Transcript Slide 1

A.P. CHEM. CH. 7
ATOMIC STRUCTURE
Particle
Wave
mass
Bohr Model
l,n
Wave-Mechanical
Model
It explained
Atom doesn’t collapse
DeBroglie
Bright-Line Spectra
H
Equations
Light
m = h/cl
lxn =c
Matter
P E= hn
E
E= mc2
l = h/mv
Named: Quantum model
Duality
of matter
Wave **
Equation
Schroedinger
Characteristics
Discrete energy levels
Electron transitions
Uncert.
Heisenberg Princ.
Equation: En=-2.178x10-18J(Z2/n2)
Flaw: Bohr didn’t know why
Observer
affects the
observed
Dx • Dmv ≥ h/4p
position
Wave function
H Y =E Y
**
orbital
Can be applied to atoms other
than hydrogen by finding:
Defined: High prob.
region
Designated by:
Quantum
#’s
Zeff = Zact - repulsive effects
n
Repulsions/
core shielding
Can be found
by knowing I.E.
equation
I.E.=
1310 kJ
mole e-
Not as low as could
be in certain
instances due to: penetration
I.E.
E.A.
size
Relate to
Chart
Know the
trends of this
l
ml
Z2eff
ms
n2
Still described
by these
Hydrogen like
orbitals
s
p
d
f
Representations
Rules for multielectronic atoms:
aufbau
Pauli
Hund’s