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ChemistryUnit4
Electron Configuration
Term | Definition |
---|---|
Quantum Mechanical model | Predicts the probability of where electrons are within an atom |
Electron Configurations | Show how electrons are distributed within an atom |
Sublevels | Correspond to the different areas an electron can be located in an atom |
Principle Energy Levels | Describe the average distance of an electron from the nucleus, energy increases the farther away you go from the nucleus |
S sublevel shape | Sphere |
P sublevel shape | Dumbbell |
D sublevel shape | Clover |
F sublevel shape | Double clover |
Atomic Orbitals | The different orientation of sublevels in 3-D Space, can only hold up to two electrons |
Sublevel Orbitals | Similar in shape, but different in orientation and size |
Aufbau Principle | Electrons enter sublevels with the lowest energy first |
Orbital Notation | Uses circles to represent atomic orbitals with a label underneath to indicate sublevel and energy level |
Pauli Principle | Atomic orbitals can hold only 2 electrons at most and they must have opposite spins |
Hund's Rule | In a sublevel with more than one orbital, put one electron into each orbital before putting 2 electrons into any one orbital |
Isoelectronic | Two atoms have the same number of electrons |
Noble Gas Configuration | Uses closest noble gas to the element you are writing the configuration for that comes before the element |
Valence Electrons | Electrons located in the outermost energy level (Responsible for bonding) |
Figure out Valence Electrons | Look at the highest numbered energy level in the entire configuration, add the electrons together |
Quantum Numbers | Used to describe the distribution of electrons in atoms |
Energy level (n) | Principle Quantum Number |
Sublevel (l) | Angular Momentum Quantum Number |
Orbital (m sub l) | Magnetic Quantum Number |
Direction (m sub s) | Electron Spin Quantum Number |