Chemistry Reference
In-Depth Information
nitrogen is connected to its bound atoms and lone electron pair in a tetrahedral
geometry. Please note that because the nitrogen is only bound to three atoms, the
tetrahedral relationship between the bound atoms and lone electron pair can also
be referred to as trigonal pyramidal (not considering the contributions of the lone
electron pair to the geometry) because the geometry represents a three-sided
pyramid.
The highlighted bond joins a methyl carbon atom to an imine nitrogen atom. The
methyl carbon atom, being joined to three hydrogen atoms and an imine nitrogen
atom, is bound to four separate atoms and is, therefore, sp
3
hybridized. The imine
nitrogen atom is bound to a methyl carbon atom through a single bond and to a
second carbon atom through a double bond. Additionally, the imine nitrogen pos-
sesses one lone electron pair. Therefore, because the imine nitrogen is bound to
two separate atoms and possesses one lone electron pair, this nitrogen is sp
2
hybri-
dized. Based on the atomic hybridizations, the methyl carbon is connected to its
bound atoms in a tetrahedral geometry, and the imine nitrogen is connected to its
bound atoms and lone electron pair in a trigonal planar geometry. Please note that
the molecular structure is referred to as bent.
The highlighted bond joins a nitrile carbon atom to a hydroxy oxygen atom. The
nitrile carbon atom, being joined to a nitrogen atom via a carbon-nitrogen triple
bond, can only be joined to one additional atom. Therefore, this atom is sp hybri-
dized. However, the hydroxy oxygen is joined to the nitrile carbon and one hydrogen
atom. Additionally, the hydroxy oxygen possesses two lone electron pairs.
Therefore, because the hydroxy oxygen is bound to two separate atoms and pos-
sesses two lone electron pairs, this oxygen is sp
3
hybridized. Based on the atomic
hybridizations, the nitrile carbon is connected to its bound atoms in a linear geome-
try, and the hydroxy oxygen is connected to its bound atoms and lone electron pairs
