2 Periodic Table 21 01 09 [Kompatibilitätsmodus]neutron/download/lehre/chemistry/old... · 2.4.1.1 Pauli‘s Rule • Within one atom electrons can not be equal in all 4 quantum

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Periodic TablePeriodic TableProf. Dr. Sabine Prys

21/01/2009 1@designed by ps

1.0 Element Abundance

466 000OEl t i th E th t i / t 277 20081 30050 00036 30028 30025 90020 900

Si Al Fe Ca Na K Mg

Elements in the Earth crust in g / t

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20 9004 4001 4001 1801 000

700520

Mg Ti H P Mn F S

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1.1 Earth's Interior

Crust 50 km

Mantle 642 kmMg, Fe, Al, Si, O (plastic)Core 2200 km

0 ºC

1000 ºC

3700 ºC

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Fe, Ni (liquid)Inner Core 3486 kmFe (solid)4300 ºC

r= 6 378 km

1.2 Matter

Matter is commonly defined as being anything that has mass and that takes up space

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3

1.3 Materials

phase: different aggregations of mattersolid – liquid - gaseous

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homogeneous materials: one phase

heterogeneous materials: more than one phase

1.4 Compounds

Chemical compound

A compound is a group of atoms with an exact number and type of atoms in it, arranged in a specific

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way, characterized by a specific melting or boiling point.

e.g. quartz crystal

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1.5 Aggregation of Matter

Bose-Einstein-Continuum

solid

solid

liquid

gaseous

melting

freezing

subliming

resubliming

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liquid

gaseous

gaseous

plasmatic

vaporizing

condensing

Ionising

recombining

1.6 Chemical Elements

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A chemical element is a fundamental substance that cannot be further refined or subdivided by chemical means. All atoms of a chemical element have the same number of protons.

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2.0 Atomic Theory

until 1887: atoms = billiard balls1886 E. Goldstein discovered positive charges within the atom1887 J.J. Thomson discovered the electron when using cathode ray tubes

THOMSONs raisin bread theory of atoms

1908 E. Rutherford interpretated his gold foil experiments by assuming a positively charged centre und negative charged surrounding electrons

RUTHERFORD’s model

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1913 Bohr postulated his model of defined electron shells1932 J. Chadwick discovered the neutron

Bohr’s Modelhttp://www.visionlearning.com/library/module_viewer.php?mid=50

2.1 BOHR‘s Atomic Theory

φ = 10-7 - 10-10 m

Nucleus:Protons (+)Neutrons (n)

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Electron Orbits:Electrons (-)

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2.2 Nuclides

Notation: ElementAtomic Mass

Notation: ElementAtomic Number

Neutron Atomic Mass Atomic Number Element

Proton1 1 H1

1

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4 2 He

12 6 C

42

126

2.2.1 Chart of the Nuclides

Isotopic NuclidesIsotopic NuclidesppAtoms which have the same atomic number but different mass numbers

He4,002602σabs < 0,05

He-30,000137σ 0,00005

He-499,99986 3β− 0,02

He-599,99986n

He-6806,7 ms β- 3,5

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H1,00794σ 0,332

H-199,985σ 0,332

H-20,015σ 0,00052

H-312,323 aβ− 0,02

n 110,25 mβ− 0,8

N

Z

7

2.2.2 Hydrogen Isotopes

11

21

Hydrogen

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1

31 T

2.3 Electron Shell

2n2n22 Electrons per ShellElectrons per Shell

n = 4 N-Shell

n = 3 M-Shell

n = 2 L-Shell

n = 1 K-Shell

E

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22

422

221

h⋅⋅⋅⋅

=⋅

⋅−=n

eZmreZE

Z = Atomic Numbere = Elementary Charger = Orbital Radiusm = Electron Massn = Shell Number

= Planck‘s Constant h

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2.3.1 Hydrogen Spectrum

Hydrogen Electron Transitions

PFUNDBRACKETT

PASCHEN

PONM

spectral serials

PASCHEN

BALMER

LYMAN

L

K

2.3.2 Quantum Mechanics

electron stationary wave

electron wave function ΨΨ ((r,Er,E))

electron orbital Ψ Ψ 22((r,Er,E))

Schrödinger‘s equation HHΨΨ = E= EΨΨ

electron energy levels EE

electron nucleus distance rr

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2.3.3 Uncertainty Principle

• position and momentum of a particle cannot both beposition and momentum of a particle cannot both be known simultaneously

• the energy-time uncertainty principle.2h

=Δ⋅Δ px

Quantum Mechanics = Probabilistic Considerations !

