Good morning! Today is November 17, 2010 (B day)
TURN IN ELECTRON CONFIGURATIONS WORKSHEET!
ChemCatalyst
Answer the following questions in your notebook:
1. What are the only possible values that the spin quantum
number, ms, can have?
2. Complete the table below:
l Letter/shape ALL possible values of ml
l=0
l=1
l=2
l=3
Electron Orbital Diagrams
Objective
• To compare and contrast the energies
of the electron orbitals on the same
energy level and on different energy
levels
Electron Configuration
• Shows the value of 2 quantum numbers
– Principal
– Azimuthal
• Does not show the value of the other
quantum numbers
– Magnetic
– Spin
Magnetic Quantum Number
• ml
• Equal to –l to l
• Tells how many ways the orbital can be
oriented (positioned)
Magnetic Quantum Number
l Letter/shape ALL possible values of ml
l=0 s 0
l=1 p -1, 0, 1
l=2 d -2, -1, 0, 1, 2
l=3 f -3, -2, -1, 0, 1, 2, 3
• One way to orient “s”
• Three ways to orient “p”
• Five ways to orient “d”
• 7 ways to orient “f”
Electron Configuration Layout
7p ___ ___ ___
6d ___ ___ ___ ___ ___
5f ___ ___ ___ ___ ___ ___ ___
7s ___
6p ___ ___ ___
5d ___ ___ ___ ___ ___
4f ___ ___ ___ ___ ___ ___ ___
6s ___
5p ___ ___ ___
4d ___ ___ ___ ___ ___
5s ___
4p ___ ___ ___
3d ___ ___ ___ ___ ___
4s ____
3p ___ ___ ___
3s ___
2p ___ ___ ___
2s ___
1s ___
The Layout
• Shows the electron configuration
arranged vertically
– Energy increases as you move up
Spin Quantum Number
• ms
• Equal to -½ or ½
Filling the Diagram
• Use arrows
– ↑and ↓
• Based on 3 rules
Aufbau Principle
• Electrons enter orbitals of lowest
energy first
Pauli Exclusion Principle
• An atomic orbital may only hold 2 electrons
• Electrons must have opposite spins
– ms = ½ or -½
– Denoted by direction of arrows
Hund’s Rule
• Every orbital of the same energy is singly
occupied before any orbital is doubly occupied
– Add up arrows first singly
– Add down arrows to double