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Rutherford theory
1. Rutherford continued Lenard's experiment by firing positively charged particles at a gold foil. 2. He discovered that most particles passed through the foil, but some were deflected or bounced back, indicating a small, dense nucleus at the atom's center. 3. This led Rutherford to propose his nuclear model of the atom, where electrons orbit a tiny, massive nucleus - overturning Thomson's "plum pudding" model. However, his theory did not explain how electrons can orbit the nucleus without radiating energy.
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Rutherford theory
- 1. RUTHERFORD THEORY AlbertC. X10/1 | Julius C. X10/13 | Nicholas S.W. X10/17 | Sinclair K. X10/19
- 2. Lenard’s Experiment Lenard’s experimentwas meant to proof that if Thomson’s atomic model is right, electrons that go through the aluminum plate should’ve experienced energy loss, so the electrons should be easily refracted. In Lenard’s experiment, he shows that Thomson’s atomic model is wrong because he found that most of the electrons were not refracted. This shows that electrons are not spread evenly.
- 3. Continuation of Lenard’sExperiment In 1911, Ernest Rutherford was interested to continue Lenard’s experiment by replacing electrons with particle which consist of positive charge. This experiment was conducted by Hans Geiger & Ernst Marsden.
- 4. Who is ErnestRutherford? He is a New Zealand-born, British chemist and physicist. In 1914, he was knighted and two years later, he was awarded the Hector Memorial Medal. Under him, Nobel Prizes were awarded to James Chadwick for discovering neutron. Rutherford remains the only science Nobel Prize winner to have performed his most famous work after receiving the prize.
- 5. Rutherford’s research • “rays”/ particles • Theory of protons • Detector for electromagnetic waves
- 6. What are rays / particles? • High speed particles • Made up of two protons and two neutrons • Is a nucleus, same as the nucleus of a common atom of helium • Don’t have electrons around it • Type of ionizing radiation • will loose all their energy in just a couple inches of travel in air
- 8. What Rutherford did? Hedirected the rays to a gold plate surrounded by screen coated with sulfide zinc which are around the plate.
- 9. What happened? 1. Someof the particles pass the empty space go trough Nucleus Particles Atoms of Gold foil
- 10. 2. Some ofthe particles that approach the nucleus are deflected Nucleus Particles Atoms of Gold foil
- 11. 3. Some ofthe particles that hits the nucleus are bounced back Particles Nucleus Atoms of Gold foil
- 12. Conclusion of Rutherford’sTheory • A large fraction of the room in an atom is empty – Indicated by most of rays pass through the plate Nucleus Particles Atoms of Gold foil
- 13. • Nucleus istiny yet very dense core of atom – Indicated by little amount of refracted rays Particles Nucleus Atoms of Gold foil
- 14. • Electrons gocircle the nucleus with high speed – Indicated by the electrons that are not attracted by protons inside the nucleus
- 15. • The chargeof the nucleus is the same as particle’s, which is positive – Indicated by the deflected rays that deflected due to repulsion forces of similar charge. Nucleus Particles Atoms of Gold foil
- 16. Rutherford’s Theory Weakness Basedon Rutherford’s theory that states electrons go around the nucleus will stay on its path is unproved. Based on physics classical mechanic law, that objects that going around on circular path will release its energy in the form of radiation, so the electron will be going closer to the nucleus. But then, Rutherford’s theory is supported by Bohr’s theorem.