2h

=Δ⋅Δ Et

2.3.4 De Broglie Hypothesis

Wave – Particle Duality

ph

=λ

λ = particle wavelength, h = planck‘s constant, p = particle momentum

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2.3.5 Stationary Wave

λ

,...4,3,2,12

=

⋅=

n

nl λ

http://uni-ka.lanable.de/html/exphys1/exse18.htm

2.3.5.1 Stationary Wave (a)

d dl

,...4,3,2,12

=

⋅=

n

nl λ

n = 1 Fundamental n = 2 1. Overtone

d d

n = 4 3. Overtonen = 3 2. Overtone

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2.3.5.2 Stationary Wave (b)

40,0045,0050 0055 00310 00315 00320,00325,00 5,0010,0015,0020,0025,0030 0035 00330 00335 00340,00345,00350,00355,00360,0050,0055,0060,0065,0070,0075,0080,0085,0090,0095,00100,00105,00110,00115,00120,00125,00130,00135,00140,00145,00150,00155,00160,00165,00170,00175,00180,00185,00190,00195,00200,00205,00210,00215,00220,00225,00230,00235,00240,00245,00250,00255,00260,00265,00270,00275,00280,00285,00290,00295,00300,00305,00310,00315,00 25,0030,0035,0040,0045,0050,0055,0060,0065,0070,0075,0080,0085,0090,0095,00100,00105,00110,00115,00120,00125,00130,00135,00140,00145,00150,00155,00160,00165,00170,00175,00180,00185,00190,00195,00200,00205,00210,00215,00220,00225,00230,00235,00240,00245,00250,00255,00260,00265,00270,00275,00280,00285,00290,00295,00300,00305,00310,00315,00320,00325,00330,00335,00340,00

,30,0035,0040,0045,0050,0055,0060,0065 0070 00295 00300 00305,00310,00315,00320,00325,00330,00335,00, 5,0010,0015,0020,0025,0030,0035,0040,0045,0050 0055 00310 00315 00320,00325,00330,00335,00340,00345,00350,00355,00360,00

n = 1 Fundamental n = 2 1. Overtone

65,0070,0075,0080,0085,0090,0095,00100,00105,00110,00115,00120,00125,00130,00135,00140,00145,00150,00155,00160,00165,00170,00175,00180,00185,00190,00195,00200,00205,00210,00215,00220,00225,00230,00235,00240,00245,00250,00255,00260,00265,00270,00275,00280,00285,00290,00295,00300,00 ,50,0055,0060,0065,0070,0075,0080,0085,0090,0095,00100,00105,00110,00115,00120,00125,00130,00135,00140,00145,00150,00155,00160,00165,00170,00175,00180,00185,00190,00195,00200,00205,00210,00215,00220,00225,00230,00235,00240,00245,00250,00255,00260,00265,00270,00275,00280,00285,00290,00295,00300,00305,00310,00315,00,

Polarcoordinate Presentation

n = 4 3. Overtonen = 3 2. Overtone

2.3.6 OrbitalsAn orbital represents the probability in space to meet an electron

s orbital, p orbital

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d orbital orbitals were calculated as <Ψ|r|Ψ>

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2.3.7 Electron Angular Momentum

Electron Mass m

Charge e

Velocity

Circle Radius

Magnetic Dipolmoment

Angular Momentum prL ×rrr

vr

rr

μr

Lr

μr

rr

vrm,-e

Angular Momentum

Linear Impact

hnvmr

vmpprL

⋅=⋅⋅⋅⋅

⋅=×=

)()2( π

rr

, not independantLr

μr

2.3.8 Electron Spin

intrinsic angular momentum (or spin angular momentum, or simply spin

Sr

21±=

⋅=

s

sS h

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2.3.9 Quantum Numbers

Quantum numbers describe values of conserved numbers in the dynamics of the quantum system. They often describe specifically the energies of electrons in atoms, but other possibilities include angular momentum spinpossibilities include angular momentum, spin etc.

