Electron Configurations, Orbital Notation and Quantum Numbers
Quantum Numbers At the conclusion of our time together, you should be able to: List and define each...
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Transcript of Quantum Numbers At the conclusion of our time together, you should be able to: List and define each...
Quantum NumbersQuantum NumbersAt the conclusion of our time At the conclusion of our time together, you should be able together, you should be able
to:to:
List and define each of the 4 quantum numbers.
Relate these numbers to the state, city, street and home address for the electron.
Give the maximum number of electrons for each level and sublevel.
Draw the basic shape of the 4 sublevels.
Principal Quantum Number - nPrincipal Quantum Number - n
Symbol = n Represents the main energy level of the electron
and its distance from the nucleus Equation: 2n2 - shows how many electrons can
be in each energy level
(e.g. 3rd energy level: 2(3)2 = 18 total possible e-
in this energy level) Your turn: How many electrons in the 4th energy
level?32
Principal Quantum Number - nPrincipal Quantum Number - n
In an address analogy, this would be the state in which the electron would probably be found. Presently, we can find electrons in 7 states.
Values are 1-7
Ex. = 1s1 (the electron configuration for H)
Principal Quantum number = 1
The First of 4 Quantum Numbers for The First of 4 Quantum Numbers for the One Electron of Hydrogenthe One Electron of Hydrogen
n (energy level)
1
The Second Quantum Number - The Second Quantum Number - ll
This number describes sublevels, shapes of these sublevels and is the Angular momentum quantum number. The number of sublevels (shapes) in an energy level equals the value of n, the principle quantum number. The first 4 sublevels are named s, p, d, f.
Each sublevel has a unique shape:
Shape of the “s” Orbital
•s for "Sphere": the simplest shape, or shape of the simplest atoms like hydrogen and helium
•Electrons don't interfere with, or block, each other from the pull of the nucleus - ball shape•Each energy level has an "s" orbital at the lowest energy within that level
•p for "Peanut/Petal": a more complex shape that occurs at energy levels 2 and above
Shapes of the “p” Orbitals
• d for "Double Peanut/Petal": a complex shape occurring at energy levels 3 and above
•The arrangement of these orbitals allows for "s" and "p" orbitals to fit closer to the middle/nucleus
Shapes of the “d” Orbitals
•f for "Flower": bizarre-shaped orbitals for electrons of very large atoms
•electrons filling these orbitals are weakly attached to the atom because they are so far away from the pull of the nucleus
Shapes of the “f” Orbitals
The Second Quantum Number - The Second Quantum Number - ll
In the address analogy, this would be the city in which the electron would probably be found. In the first state there would be 1 city, in the second state there would be 2 cities...
This number is from the formula: 0 to (n-1)
The Second Quantum Number - The Second Quantum Number - ll
The 2nd Quantum Number = 0 to (n-1) Ex. = 1s1 , s sublevel number is 0 to (1-1) = 0 p sublevel number is, 0 to (2-1) = 1 d sublevel number is, 0 to (3-1) = 2 f sublevel number is, 0 to (4-1) = 3 Therefore:
For s, l = 0For p, l = 1For d, l = 2For f, l = 3
The Second of 4 Quantum Numbers for The Second of 4 Quantum Numbers for the One Electron of Hydrogenthe One Electron of Hydrogen
n (energy level)
1
l (angular momentum,
sublevel shape)
0
Ex. = 1s1, 0 to (1-1) = 0Second Quantum number for Hydrogen = 0
The Third Quantum Number - mThe Third Quantum Number - m
This number describes orientations of the orbitals that each sublevel can have and is the Magnetic quantum number.
s has one orientation, p has three orientations , d has five orientations and f has 7 orientations.
We’ll see how we got these orientation numbers in just a moment.
The Third Quantum Number - mThe Third Quantum Number - m
In the address analogy, this would be the street on which the electron would probably be found.
In the first state there is one city. In this first city there would be one street.
In the second state there are two cities. The first city with its one street and a second city with its 3 streets for a total of 4.In the 3rd state would have the previous 4 streets plus 5 more streets from the 3rd
city for a total of 9.
The Third Quantum Number - mThe Third Quantum Number - m
3rd Quantum Number = –l to 0 to +lWe know what the shape looks like
from the second Quantum Number, now we know how many orientations of these shapes each sublevel has by plugging the l value into the formula
above.
