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Electron Configuration and
Basic Quantum Model
NC Essential Standard
1.3.2
Quantum mechanics and it relation to electron configuration
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Slide 1
Notes:
Electron Configuration and Basic
Quantum Model
This lesson is on how the electrons are arranged
and basic quantum mechanics.
Duration: 00:00:05
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Electron Configuration and
Basic Quantum Model
NC Essential Standard
1.3.2
Quantum mechanics and it relation to electron configuration
Slide 2
Notes:
Quantum Model
Quantum Model
Duration: 00:00:33
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The quantum model describes the probability of locating an
electron at any place.
Heisenberg Uncertainty Principle – it is impossible to know both
the velocity (momentum) and the position of an electron at the
same time.
– The impact of a photon of light alters the motion of the electron
in unpredictable ways, so measuring position changes velocity
Each electron is assigned four quantum numbers that describe it.
No two electrons of an atom can have the same four quantum
numbers.
Slide 3
Notes:
Principle Energy Level, n
Duration: 00:00:16
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Principle Energy Level, n
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The quantum model describes the probability of
locating an electron at any place. The
Heisenberg Uncertainty Principle – states it is
impossible to know both the velocity
(momentum) and the position of an electron at
the same time The impact of a photon of light
alters the motion of the electron in unpredictable
ways, so measuring position changes velocity.
Each electron is assigned four quantum numbers
that describe its location within the atom. No two
electrons of an atom can have the same four
quantum numbers.
Indicates main energy level occupied by eAlways a whole number (1, 2, …)
To calculated the number of electrons that a given energy level can
have. Simpley use the formula 2n2
1st level can hold 2(1)2 = 2 e2nd level can hold 2(2)2 = 8 e3rd level can hold 2(3)2 = 18 e4th level can hold 2(4)2 = 32 eThe period indicates the # of principle energy levels
The principle quantum number is represented by
the letter “n”. The n represents the energy level
being looked at as well as the number of
sublevels the energy level can have. By using
2
the formula 2n the number of electrons that an
energy level can hold can be determined.
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Slide 4
Notes:
Sublevels, l
Sublevels, l
Duration: 00:00:23
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Main energy levels are then divided into sublevels
Indicates the shape or type of orbital
– s, p, d, f
– s sublevel is spherical and holds 2 e– p sublevel is shaped like a dumbbell and holds 6 e– d holds 10 e– f holds 14 e-
Slide 5
Notes:
Orbitals, m
Duration: 00:00:14
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Orbitals, m
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Represents the orbital within the sublevel where the electron is
located
Each orbital holds a pair of electrons therefore:
– 1 s orbital
– 3 p orbitals
– 5 d orbitals
– 7 f orbitals
Slide 6
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The orbitals are the actual place electrons are
located. Each sublevel has a maximum number
of orbitals. The s has one orbit, the p has three
orbits, the d has five orbits and the f has seven
orbits.
Notes:
Spin, s
Duration: 00:00:19
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There are four shapes of sublevels which are
represented by the letter (l). The sublevels are
filled from lowest to highest energy. The lowest
energy sublevel is s which will hold 2 electrons.
The next is p which will hold 6 electrons. The
next sublevel is d which will hold 10 electrons
and finally the fourth sublevel is f and it will hold
14 electrons.
Spin, s
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Each orbital holds 2 electrons that will always spin in opposite
directions the electrons are represented by +1/2 and -1/2. Note
arrows are used in the orbital notation for example ??.
The last quantum number is called the spin
quantum number represented by the letter “s” it
has two orientations. The number values are
positive one half and negative one half. The up
arrow indicates an electron is spinning clockwise
and the down arrow indicates an electron
spinning in the counter clockwise manner.
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Slide 7
s Orbital
• The s orbital
is spherically
shaped.
There is one
s orbital for
each value n
= 1,2,3,…, of
the principle
number.
Duration: 00:00:07
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Slide 8
These are the three orientations for the orbits in
the p sublevel. Notice each orbit is in a different
orientation in space.
Duration: 00:00:09
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Slide 9
Notes:
d Orbital
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The s orbital is spherically shaped. There is one
s orbital for each value of n.
Notes:
p Orbital
Duration: 00:00:08
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Notes:
•
For each of the
values n = 3, 4, 5,…,
there are five d
orbitals. Four of the
five have similar
shapes, but differ in
orientation.
These are the five orientations for the orbits in
the d sublevel. Notice each orbit is in a different
orientation in space.
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Slide 10
Electron Configurations
Duration: 00:00:16
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Electron Configurations
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Slide 11
Electron Configurations
Duration: 00:00:33
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Slide 12
Explanation of configuration
Duration: 00:00:12
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Shows the electron arrangement in an atom, always represents the
lowest possible energies
Aufbau Principle (German for “building up”) – electrons fill orbitals
that have the lowest energies first
Notes:
Electron configurations are a way to show the
arrangement of an atoms electrons from the
lowest energy level to the highest energy level.
The Augbau Principle is a governing principle
that say that electrons will fill the lowest energy
level that can receive it first.
Notes:
The relative energies of orbitals are represented
here in two ways. The yellow brick road is the
typical representation of the energy
arrangement. The way to use the yellow brick
road is to connect the arrows from right to left.
The order for electrons is as follows.
