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Complete the lewis structure for serotonin

1. what is the geometry of nitrogen 1
2. what is the shape around oxygen
3. what is the geometry around Carbon 1
4. what is the hybridization around Carbon 2
5. how many pi bonds
6. what orbitals overlap to form the sigma bond between nitrogen 2 and carbon 2

User Jkemming
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1 Answer

4 votes

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.

User Nick Patsaris
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