Benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) consists of a six- membered ring of carbon atoms with one hydrogen bonded to each carbon. Write Lewis structures for benzene, including resonance structures.

First, we need to determine the total number of valence electrons in a benzene molecule. Each carbon atom contributes four valence electrons, and each hydrogen atom contributes one valence electron. For the benzene molecule: Total valence electrons = (6 carbon atoms * 4) + (6 hydrogen atoms * 1) = 24 + 6 = 30 valence electrons

Next, we'll draw the initial Lewis structure for the benzene molecule. Each carbon atom is connected to one hydrogen atom and two neighboring carbon atoms. To draw the initial Lewis structure: - Place six carbon atoms in a hexagonal ring. - Add one hydrogen atom to the outside of each carbon atom. - Draw single covalent bonds between each carbon and hydrogen atom and single covalent bonds between each neighboring carbon atoms.

In the initial Lewis structure, each carbon atom forms three covalent bonds and has one unpaired electron. These unpaired electrons can participate in the formation of double bonds. To identify resonance structures: - Position double bonds between alternating carbon atoms in the ring, which will create two possible structures. 1. Structure A: Double bonds between C1-C2, C3-C4, and C5-C6 2. Structure B: Double bonds between C2-C3, C4-C5, and C6-C1 - These two resonance structures indicate that the actual electron distribution in the benzene molecule is an average of structures A and B. - The real structure of benzene has bond lengths and strengths between a single bond and a double bond. Benzene is also more stable than either of these structures would indicate on their own. #Final_output#: Step-by-step solution: \[ \textbf{Step 1: Determine the total number of valence electrons}\] Total valence electrons = (6 carbon atoms * 4) + (6 hydrogen atoms * 1) = 24 + 6 = 30 valence electrons \[ \textbf{Step 2: Draw the initial Lewis structure}\] Initial Lewis structure: - Carbon atoms in a hexagonal ring - Hydrogen atom bonded to each carbon atom outside the ring - Single covalent bonds between carbon and hydrogen atoms and neighboring carbon atoms \[ \textbf{Step 3: Determine resonance structures}\] Two possible resonance structures: - Structure A: Double bonds between C1-C2, C3-C4, and C5-C6 - Structure B: Double bonds between C2-C3, C4-C5, and C6-C1 - Actual electron distribution in benzene is an average of structures A and B, with bond lengths and strengths between a single bond and a double bond.