1. ATOMICS MODELS AND ATOMICS SPECTRA Presentation by: Elena Escamilla García. 3º C

2. The Atomic Model of Thomson The atom, that Thomson discovered, was a compact atom. He believed that the atom was a sphere with positive charge into which the electrons were like a pudding plum, in which the electrons were like negative 'plums' in a pudding of positive matter (proton). The atom, that Thomson discovered, was a compact atom. He believed that the atom was a sphere with positive charge into which the electrons were like a pudding plum, in which the electrons were like negative 'plums' in a pudding of positive matter (proton).

3. Atomic model of Rutherford Rutherford bombed a fine plate of gold with alpha particles (positive load) and observed that most of the particles crossed the plate without diverting their paths. Aside from the majority, which crossed without diverting their paths, the minority bumped and were sent backwards. Rutherford bombed a fine plate of gold with alpha particles (positive load) and observed that most of the particles crossed the plate without diverting their paths. Aside from the majority, which crossed without diverting their paths, the minority bumped and were sent backwards.

4. Atomic model of Rutherford (Explanation of what happened) If the atom is compact, why did alpha particles cross the golden sheet? If the atom is compact, why did alpha particles cross the golden sheet? This is because the atom is almost empty, and for this reason the majority of the particles cross the plate without diverting their paths. This is because the atom is almost empty, and for this reason the majority of the particles cross the plate without diverting their paths. But some of the particles that crossed without diverting paths and others that bumped and went backwards. But some of the particles that crossed without diverting paths and others that bumped and went backwards. Why? Why?

5. Atomic model of Rutherford (Explanation of the happened) There was something concentrated in a point that was turning the particles aside and in addition, it had big mass because some of them (the minority) were hitting and were being sent backwards. There was something concentrated in a point that was turning the particles aside and in addition, it had big mass because some of them (the minority) were hitting and were being sent backwards. Later Rutherford to deduce that there was an atomic nucleus with protons and electrons and that the electrons were orbiting around and about the atomic nucleus, but he could not verify what in the atomic nucleus that was contributing to its great mass. Later Rutherford to deduce that there was an atomic nucleus with protons and electrons and that the electrons were orbiting around and about the atomic nucleus, but he could not verify what in the atomic nucleus that was contributing to its great mass.

6. Chadwick's Contribution to the Atomics Models Chadwick (1891-1974) discovered a new fundamental particle in atoms, the neutron, a particle with no electric charge and a mass similar to protons which were also in the nucleus. This explained the increase in mass in the atomic nucleus that Rutherford could not explain. Chadwick (1891-1974) discovered a new fundamental particle in atoms, the neutron, a particle with no electric charge and a mass similar to protons which were also in the nucleus. This explained the increase in mass in the atomic nucleus that Rutherford could not explain.

7. Atomic Model of Bohr Rutherford said that the orbit of electrons in the electronic layer or crust is possible, but Bohr later found that not all orbits are possible. There is a maximum of 7 orbits. Rutherford said that the orbit of electrons in the electronic layer or crust is possible, but Bohr later found that not all orbits are possible. There is a maximum of 7 orbits. Bohr also explained the atomic spectrum. Bohr also explained the atomic spectrum.

8. Atomics Spectrums Bohr explained the atomic spectrum. The atomic spectrum is the visual representation of the energy. There are two types of spectrums, the absorption spectrum and the emission spectrum.