2.3.9.1 Elektron Quantum Numbers

Quantum Number Symbol Values Meaningy g

principal quantum number n 1,2,3,4,5,... Nucleus Distance, Energy, Shell

azimuthal quantum number l 0,1,2, ... (n-1) Angular Momentum,Subshell

magnetic quantum number m 0,±1,±2, ... ,± l Projection of angular momentum, Energy Shift, gy

spin projection quantum number s ± ½ Intrinsic Angular Momentum,

The angular momentum corresponds to the orbital type (s,p,d,f..) The projection of the angular momentum corresponds to the orbital position

(e.g. p: x,y,z, etc) an

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2.3.10 Wave Functions

Quantum mechanical statesQΨΑ = ΨΑ(r,θ,φ) . ΨΑ(t) ΨΒ = ΨΒ(r,θ,φ) . ΨΒ(t) ΨC = ΨC(r,θ,φ) . ΨC(t)

Linear combination of states (interferences)Ψ = a . ΨΑ(r,θ,φ) + b .ΨΒ(r,θ,φ) + c .ΨC(r,θ,φ)

OrbitalsΨ2 = A2.sin2(ω.t + ϕ0) 7891011

12131415161718192021222324

2526

2728293031444546474849

50515253545556575859606162636465666768

2.4 Electron Shell Structure

Sh ll (K L M N) t i i b h ll ( d f)

n = 2n = 2

n = 3n = 3

n = 4n = 4

Shells (K, L, M, N) are containing sub shells (s, p, d, f)The filling of shells is restricted to rules

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n = 1n = 1

ss pp dd ff

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2.4.1 Configuration of shells

Notation: n l x n = shell Number

H 1 s1

He 1 s2

Li 1 s2 2 s1 valence electronsvalence electrons

Notation: n l n shell Numberl = sub shell s,p,d,f..x = number of e- per orbital population number, no exponent !

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Be 1 s2 2 s2

B 1 s2 2 s2 2p1

C 1 s2 2 s2 2p2

N 1 s2 2 s2 2p3

2.4.1.1 Pauli‘s Rule

• Within one atom electrons can not be equal in all 4 quantum numbers

x

principal quantum numberazimuthal quantum number magnetic quantum number spin projection quantum number

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2.4.1.2 HUND‘s Rule

• Orbitals of the same energy within the one subshell were first single occupiedsingle occupied

E

2.4.2 Shell Configuration for NPAULI‘s rule - HUND‘s rule

n = 2

n = 3E

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n = 1

positive spin negative spin

s p d

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E 4

2.4.3 Shell Configuration for KEnergy rule

n = 2

n = 3E

4s

n = 4

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n = 1

positive spin negative spin

s p d

2.4.4 Shell Configuration Rules

Energy rule

PAULI‘s rule

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HUND‘s rule

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Notation

2.4.5 Shell Configuration for C

NotationCC 1s1s2 2 2s2s2 2 2p2p22

6

12

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Notation

2.4.6 Shell Configuration for Na

NotationNaNa 1s1s2 2 2s2s2 2 2p2p6 6 3s3s11

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30

n = 3n = 3

n = 4n = 4

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n = 1n = 1

n = 2n = 2

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2.4.7 Shell Configuration for Ge , Sn

Ge (32) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2

= [Ar] 4s2 3d10 4p2

Sn (50)

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Sn (50)1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p2

= [Kr] 5s2 4d10 5p2

Test 1

[[ArAr] 3d] 3d1010 4s4s22 4p4p66 = ?= ?

n = 3n = 3

n = 4n = 4

[[ArAr] 3d] 3d1010 4s4s22 4p4p6 6 = ?= ?

??

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n = 1n = 1

n = 2n = 2

ss pp dd ff

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Test 2

What is the shell configuration of siliconWhat is the shell configuration of silicon

?

