Question | Answer |
Split the nucleus to discover it contains particles with no charge that have a mass approximately equal to that of protons | Chadwick |
Reacted gases to find that all matter is made of atoms that react in whole number ratios, which led to form the billard ball model. | Dalton |
Frond that electron can have diffraction and interferance like light and other electromagnetic waves. | deBroglie |
Performed the gold foil experiment to find that atoms are mostly empty space, but have a positively charge and much mass concentrated in the nucleus, | Rutherford |
Performed the oil drop experiment which allowed him to calculate the small mass of electrons. | Millikan |
Observed the spectrakl lines of hydrogen which led him to conclude that electrons are arranged in energy levels sround the nucleus and can not be between levels. | Bohr |
discovered that two electrons can occupy the same electron cloud if they have spins in opposit directions. | Pauli exclusion principle |
Performed experiments with cathode ray tube to find that atoms contain particles with a negative charge which can leave the atom | JJ Thomson |
Mathemathically calculated all known electron orbital properties | Schrodinger |
An electron occupies the lowest energy level that can recieve it | Aufbau Principle |
Orbitals of equal energy are occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin. | Hunds Rule |
It is impossible to know both the position and velocity of an electron simultaneously | Heisenberg uncertainty principle |
indicates the main energy level occupied by an electron. | Principal quantum number |
Known as sublevels, orbitals of different shapes, (s,p,d,f) | Angular Momentum quantum number |
Indicates the orientation of an orbital around the nucleus. | Magnetic quantum number |
Indicates the two possible spin states of an electron in an orbital | Spin quantum number |