Final answer:
Elements in the same group often exhibit similar properties due to the number of valence electrons, which results in comparable chemical behaviors.
Step-by-step explanation:
The key to understanding why aluminum and sulfur can seem to have similar properties lies in the concepts of valency and oxidation states. Aluminum, a member of group 13, tends to use all its valence electrons when it reacts, frequently giving compounds an oxidation state of 3+. On the other hand, sulfur is in group 16, and elements in the same group often have similar properties due to the same number of valence electrons. This can explain why some chemical properties might appear alike or why they may react in comparable ways.
However, it must be noted that aluminum and sulfur don't have identical properties; they're quite different in their natural states and typical compounds they form. Aluminum generally forms ionic bonds (e.g., AlF3, Alâ‚‚(SO4)3), whereas sulfur forms covalent bonds (e.g., in thiols like CH3SH). The comparison of their ionic radii shows that the aluminum cation has a smaller radius than its atomic radius, whereas the sulfur anion expands upon gaining electrons.
The groundbreaking discovery by Gertrude Elion and George Hitchens utilized the similarity between sulfur and oxygen, both in group 16, for their ability to interrupt cell replication, leading to significant advancements in medicine. Sulfur-based compounds were used to mimic the structure of purines in DNA, demonstrating the importance of understanding elemental similarities in the field of drug development.