periodic table1

9.17.00 1:37 PM1 3.3 Periodic Table

The Periodic The Periodic Table Table

and the Elementsand the Elements

Penny SquiresPenny SquiresPisgah High SchoolPisgah High School

20052005


The Periodic Table and the The Periodic Table and the ElementsElements

What is the periodic table ?What is the periodic table ?What information is obtained from the table ?What information is obtained from the table ?How can elemental properties be predicted base on the PT ?How can elemental properties be predicted base on the PT ?


Dmitri MendeleevDmitri Mendeleev (1869)(1869)In 1869 Mendeleev and Lothar Meyer In 1869 Mendeleev and Lothar Meyer (Germany) published nearly identical (Germany) published nearly identical classification schemes for elements known classification schemes for elements known to date. The periodic table is base on the to date. The periodic table is base on the similarity of properties and reactivities similarity of properties and reactivities exhibited by certain elements. Later, Henri exhibited by certain elements. Later, Henri Moseley ( England,1887-1915) established Moseley ( England,1887-1915) established that each elements has a unique atomic that each elements has a unique atomic number, which is how the current periodic number, which is how the current periodic table is organized.table is organized.

http://www.chem.msu.su/eng/misc/mendeleev/welcome.html


Periodic LawPeriodic Law

The Periodic Law states that when elements are arranged in order of

increasing atomic number their physical and chemical properties show a periodic

pattern.


The Periodic TableThe Periodic TableA map of the building block of matter.

1IA

18VIIIA

11H

1.00797

2IIA

Periodic Table 13IIIA

14IVA

15VA

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 109http://www.chemsoc.org/viselements/pages/periodic_table.html


ArrangementArrangement

The modern Periodic Table is arranged according to atomic number.

Remember that it is the atomic number, or nuclear charge, that determines

the identity of the element.


Periodic Table Expanded Periodic Table Expanded ViewView

The way the periodic table usually The way the periodic table usually seen is a compress view, placing seen is a compress view, placing the Lanthanides and actinides at the Lanthanides and actinides at

the bottom of the stable.the bottom of the stable.


Periodic Table: Periodic Table: Metallic Metallic arrangementarrangement

Layout of the Periodic Table: Metals vs. nonmetals

1IA

18VIIIA

12

IIA13

IIIA14

IVA15VA

16VIA

17VIIA

2

33

IIIB4

IVB5

VB6

VIB7

VIIB8 9

VIIIB10 11

IB12IIB

4

5

6

7

MetalsMetalsNonmetalsNonmetals


METALSMETALS

Hard and Shiny

3 or less valence electrons

Form + ions by losing e-

Good conductors of heat and electricity


NONMETALSNONMETALS

Gases or dull, brittle solids

5 or more valence electrons

Form - ions by gaining e-

Poor conductors of heat and electricity


MetalloidsMetalloids

Appearence will vary

3 to 7 valence electrons

Form + and/or - ions

Conduct better than nonmetals but not as well as metals


Periodic Table: The three broad Periodic Table: The three broad ClassesClasses

Main, Transition, Rare EarthMain, Transition, Rare EarthMain (Representative), Transition metals, lanthanides and actinides (rare earth)


Reading the Periodic Table: Reading the Periodic Table: ClassificationClassification

Nonmetals, Metals, Metalloids, Noble gases


Across the Periodic Across the Periodic TableTable

Periods:Periods: Are arranged horizontally across the Are arranged horizontally across the periodic table (rows 1-7)periodic table (rows 1-7)

These elements have the same number of valence shells.These elements have the same number of valence shells.1

IA18

VIIIA

12

IIA13

IIIA14

IVA15VA

16VIA

17VIIA

2

33

IIIB4

IVB5

VB6

VIB7

VIIB8 9

VIIIB10 11

IB12IIB

4

5

6

7

2nd Period

6th Period


3

p block s block

d block

f block


Down the Periodic Down the Periodic TableTable

Family:Family: Are arranged vertically down the periodic table Are arranged vertically down the periodic table (columns or (columns or group, 1- 18 or 1-8 A,B)group, 1- 18 or 1-8 A,B)These elements have the same number electrons in the outer most shells, the valence These elements have the same number electrons in the outer most shells, the valence shell.shell.

