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FACT:. Chemical reactions happen because electrons are shared or transferred from one substance to another. MAX NUMBER OF ELECTRONS IN AN ENERGY LEVEL. Write a mathematical equation that allows us to predict the Max # if we know the energy level (n). Max # = …n…. - PowerPoint PPT PresentationTRANSCRIPT
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FACT:Chemical reactions
happen because electrons are shared or transferred from one substance to another
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MAX NUMBER OF ELECTRONS IN AN ENERGY LEVEL
ENERGY LEVEL MAX # OF ELECTRONS
1 22 83 184 325 50
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Write a mathematical equation that allows us to predict the Max # if we
know the energy level (n)
ENERGY LEVEL MAX # OF ELECTRONS
1 2
2 8
3 18
4 32
5 50
Max # = …n…
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Equation to calculate Max # of e-
2n2
Where n is any energy level
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There are 4 Quantum #s and those #s are
used to describe where an electron is likely to be found at any given
time
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This is a lot like being able to use four “places” to describe EXACTLY where Mr. T should be at 8:00AM on Friday.
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The first number we already know…
The Principle Quantum #
(a.k.a. The NRG level)
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1st Quantum #Principle Quantum #
Specifies the energy level that the electron
is on
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Principle Quantum # (IDEA Academy’s Street)
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2nd Quantum #
Specifies the shape of the sub-energy level
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s and p Sub Energy Levels
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III. Quantum Mechanical Model: Atomic OrbitalsE. Shapes of orbitals
d orbitals
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ORBITALSpace occupied by a pair of electrons
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Four Sub-Energy LevelsSub NRG
LevelShape Max # of
electrons# of
Orbitals
s Sphere 2 1
p Dumbbell 6 3
d 4-Lobed 10 5
f 6-8 Lobed 14 7
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Sub-Energy Levels
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So why do electrons fill in like they do?
i.e. why is K’s last electron in the 4th NRG level?
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2 Factors Influencing Electron Placement
1.Energy Level- Closer to nucleus=easy
2. Subenergy level (shape) - spdf
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Electron ConfigurationA detailed way of
showing the order in which electrons fill in around the nucleus
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Electron Configuration Symbols
5f 3
Energy LevelSub-Energy
Level
# of e- in sub-energy
level
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Electron Configuration PT
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K
K: 2s21s2 4s13s22p6 3p6
Bohr Models
vs. e- Configs
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Write the e- config for:
H:1s1
He: 1s2
Li: 1s22s1
K: 1s22s22p63s23p64s1
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Valence Electrons
Electrons in the outermost energy
level (involved in chemical reactions)
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Noble Gas ShortcutK: 1s22s22p63s23p64s1
K: [Ar] 4s1
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Aufbau Principle
All lower energy sublevels must be full before high energy sublevels begin
filling in
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Steps for writing NGSC
1. Write the noble gas preceding the desired element [in brackets]
2. Carry on as usual
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With only the first two Quantum #s, do we have as much information as possible as to where the electrons are likely to be
found?
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3rd Quantum #m or magnetic Q#
Specifies the orientation of an orbital in space
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4th Quantum #s or spin Q#
Spin of an electron on its own axis
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Quantum Review1st Q#: Energy Level
2nd Q#: Shape of sub3rd Q#: Orientation of Orbital
4th Q#: Spin of e-
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Quantum ReviewPrinciple (n): 1, 2, 3, 4, …
Azimuthal (l): 0, 1, 2, 3
Magnetic (ml): …-2, -1, 0, 1, 2
Spin (ms): +1/2 or -1/2
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Pauli Exclusion Principle
No 2 electrons can have the same set of 4
quantum numbers
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Arrow-Orbital Diagrams
A way to show orbital filling, spin,
relative energy
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Hund’s RuleMost stable
arrangement of electrons is the one with the maximum number of
unpaired electrons
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Arrow-Orbital DiagramsE
ner
gy
1s2s 2p
3p3s4s
3d
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Lewis Electron Dot Diagrams
The easiest way to represent the # of valance electrons
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Steps for writing electron dot diagrams
1. Write the element’s symbol
2. Write out e- config
3. Count # of valence e-s (1-8)
4. Place same # of dots as e- around symbol
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Order to fill in an e- dot
Bm
12
34
5
6
7
8
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What up?
Bm
12
Why do 1 and 2 fill in on the same side?
Who do 1 and 2 represent?
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What up?
Bm
34
5
6
78
Who do 3-8 represent?
Why do 3,4,5 and 6,7,8 fill in on different sides?
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What up?
Bm
34
5
6
78
Why will you never have
more than eight dots?
12
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Examples of Lewis Electron Dots
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What is different between the dot diagrams below and the ones that we’ve been doing?
Our way accounts for Quantum #s, this way doesn’t!