Final answer:
The statement that molecules CH3 CH₂COOH and C3H6O2 could be structural isomers is true, and wave-particle duality is false for macroscopic objects. Molecular formulas require structural formulas to understand the exact arrangement of atoms.
Step-by-step explanation:
When evaluating the molecular structure of compounds, it is critical to understand that molecules with the same molecular formula may have different arrangements of atoms, leading to distinct compounds with varying properties. For instance, structural isomers are molecules that have the same molecular formula but different covalent arrangements of atoms. Consequently, the statement that molecules with formulas CH3 CH₂COOH and C3H6O2 could be structural isomers is true. This exemplifies that the molecular formula does not indicate the exact arrangement of atoms within a molecule, and additional knowledge of the structural formula is necessary to discern the specific isomers and their respective properties.
Additionally, atomic models such as the Bohr Model represent one way to visualize the structure of an atom, showing electrons in orbits around a nucleus, which aids in understanding atomic behavior. However, this model is not a precise depiction of an atom's exact structure. Understanding the concept of atoms and molecules is essential in chemistry as it forms the basis for predicting how substances will interact physically and chemically, and how they can be represented through various models such as stick, ball-and-stick, and space-filling models.
The concept of wave-particle duality is true at the quantum level but false at the macroscopic scale. This crucial principle states that microscopic particles like electrons have properties of both waves and particles, while larger objects do not exhibit such duality.