Chemistry Chapter 4.2 and 4.3

Quantum Models and Orbitals

Louis de Broglie’s research

Treats e- as waves with a certain probability of being found at different distances from the nucleus

Werner Heisenberg Principle

It is impossible to determine simultaneously both the position and velocity of an electron

Erwin Schrodinger’s research

Treated e- as waves having a certain probability of being found in orbitals at various distances from the nucleus

Orbital

A three dimensional region around the nucleus that indicates the probable location of an e-

Quantum Number 1

Principle Quantum Number

Principle Quantum Number

Indicates the main energy level around the nucleus, symbol = n

Quantum Number 2

Angular Momentum Quantum Number

Angular Momentum Quantum Number

Tells the shape of an orbital (sublevels)

S orbitals

Spherical shape, lowest E

P orbitals

Dumbbell shape, low E

D orbitals

Double dumbbell shape, high E

F orbitals

Flower shape, highest E

How many orbitals in S sublevels

1 orbital

How many orbitals in p sublevels

3 orbitals

How many orbitals in d sublevel

5 orbitals

How many orbitals in f sublevel

7 orbitals

Quantum Number 3

Magnetic Quantum Number

Mangnetic Quantum Number

Indicates the orientation in space of orbital (x, y, z axis), symbol = m

Quantum Number 4

Spin Quantum Number

Spin Quantum Number

Two e- can exist in one orbital but must have opposite spin states (+1/2; -1/2)

Hunds Rule

Each orbital receives 1 e- before receiving a second e-

aufbau Principle

e- will occupy the lowest energy position (must fill up 1s before 2s, etc)

Pauli Exclusion Principle

no two e- can have the same Spin State

Valence e-

e- in the highest main energy level