The Third Quantum Number - mThe Third Quantum Number - m
Value = –l to 0 to +l, therefore: s = ___ 0
Or just 1 orientation
The Third Quantum Number - mThe Third Quantum Number - m
Values are –l to 0 to +l, therefore: p = ___ ___ ___
-1 0 +1 Or 3 orientations
The Third Quantum Number - mThe Third Quantum Number - m
Values are –l to 0 to +l, therefore: d = ___ ___ ___ ___ ___ -2 -1 0 1 2 or 5 orientations
The Third Quantum Number - mThe Third Quantum Number - m
Values are –l to 0 to +l, therefore: f = ___ ___ ___ ___ ___ ___ ___ -3 -2 -1 0 1 2 3 or 7 orientations
The Third Quantum Number - mThe Third Quantum Number - m
Let’s Review the Values for m: s = ___ p = ___ ___ ___ 0 -1 0 +1 d = ___ ___ ___ ___ ___ -2 -1 0 1 2 f = ___ ___ ___ ___ ___ ___ ___ -3 -2 -1 0 1 2 3 Ex. = 1s1 = 0
Third Quantum number from s = 0, or 1 shape
The Third of the 4 Quantum Numbers The Third of the 4 Quantum Numbers for the One Electron of Hydrogenfor the One Electron of Hydrogen
n (energy level)
1
l (angular momentum,
sublevel shape)
0
m (magnetic, orientation)
0
The Fourth Quantum Number - sThe Fourth Quantum Number - s
This number describes the spin of the electrons in an orbital. There can be two electrons in each orbital as long as they are spinning in opposite directions.
In the address analogy, this would be the house number of the electron. There can only be 2 houses on each
street Values are +1/2 = clockwise spin -1/2 = counter clockwise spin
The Fourth Quantum Number - sThe Fourth Quantum Number - s
Ex. = 1s1 , spin is up or +1/2
Fourth Quantum number from 1 = +1/2
The Fourth of the 4 Quantum Numbers The Fourth of the 4 Quantum Numbers for the One Electron of Hydrogenfor the One Electron of Hydrogen
n (energy level)
1
l (angular momentum,
sublevel shape)
0
m (magnetic, orientation)
0
s (spin, clockwise or
counterclockwise)
+1/2
Quantum # Summary for HydrogenQuantum # Summary for Hydrogen
1s1
Hydrogen has one electron spinning in a clockwise direction in the first energy level that has one orbital and only one orientation in its s sublevel shape which is spherical.
The 4 quantum numbers for H are: 1, 0, 0, +1/2
Quantum NumbersQuantum NumbersLet’s see if you can:Let’s see if you can:
List and define each of the 4 quantum numbers.
Relate these numbers to the state, city, street and home address for the electron.
Give the maximum number of electrons for each level and sublevel.
Draw the basic shape of the 4 sublevels.
How do we know when an electron has How do we know when an electron has moved from an excited state to the moved from an excited state to the
ground state? The electron willground state? The electron will
1. Release a photon.
2. Release a specific amount of energy.
3. Release a specific color.
4. Release a quantum of energy.
5. All of the above are correct.
What does the second quantum What does the second quantum number (number (ll) describe?) describe?
1. Orbital shape.
2. Energy level.
3. Electron spin.
4. Orbital orientation.
Which quantum number has values of +½ or –½?
1. Orbital shape.
2. Energy level.
3. Electron spin.
4. Orbital orientation.
Which of the following is not a possible Which of the following is not a possible orbital shape?orbital shape?
1. s
2. p
3. z
4. f
What is currently the highest possible What is currently the highest possible principal quantum number an electron principal quantum number an electron
can have?can have?
1. No limit
2. 5
3. 6
4. 7
How many electrons will the 4How many electrons will the 4thth energy energy level hold?level hold?
1. No limit
2. 8
3. 18
4. 32
5. 50
1. sphere
2. petal
3. double petal
4. flower
5. mess
The p sublevel would look like a The p sublevel would look like a
Quantum NumbersQuantum NumbersAt the conclusion of our time At the conclusion of our time together, you should be able together, you should be able
to:to:
Continue to relate Quantum Numbers to the state, city, street and home address for the electron.
Give the 4 quantum number for every electron of every atom on the periodic table.
