00:01
For a molecule, for all the atoms in the molecule to be in the same plane, they need to be in a square planar, trigonal planar, or linear geometry.
00:11
If we draw the lewis structure for h2co, we end up with a double bond to the, of the oxygen to the carbon, and then two single bonds of hydrogen to the carbon.
00:28
This ends up being square planar, so this one is definitely, definitely has all of its atoms in the same plane.
00:42
The next is c2h6.
00:46
If we draw its lewis structure, we're going to get this, with four electron groups surrounding each carbon.
00:58
It is tetrahedral around each carbon, and tetrahedral is not planar, so these atoms would not be in the same plane.
01:09
Pf3, if we draw its lewis structure, we're going to end up with enough electrons to add to all of the fluorines, so that each fluorine has an octet, and we'll have two more that we can add to phosphorus.
01:32
So with four electron groups, one of them being a lone pair, this is trigonal, sorry, i don't know why i said square planar, this is trigonal planar, and this one is trigonal pyramidal, and if it has a pyramid shape, then the atoms are not in, all in the same plane.
01:57
Then we have c2h4, which is going to have a carbon, two carbons, doubly bonded to each other, and off of each carbon we have two hydrogens, three electron groups around each carbon, all being bonding, just like up here, gives us a trigonal planar geometry...