Transcript Quantum Numbers

QUANTUM NUMBERS
 Bohr model was 1
dimensional
 Scientist started thinking
about electrons in the forms
of waves and particles
 DeBrogile Equation
 Schroedinger Equation
 Heisenberg Uncertainty
Principle
 Narrows down location even
more than electron
configuration
QUANTUM NUMBERS
Principle quantum number
(n) = Energy level
Describes the size of orbital
Always a + whole number
Never zero
QUANTUM NUMBERS
Angular quantum
number (l) = sublevel
Describes the shape of
the orbitals
Always a whole number
Ranges from 0 to n-1
L
L
L
L
=
=
=
=
0
1
2
3
=
=
=
=
s = sphere
p = dumbbell
d = clover leaf
f = complex
shapes
QUANTUM NUMBERS
Magnetic quantum
number (m or m l ) =
orbital
Describes orientation
of orbital
Always a whole
number
Ranges from –L…L
QUANTUM NUMBERS
Spin quantum number
(s or m s )
Used to distinguish 2
electrons in each lobe
of orbital
Can only be +½ or -½
Pauli Exclusion
Principle
QUANTUM NUMBERS
 n = principle = size
 The coefficient in econfiguration
 1s 2 n= 1
 3d 10 n = 3
 l = angular = shape
S
P
D
F
L
L
L
L
=
=
=
=
0
1
2
3
 m = magnetic =
orientation
 Values range from
-L…0…+L
 s (m s ) = spin
 Up arrow = +1/2
 Down arrow = - 1/2
QUANTUM NUMBERS
 Each electron has its own unique set of quantum numbers
 Helpful to draw out the spin diagram
 Determine the quantum numbers for electrons in oxygen:
______
______
______ ______ ______
QUANTUM NUMBERS
Some helpful short cuts…
Number of orbitals in an energy level= n 2
 How many orbitals are contained in the 3 rd energy
level?
 3 rd energy level and below?
Maximum number of electrons in energy level = 2n 2
 What is the maximum number of electrons in the 2 nd
energy level?
WRITE 4 QUANTUM NUMBERS FOR EACH
ELECTRON IN A HYDROGEN ATOM
E- #
N
L
ML
Ms