The History and Structure of Atoms
The journey to understanding atomic structure is like a detective story spanning centuries. It started with the ancient Greeks, then Dalton in the 1800s suggested atoms were tiny, hard spheres. J.J. Thompson discovered the electron and created the "plum pudding model" - imagine a sphere of positive charge with electrons dotted throughout.
Everything changed when Rutherford and his team did the famous gold foil experiment, discovering the nucleus with its positively charged protons. Later, Bohr suggested electrons orbit the nucleus at fixed distances in shells, and finally Chadwick discovered the neutron in 1932.
Now we know atoms contain three key particles: protons charge+1,mass1, neutrons (charge 0, mass 1), and electrons charge−1,virtuallynomass. The atomic number tells you how many protons an atom has, whilst the mass number is protons plus neutrons.
Isotopes are atoms of the same element with different numbers of neutrons - they have identical chemical properties but different physical properties like density. Remember, it's the number of electrons in an atom's outermost shell that determines how an element reacts!
💡 Quick Tip: Atoms normally have equal numbers of protons and electrons, so they have no overall charge. When they gain or lose electrons, they become ions!