3.  Democritus  400 B.C. - thought matter could not be divided indefinitely  This led to the idea of atoms in a void  Aristotle  Believed that matter was made of a combination of four “elements”: earth, fire, water, air  Aristotle was wrong. However, his theory persisted for 2000 years. Democritus Aristotle fire air water earth

4.  1800 -Dalton proposed a modern atomic model based on experimentation not on pure reason  His ideas account for the law of conservation of mass (atoms are neither created nor destroyed) and the law of constant composition (elements combine in fixed ratios). All matter is made of atoms Atoms of an element are identical. Each element has different atoms. Atoms of different elements combine in constant ratios to form compounds. Atoms are rearranged in reactions.

5.  Accidental discovery of the cathode ray  Discovery led to the development of the television

6.  Joseph John Thompson  found that atoms could sometimes eject a far smaller negative particle which he called an ELECTRON PLUM PUDDING MODEL Robert Millikan - Developed the charge of an atom… e-

7. Most particles passed through So, atoms are mostly empty space Some positive  -particles deflected or bounced back! Thus, a “nucleus” is positive & holds most of an atom’s mass Radioactive substance path of invisible  - particles  Rutherford shot alpha (  ) particles at gold foil Lead block Zinc sulfide screen Thin gold foil

8. There are 2 types of spectra: continuous spectra & line spectra It’s when electrons fall back down that they release a photon. These jumps down from “shell” to “shell” account for the line spectra seen in gas discharge tubes (through spectroscopes). Electrons orbit the nucleus in “shells” Electrons can be bumped up to a higher shell if hit by an electron or a photon of light

9. HELIUM ATOM + N N + - - proton electron neutron Shell

10. ATOMIC STRUCTURE Particle proton neutron electron Charge + charge - charge No charge 1 1 nil Mass

11. ATOMIC STRUCTURE the number of protons in an atom the number of protons and neutrons in an atom He 2 4 Atomic mass Atomic number number of electrons = number of protons

12.  There are 3 types of subatomic particles.  You know about electrons (e – ) & protons (p + )  Neutrons (n 0 ) were also shown to exist (1930s).  They have: no charge, a mass similar to protons  Elements are often symbolized with their mass number and atomic number E.g. Oxygen: O 16 8 The Periodic Table gives you all this information For now, round the mass # to a whole number # of protons = # of electrons = atomic number mass number – atomic number = # of neutrons Nuclear Symbol

13. Br Ar Ca e–e– n0n0 p+p+ MassAtomic Practice