Radioactivity - Atomic Structure

With the fall of the Greek civilisation, many scientific ideas were lost, at least to the western European countries. This started to change in the seventeenth century and some very clever and well-educated people had the time and money to think about science. One of these, a man called John Dalton, revived the idea of atoms. He came up with a model that suggested that atoms were the building blocks of all chemicals and were small, hard spheres that joined together in specific proportions. As with the Greeks, there was no way of testing this or proving this at the time. But this model of atoms seemed to work quite well, especially when Italian scientist, Amedeo Avogadro, modified it slightly to apply to gases, which was the main flaw.

During most of the 19th century, scientists believed that atoms of different elements were made up from different numbers of hydrogen atoms. We now know that it wasn't far off being the truth as a hydrogen atom is one proton with one electron. Then, at the end of the nineteenth century, a scientist called J. J. Thompson discovered the electron which was clearly a lot smaller than an atom. This showed that atoms were not the smallest particles of matter. He suggested that rather than being solid spheres, atoms were spheres of positive charge with the negatively-charged electrons spread through it. This model was replaced about a decade later when Ernest Rutherford discovered that most of the mass of an atom is contained in a small nucleus at the very centre. It is still a bit strange to think of atoms being mainly empty space. Eight years later, Rutherford carried out experiments with radioactive materials that proved that the hydrogen atom was indeed present in other elements and this is regarded as being the discovery of the proton. Rutherford also suggested the idea of neutrons but it wasn't until 1932 that the neutron was finally discovered.