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Chemical bonds are the glue keeping atoms together to form molecules and compounds. They are the result of the attraction between the positively charged nuclei and the electrons of different atoms. The most common types include ionic, covalent, and metallic bonds. When atoms bond together, they can achieve a more stable electron configuration, which is often the octet rule for many elements - having eight electrons in their outer shell.

Breaking these bonds requires energy since you're overcoming the attraction forces that stabilize the molecule. In the context of the exercise, to cleave the compound into its elemental parts, you'd need to disrupt these bonds, necessitating a chemical change.

Compound decomposition, also known as chemical decomposition, is the process in which a compound breaks down into its constituent elements or simpler compounds. This can occur in various ways, such as electrolysis, where an electric current causes the compound to separate, or thermal decomposition, where heat breaks down the chemical bonds.

When a compound decomposes, the original chemical bonds are broken, and new bonds might form if decomposition leads to the creation of simpler compounds. This contrasts with the original exercise where we consider the breakdown into pure elements, an unequivocal sign of chemical change since the original substance's properties completely alter.

A physical change might seem dramatic, but it's all about appearances as it doesn't alter the internal structure of a substance. Examples include changes in state, such as melting ice or tearing a piece of paper. Despite the visual or physical transformation, the substance's chemical makeup remains untouched.

Understanding the difference between physical and chemical changes is integral in chemistry. A simple way to remember is: if the change you observe doesn't create a new substance, it's likely just a physical change. Thus, physical changes are usually reversible, while chemical changes, such as breaking the bonds within a compound to retrieve the individual elements, are not easily reversible, marking a fundamental distinction in the study of matter.