Chemistry Definitions 3
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Created by:
Gizmo-chan on September 12, 2011
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8 terms
Terms | Definitions |
|---|---|
 Orbitals | regions where elecrons are found, located at various distances from the nucleus |
| Principal Quantum Number | (n) Describes the energy level in which the electron can be found Possible values=(1, 2, 3, 4, 5, 6, 7) |
| Azimuthal Quantum Number | (l) Describes the shape of the orbital 0=s orbital 1=p orbital 2=d orbital 3=f orbital |
| Magnetic Quantum Number | (m_l) The orientation of the orbital in space Possible values=(-1, 0, 1) |
| Spin Quantum Number | (m_s) Describes the apparent spin of the electron Possible values=(+1/2 or -1/2) |
| Aufbau Principle | a principle that states electrons occupy the orbitals of lowest energy first (one of the 3 Laws of Electron Configuration) |
| Pauli Exclusion Principle | a principle that states an atomic orbital may contain, at most, two electrons (one of the 3 Laws of Electron Configuration) |
| Hund's Rule | a rule that states that only one electron must occupy all orbitals of equivalent energy in an energy level of an atom before "doubling up" may occur |
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