Section 1 – History of the Periodic Table

Objectives:1. Explore the scientific theory of atoms (also known as the atomic

theory) by describing changes in the atomic model over time and why those changes were necessary based on new evidence.

2. Become familiar with the scientists that helped these changes come about.

3. Explore the differences between modern periodic table and the historic periodic tables.

• By 1860, more than 60 elements had been discovered.

• Chemists had a hard time determining properties of the elements and compounds that the elements formed.

• They also had no accurate way to determine

atomic mass or the number of atoms that made up an element, so each scientist used a different atomic mass – making it nearly impossible for one chemist to understand the results of another.

• In 1860, chemists assembled at the First International Congress of Chemists in Germany to settle the issue of atomic mass.

• Russian chemist Dmitri Mendeleev included the new values from the conference in a chemistry textbook that he was writing.

• He hoped to organize the elements according to their properties.

• He did this by placing the elements on cards and arranged them according to atomic mass and properties, looking for trends.

• He noticed that when the elements were arranged by increasing atomic mass, similarities in the chemical properties appeared at regular intervals – these patterns are periodic.

Mendeleev and Chemical Periodicity:

List 3 examples of phenomena that occur periodically:

1.

2.

3.

Brainstorming:

List 3 examples of phenomena that occur periodically:

1. Phases of the moon

2. Magazine Publications (monthly)

3. Tides (high tide & low tide)

**Keep these examples in mind as we cover the arrangement of the elements on the

periodic table**

Brainstorming:

• Mendeleev created a table in which the elements were grouped together by similar properties – a periodic table of elements.

• This table was published in 1869 and the properties were similar as you read horizontally across the table.

• This procedure left many empty spaces, but he predicted that elements would be discovered and would fill those places - all three were discovered by 1886.

Mendeleev and Chemical Periodicity Cont.:

• Moseley was working with 38 different metals and discovered a pattern that was had not been recognized – elements fit better when they were arranged by increasing nuclear charge (# of protons in nucleus)

• Moseley’s work led to:a. Modern definition of atomic number b. Recognition that atomic number – NOT atomic

mass – is basis for organization of periodic table

• Periodic Law – the physical and chemical properties of the elements are periodic functions of their atomic numbers (# of protons).

Moseley and the Periodic Law:

P

Zn As

Sb

Pt Bi

Midd. -1700

Cr Mn

Li

K

N O F

Na

BBe

H

Al Si Cl

Ca Ti V Co Ni Se Br

Sr Y Zr Nb Mo Rh Pd Cd Te I

Ba Ta W Os Ir

Mg

Ce Tb Er

Th U

1735-1843

Discovering the Periodic Table

C

S

Fe Cu

Ag Sn

Au Hg Pb

Ancient Times

He

Sc Ga Ge

Rb Ru In

Cs Tl

Pr Nd Sm Gd Dy Ho Tm Yb

La

1843-1886 Ne

Ar

Kr

Xe

Po Rn

Ra

Eu Lu

Pa

Ac

1894-1918

Tc

Hf Re At

Fr

Pm

Np Pu Am Cm Bk Cf Es Fm Md No Lr

1923-1961

Rf Db Sg Bh Hs Mt

1965-

Journal of Chemical Education, Sept. 1989

Lr103

No102

Md101

Fm100

Es99

Cf98

Bk97

Cm96

Am95

Pu94

Np93

U92

Pa91

Th90

Lu71

Tm69

Yb70

Er68

Ho67

Dy66

Tb65

Gd64

Eu63

Sm62

Pm61

Nd60

Pr59

Ce58

He2

Ne10

Ar18

Kr36

Xe54

Rn86

At85

I53

Br35

Cl17

F9

Po84

Te52

Se34

O8

Bi83

Sb51

As33

N7

Pb82

Tc43

Ta73

Hg80

Mt109

Hs108

Bh107

Sg106

Db105

Rf104

Ac89

La57

Hf72

W74

Re75

Os76

Ir77

Rh45

Ru44

Mo42

Nb41

V23

Li3

Fr87

Cs55

H 1

Na11

K19

Rb37

Mn25

Co27

Pd46

Au79

Cd48

Zn30

Cu29

C6

B5

Al13

S16

P15

Si14

Ge32

Sn50

Ag47

Pt78

Fe26

Ni28

Cr24

Ti22

Sc21

Zr41

Y39

Ga31

In49

Tl81

Mg12

Ca20

Sr38

Ba56

Ra88

Be4

Other Physical DATA

Periodic table – an arrangement of the elements in order of their atomic number so that elements with similar properties fall in the same column or group.

The Noble Gases - 1894• Noble gases were the most significant addition to

the periodic table.

• John William Strutt and Sir William Ramsay discovered Argon – a gas in the atmosphere that had not been noticed because it is unreactive – and Helium – a component of the sun.

• Ramsey added a new group to the table to fit these gases.

The Modern Periodic Table

Lanthanides/ Actinides – early 1900s

• These are the 14 elements with atomic number from 58 to 71 (lanthanides) and 90 to 103 (actinides) that have very similar properties.

• They are placed below the table to save space

Dutch Periodic Table

106107

108

109

110

111

112

113

114

115116

117 118

Strong, Journal of Chemical Education, Sept. 1989, page 743

Chinese Periodic Table

http://www.limestone.on.ca/ibuild/davies/chinesept.html

Stowe’s Periodic Table

Benfrey’s Periodic Table

developed by Mohd Abubakr, Hyderabad, India

Misconceptions:

- Something does not have to very uniformly to be periodic. It just has to have a similar pattern.