1IA

18VIIIA

12

IIA13

IIIA14

IVA15VA

16VIA

17VIIA

2

33

IIIB4

IVB5

VB6

VIB7

VIIB8 9

VIIIB10 11

IB12IIB

4

5

6

7

Alkali Family: 1 e- in the valence shell

Alkali Family: 1 e- in the valence shell

Halogen Family: 7 e- in the valence shell

Halogen Family: 7 e- in the valence shell


Infamous Families of the Periodic Infamous Families of the Periodic TableTable

Notable families of the Periodic Table and some important members:

1IA

18VIIIA

12

IIA13

IIIA14

IVA15VA

16VIA

17VIIA

2

33

IIIB4

IVB5

VB6

VIB7

VIIB8 9

VIIIB10 11

IB12IIB

4

5

6

7

Alkali

Alkaline (earth)

Transition MetalsTransition Metals

Noble GasNoble GasHalogenHalogen

ChalcogensChalcogens


Hydrogen:Hydrogen:

A Unique Element 1s1 Shown Over Group 1A & 7A

Hydrogen is neither an alkali metal nor a halogen

However, hydrogen does show reactions that are similar to both alkali metals and halogens

H . + . Cl : H : Cl :

H . + e- H : - or H - called hydride

Hydrogen can also gain an electron to form an ion with a 1- charge


Group 1A: Alkali MetalsGroup 1A: Alkali MetalsReact with water easily to lose a valence electron.

Form a +1 ion

Soft

Found in nature combined with other elements

Good conductors of heat and electricity


Group 2A: Alkaline Earth Group 2A: Alkaline Earth MetalsMetals

Forms compounds with Oxygen (Oxides)

React with water

Shiny solids that are heavier than Alkalis

React with Oxygen or other metals found in the earth

Lose valance electrons to form +2 ions

Ca (g) Ca+ (g) + e-

Ca+ (g) Ca2+ (g) + e-

First Ionization Step

Second Ionization Step


Group 3A: Boron GroupGroup 3A: Boron GroupAlways found combined with other elements in nature.

Found as oxides in the earth’s crust.

B, Al, Ga, and In form +3 ions

Tl only forms a +1 ion


Group 4A: Carbon GroupGroup 4A: Carbon Group

Few rules apply to this group!!!!


Group 5A: Nitrogen GroupGroup 5A: Nitrogen GroupWide variety of Chemical and Physical properties.

N forms a –3 ion

Bi forms a +3 ion


Group 6A: Oxygen Group or Group 6A: Oxygen Group or ChalcogensChalcogens

Act like nonmetals

Tend to gain 2 e- to form –2 ions.

Can also share 2 e-


Group 7A: HalogensGroup 7A: HalogensForm compounds with almost all metals

Salts (NaCl)

Have different Physical properties

Very reactive and found combined in nature

Tend to share or gain 1 e- to form a –1 ion


Group 8A: Noble GasesGroup 8A: Noble Gases

•Colorless

•Unreactive

•Last to be discovered

•Rarely react (1st time was in a lab in 1962)


Transition MetalsTransition Metals1. Lanthanides –

Named because they follow lanthanumSilvery metals with high melting pointsFound mixed in nature – very hard to seperate

2. Actinide – Named because they follow actinium

Radioactive elementsOnly 3 exist in nature – the rest are synthetic


Transition Metals (cont.)Transition Metals (cont.)Share conductivity, luster and malleability with other metals.

