Quantum Theory
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Created by:
dhanushyab on September 26, 2011
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70 terms
Terms | Definitions |
|---|---|
 Democritus | First coined the term 'atoms' |
| Einstein | Explained the "photoelectric effect" by proposing that light is both a wave and a particle |
| Planck | proposed that atoms accept ONLY specific amounts of energy called quanta |
| Dalton | proposed that all matter is made up of atoms and established ideas about how atoms combine to form compounds in definite proportions. |
| Bohr | proposed that electrons orbit the nucleus in circular orbits (solar system model) |
| Thomson | positive and negative charges make up his plum pudding model. |
| Millikan | determined the mass to charge ratio of an electron |
| Rutherford | discovered the nucleus |
| Photoelectric Effect | uses stopping voltage to determine the energy of electrons, and enabled Planck's constant to directly relate frequency to energy. |
| increases | As energy increases, frequency______? |
| Red | Which has lower energy? Red of Violet? |
| Wavelength | Distance between corresponding points on adjacent waves. Length of one complete wave. |
| Frequency | number of waves that pass a point during a certain time period. Defined as the number of waves that pass a given point in a specific time (1 second) |
| Amplitude | distance from the origin to the trough or crest. |
| Quanta | energy that is emitted in small specific amounts. |
| Photoelectric Effect | the emission of electrons from a metal when light shines on a metal. |
| Frequency+wavelength formula | C=λv |
| Inversely | Frequency+wavelength are_____proportional. |
| Higher | Low energy waves have _____ frequencies. |
| Length of visible spectrum | 400nm-700nm |
| Violet | Which has higher energy? Red or Violet? |
| Photon | bundles of light energy that is emitted by electrons as they go from higher energy levels to lower energy levels. Particle of electromagnetic radiation having zero mass and carrying a quantum of energy. |
| Each element has a unique bright-line emission spectrum | What is the significance of the Line Emission Spectrum? |
| Proportional | Energy of a photon is ______ to its frequency. |
| Energy+Frequency Formula | E=hv |
| Energy+wavelength Formula | E=hc/λ |
| Hertz (Hz) | what is frequency measured in? |
| Joules (J) | what is energy measured in? |
| meters, nm, etc | what is wavelength measured in? |
| Planck's constant | 6.6262*10^34 J.s |
| C=speed of light | 3.00*10^8 |
| Orbital | region in space where there is 90% probability of finding an electron. "electron cloud" |
| Two | Each orbital can hold___electrons |
| Two | The S sublevel has____electrons |
| One | The S sublevel has___orbitals |
| Three | The P sublevel has______orbitals |
| Six | The P sublevel has_____electrons |
| Five | The D sublevel has____orbitals |
| Ten | The D sublevel has____electrons |
| Photon | When the electrons falls to a lower energy level, a _____ is emitted. |
| Size of the orbital | What does the energy level tell you? |
| Aufbau Principle | electrons fill the lowest energy orbitals first. An electron occupies the lowest-energy orbital that can receive it. |
| Pauli's Exclusion Principle | Each orbital can hold TWO electrons, but they must have opposite spins. |
| Hund's Rule | Within a sublevel,place one electron per orbital before pairing them up. "urinal analogy" |
| Ground State | lowest energy state of an atom |
| Excited State | a state in which an atom has a higher potential energy that it has in its ground state. |
| Principle quantum number | symbolized by n, indicates the main energy level occupied by the electron. |
| Angular momentum number | symbolized by l, indicates the shape of the orbital s-spherical p-dumbbell |
| Magnetic quantum number | symbolized by m, indicates the orientation of an orbital around the nucleus. |
| Spin quantum number | has only two possible values (+1/2, or -1/2) which indicate the two fundamental spin states of an electron in an orbital |
| Higher | As the wavelenght become shorter, the energy is______. |
| Bohr Model | electrons orbit the nucleus in circular paths of fixed energy. |
| Quantum Numbers | specify the "address" of each electron in an atom |
| S-orbitals | electrons are found within a sphere around the nucleus |
| D-orbitals | most appear to be the combination of two p-orbitals, "daisy" |
| P-orbital | orbital that look like "dumbbells or propellers" or tear drops. |
| F-orbitals | really complicating structure. |
| n | # of sublevels per level |
| n^2 | # of orbitals per level |
| Dalton | All atoms of the same element are identical, other atoms are different. Proposed that atoms are small, uniformely dense, and indivisible. |
| Crooke & Thomson | used a cathode ray tube. Determined that atoms also contain witin themselves small negatively charged particles. They discovered the electron, the 'first' subatomic particle. |
| Rutherford | He tested Thomson's model with the gold foil experiment. According to Thomson's model, radiation particles should not be deflected. but in his experiment, some radiation was deflected. |
| Chadwick | Discovered the neutron. He reevaluates data and proposes that the radiation was actually a "massive" particle. |
| Planck | will only accept energy in small 'quantized' packets. |
| Broglie | Applied wave-particle theory to electrons. Found that electrons exhibit wave properties. |
| Schrodinger | The wavefunction helps describes the location of the electron, and its probable location. Electrons have a wavelenght. |
| Ion electron configuration | write the electron configuration for the closest Noble Gas |
| Ion formation | Atoms gain or lose electrons to become more stable. |
| Heisenberg Uncertainty Principle | impossible to know both the velocity and position of an electron at the same time. |
| Pauli Exclusion Principle | no to electrons in an atom can have the same 4 quantum numbers. |
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