light and energy in 1900 max planck helped us move toward a better understanding of electromagnetic...

Light and Energy

In 1900 Max Planck helped us move toward a better

understanding of electromagnetic radiation.

Matter can gain or lose energy only in small, specific amounts called quanta.

A quantum is the minimum amount of energy that can be gained or lost by

an atom.

Atomic Emission SpectrumAtomic Emission Spectrum

Electrons gain energy and ‘jump’ to a higher energy level.

This is an unstable excited state. The electrons release energy when they return

to their ground state. We see this energy as light.

The Bohr Quantum ModelThe Bohr Quantum Model

The electron in a hydrogen atom moves around the nucleus only in certain allowed circular orbits

Ground State: The lowest possible energy level.

Excited State: Higher energy level.

Atomic Emission SpectraAtomic Emission Spectra

Wave-Particle Duality Theory Wave-Particle Duality Theory (Einstein)(Einstein)

Is energy a wave like light, or a particle?

BOTH

Atomic Theory

Louis de Broglie (1892 – 1987)

•Matter has characteristics of both waves

and particles

•Electrons move in wavelike motion in the

•circular orbits

Heisenberg Uncertainty PrincipleHeisenberg Uncertainty Principle

There is a fundamental limitation to just how precisely we can know

both the position and momentum of a particle at a given time

SchrodingerSchrodinger

Came up with an equation to describe the probability of finding an electron within a 3D area of space.

These equations are called wavefunctions. The wavefunctions describe orbitals.

Orbitals are the building block of electron arrangement.

The Quantum Model!The Quantum Model!

Atomic orbitals are used to describe the possible position and energy of an electron.

OrbitalsOrbitals

The location of an electron is described with 4 terms.

- Energy Level

- Sublevel

- Orbital

- Spin

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 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


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 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 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.


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.


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.


Value = –l to 0 to +l, therefore: s = ___ 0

Or just 1 orientation


Values are –l to 0 to +l, therefore: p = ___ ___ ___

-1 0 +1 Or 3 orientations


Values are –l to 0 to +l, therefore: d = ___ ___ ___ ___ ___ -2 -1 0 1 2 or 5 orientations


Values are –l to 0 to +l, therefore: f = ___ ___ ___ ___ ___ ___ ___ -3 -2 -1 0 1 2 3 or 7 orientations


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:


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


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.


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.


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


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?


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.


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


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


Also note that according to the Aufbau Principle, after 6s should fill 4f and then 5d.


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


List and define the 4 principles that are part of 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

light and energy in 1900 max planck helped us move toward a better understanding of electromagnetic...

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