Transcript Slide 1

A.P. CHEM. CH. 7
ATOMIC STRUCTURE
Particle
Bohr Model
Wave
mass
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
USE SPECIAL
PENS OR
PENCILS IN THE
BINS TO FILL IN
OVERVIEW!
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
**
Defined:
orbital
Can be applied to atoms other
than hydrogen by finding:
High prob.
region in space
where the
electron is
likely to be
found.
Zeff = Zact - repulsive effects
Repulsions/
core shielding
Can be found
by knowing I.E.
equation
I.E.=
Z2eff
1310 kJ
mole e-
n2
evidence
Not as low as could PHOTOELECTRON
SPRECTOSCOPY
be in certain
instances due to: penetration
I.E.
E.A.
size
Relate to
Chart
Know the
trends of this
Hydrogen like
orbitals
s
p
d
f
Representations
Rules for multielectronic atoms:
aufbau
Pauli
Hund’s
phosphorous
This is the photoelectron spectrum for _______________________
1000
5000
100
1000
100
0
(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
phosphorous
This is the photoelectron spectrum for _______________________
5000
1000
100
1000
100
0
(eV)
If the photoelectron spectrum for sulfur was shown above,
Due to more
the peak for the 1s orbital would
A.) shift more to the
B.) shift more to the
protons in the
right than in phosphorous. nucleus…no
change in core
left than in phosphorous. shielding or
repulsions!
C.) not shift compared to phosphorous.
D.) not be able to be compared to phosphorous.
phosphorous
This is the photoelectron spectrum for _______________________
5000
1000
100
1000
100
0
(eV)
If the photoelectron spectrum for sulfur was shown above,
the peak for the 3p orbital would
Due to significant
repulsion when an
A.) shift more to the right than in phosphorous.electron is added to
B.) shift more to the left than in phosphorous. an orbital in a set of
degenerate orbitals
that had previously
C.) not shift compared to phosphorous.
had only one!
D.) not be able to be compared to phosphorous.
Practice Problem: Chapter 7 A.P. Chemistry
Let’s look at the atom beryllium.
1s22s2
Write out the ground state configuration notation for Be: _____________________
Record the second and third ionization energies for Be: I.E.2= ________________
1757.1 kJ/mol
14848.7 kJ/mol
I.E.3= ________________
<1757.1 kJ/mol (the actual value = 899.5
Predict a value for I.E.1 = _________________
_____________)
kJ/mol
Zeff ( For the remaining electron) = _______________
4
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?
E4 = (-2.178x10-18 J)(42/42)= -2.178x10-18 J
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
c/n = l l = 2.54x10-7 m
Find the
difference
violet