Download Heisenberg uncertainty principle

Electrons
What causes what you are
seeing?
Sample
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Electron Configuration
Mapping the electrons
Electron Configuration
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The way electrons are arranged
around the nucleus.
Quantum Mechanical Model
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1920’s
Werner Heisenberg (Uncertainty Principle)
Louis de Broglie (electron has wave
properties)
Erwin Schrodinger (mathematical equations
using probability, quantum numbers)
Heisenberg uncertainty
principle
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it is impossible to
determine simultaneously both the
position and velocity of an electron or
any other particle with any great degree
of accuracy or certainty.
Erwin Schrodinger
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Formulated equation that describes behavior and
energies of subatomic particles.
Incorporates both particle and wave behavior in
terms of wave function:
is proportional to the probability of finding an
electron.
Leads to Quantum Mechanics: we cannot pinpoint an
electron in an atom but we can define the region
where electrons can be in a particular time………
called a Probability map….a 3-dimensional area in
space called an ORBITAL
Like building a house…..
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Orbitals are like a house.
There are floors, rooms, closets and
balconies.
Keep that in mind……
Principal Quantum Number, n
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Indicates main energy levels
n = 1, 2, 3, 4…
This is like how many floors your house has
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Each main energy level has sub-levels
This is like what kind of rooms are on
each floor
Energy Sublevels
s
p
d
f
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The principle quantum number, n,
determines the number of sublevels
within the principle energy level.
Basically each floor can only have certain
types of rooms-answer questions….
Orbital Quantum Number, ℓ
(Angular Momentum Quantum Number)
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Indicates shape of orbital sublevels
ℓ = n-1
ℓ
sublevel
0
1
2
3
4
s
p
d
f
g
Orbital
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The space where there is a high
probability that it is occupied by a pair
of electrons. How many in a pair?
Orbitals are solutions of Schrodinger’s
equations.
Orbitals
Visualizing the orbitals
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Back to the house……
Orbitals are the rooms that hold 2 people per
room.
Orbitals in Sublevels
Sublevel
s
p
d
f
# Orbitals
1
3
5
7
# electrons
2
6
10
14
Three rules are used to build
the electron configuration:
Aufbau principle
 Pauli Exclusion Principle
 Hund’s Rule
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Aufbau Principle
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Electrons occupy orbitals of lower
energy first.
Like building a house- lower floors fill
up first
Orbital
Diagram
Filling Order diagram
-Pauli Exclusion Principle
(Wolfgang Pauli, Austria, 1900-1958)
-Electron Spin Quantum Number
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An orbital can hold only two electrons and
they must have opposite spin.
Electron Spin Quantum Number (ms):
+1/2, -1/2
Imagine people in a house one on feet……
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Hund’s Rule
In a set of orbitals, the electrons will fill the
orbitals in a way that would give the
maximum number of parallel spins
(maximum number of unpaired electrons).
Analogy: Students could fill each seat of a
school bus, one person at a time, before
doubling up.
Orbital
Diagram for
Hydrogen
Orbital
Diagram
for Helium
Orbital
Diagram
for Lithium
Orbital
Diagram
for
Beryllium
Orbital
Diagram
for Boron
Orbital
Diagram
for Carbon
Orbital
Diagram
for
Nitrogen
Rappers Resort
Orbital
Diagram
Orbital
Diagram
for Fluorine
Notations of Electron
Configurations
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Standard
Shorthand
Standard Notation – electron
configurations
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If I had to send mail to someone living
in the house you just built how would I
address the envelope?
I would have to do the following.
Floors I have to climb to get to you
Type of rooms I pass
How many people are living in the
rooms
Match up
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Who is who in this situation?
Floors I have to climb
electrons
Type of rooms I pass
Principle energy levels
How many people are living
in the rooms
orbitals
ALWAYS!!!
ROW
BLOCK
# OF BLOCKS
Color it in!
What do you notice about the
d block?
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the d block ______________
________ so instead of 4d it is _____.
Why? It’s like closets in bedrooms.
Standard Notation
of Fluorine
2
1s
Number of electrons
in the sub level 2,2,5
2
2s
5
2p
Sublevels
Practice
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He
Li
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P
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O
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Fe
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Shorthand Notation- Noble
gas configurations
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Use the last noble gas that is located in
the periodic table right before the
element.
Write the symbol of the noble gas in
brackets.
Write the remaining configuration after
the brackets.
Ex: Fluorine: [He] 2s2 2p5
Practice
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Ca
Al
Br
Cu
Lewis Dot Structures
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Models to show how many valence
electrons are in the A group elements.
This doesn’t apply to group B
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Group # = Dots!
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Examples
You try!
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Xe
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Cs
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Sr
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I
Electrons get excited!
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Electrons can gain energy and move to
an excited state and emit energy in
specific wavelengths of light we can
see!
How?
Ground state
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Electrons have a ground state – or a
state in which they normally exist.
When energy is added to the system
they jump to the next level
ON the RETURN to ground level they
emit light in our visible spectrum.
Visible spectrum
Flame test.
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We are going to solve a crime…….
See flame test worksheets
That’s it
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Good luck on your test!