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2.5 H2O Binding Orbitals

NotationNotationOO 1s1s2 2 2s2s2 2 2p2p44

HH 1s1s11

168

11

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Periods

3.0 Periodic Table of Elements (PT)

Main GroupsI II III IIII V VI VII VIII

1 1 H 2 He2 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10Ne3 11 Na 12Mg 13Al 14Si 15P 16 S 17Cl 18 Ar4 19 K 20Ca 31Ga 32Ge 33As 34Se 35Br 36Kr19 20 31 32 33 34 35 36

5 37 Rb 38Sr 49 In 50 Sn 51Sb 52 Te 53I 54 Xe6 55 Cs 56Ba 81Tl 82 Pb 83Bi 84Po 85At 86Rn7 87 Fr 88Ra 113 114 115 116 117 118

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3.1 Main Group Elements (s,p)

I Alkali metal elements V Nitrogen groupI Alkali metal elements V Nitrogen group Li, Na, K, Rb, Cs, Fr N, P, As, Sb, Bivery reactive metals increasing metallic properties

II Alkaline earth elements VI Chalcogens Be, Mg, Ca, Ba, Sr, Ra O, S, Se, Te, Poless very reactive metals ore-former

III Earth elements VII Halogens B Al G I Tl F Cl B I At

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B, Al, Ga, In, Tl F, Cl, Br, I, Atlight metals salt-former

IIII Carbon group VIII Noble gases C, Si, Ge, Sn, Pb He, Ne, Ar, Kr,Xe, Rnincreasing metallic properties inert elements

valence electrons: s, valence electrons: s, pp

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3.1.1 Examples: CaF2 Fluorite

Chemical Formula: CaF2Molecular Weight: 78.07 g/m Calcium 51.33 % Ca Fluorine 48.67 % FSynonym: Fluorite Spar Locality:

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ycommon world wideEnvironment: low temperature vein deposits

Chemical Formula: PbS

3.1.2 Examples: Lead Glance –PbS

Chemical Formula: PbSMolecular Weight 239.27 g/mLead 86.60 % PbSulphur 13.40 % S Synonym: “galena” ,Blue Lead, Lead Glance Locality:

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yCommon world wide Environment: Lead sulphide ore veins, isseminated in igneous + sedimentary rocks.

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3.1.3 Examples: CaCO3Calcite

Molecular Weight 100 09 g/m

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Molecular Weight 100.09 g/mCalcium 40.04 % Ca Carbon 12.00 % C Oxygen 47.96 % O Synonyms: Glendonite - pseusomorph Nicols, Travertine Locality: Common world wide. Environment: Found in sedimentary, igneous, and metamorphic rocks.

3.2 Transition Metal Elements (s,d)

Scandium-Group IIIb Sc s2p6d1

Sc 1s2 2s2 p6 3s2 p6 d1 4s2

Y 1s2 2s2 p6 3s2 p6 d10 4s2 p6 d1 5s2

La 1s2 2s2 p6 3s2 p6 d10 4s2 p6 d10 5s2 p6 d1 6s2

Ac 1s2 2s2 p6 3s2 p6 d10 4s2 p6 d10 5s2 p6 d10 6s2 p6 d1 7s2

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valence electrons: s, dvalence electrons: s, d

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FeO Fe O Fe O

3.2.2 Examples: Iron Minerals

FeO Fe2O3 Fe3O4

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Hematite Fe2O3 Magnetite: Fe3O4 (magnetic)

3.2.3 Examples: Pyrite FeS2

Chemical Formula: FeS2Molecular Weight 119.98 g/m Iron 46.55 % FeSulphur 53.45 % S Synonym: Fool's Gold Locality:

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yCommon world wide Environment: sedimentary magmatic, metamorphic, and hydrothermal.

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3.3 Lanthanoids und Actinoids(f)

5757LaLa Xe 5d1 6s2

5858CeCe Xe 4f2 6s2

5959PrPr Xe 4f3 6s2

8989AcAc Rn 6d1 7s2

9090ThTh Rn 6d2 7s2

9191PaPa Rn 5f2 6d1 7s2

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6060NdNd Xe 4f4 6s29292UU Rn 5f3 6d1 7s2

valence electrons: s, d, fvalence electrons: s, d, f

3.3.1 Webelements (1)

http://www.webelements.com

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3.3.2 Webelements (2)

