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ATOMIC HISTORY & ISOTOPES

This overview investigates key experiments that shaped atomic theory, beginning with J.J. Thomson's cathode ray tube experiment, which illuminated the existence of negatively charged electrons. Thomson's "Plum Pudding Model" depicted electrons embedded in a positively charged matrix. Following this, Ernest Rutherford's Gold Foil Experiment revealed the existence of a small, dense nucleus, challenging previous atom models by demonstrating the atom's vast empty space. Additionally, the concept of isotopes is explained, highlighting their properties and methods for calculating relative mass and abundance.

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ATOMIC HISTORY & ISOTOPES

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  1. ATOMIC HISTORY & ISOTOPES

  2. Thomson’s experiment involved a cathode ray tube with a gas at low pressure. The gas flowed from the negative end to the positive end of the tube. Because the gas consisted of electrons, it was repelled by the negative end of the magnet and attracted by the positive end of the magnet showing that an electron is negatively charged

  3. THOMSON’S MODEL IS CALLED THE PLUM PUDDING MODEL Thomson explained that the model was like plums representing the electrons in pudding represented as protons

  4. Rutherford’s Gold Foil experiment involved shooting positively charged alpha particles through a thin piece of gold foil. He expected the alpha particles to pass straight through or get struck in the positive part. Instead most alpha particles passed straight through but a few were deflected or bounced straight back. This lead to the conclusion that an atom is mostly empty space but has a very small positively charged center (nucleus)

  5. ISOTOPES ISOTOPES: Describe an isotope, compare the properties of the isotope of an element and deduce the symbol of an isotope given its mass number and atomic number. RELATIVE MASS (AVERAGE ATOMIC MASS): Calculate the non integer relative mass and abundance of isotopes from given data.

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