Periodic table of elements - DEOS / ДЕОС

Periodic table of elements

Periodic Table The periodic table organizes the elements in a particular

way. A great deal of information about an element can begathered from its position in the period table.

For example, you can predict with reasonably goodaccuracy the physical and chemical properties of theelement. You can also predict what other elements aparticular element will react with chemically.

Understanding the organization and plan of the periodictable will help you obtain basic information about each ofthe 118 known elements.

Dmitri Mendeleev (1869)In 1869 Mendeleev and Lothar Meyer

(Germany) published nearly identicalclassification schemes for elements known todate. The periodic table is based on thesimilarity of properties and reactivitiesexhibited by certain elements. Later, HenriMoseley ( England, 1887-1915) established thateach elements has a unique atomic number,which is how the current periodic table isorganized.

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Key to the Periodic Table

Elements are organized on thetable according to their atomicnumber, usually found near thetop of the square. The atomic number refers to

how many protons an atom ofthat element has.

For instance, hydrogen has 1proton, so it’s atomic numberis 1.

The atomic number is uniqueto that element. No twoelements have the sameatomic number.

What’s in a square?

Different periodic tables can include various bits of information, but usually: atomic number symbol atomic mass number of valence

electrons state of matter at room

temperature.

The Periodic Table A map of the building block of matter.

1IA

18VIIIA

11H

1.00797

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

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Periodic Table Expanded ViewThe way the periodic table usually seen is a compress view, placing theLanthanides and actinides at the bottom of the stable.The Periodic Table can be arrange by subshells. The s-block is Group IA andIIA, the p-block is Group IIIA - VIIIA. The d-block is the transition metals,and the f-block are the Lanthanides and Actinide metals

Periodic Table: The three broad ClassesMain, Transition, Rare Earth

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

Reading the Periodic Table: Classification Nonmetals, Metals,

Metalloids, Noble gases

Across the Periodic Table Periods: Are arranged horizontally across the periodic table (rows 1-7) These elements have the same number of valence shells.

1IA

18VIIIA

1 2IIA

13IIIA

14IVA

15VA

16VIA

17VIIA

2

3 3IIIB

4IVB

5VB

6VIB

7VIIB

8 9VIIIB

10 11IB

12IIB

4

5

6

7

2nd Period

6th Period

Each horizontal row of elements is called a period. The elements in a period are not alike in properties. In fact, the properties change greatly across even given

row. The first element in a period is always an extremely active

solid. The last element in a period, is always an inactivegas.

Periods

Reading the Periodic Table: Categorization

Down the Periodic TableFamily: Are arranged vertically down the periodic table (columns orgroup, 1- 18 or 1-8 A,B)These elements have the same number of electrons in the outer mostshells, the valence shell.

1IA

18VIIIA

1 2IIA

13IIIA

14IVA

15VA

16VIA

17VIIA

2

3 3IIIB

4IVB

5VB

6VIB

7VIIB

8 9VIIIB

10 11IB

12IIB

4

5

6

7

Alkali Family: 1 e- in the valence shell

Halogen Family: 7 e- in the valence shell

Families Columns of elements are called groups or families. Elements in each family have similar but not identical

properties. For example, lithium (Li), sodium (Na), potassium (K),

and other members of family IA are all soft, white,shiny metals.

All elements in a family have the same number ofvalence electrons.

Reading the Periodic Table: Categorization

Period #energy level (subtract for d & f)

A/B Group # total # of valence e-

Column within sublevel block# of e- in sublevel

Reading the Periodic Table: Periodic Patterns

s-block1st Period

1s1 1st column of s-block

1 2 3 4 5 6 7

Periodic Patterns Example - Hydrogen

Periodic Tablee- configuration from the periodic table

B2p1

1IA

18VIIIA

1 2IIA

13IIIA

14IVA

15VA

16VIA

17VIIA

2

3 3IIIB

4IVB

5VB

6VIB

7VIIB

8 9VIIIB

10 11IB

12IIB

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 behavior The periodic table can be classified by the behavior of their electrons

1IA

18VIIIA

1 2IIA

13IIIA

14IVA

15VA

16VIA

17VIIA

2

3 3IIIB

4IVB

5VB

6VIB

7VIIB

8 9VIIIB

10 11IB

12IIB

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

Metals

Alkali Metals

They are the most reactivemetals.

They react violently with water.

Alkali metals are never found asfree elements in nature. Theyare always bonded with anotherelement.

Alkaline Earth Metals

They are never found uncombined in nature. They have two valence electrons. Alkaline earth metals include magnesium and

calcium, among others.

Properties of Metalloids

Metalloids (metal-like) haveproperties of both metalsand non-metals.

They are solids that can beshiny or dull.

They conduct heat andelectricity better than non-metals but not as well asmetals.

They are ductile andmalleable.

Silicon

Transition Metals

Transition Elements include those elements in the Bfamilies.

These are the metals you are probably most familiar:copper, tin, zinc, iron, nickel, gold, and silver.

They are good conductors of heat and electricity.

Transition Elements

Transition elements have propertiessimilar to one another and to othermetals, but their properties do not fitin with those of any other family.

Many transition metals combinechemically with oxygen to formcompounds called oxides.

Boron Family

The Boron Family is namedafter the first element inthe family.