http://www.webelements.com

4.0 Periodic Properties atomic diameter

I II III IIII V VI VII VIII1 1 H 2 He

2 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10Ne

3 11 Na 12Mg 13Al 14Si 15P 16 S 17Cl 18 Ar

4 K Ca Ga Ge As Se Br Kr4 19 K 20Ca 31Ga 32Ge 33As 34Se 35Br 36Kr

5 37 Rb 38Sr 49 In 50 Sn 51Sb 52 Te 53I 54 Xe

6 55 Cs 56Ba 81Tl 82 Pb 83Bi 84Po 85At 86Rn

7 87 Fr 88Ra 113 114 115 116 117 118

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4.1 Ionisation Energy

ΔEI

Na Na+ + e-

Cat ion

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ΔEI = ionisation energy = 8,3 . 10-19 J (per atom)

increases with Zdecreases with increasing rAtom

decreases: s>p>d>f

4.1.1 Ionisation Energy Curve

He

Ne

ArKr

XeRn

HF

Cl BrHg

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RnZn Cd Hg

Li Na K Rb Cs

10 20 30 40 50 60 70Atomic Number

28

4.1.2 PT Ionisation Energy


2 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10Ne

3 11 Na 12Mg 13Al 14Si 15P 16 S 17Cl 18 Ar

4 K Ca Ga Ge As Se Br Kr

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4 19 K 20Ca 31Ga 32Ge 33As 34Se 35Br 36Kr



7 87 Fr 88Ra 113 114 115 116 117 118

Ionization Energy of Elements Z = 1, ..12Z Element ionization energy in eV for removel of electron x

4.1.3 Higher Ionisation Energies

Z Element ionization energy in eV for removel of electron x1 2 3 4 5 6 7

1 H 13,62 He 24,6 54,43 Li 5,4 75,6 122,44 Be 9,3 18,2 153,9 217,75 B 8,3 25,1 37,9 259,3 340,16 C 11,3 24,4 47,9 64,5 391,9 489,86 C 11,3 24,4 47,9 64,5 391,9 489,87 N 14,5 29,6 47,4 77,5 97,9 551,9 666,88 O 13,6 35,2 54,9 77,4 113,9 138,1 739,19 F 17,4 35,0 62,6 87,2 114,2 157,1 185,110 Ne 21,6 41,0 64,0 97,1 126,4 157,9 207,011 Na 5,1 47,3 71,6 98,9 138,6 172,4 208,412 Mg 7,6 15,0 80,1 109,3 141,2 186,7 225,3

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4.2 Electron Affinity

Cl. + e- Cl-

Anion

ΔEE = Electron Affinity = - 6,0 . 10-19 J (per atom)

ΔEE

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E y (p )

(kJ / mol)H - 72F -333Cl -364Br -342I -295

Test 3

Which are the corresponding energies ?Which are the corresponding energies ?

Cl+ + e- Cl.

Cl. + e- Cl-

Cl. Cl+ + e-

Cl- Cl. + e-

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Cl Cl e

??

30

b EN

4.3 Electronegativity

number: EN

Atom 1 binding electrons Atom 2attraction to binding electrons

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EN H 2,1Fr 0,7F 4,0Cl 3,0Br 2,8I 2,4

[ ]IE EEEN Δ+Δ21~

Mulliken, 1966:

4.3.1 Electronegativity in the PT


2 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10Ne

3 11 Na 12Mg 13Al 14Si 15P 16 S 17Cl 18 Ar

4 K Ca Ga Ge As Se Br Kr

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7 87 Fr 88Ra 113 114 115 116 117 118

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4.3.2 Electronegativity Curve

1,52

2,53

3,54

4,5

Elek

tron

egat

ivitä

t

Cl

F

BrI

Ele

ctro

neg

ativ

ity

00,5

1

1 51 101

Ordnungszahl21/01/2009 61Atomic Number

H2,1

4.3.2.1 Electronegativity Examples

Li1,0

Be1,5

B2,0

C2,5

N3,0

O3,5

F4,0

Na0,9

Mg1,2

Al1,5

Si1,8

P2,1

S2,5

Cl3,0

K0,8

Ca1,0

Sc1,3

Ti1,6

Ge1,7

As2,0

Se2,4

Br2,8

Rb0,8

Sr1,0

Y1,3

Zr1,6

Sn1,7

Sb1,8

Te2,1

I2,4

Cs0,7

Ba0,9 EN

1 2 3 4

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4.3.3 Metal Properties

electricalconductor

~ 1/Tplasticdeformations

large atomic radii

atomic lattice

thermalconductor

supraconductivity

low ionisation energies

metalshining

4.4 Metal Behaviour

metal behaviour non metal behaviour


2 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10Ne

3 11 Na 12Mg 13Al 14Si 15P 16 S 17Cl 18 Ar


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Metals Semi-metals Non-metals