Let’s Try HeliumLet’s Try Helium
H is 1s1
He has 2 electrons, can we add another electron spinning in the other direction in the first energy level of the s sublevel with its 1 spherical orbital?
Yes, He is 1s2
He has 2 electrons spinning in opposite directions in the s sublevel with its spherical shape with 1 orientation.
Remember the Quantum # Summary Remember the Quantum # Summary for Hydrogenfor Hydrogen
1s1
Hydrogen has one electron spinning in a clockwise direction in the first energy level that has one spherical orbital in its s sublevel.
The 4 quantum numbers for H are: 1, 0, 0, +1/2
The Pauli Exclusion PrincipleThe Pauli Exclusion Principle
No two electrons in an atom can have the same set of four quantum numbers.
Therefore, the second electron that He has must have a different set of 4 Quantum Numbers.
What would they be??
The 4 Quantum Numbers of HeliumThe 4 Quantum Numbers of Helium
n
1
l 0
m
0
s-1/2
The 4 Quantum Numbers of HeliumThe 4 Quantum Numbers of Helium
No two electrons in an atom can have the same set of four quantum numbers.
What principle?? Pauli Exclusion Principle Therefore, the second electron that He has must
have a different set of 4 Quantum Numbers. What would they be?? 1, 0, 0, -1/2
Let’s Try LithiumLet’s Try Lithium
He is 1s2
He has 2 electrons, can we add another electron spinning in another direction in the first energy level of the s sublevel with its 1 spherical orbital?
No, the third electron must go to the 2nd energy level which has 2 sublevels, s and p, s with its one spherical orbital and p with its 3 orientations of its petal shaped orbitals.
Let’s Try LithiumLet’s Try Lithium
So the address for all 3 electrons of Li is:
1s2 2s1
This is called the electron configuration for Li and basically says that the first two electrons of Li are in the s sublevel with its one spherical shape with the 3rd electron in the 2 energy level, s sublevel with its bigger spherical shape.
The Quantum #’s of the 3rd electron:
The 4 Quantum Numbers for the 3The 4 Quantum Numbers for the 3rdrd Electron of LithiumElectron of Lithium
n
2
l0
m
0
s+1/2
Now Beryllium:Now Beryllium:
Add one more electron to Li : 1s2 2s1? Where would it go?? 1s2 2s2
The 2s sublevel with its one spherical orbital can hold 2 electrons spinning in opposite directions.
The Quantum #’s of the 4th electron:
The 4 Quantum Numbers for the 4The 4 Quantum Numbers for the 4thth Electron of BerylliumElectron of Beryllium
n
2
l0
m
0
s-1/2
What About Boron:What About Boron:
Add one more electron to Be: 1s2 2s2? Where would it go?? 1s2 2s3 ? No 1s2 2s2 2p1
The 2s sublevel with its one spherical orbital is full. We must now start filling the 2p sublevel with its 3 orbitals
The Quantum #’s of the 5th electron:
The Electrons of the 2The Electrons of the 2ndnd Energy Level Energy Level for Boronfor Boron
s = ___ p = ___ ___ ___ 0 -1 0 +1
The 4 Quantum Numbers for the 5The 4 Quantum Numbers for the 5thth Electron of BoronElectron of Boron
n
2
l1
m
-1
s+1/2
Let’s Move to Carbon:Let’s Move to Carbon:
Add one more electron to B: 1s2 2s2 2p2
The 2p sublevel has 3 orbitals. However, we can’t put another electron in the first orbital of p. Why?
Hund’s Rule: Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron.
The Electrons of the 2The Electrons of the 2ndnd Energy Level Energy Level for Carbonfor Carbon
s = ___ p = ___ ___ ___ 0 -1 0 +1
The 4 Quantum Numbers for the 6The 4 Quantum Numbers for the 6thth Electron of CarbonElectron of Carbon
n
2
l1
m
0
s+1/2
Nitrogen:Nitrogen:
Add one more electron to C: 1s2 2s2 2p3
The 3rd electron in the p sublevel must go into the 3rd orbital. Why?
Again Hund’s Rule: Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron.
The Electrons of the 2The Electrons of the 2ndnd Energy Level Energy Level for Carbonfor Carbon
s = ___ p = ___ ___ ___ 0 -1 0 +1
The 4 Quantum Numbers for the 7The 4 Quantum Numbers for the 7thth Electron of NitrogenElectron of Nitrogen
n
2
l1
m
1
s+1/2
Oxygen:Oxygen:
Add one more electron to N: 1s2 2s2 2p4
The 4th electron in the p sublevel must begin to double up the electrons of the three p orbitals.
