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Chemistry Unit 5
| Question | Answer |
|---|---|
| Quantum Mechanical Model | Uses probability to predict the location of an electron |
| De Broglie | Dual nature of an electron as a particle and wave. |
| Heisenberg Uncertainty Principle | We cannot measure both an electrons location and velocity. |
| Einstein | Dual nature of light as a wave and particle |
| Schrodinger | Developed an equation to give the probability of an electron's position in space. |
| Orbital | Area which a max of two electrons will most likely be. |
| S Orbital | 1 type, 2 electrons; Least energy orbital. |
| P Orbitals | 3 types (x,y,z), 6 electrons. |
| D Orbitals | 5 types, 10 electrons. |
| F Orbitals | 7 types, 14 electrons; Highest energy. |
| What happens to an electron as it moves farther from the nucleus? | It gains energy, also it can only move to quantum amounts. |
| Aufbau Principle | Electrons are found in lower energy orbitals before higher energy orbitals (1s,2s,2p, etc) |
| Pauli Exclusion Principle | For 2 electrons to occupy the same orbital, they must have opposite spins. |
| Hund's Rule | For equal energy orbitals there must be 1 electron in each before they gain another. Ex (1/3p, 1/3p, 1/3p) not (2/3p, 1/3p, 0/3p) |
| Valance electrons | Found by adding up all of the electrons in all orbitals of the highest energy level. |
| Core electrons | Electrons that aren't at the highest energy level. (Non-Valance) |
| Exceptions for orbit electron counts | Copper (Cu) and Chromium (Cr) both have an electron move from the 4s to the 3d to make it more stable. |
Created by:
Bhi