Chemistry Chapter 13
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34 terms
Terms | Definitions |
|---|---|
 Democritus | first thought atom was a solid, indestructible, indivisible mass |
| solid; indestructible; indivisible | Democritus thought the atom was a ... , ... , ... mass. |
| J.J. Thomson | said that the atomic model did not take into account electrons and protons |
| electrons; protons | J.J. Thomson said that the atomic model did not take into account ... and ... |
| Ernest Rutherford | proposed that electrons surrounded a dense, positively charged nucleus and the rest of the atom was empty space |
| Niels Bohr | said that electrons were arranged in orbits around the nucleus |
| Niels Bohr | said that electrons in a particular path have a fixed energy |
| fixed energy | Niels Bohr said that electrons in a particular path have a ... ... |
| energy level | region around the nucleus where the electron is likely to be moving |
| greater | Energy levels are more closely spaced the ... the distance from the nucleus. |
| more | the higher the energy level, the ... energy the electron has. |
| quantum | amount of energy required to move an electron from one energy level to the next higher one |
| quantum leap | an abrupt change of energy levels |
| quantum mechanical model | the present day atomic model |
| most probable location | The quantum mechanical model does not show paths, instead it shows the ... ... ... of an electron. |
| higher | The denser the place in the cloud of the electron cloud model, the ... the probability of finding an electron. |
| Schrodinger | came up with the mathematical equation showing energy and location of electron |
| energy; location | Schrodinger came up with a mathematical equation showing the ... and ... of electron |
| principal quantum number | principal energy level or shell |
| sublevels | number of ... is the same as the principal quantum number |
| atomic orbitals | regions within a sublevel where electrons can be found |
| two | maximum of ... electrons per orbital |
| ground state | lowest possible energy state |
| unstable | high energy systems are ... |
| electron configurations | ways in which electrons are arranged around the nucleus of atoms |
| Aufbau Principle | electrons enter orbitals of lowest energy first |
| overlap | energy levels can ... |
| Pauli Exclusion Principle | for two electrons to occupy the same orbital, they must have opposite spins |
| orbital pair | two oppositely spinning electrons occupying the same orbital |
| Hund's Rule | before a second electron can be placed in any orbital, all orbitals of that sublevel must contain at least one electron |
| electrons | For neutral atoms, the sum of the superscripts is the number of ... in the atom. |
| valence shell | outermost principal energy level of an atom that includes at least one electron |
| valence electrons | electrons in the valence shell |
| excited state | condition of an atom whose electrons are at higher energy levels than the ones they normally occupy |
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