Final answer:
Dalton's original atomic theory incorrectly stated that all atoms of the same element are identical and that atoms of different elements are entirely distinct. Instead, modern atomic theory recognizes the existence of isotopes and the ability of atoms to undergo subatomic division as well as transformation through nuclear reactions. Furthermore, atoms of different elements can have isotopes with the same atomic mass.
Step-by-step explanation:
Dalton's Original Atomic Theory vs Modern Understanding
Several statements in Dalton's original atomic theory have been proven to be incorrect as modern atomic theory has advanced. One key aspect that Dalton got wrong is the notion that all atoms of the same element are identical. Modern science has shown that atoms of the same element can exist in different forms known as isotopes, which have the same number of protons but a different number of neutrons, resulting in different masses.
Furthermore, Dalton believed that atoms of different elements are different in all respects. However, there are cases where atoms of different elements share some similarities, such as argon and calcium both having isotopes with an atomic mass of 40 amu. These discoveries demonstrate that Dalton's idea about absolute uniqueness in atomic mass among different elements does not always hold true.
An important part of modern atomic theory is the understanding of subatomic particles. Dalton thought that atoms were indivisible units, but we now know they can be broken down into protons, neutrons, and electrons. As for the creation or destruction of atoms, Dalton did not believe it was possible, yet modern techniques like nuclear fission and fusion allow for atoms to be split or combined, effectively changing one element into another.
The three known isotopes of hydrogen are Protium (^1H), Deuterium (^2H), and Tritium (^3H). These isotopes highlight the variation that can exist within the atoms of a single element.