7 87 Fr 88Ra 113 114 115 116 117 118

33

4.4.1 Metal Classifications

Densityy

Galvanic Corrosion Potential ChartK N M Al Z F Pb C A A

light metals heavy metalsρ < 4 - 5 g/cm3 ρ > 4 - 5 g/cm3

e.g. Al, Mg e.g. Pb, Cd

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K, Na, Mg, Al, Zn, Fe, Pb, Cu, Ag, Au Anodic

least noblecorroded metals

Cathodicmost nobleprotected metals

4.5 Semi-Metals


2 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10Ne

3 11 Na 12Mg 13Al 14Si 15P 16 S 17Cl 18 Ar



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conductivity increases with temperature, various modifications, e.g. crystalline, amorphous, semiconductor behaviour, electron conductivity,

defect electron conductivity


7 87 Fr 88Ra 113 114 115 116 117 118

34

Test 4

Explain the semiconductor‘s energy bands

21/01/2009 67

??

4.5.2 Dopants


2 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10Ne

3 11 Na 12Mg 13Al 14Si 15P 16 S 17Cl 18 Ar



21/01/200968

p-type dopants n-type dopantsacceptor atoms donator atoms


7 87 Fr 88Ra 113 114 115 116 117 118

35

4.5.3 Semiconductor Materials 1

• Group IV elemental semiconductors – Diamond (C) – Silicon (Si) – Germanium (Ge)

G IV d i d t• Group IV compound semiconductors – Silicon carbide (SiC) – Silicon germanide (SiGe)

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• III-V semiconductorsIII V semiconductors– Aluminium antimonide

(AlSb) – Aluminium arsenide

(AlAs) – Aluminium nitride (AlN) – Aluminium phosphide

(AlP)

– Gallium antimonide(GaSb)

– Gallium arsenide (GaAs) – Gallium nitride (GaN) – Gallium phosphide (GaP) – Indium antimonide (InSb)

(AlP) – Boron nitride (BN) – Boron phosphide (BP) – Boron arsenide (BAs) – phosphide (InP)

– Indium arsenide (InAs) – Indium nitride (InN)

21/01/200970

36


• III-V ternary semiconductor alloys – Aluminium gallium arsenide (AlGaAs, AlxGa1-xAs) – Indium gallium arsenide (InGaAs, InxGa1-xAs) – Indium gallium phosphide (InGaP) – Aluminium indium arsenide (AlInAs) – Aluminium indium antimonide (AlInSb) – Gallium arsenide nitride (GaAsN)

Gallium arsenide phosphide (GaAsP)– Gallium arsenide phosphide (GaAsP) – Aluminium gallium nitride (AlGaN) – Aluminium gallium phosphide (AlGaP) – Indium gallium nitride (InGaN) – Indium arsenide antimonide (InAsSb) – Indium gallium antimonide (InGaSb) 21/01/2009 71


• III-V quaternary semiconductor alloys – Aluminium gallium indium phosphide (AlGaInP, also

InAlGaP, InGaAlP, AlInGaP) – Aluminium gallium arsenide phosphide (AlGaAsP) – Indium gallium arsenide phosphide (InGaAsP) – Aluminium indium arsenide phosphide (AlInAsP)

Aluminium gallium arsenide nitride (AlGaAsN)– Aluminium gallium arsenide nitride (AlGaAsN) – Indium gallium arsenide nitride (InGaAsN) – Indium aluminium arsenide nitride (InAlAsN) – Gallium arsenide antimonide nitride (GaAsSbN)

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37


• III-V quinary semiconductor alloys – Gallium indium nitride arsenide antimonide (GaInNAsSb) – Gallium indium arsenide antimonide phosphide

(GaInAsSbP)

