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
Planck’s Constant
6.626x10^-34
Energy of a quantum
E=(planck’s constant)(frequency)
When given nanometers , to get to meters you must…
Divide by 10^9
Exceptions to the Aufbau Principle
Electron configurations of copper and chromium
Heisenberg Uncertainty Principle
States that it is not possible to know the velocity and position of an electron at the same time
The quantum mechanical model replaced
Bohr’s model