- As you read through the articles, make sure you are aware that changes have been made - the periodic table has been modified to fit new evidence.

Group assignments:• Individually read the two articles that you have

been given.

• Once you have read the articles, please discuss them with your group members and create two charts on your bell ringer paper :

1. Venn Diagram:• Compare historic periodic tables vs. the

Modern Periodic table • The overlap will represent what has

stayed the same.2. Concept Map:

• Periodic Table is your Heading • Relate it to:

• The scientists involved • Problems/predictions that occurred • Changes made over time

Groups for Assignment:Group 11. Anna Ashley2. Bobby Beeton3. Kaylee Madere

Group 21. Kellie Fahy2. Rachel Loughney3. Nicholas White

Group 3:1. Joey Winston 2. Madeline Mulder3. Sierra Lloyd

Group 41. Zach Jowers2. Matthew Holt3. Chanteria Hamm

Group 5

1. Moriah Fobbs 2. Cody Frizzelle3. Garret Siegel

Group 6 1. Noah Mobley2. Edin McKuhen3. Jonah Hooton

Group 71. Zachary Bradley 2. Sean Chancellor3. Victoria Worley

Group 81. Spencer Carr2. Brandon Castelin3. Alex Hill4. Nancy Tanner

Section 2 – Electron Configuration and the Periodic

Table Objectives:1. Relate the properties of atoms and their position in the

periodic table to the arrangement of their electrons. 2. The student will organize information to show understanding

or relationships among facts, ideas, and events (representing key points within text through charting, mapping, paraphrasing, summarizing, comparing, contrasting, or outlining)

Groups of Elements1

2

3

4

5

6

7

*

W

W

*

Li

3

He

2

C

6

N

7

O

8

F

9

Ne

10

Na

11

B

5

Be

4

H

1

Al

13

Si

14

P

15

S

16

Cl

17

Ar

18

K

19

Ca

20

Sc

21

Ti

22

V

23

Cr

24

Mn

25

Fe

26

Co

27

Ni

28

Cu

29

Zn

30

Ga

31

Ge

32

As

33

Se

34

Br

35

Kr

36

Rb

37

Sr

38

Y

39

Zr

40

Nb

41

Mo

42

Tc

43

Ru

44

Rh

45

Pd

46

Ag

47

Cd

48

In

49

Sn

50

Sb

51

Te

52

I

53

Xe

54

Cs

55

Ba

56

Hf

72

Ta

73

W

74

Re

75

Os

76

Ir

77

Pt

78

Au

79

Hg

80

Tl

81

Pb

82

Bi

83

Po

84

At

85

Rn

86

Fr

87

Ra

88

Rf

104

Db

105

Sg

106

Bh

107

Hs

108

Mt

109

Mg

12

Ce

58

Pr

59

Nd

60

Pm

61

Sm

62

Eu

63

Gd

64

Tb

65

Dy

66

Ho

67

Er

68

Tm

69

Yb

70

Lu

71

Th

90

Pa

91

U

92

Np

93

Pu

94

Am

95

Cm

96

Bk

97

Cf

98

Es

99

Fm

100

Md

101

No

102

Lr

103

La

57

Ac

89

1

2

3

4

5

6

7

*

W

1A

2A

1A

2A

3A

4A

5A

6A

7A

8A

Alkali metals

Alkaline earth metals

Transition metals

Inner transition metals

Boron group

Carbon group

Nitrogen group

Oxygen group

Halogens

Noble gases

Hydrogen

3B 5B 6B 7B 8B 1B 2B

3A 4A 5A 6A 7A

8A

4B

Rn

86

Xe

54

Kr

36

Ar

18

Ne

10

He

2

Mt

109

Hs

108

Bh

107

Sg

106

Rf

104

Db

105

Hg

80

Au

79

Pt

78

Ir

77

Os

76

Re

75

W

74

Ta

73

Hf

72

Cd

48

Ag

47

Pd

46

Rh

45

Ru

44

Tc

43

Mo

42

Nb

41

B

5

Zr

40

Y

39

Zn

30

Cu

29

Co

27

Ni

28

Fe

26

Mn

25

Cr

24

V

23

Ti

22

Sc

21

Ac

89

Th

90

Pa

91

U

92

Np

93

Pu

94

Am

95

Cm

96

Bk

97

Cf

98

Es

99

Fm

100

Md

101

No

102

Lr

103

O

8

S

16

Se

34

Te

52

As

33

P

15

N

7

Sb

51

Bi

83

Po

84

Groups of Elements1

2

3

4

5

6

7

*

W

W

*

Li

3

C

6

F

9

Na

11

Be

4

H

1

Al

13

Si

14

Cl

17

K

19

Ca

20

Ga

31

Ge

32

Br

35

Rb

37

Sr

38

In

49

Sn

50

I

53

Cs

55

Ba

56

Tl

81

Pb

82

At

85

Fr

87

Ra

88

Mg

12

Ce

58

Pr

59

Nd

60

Pm

61

Sm

62

Eu

63

Gd

64

Tb

65

Dy

66

Ho

67

Er

68

Tm

69

Yb

70

Lu

71

La

57

1

2

3

4

5

6

7

*

W

Alkali metals

Alkaline earth metals

Transition metals

Other metals

Lanthanides

HalogensOther non-metals

Noble gases Actinides

1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17IA IIA IIIB IVB VB VIB VIIB VIIIB IB IIB IIIA IVA VA VIA VIIA VIIIA

18