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If you're drawing a Lewis Structure and a molecule doesn't have enough electrons to make a complete octet but its still relatively stable, like BF3, that would be a great candidate for a coordinate covalent bond. If a molecule with a free lone pair is there, like F- or ammonia, NH3, that molecule would donate both of the electrons needed for the coordinate covalent bond to form.
Basically, a coordinate covalent bond is not a typical bond. Instead of atoms each sharing two electrons, one of the atoms donates two electrons to share. I think this type of bond can be seen with an element that needs two more electrons to complete an octet. An example of this would be BF3 to BF4-
Coordinate covalent bond is when one atom shares two electrons (the donor) and the accepting atom just takes them. This often occurs when the acceptor does not get the 8 electrons (octet guideline) from the bonds with the other atoms.
Coordinate covalent bonds are also common between lewis acids and bases. Since lewis acids are electron pair acceptors and lewis bases are electron pair donors, the lewis base will donate both of its electrons to form a coordinate covalent bond with the lewis acid.
coordinate covalent bonds are when a lone element like F comes and donates both of their electrons to create covalent bond. Basically, the electrons are not shared and one of the compounds donates their two electrons to create a bond. This happens where there are partial positive and negative charges.
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