1. Bohr Model l , n l x n Light hn Matter
A.P. CHEM. CH. 7
ATOMIC STRUCTURE
Background Info
Duality
Particle
Wave-Mechanical Model
Bohr Model
Wave
mass
l , n
It explained
Duality of matter
U.V. catastrophe/ photelelectric effect
Atom doesn’t collapse
DeBroglie
Planck / Einstein
Young
Double Slit
Dalton
Bright-Line Spectra
DeBroglie
Equations H
Wave ** Equation
l x n
= c
Named:
Quantum model
Schroedinger
Light hn
Matter P E=
Characteristics E E=
mc2
m = h/cl
Discrete energy levels
l = h/mv
Uncert. Princ.
Electron transitions
Heisenberg
USE SPECIAL PENS OR PENCILS IN THE BINS TO FILL IN OVERVIEW!
Equation:
En=-2.178x10-18J(Z2/n2)
Observer affects the observed
Flaw:
Bohr didn’t know why
Dx • Dmv ≥ h/4p

2. H Y E Y I.E.= Zeff Zact - repulsive effects Z2eff penetration s aufbau
position
High prob. region in space where the electron is likely to be found.
Wave function **
H Y E Y =
Defined:
orbital
Can be applied to atoms other than hydrogen by finding:
Zeff
Zact - repulsive effects =
Repulsions/ core shielding
Can be found by knowing I.E. equation
Z2eff
I.E.=
1310 kJ
mole e- n2
Config. Not.
Orbital. Not.
evidence
Not as low as could be in certain instances due to:
PHOTOELECTRON SPRECTOSCOPY
Hydrogen like orbitals
penetration
Representations s
Rules for multielectronic atoms:
I.E.
aufbau
Relate to Chart
E.A.
Know the trends of this p
Pauli
size d
Hund’s f

3. This is the photoelectron spectrum for _______________________
phosphorous
1000
5000
100
1000
100
(eV)
The peak on the spectrum to which the arrow is pointing would be associated with electrons in which sublevel?
A.) 1s
B.) 2s
C.) 3s
D.) 3p

4. A.) shift more to the right than in phosphorous.
This is the photoelectron spectrum for _______________________
phosphorous
1000
5000
100
1000
100
(eV)
If the photoelectron spectrum for sulfur was shown above, the peak for the 1s orbital would
A.) shift more to the right than in phosphorous.
B.) shift more to the left than in phosphorous.
C.) not shift compared to phosphorous.
D.) not be able to be compared to phosphorous.
Due to more protons in the nucleus…no change in core shielding or repulsions!

5. A.) shift more to the right than in phosphorous.
This is the photoelectron spectrum for _______________________
phosphorous
1000
5000
100
1000
100
(eV)
If the photoelectron spectrum for sulfur was shown above, the peak for the 3p orbital would
A.) shift more to the right than in phosphorous.
B.) shift more to the left than in phosphorous.
C.) not shift compared to phosphorous.
D.) not be able to be compared to phosphorous.
Due to significant repulsion when an electron is added to an orbital in a set of degenerate orbitals that had previously had only one!

6. …nearly violet 1s22s2 1757.1 kJ/mol 14848.7 kJ/mol 4
Practice Problem: Chapter 7 A.P. Chemistry
Let’s look at the atom beryllium.
Write out the ground state configuration notation for Be: _____________________
Record the second and third ionization energies for Be: I.E.2= ________________
I.E.3= ________________
Predict a value for I.E.1 = _________________ (the actual value = _____________)
Zeff ( ) = _______________
One of the emission spectral lines for Be3+ [that’s nearly a color we can see] results from an electronic transition from n=5 to n=4. Is the transition’s associated “color” nearly red or nearly violet?
1s22s2
kJ/mol
kJ/mol
< kJ/mol
899.5 kJ/mol 4
For the remaining electron
E4 = (-2.178x10-18 J)(42/42)
= x10-18 J
Find the difference
E5 = (-2.178x10-18 J)(42/52)=
-1.394x10-18 J
E (released) =7.84x10-19 J
- 7.84x10-19 J
E =h n
n = 1.18x1015/s
…nearly violet
c/n = l
l = 2.54x10-7 m