The Electrons of the 2The Electrons of the 2ndnd Energy Level Energy Level for Carbonfor Carbon
s = ___ p = ___ ___ ___ 0 -1 0 +1
The 4 Quantum Numbers for the 8The 4 Quantum Numbers for the 8thth Electron of OxygenElectron of Oxygen
n
2
l1
m
-1
s-1/2
Fluorine:Fluorine:
Add one more electron to O: 1s2 2s2 2p5
Where would the 5th electron for the 2p orbitals go?
The Electrons of the 2The Electrons of the 2ndnd Energy Level Energy Level for Fluorinefor Fluorine
s = ___ p = ___ ___ ___ 0 -1 0 +1
The 4 Quantum Numbers for the 9The 4 Quantum Numbers for the 9thth Electron of FluorineElectron of Fluorine
n
2
l1
m
0
s-1/2
Neon:Neon:
Add one more electron to F: 1s2 2s2 2p6
Where would the 6th electron for the 2p orbitals go?
The Electrons of the 2The Electrons of the 2ndnd Energy Level Energy Level for Neonfor Neon
s = ___ p = ___ ___ ___ 0 -1 0 +1
The 4 Quantum Numbers for the 10The 4 Quantum Numbers for the 10thth Electron of NeonElectron of Neon
n
2
l1
m
1
s-1/2
What About Sodium:What About Sodium:
Add one more electron to Ne: 1s2 2s2 2p7 No!! The 2p sublevel with its 3 orbitals
is full. We must now go to the 3rd energy level with its 3 sublevels, s, p, and d, and start filling electrons all over again!
The Electrons of the 3The Electrons of the 3rdrd Energy Level Energy Level for Sodiumfor Sodium
s = ___ p = ___ ___ ___ 0 -1 0 +1
d = ___ ___ ___ ___ ___ -2 -1 0 1 2
The 4 Quantum Numbers for the 11The 4 Quantum Numbers for the 11thth Electron of SodiumElectron of Sodium
n
3
l0
m
0
s+1/2
What About Magnesium:What About Magnesium:
Add one more electron to Na: 1s2 2s2 2p6 3s2
Remember, the s sublevel with its one spherical orbital can have one more electron.
The Electrons of the 3The Electrons of the 3rdrd Energy Level Energy Level for Magnesiumfor Magnesium
s = ___ p = ___ ___ ___ 0 -1 0 +1
d = ___ ___ ___ ___ ___ -2 -1 0 1 2
The 4 Quantum Numbers for the 12The 4 Quantum Numbers for the 12thth Electron of MagnesiumElectron of Magnesium
n
3
l0
m
0
s-1/2
Aluminum:Aluminum:
Add one more electron to Mg:
1s2 2s2 2p6 3s2 3p1
Remember, the s sublevel with its one spherical orbital can only have 2 electrons. The next electron must start to fill the 3p sublevel with its 3 orbitals.
The Electrons of the 3The Electrons of the 3rdrd Energy Level Energy Level for Aluminumfor Aluminum
s = ___ p = ___ ___ ___ 0 -1 0 +1
d = ___ ___ ___ ___ ___ -2 -1 0 1 2
The 4 Quantum Numbers for the 13The 4 Quantum Numbers for the 13thth Electron of AluminumElectron of Aluminum
n
3
l1
m
-1
s+1/2
Silicon to Argon:Silicon to Argon:
Keep adding one more electron to Al:
1s2 2s2 2p6 3s2 3p2-6
Remember Hund’s rule. We will put one electron in each of the p orbitals and then come back to double up.
The Electrons of the 3The Electrons of the 3rdrd Energy Level Energy Level for Silicon to Argonfor Silicon to Argon
s = ___ p = ___ ___ ___ 0 -1 0 +1
d = ___ ___ ___ ___ ___ -2 -1 0 1 2
The 4 Quantum Numbers for the 18The 4 Quantum Numbers for the 18thth Electron of ArgonElectron of Argon
n
3
l1
m
1
s-1/2
Quantum NumbersQuantum NumbersLet’s see if you can:Let’s see if you can:
Continue to relate Quantum Numbers to the state, city, street and home address for the electron.
