how did the discovery of nutrons change the atomic model
The discovery of neutrons had a profound impact on the atomic model and our understanding of the atom's structure. Prior to the discovery of neutrons, the atomic model proposed by J.J. Thomson in 1904 depicted atoms as a positively-charged "pudding" with negatively-charged electrons scattered throughout the atom. This model was further refined by Ernest Rutherford's gold foil experiment in 1911, which led to the development of the nuclear model. According to this model, atoms consist of a small, dense, positively-charged nucleus at the center, with negatively-charged electrons orbiting around it.
The discovery of neutrons in 1932 by James Chadwick revolutionized the atomic model by revealing the presence of a neutral particle within the atom. Neutrons are subatomic particles with no electrical charge, located within the nucleus along with positively-charged protons. The existence of neutrons explained some of the limitations and discrepancies observed in the nuclear model.
With the discovery of neutrons, the atomic model was revised to include three subatomic particles: protons, neutrons, and electrons. The positively-charged protons and electrically-neutral neutrons are located in the nucleus, while the negatively-charged electrons orbit around the nucleus in specific energy levels or shells. This revised atomic model, known as the "electron cloud model" or the "quantum mechanical model," accurately describes the distribution of subatomic particles and the behavior of atoms.
In summary, the discovery of neutrons led to an updated atomic model that incorporated all three subatomic particles, providing a more complete understanding of atomic structure and behavior.