The modern-day quantum model of the atom is considered superior to John Dalton's model because it:

• A. describes atoms as indivisible solid spheres
• B. does not account for the existence of subatomic particles
• C. states that atoms of the same element have identical masses
• D. explains the behavior of electrons using probability distributions and wave functions

Answer: (D)

Verified step by step guidance

1. Understand that John Dalton's atomic model described atoms as indivisible solid spheres without internal structure or subatomic particles.
2. Recognize that the modern quantum model introduces the concept of electrons behaving both as particles and waves, which cannot be precisely located but are described by probability distributions.
3. Learn that the quantum model uses wave functions (solutions to the Schrödinger equation) to predict the likelihood of finding an electron in a particular region around the nucleus.
4. Note that this probabilistic approach explains atomic behavior and chemical properties more accurately than Dalton's model, which lacked any description of electron behavior.
5. Conclude that the superiority of the quantum model lies in its ability to explain electron behavior through probability distributions and wave functions, rather than treating atoms as indivisible solid spheres.