Give the 4 quantum number for every electron of every atom on the periodic table.
The 5f sublevel with its orbitals would The 5f sublevel with its orbitals would look like a look like a
1. sphere
2. petal
3. double petal
4. flower
5. mess
How many orbitals are in the 5f How many orbitals are in the 5f sublevel? sublevel?
1. No limit
2. 1
3. 3
4. 5
5. 7
How many electrons will the 4f How many electrons will the 4f sublevel hold?sublevel hold?
1. 2
2. 6
3. 10
4. 14
5. 18
1. 1
2. 2
3. 3
4. 4
5. 5
In the address analogy, the first In the address analogy, the first quantum number is the state and the quantum number is the state and the second quantum number is the city. second quantum number is the city.
How many cities are there in the How many cities are there in the second state?second state?
1. 1
2. 2
3. 3
4. 4
5. 5
In the address analogy, the second In the address analogy, the second state can have how many total state can have how many total
streets?streets?
Quantum NumbersQuantum NumbersAt the conclusion of our time At the conclusion of our time together, you should be able together, you should be able
to:to:
Explain the Aufbau principle and the diagonal rule.
Use Hund’s rule in an orbital filling diagram.
Give the quantum numbers for every electron of every atom on the periodic table.
Draw the electron configuration and orbital notation for every element.
Now Potassium:Now Potassium:
We should now start to fill the 3d sublevel with its 5 orbitals.
1s2 2s2 2p6 3s2 3p6 3d1
But now we must consider the Aufbau Principle:
An electron will occupy the lowest energy level orbital that can receive it.
Look at the energy needed for 3d vs. 4s:
??????
The Aufbau PrincipleThe Aufbau Principle
You will need to remember this chart so that you place electrons in the correct order.
An easy way to remember the filling order is to follow the diagonal rule.
Check it out on the next slide:
Maybe You’ve Seen Maybe You’ve Seen This Chart???This Chart???ss
s 3p 3ds 3p 3d
s 2ps 2p
s 4p 4d 4fs 4p 4d 4f
s 5p 5d 5f 5g?s 5p 5d 5f 5g?
s 6p 6d 6f 6g? 6h?s 6p 6d 6f 6g? 6h?
s 7p 7d 7f 7g? 7h? 7i?s 7p 7d 7f 7g? 7h? 7i?
11
22
33
44
55
66
77
It Represents the It Represents the Diagonal RuleDiagonal Rule
Steps:
1. Write the energy levels top to bottom.
2. Write the orbitals in s, p, d, f order. Write the same number of orbitals as the energy level.
3. Draw diagonal lines from the top right to the bottom left.
4. To get the correct order, follow the arrows!
Diagonal RuleDiagonal Rule
ss
s 3p 3ds 3p 3d
s 2ps 2p
s 4p 4d 4fs 4p 4d 4f
s 5p 5d 5f 5g?s 5p 5d 5f 5g?
s 6p 6d 6f 6g? 6h?s 6p 6d 6f 6g? 6h?
s 7p 7d 7f 7g? 7h? 7i?s 7p 7d 7f 7g? 7h? 7i?
11
22
33
44
55
66
77
By this point, we are By this point, we are past the current past the current periodic table so we periodic table so we can stop.can stop.
The Aufbau PrincipleThe Aufbau Principle
But there is even an easier way to remember the filling order.
Have you noticed areas in the periodic table where certain sublevels are filling??
Check it out on the next slide:
The 4 Blocks of the Periodic TableThe 4 Blocks of the Periodic Table
The Aufbau PrincipleThe Aufbau Principle
So, what block is always filling on the left side of the periodic table??
The s block!! What period is it?? The 4th!! Therefore, 4s will begin filling before we fill 3d!!!
So is Potassium?So is Potassium?
1s2 2s2 2p6 3s2 3p6 3d1
No!!! 1s2 2s2 2p6 3s2 3p6 4s1
The Electrons of the 4The Electrons of the 4rdrd Energy Level Energy Level for Potassium and Calciumfor Potassium and Calcium
s = ___ p = ___ ___ ___ 0 -1 0 +1
d = ___ ___ ___ ___ ___ -2 -1 0 1 2
The 4 Quantum Numbers for the 20The 4 Quantum Numbers for the 20thth Electron of CalciumElectron of Calcium
n
4
l0
m
0
s-1/2
The “D” Block ElectronsThe “D” Block Electrons
The next electron for Scandium will now start to fill the “D” block.
