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| Could not explain the chemical properties of an element |
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| Proposed that an electron is found only in specific circular paths, or orbits, around the nucleus |
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| Determines the allowed energies an electron can have and how like.y it is to find an electronic various locations around the nucleus |
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| Each energy us level corresponds to an orbital of a different shape, which describes where the electron is likely to be found |
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Tell you how to find the electron configurations of an atom
They Re aufbau principle, the Pauli exclusion principle and Hunds rule |
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| Exceptional electron configurations |
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| Some actual configurations differ from those assigned using the affability principle because half filled sun levels are not as stable as filled us levels, but they are never more stable than other configurations |
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| Product of frequency and wavelength always equals a constant |
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| Wavelength and frequency of light are inversely proportional to each other. As the wavelength of light increases, the frequency decreases. |
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| When atoms absorb energy, electrons move into higher energy levels. These electrons then lose energy by emitting light when they return to lower energy levels |
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| The light emitted by an electron moving from a higher to a lower energy level has a frequency directly proportional to the energy change of the electron. |
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| Classical mechanics adequately describes the motions of bodies larger than atoms, while quantum mechanics describes the motions of subatomic particles and atoms as waves |
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| Process in which electrons are ejected by metals when certain wavelengths of light shine on them |
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| Predicts that all matter exhibits wavelike motions |
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| Principle energy levels, sublevels and orbitals |
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Prin. energy level. #sublevels. Type sub level
n = 1. 1. 1s (1 orbital)
n = 2. 2. 2s (1 orbital) 2p (3 orbitals)
n = 3. 3. 3s (1 orbital), 3p (3 orbitals)
3d (5orbitals)
n= 4. 4. 4s (1 orbital) 4p (3 orbitals)
4d (5 orbitals) 4f (7 orbitals) |
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