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Gen Chem chpt3
Quantum Theory chpt3
| Question | Answer |
|---|---|
| Define these terms: Potential and Kinetic Energy and the Law of Conservation | Potential- energy that is stored Kinetic- energy that is in motion law of conservation- energy cannot be created nor destroyed |
| Thermal Energy | is a form of kinetic energy |
| Chemical Energy and electrostatic energy | are forms of potential energy |
| what we commonly refer to as "light" | is the visible portion of electromagnetic spectrum |
| electromagnetic waves | have electric and magnetic components that mutually perpendicular and in phase |
| black body radiation | electromagnetic radiation given off by a solid when it is heated |
| Max Planck | proposed that energy like matter is composed of "quanta" |
| Einstein | used Planck's quantum theory to explain the photoelectric effect |
| Photoelectric effect | electrons are emitted of a certain minimum frequency, shines on a metal surface |
| threshold frequency | minimum frequency of light required to eject an electron form the surface of a metal in the photoelectric effect |
| photon | a quantum of light |
| emission spectrum | the light given off by an object when its excited thermally and is continuous |
| the ground state | the lowest possible energy state for an atom |
| the excited state | any energy level higher than the ground state |
| node | standing wave has zero amplitude |
| De Broglie wavelength | wavelength associated with a particle of very small mass. |
| De Broglie | proposed that light could have particle-like behavior and after conducting experiments, it showed that electrons could exhibit diffraction - a property of waves |
| Heisenberg Uncertainty principle | the product of the uncertainty of a location and the uncertainty of the momentum of a very small particle must have a certain minimum value, meaning you cannot know both the location and the momentum |
| electron density | the probability of finding an electron in a particular region in an atom |
| atomic orbital | the region of a 3-D space define by the square of a wave function |
| the atomic orbital is defined by: | quantum numbers: the principle quantum number, (n) the angular quantum number (l), and the magnetic quantum number (ml) |
| principle quantum number | indicates the distance from the nucleus (n) |
| angular quantum number | indicates the shape of an orbital (l) |
| magnetic quantum number | indicates the orbital's orientation in space (ml) |
| electron spin quantum number s | two electrons that occupy the same atomic orbital in the ground state (ms) |
| s orbital | 0 |
| p orbital | 1 |
| d orbital | 2 |
| f orbital | 3 |
| line spectra | The emission or absorption of light only at discrete wavelengths. |
Created by:
landryw
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