Please note that the energy level for the d sublevel is not 4. We have not filled 3d yet.
Therefore, the “D” block will always be one energy level behind the current energy level.
• d for "Double Peanut/Petal": complex shape occurring at energy levels 3 and above
•How many orbitals (orientations) does “d” have?•5
Remember the Shape of the “d” Orbitals
So for Scandium to ZincSo for Scandium to Zinc
Following Hund’s Rule, we will put one electron in each of the 3d orbitals before we begin to double up the electrons in each orbital.
Remember that the “d” block is always one energy level behind.
The Electrons of the 3The Electrons of the 3rdrd Energy Level Energy Level for Scandium to Zincfor Scandium to Zinc
s = ___ p = ___ ___ ___ 0 -1 0 +1
d = ___ ___ ___ ___ ___ -2 -1 0 1 2
The 4 Quantum Numbers for the The 4 Quantum Numbers for the Circled Electron of ZincCircled Electron of Zinc
n
3
l2
m
1
s+1/2
Gallium to KryptonGallium to Krypton
So, what block is always filling on the right side of the periodic table??
The p block!! What period is it?? Back to the 4th!! Therefore, 4p will begin filling after we fill 3d!!!
The Electrons of the 4The Electrons of the 4rdrd Energy Level Energy Level for Gallium to Kryptonfor Gallium to Krypton
s = ___ p = ___ ___ ___ 0 -1 0 +1
d = ___ ___ ___ ___ ___ -2 -1 0 1 2
The 4 Quantum Numbers for the The 4 Quantum Numbers for the Circled Electron of KryptonCircled Electron of Krypton
n
4
l1
m
-1
s-1/2
Rubidium and StrontiumRubidium and Strontium
So, what block is always filling on the left side of the periodic table??
The s block!! What period is it?? 5th!! Remember, the 4th energy level has 4 sublevels,
s, p, d, and f. Because of the Aufbau Principle, d and f will fill later.
Rubidium and StrontiumRubidium and Strontium
Let’s do the electron configuration for these two elements
1s2 2s2 2p6 3s2 3p6 4s2 3d10
4p6
5s1
or 5s2
How About Yttrium to Cadmium?How About Yttrium to Cadmium?
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2
4d1-10
Indium to Xenon?Indium to Xenon?
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10
5p1-6
Cesium and Barium?Cesium and Barium?
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6
6s1-2
Now do the 4 quantum numbers for 55th electron of Barium.
The 4 Quantum Numbers for the The 4 Quantum Numbers for the Circled Electron (55Circled Electron (55thth) of Barium) of Barium
n
6
l0
m
0
s+1/2
The “F” Block ElementsThe “F” Block Elements
Now we come to a confusing part of the periodic table.
Note that element #57, Lanthanum, is in the “d” block but the next element #58, Cerium, drops down to the “f” block.
The Periodic TableThe Periodic Table
The “F” Block ElementsThe “F” Block Elements
Also note that according to the Aufbau Principle, after 6s should fill 4f and then 5d.
The “F” Block ElementsThe “F” Block Elements
Recent discoveries suggest that Lanthanum is not the first element of the 4f block as previously thought, but really is the first element of the 5d block.
From there we will move to the 4f block.
Lanthanum?Lanthanum?
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
5d1
Then Cerium is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
5d1
4f1
The Rest of the 4f BlockThe Rest of the 4f Block#58 Praseodymium to #71 Lutetium#58 Praseodymium to #71 Lutetium
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
5d1
4f1-14
The Electrons of the 4The Electrons of the 4f Sublevelf Sublevel
6s = ___ 6p = ___ ___ ___ 0 -1 0 +1
5d = ___ ___ ___ ___ ___ -2 -1 0 1 2
4f = ___ ___ ___ ___ ___ ___ ___ -3 -2 -1 0 1 2 3
The 4 Quantum Numbers for the The 4 Quantum Numbers for the Circled Electron (67Circled Electron (67thth) of Lutetium) of Lutetium
n
4
l3
m
-1
s-1/2
Now Back to the “D” Block ElementsNow Back to the “D” Block Elements
As we follow the numbers on the Periodic Table, you will see that element #72, Hafnium, is back in the “d” block.
