Block 26: Th 11/7 or F 11/8

• Sapling #11 due T 11/12• Flame test lab due next class

• Debrief flame test

Quantum Mechanical Model, Electron Configuration and

Orbital Diagrams

Add to your electrons notesDraw a line and put today’s date: 11/7 or 11/8

Quantum Mechanical Model

Image from the Higher Education Academy Physical Sciences Centre

Max Planck and Werner Heisenberg

expanded upon Bohr’s model

There are energy levels, but they are not circular orbits

They are regions in which you may find

electrons in the electron cloud

Bohr

Quantum

Electrons are organized in three ways1st = Energy levels

each atom contains energy levels;

which generally correspond to the rows of

the PT

2nd = Sublevels

each energy level contain sublevels; they are divided into blocks

called s, p, d and f

3rd = Orbitals

each sublevel contain orbitals; an orbital is the space

occupied by two (a pair of) electrons

It’s like an address!

Electron Sublevels

Start on energy level:

1 and up

2 and up

3 and up

4 and up

# of orbitals 1 orbital

3 orbitals

5 orbitals

7 orbitals

How many electrons can it

hold?

2 e- 6 e- 10 e- 14 e-

Sublevel s p d f

What do orbitals look like?

orbital on s sublevel(one per sublevel)

orbitals on p sublevel (three per sublevel)

(remember two electrons fit in each orbital)

What do orbitals look like?

orbitals on d sublevel(five per sublevel)

What do orbitals look like?

orbitals on f sublevel(seven per sublevel)

Since sublevels and orbitals are too complicated to draw all the time, we simplify with orbital diagrams.

Each orbital is represented by a box.

Each electron is represented by an up or down arrow.

(means 2 electrons)

s sublevels sublevel has one orbital, so we draw one box.

p sublevel

p sublevel has 3 orbitals, so we draw 3 boxes.

d sublevel

d sublevel has 5 orbitals, so we draw 5 boxes.

f sublevel

f sublevel has 7 orbitals, so we draw 7 boxes.

Orbital and sublevel information is like a map, telling you where

an electron can be found in an atom.

There are three rules that govern why an electron will be in one sublevel

rather than another:

1.Pauli Exclusion Principle

2.Hund’s Rule

3.Aufbau Principle

Pauli Exclusion Principle:

No two electrons can have the same set of quantum numbers (basically, “orbital address”).

What that means is that 2 electrons may occupy one orbital, but they must have

opposite spin direction.

This is why we draw electrons as arrows facing opposite directions when they share a box:

Hund’s Rule:Before 2 electrons will occupy the same orbital

of a sublevel, there must be at least one electron in every orbital of that sub level.

WRONG -This is not stable.Electrons repel each other.

RIGHT -This is stable.

Hund’s Rule paraphrased – spread them out before you pair them up!

Example: 4 electrons in a d sublevel

Aufbau Principle: Each electron must occupy

the lowest energy orbital available. Not all sublevels and orbitals have the same energy!

s p d f

energy increases

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p

This chart shows the order that electrons fill sublevels.

Although the d and f sublevels are on lower energy levels, they have high energy and do not fill until after

the s and p for higher energy levels.

Using the Aufbau Diagram

• Add electrons in the order of the arrows you drew

• Remember sublevels and electrons– s holds 2 electrons– p holds 6 electrons– d holds 10 electrons– f holds 14 electrons

The number of columns in each block corresponds

to the number of electrons that fit in that sublevel1 2 2

3 4 5 6 7 8 9 10

11 12 13 14 15 16 17 18

19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36

37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

55 56 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86

87 88 89 90 91 92 93 94 95 96 97 98 99

1 2 2

3 4 5 6 7 8 9 10

11 12 13 14 15 16 17 18

19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36

37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

55 56 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86

87 88 103 104 105 106 107 108 109 110 111

57 58 59 60 61 62 63 64 65 66 67 68 69 70

89 90 91 92 93 94 95 96 97 98 99 100 101 102

Full Length Periodic Table

Condensed Periodic Table s-block

p-block

d-block

f-block

Color Code Key

1

2 3 4 5 6 7

1 2 3 4 5 6 7

1 2 3 4 5 6 7

1 2 3 4 5 6 7

1 2 2

3 4 5 6 7 8 9 10

11 12 13 14 15 16 17 18

19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36

37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

55 56 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86

87 88 89 90 91 92 93 94 95 96 97 98 99

1 2 2

3 4 5 6 7 8 9 10

11 12 13 14 15 16 17 18

19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36

37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

55 56 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86

87 88 103 104 105 106 107 108 109 110 111

57 58 59 60 61 62 63 64 65 66 67 68 69 70

89 90 91 92 93 94 95 96 97 98 99 100 101 102

Full Length Periodic Table

Condensed Periodic Table s-block

p-block

d-block

f-block

Color Code Key

1

2 3 4 5 6 7

1 2 3 4 5 6 7

1 2 3 4 5 6 7

1 2 3 4 5 6 7

The period number tells you the energy level

The block tells you the sublevels

Each square can mean the position

of one electron

You can use the periodic table like a game board to see the order in which the sublevels fill.

