Chapter 5 Quantum Mechanics Flashcards
Quantum
The amount of energy required to move an electron from one energy level to another energy level .
Pauli Exclusion Principle
1) An atomic orbital may hold at most 2 electrons.
2) If 2 e- occupy the same orbital they must have opposite spins.
Aufbau Principle
e- occupy orbitals of lowest energy level FIRST.
Sub level : Orbitals
S : 1 P : 3 D : 5 F : 7 Divide max e- by 2 .
Electron configuration
The most stable arrangement of e- in sublevels & orbitals
Orbitals
S: max 2e-
P: max 6e-
D: max 10e-
F: max 14 e-
Scrodinger
Use theoretical calculations & experimental results to make a math equation stating the behavior of an electron in a hydrogen atom
Limitations of Rutherford’s atomic model…
1) explained only a few simple properties of atoms
2) it could not explain the chemical properties of elements
Energy Levels
The fixed energies am electron can have
Valence Electrons
e- located in the outermost energy level of an atom.
Hund’s Rule
e- occupy orbitals of the same energy in a way that makes the # of e- with the same spin direction as large as possible.
Bohr
Suggested that e- travel in a fixed path around the nucleus (think of Jimmy Neutron)
Atomic Orbital
A region of space in which there’s a high probability of finding an electron.
Electronic Transition
Light is emitted as e- drops down to lower energy state.
Speed of light
(C) 3x10^8
