons because it shares six with the three Hydrogens and two are left over.
When you look at a lewis structure, the lone pairs are the dots around the electrons, NOT the electrons that are shared through the line. Also, if there are 4 dots (example: Oxygen has one line representing two shared electrons and four dots around the electron) that means there are 4 lone pairs, NOT two pairs.
Katherine Brenner 3H wrote:Will you have lone pairs during an ionic bond?
In covalent Lewis Dot Structures, we usually look at shared electrons vs. lone pairs, but in ionic bonds, we don't have those shared electrons, so technically all the electrons are lone pairs.
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