An element’s location within that block tells you how many electrons it has in that sublevel

1 2 2

3 4 5 6 7 8 9 10

11 12 13 14 15 16 17 18

19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36

37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

55 56 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86

87 88 89 90 91 92 93 94 95 96 97 98 99

1 2 2

3 4 5 6 7 8 9 10

11 12 13 14 15 16 17 18

19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36

37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

55 56 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86

87 88 103 104 105 106 107 108 109 110 111

57 58 59 60 61 62 63 64 65 66 67 68 69 70

89 90 91 92 93 94 95 96 97 98 99 100 101 102

Full Length Periodic Table

Condensed Periodic Table s-block

p-block

d-block

f-block

Color Code Key

1

2 3 4 5 6 7

1 2 3 4 5 6 7

1 2 3 4 5 6 7

1 2 3 4 5 6 7

1 2 2

3 4 5 6 7 8 9 10

11 12 13 14 15 16 17 18

19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36

37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

55 56 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86

87 88 89 90 91 92 93 94 95 96 97 98 99

1 2 2

3 4 5 6 7 8 9 10

11 12 13 14 15 16 17 18

19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36

37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

55 56 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86

87 88 103 104 105 106 107 108 109 110 111

57 58 59 60 61 62 63 64 65 66 67 68 69 70

89 90 91 92 93 94 95 96 97 98 99 100 101 102

Full Length Periodic Table

Condensed Periodic Table s-block

p-block

d-block

f-block

Color Code Key

1

2 3 4 5 6 7

1 2 3 4 5 6 7

1 2 3 4 5 6 7

1 2 3 4 5 6 7

Example: Nitrogen is in the 3rd column of the p block.It has 3 electrons in the p sublevel

Example: Manganese has 25 electrons. Draw its orbital diagram.

Use Aufbau Principle to determine sublevel and orbital order.

1s

2s

3s

2p

3p

3d4s

Example: Manganese has 25 electrons. Draw its orbital diagram.

1s

2s

3s

2p

3p

3d

4s

Use Pauli Exclusion Principle to place arrows facing the opposite direction in each orbital.

Your Turn: Nickel has 28 electrons. Draw its orbital diagram.

1s

2s

3s

2p

3p

3d4s

• Orbital Notation Practice Website

History of the Periodic Table

More information can be foundin Chapter 6 of your text

1790 –– He was the first to organize the elements.

At the time, only 23 elements were known.

He arranged them into a list.

Distinguished metals from nonmetals.

Antoine Lavoisier

Image by Peter van der Krogt  

Image from Science Shorts

John Newlands• 1864 –– At this time, 70 elements were known. • The list was too unorganized for that many

elements, so he created a table. • He noticed that properties of the elements

repeated every 8 elements when they were arranged by increasing atomic mass.

• He called this observation the Law of Octaves.

• This law was not widely accepted, but it was mostly correct.

Photo from chemsoc

H F ?Li NaBe MgB AlC SiN PO S

octa

vePredict which element will go here.

H F ClLi NaBe MgB AlC SiN PO S

octa

ve

H F ClLi Na ?Be MgB AlC SiN PO S

octa

ve

Predict which element will go here.

H F ClLi Na KBe MgB AlC SiN PO S

octa

veWhat does the Newlands Table have in common with the current periodic table?

H F ClLi Na KBe MgB AlC SiN PO S

octa

veElements with the same number of Valence

electrons are in the same row.

Photo from chemsoc Photo from jergym Czech Republic

Lothar Meyer and Dmitri Mendeleev

They worked on the same type of table, but not together.

Mendeleev published his ideas first, so he usually gets the credit.

In 1869

Lothar Meyer and Dmitri Mendeleev

They arranged the periodic table by atomic mass horizontally rather than vertically.

He Li Be B C N O F

Lothar Meyer and Dmitri Mendeleev

Predict which element will go here.

He Li Be B C N O F

?

Lothar Meyer and Dmitri Mendeleev

He Li Be B C N O F

Ne

He Li Be B C N O F

Ne Na Mg Al Si P S Cl

Ar K Ca Sc Ti Cr Mn

What does the Mendeleev Table have in common with the current periodic table?

He Li Be B C N O F

Ne Na Mg Al Si P S Cl

Ar K Ca Sc Ti Cr Mn

Columns were arranged so that all elements in a column have similar chemical and physical

properties.

What do these three elements have in common?

They are all Noble/ Inert Gases

Lothar Meyer and Dmitri Mendeleev

He Li Be B C N O F

Ne Na Mg Al Si P S Cl

Ar K Ca Sc Ti Cr Mn

They were able to predict the existence of undiscovered elements based on blank spaces

in the periodic table.

Henry Moseley

Moseley observed that

some elements seemed to be in

the wrong column based on

their activity.

Photo from chemsoc

Henry Moseley

Fe55.845

Ni58.693

Co58.933

Cu63.546

Ru101.07

Rh102.906

Pd106.42

Ag107.868

Os190.23

Ir192.217

Pt195.078

Au196.967

For example, Nickel reacts more like Platinum.

26Fe

55.845

28Ni

58.693

27Co

58.933

29Cu

63.54644Ru

101.07

45Rh

102.906

46Pd

106.42

47Ag

107.86876Os

190.23

77Ir

192.217

78Pt

195.078

79Au

196.967

Moseley decided to order the table by Atomic Number rather than atomic mass.

26Fe

55.845

27Co

58.933

28Ni

58.693

29Cu

63.54644Ru

101.07

45Rh

102.906

46Pd

106.42

47Ag

107.86876Os

190.23

77Ir

192.217

78Pt

195.078

79Au

196.967

Moseley decided to order the table by Atomic Number rather than atomic mass.

Glen Seaborg

1940 - synthesized Np and Pu

Decided they must go in a new block of the Periodic table called

Actinides. Seaborg was awarded

a Nobel Prize in 1951.

ReviewWho made the first organized

chart of elements?

Antione Laviosier, list of 23 elements

Review

Who made the first chart in Table form?

John Newlands, based on his Law of Octaves

Review

Lothar Meyer and Dmitri Mendeleev, but they did not work together

Who first organized the table in horizontal rows?

ReviewWho arranged the table the way it is used

today?Henry Moseley, arranged it by atomic number