Atoms in this family have 3valence electrons.

This family includes ametalloid (boron), and therest are metals.

This family includes themost abundant metal in theearth’s crust (aluminum).

Properties of Non-Metals

Non-metals are poorconductors of heat andelectricity.

Non-metals are notductile or malleable.

Solid non-metals arebrittle and break easily.

They are dull. Many non-metals are

gases.Sulfur

Carbon Family

Atoms of this family have4 valence electrons.

This family includes anon-metal (carbon),metalloids, and metals.

The element carbon iscalled the “basis of life.”There is an entire branchof chemistry devoted tocarbon compounds calledorganic chemistry.

Oxygen Family

Atoms of this family have 6valence electrons.

Most elements in this familyshare electrons whenforming compounds.

Oxygen is the most abundantelement in the earth’s crust.It is extremely active andcombines with almost allelements.

Halogen Family

The elements in thisfamily are fluorine,chlorine, bromine,iodine, and astatine.

Halogens have 7 valenceelectrons, whichexplains why they arethe most active non-metals. They are neverfound free in nature.

Halogen atoms only need togain 1 electron to fill theiroutermost energy level.They react with alkalimetals to form salts.

Noble Gases

Noble Gases are colorless gases that are extremelyun-reactive.

One important property of the noble gases is theirinactivity. They are inactive because their outermostenergy level is full.

Because they do not readily combine with otherelements to form compounds, the noble gases arecalled inert.

The family of noble gases includes helium, neon,argon, krypton, xenon, and radon.

All the noble gases are found in small amounts in theearth's atmosphere.

Rare Earth Elements

The thirty rare earth elements are composed of thelanthanide and actinide series.

One element of the lanthanide series and most of theelements in the actinide series are called trans-uranium,which means synthetic or man-made.

Periodic TrendsElectronegativity – a chemical property describing an atom's ability toattract and bind with electrons.Atomic Radius - a term used to describe the size of the atom. Thereis no standard definition for this value - it may refer to the ionicradius, covalent radius, metallic radius, or van der Waals radius.Ionization potential (ionization energy (Ei)) - is qualitatively definedas the minimum amount of energy required to remove the most looselybound electron, the valence electron, of an isolated neutral gaseousatom to form a cation.Electron Affinity - the electron affinity (Eea) of an atom or moleculeis defined as the amount of energy released or spent when an electronis added to a neutral atom or molecule in the gaseous state to form anegative ion.Melting Point - the amount of energy required to break a bond(s) tochange the solid phase of a substance to a liquid.

1. Trend in Electronegativity From left to right across a period of elements, electronegativity

increases. From top to bottom down a group, electronegativity decreases. Important exceptions of the above rules include the noble gases,

lanthanides, and actinides. As for the transition metals, although they have

electronegativity values, there is little variance among them acrossthe period and up and down a group.

2. Trend in Atomic RadiusAtomic Radius: The size of an atomic specie as determined by the boundaries ofthe valence e-. Largest atomic species are those found in the SWcorner since these atoms have the largest n, but the smallest Zeff.

Presenter

Presentation Notes

No matter what criteria you use to describe the atomic radius, the size of the atom is dependent on how far out the electrons extend. The atomic radius of an element tends to increase as one goes down an element group. The reason is that the electrons become more tightly packed as you move across the periodic table, so while there are more electrons for elements of increasing atomic number, the atomic radius actually may decrease. The atomic radius moving down an element period or column tends to increase because an additional electron shell is added for each new row. In general, the largest atoms are at the bottom left side of the periodic table.

3. Trend in Ionization PotentialIonization potential:

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

4. Trend in Electron Affinity

Electron Affinity:

The energy releasewhen an electron isadded to an atom.Most favorable towardNE corner of PT sincethese atoms have agreat affinity for e-.

Presenter

Presentation Notes

Although Eea varies greatly across the periodic table, some patterns emerge. Generally, nonmetals have more positive Eea than metals. Atoms whose anions are more stable than neutral atoms have a greater Eea. Chlorine most strongly attracts extra electrons; mercury most weakly attracts an extra electron. The electron affinities of the noble gases have not been conclusively measured, so they may or may not have slightly negative values. Eea generally increases across a period (row) in the periodic table prior to reaching group 18. This is caused by the filling of the valence shell of the atom; a group 17 atom releases more energy than a group 1 atom on gaining an electron because it obtains a filled valence shell and therefore is more stable. In group 18, the valence shell is full, meaning that added electrons are unstable, tending to be ejected very quickly. Counterintuitively, Eea does not decrease when progressing down the rows of the periodic table, as can be clearly seen in the group 2 data. Thus, electron affinity follows the same "left-right" trend as electronegativity, but not the "up-down" trend.

5. Trend in Melting point

Melting points are varied and do not generally form adistinguishable trend across the periodic table. However,certain conclusions can be drawn from the graph below.Metals generally possess a high melting point.Most non-metals possess low melting points. The non-metal carbon possesses the highest boiling

point of all the elements. The semi-metal boron alsopossesses a high melting point.

Summary of Trend Periodic Table and Periodic Trends

Atomic Radius: Largest toward SW corner of PT

Ionization Energy: Largest toward NE of PTElectron Affinity: Most favorable NE of PT

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Periodic table of elements - DEOS / ДЕОС