Final answer:
The breaking up of carbon bonds leading to smaller molecules involves considerations of entropy and bond dissociation energy. Entropy is a measure of molecular disorder that changes with the state of matter. Bond dissociation energy specifics how much energy is needed to break different types of chemical bonds, influencing molecular stability.
Step-by-step explanation:
The assertion that molecules simply break into smaller ones and carbon bonds break up is not entirely accurate. The process involves more, particularly when considering entropy and bond dissociation energy.
Entropy, which is a measure of the disorder or randomness in a system, tends to increase when a substance goes from a solid to a liquid to a gas.
Gas molecules, having more translational, rotational, and vibrational energy, embody higher entropy than those in a liquid state. When a decomposition reaction occurs, entropy may decrease if the number of gas molecules reduces, since fewer molecules means less energy and lower entropy overall.
The concept of bond dissociation energy is also crucial in understanding molecular stability. When energy is added to a molecule, the bonds can break, and atoms separate. The amount of energy required to break these bonds is specific to the type of bond. For instance, a carbon-carbon (C-C) bond requires about 80 kcal/mol to break, while a carbon-carbon double bond (C=C) needs roughly 145 kcal/mol, indicating that a C=C bond is stronger than a C-C bond.
Moreover, in hydrocarbon chains, the type of carbon-carbon bonds (single, double, or triple) significantly affects the molecule's geometry and its properties. This illustrates that the geometry and stability of organic molecules are subject to the nature and strength of the bonds they contain, not simply to the process of breaking down into smaller molecules.