Benzene, formula \(\mathrm{C}_{6} \mathrm{H}_{6}\), is a perfect closed hexagon of carbon atoms, each with one hydrogen atom attached. Draw a dot diagram for this molecule, and include any resonanace forms if

Valence electrons are at the heart of understanding chemical reactions. These outermost electrons play the pivotal role in the formation of chemical bonds. Benzene, with the chemical formula \(\mathrm{C}_{6}\mathrm{H}_{6}\), features carbon and hydrogen atoms. Carbon, with four valence electrons, and hydrogen with one, sets the stage for determining the bonding possibilities. The total count of valence electrons is calculated by adding the valence electrons from all atoms. For benzene, this sum reaches 30 valence electrons:\[ 6(4\,\text{ from carbon}) + 6(1\,\text{ from hydrogen}) = 30 \]
Understanding valence electrons helps in predicting how atoms will interact and bond within a molecule. The accurate account of these electrons is critical in constructing the Lewis dot structure, which is a visual representation of atomic bonding and electron arrangement.

Chemical bonding is the force of attraction that holds atoms together in a molecule. It often involves sharing or transferring of valence electrons to achieve a stable electron configuration. In benzene, each carbon atom is bonded to one hydrogen atom and two neighboring carbon atoms. To build the molecular structure, one must consider that single covalent bonds form when two electrons are shared between two atoms. Benzene is unique in its bonding because it contains alternating double bonds. It's these connections that hold the hexagonal structure of benzene together and give it unique stability and chemical properties.
When depicting chemical bonding in the Lewis dot structure, a single line represents two shared electrons, forming a bond. Whereas, a double line reflects a double bond, sharing four electrons. These visual symbols are fundamental for students to grasp as they begin to draw and interpret the molecular structures.

Resonance structures highlight the concept that some molecules can't be adequately described by a single Lewis structure. Instead, they have multiple contributing forms. For benzene, this is especially pertinent, given its ring structure with alternating single and double bonds. The true structure of benzene is a hybrid of two equivalent Lewis structures where the double bonds can be in different positions. To represent this, chemists draw the resonance forms of benzene, which involve three alternating double bonds that shift their position around the ring – a phenomenon that delocalizes the electrons.
In the case of benzene, a double-headed arrow is placed between the two structures to indicate that the molecule's actual electronic structure is a hybrid of both forms. This accounts for its unusual stability and is a crucial aspect of chemical bonding in aromatic compounds.

The octet rule explains the tendency of atoms to prefer having eight electrons in their valence shell to achieve a noble gas-like electronic configuration, which is synonymous with chemical stability. In the context of benzene, the carbon atoms follow the octet rule, each having an arrangement of eight electrons around it. This includes one bond with hydrogen and three bonds with other carbon atoms (two single bonds and one part of a double bond).
Lewis structures are guided by the octet rule, which is why in the construction for benzene, it is imperative to ensure that every carbon atom is surrounded by eight electrons. Exceptions to the octet rule, such as in the case of hydrogen atoms which follow the duet rule (preferring two electrons), must also be recognized when constructing and verifying the correctness of the structure.