The Periodic

TableHETINY MUTHIA RAHMY

3315110318

Chemistry Education 2011Faculty of Mathematic and Sciences

• The periodic table organizes the elements in a particular way.

• A great deal of information about an element can be gathered from its position in the periodic table.1

IA18

VIIIA

11

H1.00797

2IIA Periodic Table 13

IIIA14

IVA15VA

16VIA

17VIIA

2He

4.0026

23

Li6.939

4Be

9.0122

5B

10.811

6C

12.0112

7N

14.0067

8O

15.9994

9F

18.9984

10Ne

20.179

311

Na22.9898

12Mg24.305

3IIIB

4IVB

5VB

6VIB

7VIIB

8 9VIIIB

10 11IB

12IIB

13Al

26.9815

14Si

28.086

15P

30.9738

16S

32.064

17Cl

35.453

18Ar

39.948

419K

39.102

20Ca40.08

21Sc

44.956

22Ti

47.90

23V

50.942

24Cr

51.996

25Mn

54.9380

26Fe

55.847

27Co

58.9332

28Ni58.71

29Cu63.54

30Zn65.37

31Ga65.37

32Ge72.59

33As

74.9216

34Se78.96

35Br

79.909

36Kr83.80

537

Rb85.47

38Sr87.62

39Y

88.905

40Zr91.22

41Nb

92.906

42Mo95.94

43Tc[99]

44Ru

101.07

45Rh

102.905

46Pd106.4

47Ag

107.870

48Cd

112.40

49In

114.82

50Sn

118.69

51Sb

121.75

52Te

127.60

53I

126.904

54Xe

131.30

655Cs

132.905

56Ba

137.34

57La

138.91

72Hf

178.49

73Ta

180.948

74W

183.85

75Re186.2

76Os190.2

77Ir

192.2

78Pt

195.09

79Au

196.967

80Hg200.59

81Tl

204.37

82Pb

207.19

83Bi

208.980

84Po[210]

85At[210]

86Rn[222]

787Fr[223]

88Ra[226]

89Ac[227]

104Ku[260]

105 106 107 108 109

The

Perio

dic

Tabl

e

Properties of the Elements

Metallic Character

Groups and Periods

Check the Electron

ConfigurationPeriodic Trends

How do you read the PERIODIC TABLE?

Properties of Element

• the number of protons found in the nucleus of an atom of that particular element

Atomic Number

• made up of only one capital letter and, in some cases, one or more lowercase letters

Elemental

Symbol• Average of relative

atomic mass from 1/12 of atomic mass Carbon-12

Atomic Mass

Metallic Character

Metals• elements with relatively few valence

electrons, which tend to form positive ions by losing one or more electrons

Non-metals

• elements that have more valence electrons ad tend to form negative ions by gaining one or more electrons

Semimetals

(Metalloids)

• tend to have some characteristics of metals and some of nonmetals

Properties of Metals• Good conductors of heat

and electricity.• Metals are shiny.• Ductile (can be stretched

into thin wires).• Malleable (can be pounded

into thin sheets).• A chemical property of

metal is its reaction with water which results in corrosion.

Properties of Non-Metals• Poor conductors of

heat and electricity.• Non-metals are not

ductile or malleable.• Solid non-metals are

brittle and break easily.

• Many non-metals are gases.

Sulfur

Properties of Metalloids• Metalloids (metal-like) have

properties of both metals and non-metals.

• They are solids that can be shiny or dull.

• They conduct heat and electricity better than non-metals but not as well as metals.

• They are ductile and malleable.Silicon

Groups

• The columns of elements with similar properties

Group IA Alkali Metals

Group IIA Alkaline Earth Metals

Group VIIA Halogens

Group VIIIA Noble Gases

Group IB until VIIIB Transition Metals

Special Group Names

Periods

• Each row (or period) is the energy level for s and p orbitals.

1

2

3

4

5

6

7

Period Number

Check the Electron Configuration

The “s” sublevelels hold 2 electronsthe “s” section is made up of 2 columnsThe “p” sublevels hold 6 electrons

the “p” section is made up of 6 columnsThe “d” sublevels hold up to 10 electrons

the “d” section is made up of 10 columnsThe “f” sublevels hold up to 14 electrons

The “f” section is made up of 14 columns

lanthanides

actinides

‘s’-groups ‘p’-groups

d-transition elements

f-transition elements

• For example, Rubidium (Rb) is in the fifth period and in the first column of the “s” section of the periodic table. • This tell us that the valence configuration of

rubidium must end in 5s1. • When we construct the full electron

configuration of rubidium, with its 37 electrons, we get 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1.

• Atomic Radius or atomic size is the distance from center of the nucleus to the outermost shell of an atom

Atomic Radius

• The energy required to remove an electron from an atom. (measured in kilojoules, kJ)

Ionization Energy

Periodic Trends

Atomic Sizes for Groups &Periods

Electron Affinity

• Electron affinity is the energy release when an atom gains an electron (also measured in kJ)

Electro-negativity

•Electronegativity is preference of atom to gain electron

Summary of Periodic Trends

Thanks for your attention