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Unsaturated hydrocarbons are organic compounds that contain at least one carbon-carbon double or triple bond in their structure, which means they have fewer hydrogen atoms than their saturated counterparts. These compounds are highly reactive due to the presence of these multiple bonds, making them key players in chemical reactions such as polymerization and hydrogenation.

In the case of hexene, we are dealing with an alkene, which is a type of unsaturated hydrocarbon with one or more double bonds. The presence of a double bond provides different points of reactivity, allowing for various isomers to be formed. This variation gives rise to a rich chemistry where the position of the double bond, as seen in 2-hexene and 3-hexene, significantly affects the molecule's properties and reactions.

The structural formula of a molecule represents the arrangement of atoms within it. Unlike the molecular formula, which only tells us the number of each type of atom present, the structural formula gives us a visual representation, showing how those atoms are connected to one another.

For instance, when comparing 2-hexene to 3-hexene, both share the same molecular formula of C₆H₁₂, suggesting they have identical numbers of carbon and hydrogen atoms. However, when we scrutinize their structural formulas, we notice a key difference in the positioning of the double bond. This slight variance leads to the individual molecules exhibiting distinct properties, such as differences in boiling points and reactivity, despite their common molecular composition.

A molecular formula indicates the number and types of atoms present in a molecule but does not reveal any information about the arrangement of these atoms. It serves as a compact way to show what a substance is made of. For example, the molecular formula C₆H₁₂ represents a molecule that has six carbon atoms and twelve hydrogen atoms.

The molecular formula is crucial in identifying different isomers, as isomers share the same molecular formula while having different structures. The exercise comparing 2-hexene and 3-hexene perfectly exemplifies the concept of isomerism: despite possessing the same molecular formula, the atoms are arranged differently resulting in unique chemicals with distinct physical and chemical characteristics.