Final answer:
To complete the Lewis structure for serotonin, consider valence electrons and form sigma and pi bonds. A sigma bond involves orbital overlap while pi bonds result from the side-by-side overlap of p orbitals. The sigma bond between nitrogen and carbon involves the overlap of sp hybridized orbitals.
Step-by-step explanation:
To complete the Lewis structure for serotonin, you need to follow the standard rules for drawing Lewis structures, considering valence electrons and the octet rule. Serotonin has a complex structure that includes several nitrogen and carbon atoms, each of which can form sigma and pi bonds.
A sigma bond (σ bond) is formed by the head-to-head overlap of orbitals, typically s-s or s-p orbital overlap, and constitutes a single bond between atoms. In contrast, a pi bond (π bond) involves the side-to-side overlap of p orbitals. In molecules like HCN, there is one σ bond and two π bonds. For the molecule N₂, the triple bond consists of one σ bond and two π bonds, which arises from the side-by-side overlap of p orbitals as described in valence bond theory.
When discussing the sigma bond between nitrogen and carbon atoms, as in nitrogen 2 and carbon 2, it's generally the overlap of an sp² or sp hybrid orbital of nitrogen with an sp² or sp hybrid orbital of carbon that forms this type of bond.