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On the basis of their macroscopic properties, it seems impropable that diamonds and graphite are made of exactly the same atoms. This begs the question, how do we know that diamonds are indeed carbon? Surprisingly, this has been known for over 200 years. In 1772 (before the signing of the Declaration of Independence) a talented French chemist, Antoine Lavoisier, burned diamond (ca. 150 milligrams) in a sealed container. Diamonds do not burn readily, so Lavoisier used the high heat provided by a large lens placed in the sunlight. By a simple analysis of the gases produced by burning, Lavoisier determined that the gas we now know as CO2 was produced. Furthermore, the same amount of this gas was produced when 150 milligrams of amorphous carbon in the form of charcoal was burned. Thus, Lavoisier concluded that charcoal and diamond are the same. However Lavoisier was reluctant to publicize such a radical and counterintuitive result. It took more than 20 years before Lavoisier's conclusions were confirmed by Tenant, an English chemist. Let us examine Lavoisier's conclusion in the context of the times. Lavoisier's discovery predated Dalton's formulation that all matter is made of elements by 29 years and Mendeleev's formulation of the periodic table by almost 100 years. Our modern understanding of chemistry allows us to formulate Lavoisier's experiments in a compact way, the chemical equation.
These equations indicate that burning either diamond or graphite causes the bonds of the reactants (the carbon material and dioxygen) to be rearranged to form the product (CO2) and energy in the form of heat. In general, a chemical reaction involves changes in the bonding between atoms in going from reactants to products. Let's contrast these combustion equations with the analogous equation for burning buckyballs.
Note how the buckyball equation has a subscript of 60 on the carbon, indicating that this form of carbon is molecular. As a result, 60 dioxygen molecules are required to convert the sixty atoms of carbon in each buckyball into 60 molecules of CO2. In a proper, balanced chemical equation the number and types of atoms on the reactant (left) side of the equation equal those on the product (right) side. Because heat is released in this chemical reaction, heat is written as a product. Reactions that generate heat are called exothermic.