Benzene is a cyclic compound with the molecular formula C6H6. To draw the Lewis dot structure for benzene, we need to consider the arrangement and sharing of its valence electrons, particularly among the carbon atoms and the hydrogen atoms.
1. **Count the Valence Electrons**: Each carbon atom has 4 valence electrons, and each hydrogen atom has 1 valence electron. Therefore, for benzene, we have:
- Carbon: 6 x 4 = 24 valence electrons
- Hydrogen: 6 x 1 = 6 valence electrons
Total: 24 + 6 = 30 valence electrons
2. **Arrange the Carbon Atoms in a Ring**: Benzene is a cyclic compound, so we will arrange 6 carbon atoms in a hexagonal shape, connecting each carbon with a single bond.
3. **Add Hydrogen Atoms**: Each carbon atom in benzene is bonded to one hydrogen atom. Thus, we place one hydrogen atom around each carbon atom.
4. **Distribute Electrons and Create Double Bonds**: To accurately represent benzene, we must show the delocalization of electrons. Benzene has alternating single and double bonds between carbon atoms. However, it is often represented with a circle inside the hexagon to indicate that all carbon-carbon bonds are equivalent due to resonance. Each carbon will share its electrons with its neighbors.
5. **Final Structure**: The final Lewis structure for benzene can be depicted as follows:
H H
\ /
C--C
/ \
H-C C-H
\ /
C--C
/ \
H H
In this structure, each line represents a pair of shared electrons, and the arrangement showcases how the electrons are shared among carbon and hydrogen atoms, illustrating the delocalized nature of the pi electrons in the benzene ring.