Therefore, Hafnium’s configuration would be: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
5d1 4f14
5d2
Right?? Wrong!!
Now Back to the “D” Block ElementsNow Back to the “D” Block Elements
Why? Count the total electrons… 73 not 72 Why? Because 5d2 includes 5d1
I’ve counted 5d1 twice!! Therefore, I must do this 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
5d1 4f14 5d2
The Rest of the “D” Block ElementsThe Rest of the “D” Block Elements
Tantalum to Mercury 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
5d1 4f14 5d3-10
Now to the 6p Block ElementsNow to the 6p Block Elements
Thallium to Radon 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
5d1 4f14 5d10
6p1-6
What’s NextWhat’s Next
#87 - #88, Francium and Radium 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
5d1 4f14 5d10 6p1-6
7s1-2
Now We Run into the Crazy AreaNow We Run into the Crazy Area
#89, Actinium 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
5d1 4f14 5d10 6p1-6 7s2
6d1
#90 - #103, Thorium to Lawrencium 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
5d1 4f14 5d10 6p1-6 7s2 6d1
5f1-14
Finally, We Finish Up in the D BlockFinally, We Finish Up in the D Block
#104 - #112, Rutherfordium to Copernicium Don’t forget to cross out the 6d1 electron when
you come back to the “d” block 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
5d1 4f14 5d10 6p1-6 7s2 6d1 5f14
6d2-10
Quantum NumbersQuantum NumbersLet’s see if you can:Let’s see if you can:
List and define the 4 principles that are part of quantum numbers.
List and define each of the 4 quantum numbers.
Give the quantum number for every electron of every atom on the periodic table.
Your TurnYour Turn
Let’s see if you can do the last 4 orbital filling diagrams and the 4 quantum numbers for the last electron of #112, Copernicium
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
5d1 4f14 5d10 6p1-6 7s2 6d1 5f14 6d10
The Electrons of the 4 Configurations The Electrons of the 4 Configurations for Coperniciumfor Copernicium
7s = ___ 6p = ___ ___ ___ 0 -1 0 +1
6d = ___ ___ ___ ___ ___ -2 -1 0 1 2
5f = ___ ___ ___ ___ ___ ___ ___ -3 -2 -1 0 1 2 3
The 4 Quantum Numbers for the The 4 Quantum Numbers for the Circled Electron (112Circled Electron (112thth) of Copernicium) of Copernicium
n
6
l2
m
2
s-1/2
It is impossible to determine both the position and the momentum of an electron at the same time.
An electron occupies the lowest energy level available.
No two electrons in the same atom can have the same set of four quantum numbers.
In other words, no two electrons can be in the same place at the same time.
Orbitals of equal energy are each occupied by ONE electron before any orbital is occupied by a SECOND electron
All electrons in a single occupied orbital must have the same spin.
Symbol = n Represents the main energy level of the
electron Range = 1- 7 Ex. = 3s2
Principal Quantum number = 3
Symbol = l (small letter L) Represents the shape of the orbital (also called
sublevel) Range = 0 – n-1 (whole number) Shapes: 0 = s (sphere) 1 = p (petal)
2 = d (double petal) 3 = f (flower) Ex. = 3s2
AM Quantum number = 0
Symbol = m Represents the orientation of the orbital around
the nucleus Each line holds 2 electrons m = -l to +l; Therefore: s = 0, p = 3, d =
5…___ = s
0___ ___ ___ = p
-1 0 +1
___ ___ ___ ___ ___ = d
-2 -1 0 +1 +2
___ ___ ___ ___ ___ ___ ___ = f
-3 -2 -1 0 +1 +2 +3
Ex. = 3s2
Magnetic Quantum number = 0
2 Spin States Clockwise spin = +1/2 (upward
arrow) Counterclockwise spin = -1/2 (downward
arrow)A single orbital can hold two electrons, but they
must have opposite spins Ex. = 3s2
Spin Quantum number = -1/2
Congratulations!!!!Congratulations!!!!
You can now do the complete electron configurations, orbital notations and give 4 quantum numbers (addresses) for every electron of every element on the periodic table!!!
GRADING SCALE
• A = upright and taking air
• B = eyes notable open
• C = responding to the environment
• D = comatose
• F = decomposed