Final answer:
The molecules in parts (a) and (b) are related by intermolecular forces, which are weaker interactions between molecules, and intramolecular forces, which are stronger and hold the atoms within a molecule together. Examples include hydrogen bonds and covalent bonds, respectively. The relationship type determines the molecular properties like polarity and overall stability.
Step-by-step explanation:
Understanding Molecular Relationships
The molecules drawn in parts (a) and (b) are related through what are known as either intermolecular forces or intramolecular forces. Intermolecular forces are relatively weak interactions such as hydrogen bonds, electrostatic interactions, and Van der Waals forces that occur between molecules. These forces can collectively have a significant impact despite their individual weakness, as seen in the stability of DNA's double helix structure. Intramolecular forces, on the other hand, are strong bonds that hold the atoms within a single molecule together, such as covalent bonds.
The relationship between two molecules can be characterized by their polarity, which indicates how the electrons are shared or distributed between atoms. Polar molecules have a distinct distribution of electrical charge and will align with each other to maximize attraction. Nonpolar molecules have a uniform distribution of electrical charge and therefore do not have distinct poles.
In nucleic acids, such as DNA or RNA, nucleotides are held together by a specific type of covalent bond known as a phosphodiester bond, which is a strong intramolecular force. When describing the overall stability of molecular structures, we also consider the relative strength of the bonds and how they contribute to the molecules' properties. For example, covalent molecular structures like oxygen (O₂), water (H₂O), and octane (C8H18) are examples of individual molecules held together by strong covalent bonds.