Actually I am looking at VSEPR chart now, but SP2 is trigonal planar with 3 sigma bonds, but bent or angular with two bond with one loan pair which give us <120
(and there is a lone pair on nitrogen Jbarr29) Nitrogen has 5 valence electrons. It usually it makes 3 bonds, like it did here, and the last 2 are a lone pair.
This is in chad's first organic chem video. The molecule has 3 electron domains. 1 from the double bond (we count it as one), a lone pair on N, and the H. 3 electron domains = sp2 = 120 degrees. Think of it as a wheel. A wheel adds up to 360 degrees. If you have 3 things then 360/3 = 120. For other molecules this gets more confusing since they can do 3d structures etc.
Notice the above method uses Molecular orbital theory, but there is another theory which you are using, the VSEPR.
If you are using the VSEPR model. Does this problem ask for the geometry of the electrons or the molecule? Because if it asks for electrons then it is trigonal planar and 120 degrees. If it is asking about the molecule then it is bent and less than 120 degrees and you ignore the lone pair. Here is a table
http://intro.chem.okstate.edu/1314f00/lecture/chapter10/vsepr.html
For example look at this taken from wikipedia:
The
ammonia molecule (NH3) has three pairs of electrons involved in bonding, but there is a lone pair of electrons on the nitrogen atom. It is not bonded with another atom; however, it influences the overall shape through repulsions. There are four regions of electron density. Therefore, the overall orientation of the regions of electron density is tetrahedral. On the other hand, there are only three outer atoms (the lone pair does not count, count only the H's). This is referred to as an AX3E type molecule because the lone pair is represented by an E. The observed shape of the molecule is a trigonal pyramid, because the lone pair is not "visible" in experimental methods used to determine molecular geometry. The shape of a molecule is found from the relationship of the atoms even though it can be influenced by lone pairs of electrons.