Bupropion, marketed as Wellbutrin, is a heavily prescribed medication used in the treatment of depression. Complete the following electron-dot structure for Bupropion by adding lone pairs of electrons.
(a) How many s and how many p bonds are in the molecule?

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Identify the types of bonds present in the molecule. In organic molecules, single bonds are typically sigma (\(\sigma\)) bonds, while double and triple bonds consist of one \(\sigma\) bond and one or two pi (\(\pi\)) bonds, respectively.

Count the number of single bonds in the Bupropion structure. Each single bond represents one \(\sigma\) bond.

Identify any double or triple bonds in the structure. For each double bond, count one \(\sigma\) bond and one \(\pi\) bond. For each triple bond, count one \(\sigma\) bond and two \(\pi\) bonds.

Sum the total number of \(\sigma\) bonds from single, double, and triple bonds to find the total number of \(\sigma\) bonds in the molecule.

Sum the total number of \(\pi\) bonds from double and triple bonds to find the total number of \(\pi\) bonds in the molecule.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electron-Dot Structures

Electron-dot structures, also known as Lewis structures, represent the valence electrons of atoms within a molecule. They illustrate how atoms are bonded together and show lone pairs of electrons that are not involved in bonding. Understanding how to draw these structures is essential for visualizing molecular geometry and predicting reactivity.

Types of Chemical Bonds

Chemical bonds can be classified into two main types: covalent bonds, which involve the sharing of electron pairs between atoms, and ionic bonds, which involve the transfer of electrons. In covalent bonds, the number of shared electron pairs determines whether the bond is a single (one pair), double (two pairs), or triple bond (three pairs). Recognizing these types is crucial for analyzing molecular structures.

Bonding and Lone Pairs

In a molecule, bonding pairs of electrons are involved in forming bonds between atoms, while lone pairs are pairs of valence electrons that are not shared with other atoms. The presence of lone pairs can influence the shape and polarity of the molecule, as well as its reactivity. Identifying the number of bonding and lone pairs is key to understanding the overall structure and behavior of the molecule.

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