Short instructional video explaining the Lewis structure of methanal (CH2O). Speakers (Charles Collingwood and a second speaker) outline atom counts, electron pairing and bonding: carbon forms a double bond to oxygen, two single bonds to hydrogens; oxygen has two lone pairs; the central carbon is trigonal planar with three regions of electron density.
The Lewis structure of methanal. Methanal has the formula CH2O.
So we need one carbon, one oxygen and two hydrogens. Now, the hydrogens must be bonded to.
The carbon or else the carbon wouldn't achieve enough bonds.
Carbon starts off with four electrons, and.
To bond to oxygen, it can use two pairs of electrons. Oxygen then is used up two of its electrons. It has got six electrons in the outer shell. It's used up two, so it has four more electrons. We can put two more electrons here.
And here on the oxygen.
This leaves the carbon, which has used two of its electrons. It's left with two more. That allows it to bond to.
A hydrogen. The hydrogen provides one electron and another hydrogen.
Provides another electron. So this is the Lewis structure. This oxygen has three regions of electron density around it. One double bond, two lone pairs. The carbon atom here has 1, 2, 3 regions. The central carbon atom. This means that the shape of the central carbon atom is trigonal planar.
