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In 1904, J.J Thompson suggested the plum-pudding model for an atom. In this model, the electrons were negatively charged corpuscles (plums) in a large positively charged sphere (pudding)

After the alpha-scattering experiment, Rutherford concluded in 1911 that an atom consisted of a very dense and positively charged nucleus, with electrons orbiting it in definite shells: This meant that the atom was mostly empty space.

With the advent of quantum mechanics, the atomic model had to be changed: This model is more or less what is still used today and what is being taught to students (I myself learnt this model at school!). It defines the atom as consisting a very dense and positively charged nucleus, just like Rutherford's model, but with electrons in orbtals. Orbitals are regions around the nucleus where there is the highest probability of finding an electron. This means that the position of an electron at any instant cannot be exactly determined with much precision: We can only calculate the maximum probability of finding an electron by solving complex quantum mechanics equations.

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