[nerd32]

Im having some trouble on my chem work

From the resonance structure in the picture above, im supposed to determine the hybridizations and geometries about the carbon and oxygen atom that have arrows pointing to them.
I got the geometry for the carbon atom to be trigonal planar, but i don't know how to find the geometry for the oxygen atom.(basically determine the number of bonding and lone electron pairs)

[Boxxxed]

Find out how many electron clouds around oxygen with lewis diagram

[nerd32]

yeah, i figured it out


Also, how do I tell if the atoms are in the same plane...Im not by my book right now but I assume that the molecular geometry will tell me?

[Boxxxed]

Look at the electron geometry first if there are lone pairs. The lone pairs on the central atom will influence the molecular geometry.

For example if there are 3 electron clouds, 1 of them a lone pair then the electron geometry would be trigonal planar, but the molecular geometry doesn't count the lone pair and so it would be a bent molecule. Electron clouds will space themselves out as far from eachother as possible. Lone pairs and double bonds have greater repulsion effect than single bonds

In this case, ignore the fact that there are single and double bonds in this molecule and focus solely on the orientation of the lone pair to the bonds themselves.

[rabolisk]

sp2 hybridized carbons will have a trigonal planar geometry if it is bonded to three atoms and will be in the same plane as these three atoms. It only makes sense since the geometry is called trigonal planar. It must be true, then, that two sp2 hybridized carbons with an atom in between them will be in the same plane. Of course, this extends to atoms other than just carbon.