2. Daltons Atomic Theory All matter is composed of extremely small particles called atoms All atoms of a particular element are identical, but the atoms of one element differ from the atom of each other.
3. Atoms of different elements combine with each other in certain whole-number proportion to form a compound. In a chemical reaction, atoms are rearranged to form new compounds; they are not created, destroyed, or change into atoms of any elements
4. Law of Conservation of Mass In a chemical reaction, matter is neither created nor destroyed, or, more accurately stated: there is no detectable change in mass during an ordinary chemical reaction
5. Law of Definite Proportions The different samples of any pure compound contains the same proportions by mass.
6. Law of Multiple Proportions The masses of an element that can be combine with a fixed mass are in a ratio of small numbers.
8. Thompson’s Model The Plum-Pudding Model Atom were composed primarily of very positively charged blob. Embedded on the blob were negatively charged electrons.
10. Nuclear Model Rutherford’s gold foil experiment proved that most of the atom’s mass is found in very small volume called the nucleus.
11. Bohr’s Model Planetary Model Electrons has several possible orbits at different distances from the nucleus and that electron had to be in one specific orbit or another, but this could not exist between orbits.
12. Radioactivity A property exhibited by substances that undergoes spontaneous emission of high energy radiation from nucleus of an unstable atom.
13. Assignment James Chadwick Ernest Rutherford Anton Lavoisier Moseley J.J. Thompson Dalton Antoine Henri Becquerel