Close in atomic size, electronegativity and ionization energy

Different physical properties (determined by their electron configuration)

Can lose 2 e- to form +2 ion or 3 to form a +3 ion


Periodic TablePeriodic Table ee-- configuration from the periodic configuration from the periodic

periodic tableperiodic table

B2p1

1IA

18VIIIA

12

IIA13

IIIA14

IVA15VA

16VIA

17VIIA

2

33

IIIB4

IVB5

VB6

VIB7

VIIB8 9

VIIIB10 11

IB12IIB

4

5

6

7

H1s1

Li2s1

Na3s1

K4s1

Rb5s1

Cs6s1

Fr7s1

Be2s2

Mg3s2

Ca4s2

Sr5s2

Ba6s2

Ra7s2

Sc3d1

Ti3d2

V3d3

Cr4s13d5

Mn3d5

Fe3d6

Co3d7

Ni3d8

Zn3d10

Cu4s13d10

B2p1

C2p2

N2p3

O2p4

F2p5

Ne2p6

He1s2

Al3p1

Ga4p1

In5p1

Tl6p1

Si3p2

Ge4p2

Sn5p2

Pb6p2

P3p3

As4p3

Sb5p3

Bi6p3

S3p4

Se4p4

Te5p4

Po6p4

Cl3p5

Be4p5

I5p5

At6p5

Ar3p6

Kr4p6

Xe5p6

Rn6p6

Y4d1

La5d1

Ac6d1

Cd4d10

Hg5d10

Ag5s14d10

Au6s15d10

Zr4d2

Hf5d2

Rf6d2

Nb4d3

Ta5d3

Db6d3

Mo5s14d5

W6s15d5

Sg7s16d5

Tc4d5

Re5d5

Bh6d5

Ru4d6

Os5d6

Hs6d6

Rh4d7

Ir5d7

Mt6d7

Ni4d8

Ni5d8


Periodic Table: electron Periodic Table: electron behaviorbehaviorThe periodic table can be classified by the behavior of their electrons

1IA

18VIIIA

12

IIA13

IIIA14

IVA15VA

16VIA

17VIIA

2

33

IIIB4

IVB5

VB6

VIB7

VIIB8 9

VIIIB10 11

IB12IIB

4

5

6

7

West (South) Mid-plains East (North)METALS

AlkaliAlkaline

Transition

METALLOID NON-METALSNoble gasHalogensCalcogens

These elementstend to give up

e- and formCATIONS

These elementswill give up e- or

accept e-

These elementstend to accept

e- and formANIONS


2. Trend in 2. Trend in Atomic RadiusAtomic RadiusAtomic Radius: Atomic Radius:

The size of at atomic specie as determine by the boundaries of the valence e-. Largest atomic species are those found in the SW corner since these atoms have the largest n, but the smallest Zeff.


3. Trend in 3. Trend in Ionization Ionization PotentialPotential

Ionization potential: Ionization potential:

The energy required to remove the valence electron from an atomic specie. Largest toward NE corner of PT since these atoms hold on to their valence e- the tightest.


4. Trend in 4. Trend in Electron AffinityElectron Affinity

Electron Affinity: Electron Affinity:

The energy release when an electron is added to an atom. Most favorable toward NE corner of PT since these atoms have a great affinity for e-.


Summary of TrendSummary of TrendPeriodic Table and Periodic Trends1. Electron Configuration

2. Atomic Radius: Largest toward SW corner of PT2. Atomic Radius: Largest toward SW corner of PT

3. Ionization Energy: Largest toward NE of PT3. Ionization Energy: Largest toward NE of PT4. Electron Affinity: Most favorable NE of PT4. Electron Affinity: Most favorable NE of PT


SummarySummary

Periodic TablePeriodic Table: Map of the Building block of matter

TypeType: Metal, metalloid and NonmetalGroupings: Representative or main, transition and Lanthanide/Actanides

FamilyFamily: Elements in the same column have similar chemical property because of similar valence electronsAlkali, Alkaline, chalcogens, halogens, noble gases

PeriodPeriod:: Elements in the same row have valence electrons in the same shell.

periodic table1

Education

periodic table9

periodic table family

current periodic table

periodic table isbase

periodic table periods

periodic tableand

periodic tablecolumns

theperiodic table rows