1s,2s,2p,3s, 3p, 4s, 3d, and so on. The green
image, lines them up in a simple flow diagram for
you to follow. Note as the atom get larger, they
start to overlap.
Notes:
The large number represents the energy level,
the small letter represents the sublevel and its
shape and the superscript number represents
the number of electrons in the orbit.
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Slide 13
Practice
Write electron configurations
Duration: 00:00:07
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Practice
Write electron configurations
– Pb:
• 1s22s22p63s23p6
Note All the superscripts should add up to the
number of electrons
Slide 14
Here are some examples of how electron
configurations are done. We just need to
account for all the electrons and their locations.
Since they fill up the lower levels first, only the
last shell (Valence electrons) varies from the
previous element’s configuration
Duration: 00:00:17
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Slide 15
Notes:
Practice
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The first representation of electron configuration
shows the location of each of the atoms
electrons.
Notes:
Electron Configurations
Duration: 00:00:07
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Notes:
Practice
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Write the electron configuration for
C
N
O
F
Ne
Na
Mg
Al
Here is some practice for you to try. Once you
have finished go to the next slide and check your
answers.
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Slide 16
Notes:
Practice
Duration: 00:00:04
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Practice
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Write the electron configuration for
C: 1s2 2s2 2p2
N: 1s2 2s2 2p3
O: 1s2 2s2 2p4
F: 1s2 2s2 2p5
Ne: 1s2 2s2 2p6
Na: 1s2 2s2 2p6 3s1
Mg: 1s2 2s2 2p6 3s2
Al: 1s2 2s2 2p6 3s2 3p1
Slide 17
Refer to this Periodic Table when
writing electron configurations
Duration: 00:00:37
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Here are the answers from the previous slide.
Notes:
Refer to this Periodic Table when writing
electron configurations
The numbers in
front of the “s”
and “p” are the
same as the row #
P1 p2 p3 p4 p5 p6
Refer to this periodic table. The number in front
of the s and p sublevel corresponds to the row.
The number in front of the d sublevel is 1 behind
the row number. The number in front of the f
sublevel is 2 behind the row number. The
exponents represent the number of electrons in
1
that particular sublevel, so you can have an s or
2
1
6
1
10
1
14
s , a p through p , d – d , and f – f These
regions are called the s, p, d, f, blocks.
Slide 18
Shorthand Notation
Duration: 00:00:11
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Notes:
The second representation is called a shorthand
notation which substitutes in a noble gas symbol
to represent previously filled energy levels.
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Slide 19
Notes:
Examples
Here are some examples of shorthand notation.
Duration: 00:00:04
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Slide 20
Notes:
Practice
Shorthand Notation Practice
Duration: 00:00:06
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Practice using shorthand notation and then
check you answers with the next slide.
B
Ar
K
Ca
H
Mg
Slide 21
Practice Answers
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Notes:
Here are the answers to the shorthand notation
practice. Check over your work and redo if
necessary.
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Slide 22
Notes:
Orbital notation
Orbital notation uses lines to represent orbits.
Below the line is number of the energy level and
the letter that represents the sublevel Lastly the
arrows represent the spin of each electron.
Duration: 00:00:13
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Slide 23
Notes:
Orbital Notation
Duration: 00:00:10
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Orbital Notation
• Orbital notation uses lines to represent orbits
and arrows to represent the spin of each
electron.
• oxygen has a total of 8 e-
The next governing law is Hund’s rule. This rule
states that multiple orbits with the same energy
will each receive one electron before any of them
receive a second.
The e- configuration for O:
1s2 2s2 2p4
Hund’s Rule: e- spread out within equivalent orbitals
??
??
??
?
?
1s
2s
3s
3s
3p
Slide 24
Sample Orbital Notation
Examples
Duration: 00:00:13
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He
Be
Notes:
Here are some examples of orbital notation.
Notice that Fluorine is in the excited state. We
can tell by the missing arrow in 2s has moved to
make the sixth electron in 2p.
N
F
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Slide 25
Practice Orbital Notation
Practice
Practice
Duration: 00:00:06
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Element
Notes:
Practice this orbital notation then check your
answers with the next slide.
Orbital Notation
Li
C
Al
O
Slide 26
Notes:
Practice Answers
Check your answers with these and if necessary
redo.
Duration: 00:00:05
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Slide 27
Mixed practice
Mixed Practice
Duration: 00:00:12
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Symbol Group# Valence
e[Ar]4s2
[Ne]3s23p3
Notes:
Period
S,p,d,f
block
Highest
energy
level
The electron configuration can help you
determine information about the atoms identity.
Use you periodic table to fill in this chart. The
check your answers with the next slide.
[He]2s22p5
1s22s2
1s22s22p3
1s22s22p63s23p1
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Slide 28
Notes:
Practice Answers
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[Ar]4s2
Symbol
Group#
Valence Period S,p,d,f
eblock
Highest
energy
level
Ca
2
2
4
s
4
[Ne]3s23p3
P
5A /15
5
3
p
3
[He]2s22p5
O
6A /16
7
2
p
4
1s22s2
Be
2
2
2
s
2
1s22s22p3
N
5A /15
5
2
p
2
1s22s22p63s23p1
Al
3A /13
3
3
p
3
Check your answers to see how you have done.
If necessary redo.
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