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• II-VI semiconductors– Cadmium selenide (CdSe) – Cadmium sulfide (CdS) – Cadmium telluride (CdTe) – Zinc oxide (ZnO)

Zi l id (Z S )– Zinc selenide (ZnSe) – Zinc sulfide (ZnS) – Zinc telluride (ZnTe)

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38


• II-VI ternary alloy semiconductors – Cadmium zinc telluride (CdZnTe, CZT) – Mercury cadmium telluride (HgCdTe) – Mercury zinc telluride (HgZnTe) – Mercury zinc selenide (HgZnSe)

I VII semiconductors• I-VII semiconductors – Cuprous chloride (CuCl)

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• IV-VI semiconductors – Lead selenide (PbSe) – Lead sulfide (PbS) – Lead telluride (PbTe) – Tin sulfide (SnS) – Tin telluride (SnTe)

• IV-VI ternary semiconductors – lead tin telluride (PbSnTe) – Thallium tin telluride (Tl2SnTe5) – Thallium germanium telluride (Tl2GeTe5)

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• V-VI semiconductors – Bismuth telluride (Bi2Te3)

• II-V semiconductors – Cadmium phosphide (Cd3P2) – Cadmium arsenide (Cd3As2) – Cadmium antimonide (Cd3Sb2)Cadmium antimonide (Cd3Sb2) – Zinc phosphide (Zn3P2) – Zinc arsenide (Zn3As2) – Zinc antimonide (Zn3Sb2)

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• Layered semiconductorsLayered semiconductors – Lead(II) iodide (PbI2) – Molybdenum disulfide (MoS2) – Gallium Selenide (GaSe) – Tin sulfide (SnS) – Bismuth Sulfide (Bi2S3)

• OthersOthers – Copper indium gallium selenide (CIGS) – Platinum silicide (PtSi) – Bismuth(III) iodide (BiI3) – Mercury(II) iodide (HgI2) – Thallium(I) bromide (TlBr) 21/01/2009 78

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• Miscellaneous oxides – Titanium dioxide: anatase (TiO2) – Copper(I) oxide (Cu2O) – Copper(II) oxide (CuO) – Uranium dioxide (UO2) – Uranium trioxide (UO3)Uranium trioxide (UO3)

• Organic semiconductors• Magnetic semiconductors

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Exercises

1. Explain the different quantum numbers ? 2. What was the conclusion of the RUTHERFORD experiment ?3. How many electrons can be found in the L-shell ?4. List some Lanthanoids ?5. What does HUND’s rule say ? What does PAULI’s rule6. Which orbitals are valence orbitals in (a) main group elements

(b) in transition group group elements (c) in Lanthanoids?7. What is the meaning of electronegativity ?

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8. How many oxygen atoms can be bond by silicon ?9. What are ore-former ?10. What is the galvanic corrosion potential chart ?11. What is a heavy metal ?12. Where are the semi-metals located in the periodic table ?

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Literature

E. Lindner; Chemie für Ingenieure; M. Lindner Verlag, 1993P.W. Atkins & J.A. Beran; Chemie einfach alles; VCH, 1996W. Schröter et. al; Taschenbuch der Chemie; Verlag Harry Deutsch, 1990 Römpp; Chemie Lexikon, 9. Auflage; Thieme Verlag, 1990 Linus Pauling; Grundlagen der Chemie; Verlag Chemie, 1973B. Bröcker; DTV-Atlas zur Atomphysik; DTV Verlag 1993

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Web-Links

• http://www.johnbetts-fineminerals.com/jhbnyc/quartz.htm• http://webmineral.com/data/Fluorite.shtml• http://webmineral.com/data/Pyrite.shtml• http://www.csun.edu/~vceed002/chem.html• http://www.chemtutor.com/• http://users.senet.com.au/~rowanb/chem/chembond.htm• http://www.seismo.unr.edu/ftp/pub/louie/class/100/100-earthquakes.html• http://atlasinfo cern ch/Atlas/documentation/EDUC/physics1 html

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http://atlasinfo.cern.ch/Atlas/documentation/EDUC/physics1.html• http://users.senet.com.au/~rowanb/chem/• http://newton.ex.ac.uk/aip/physnews.412.html#1• http://www.visionlearning.com/library/module_viewer.php?mid=50• http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch6/graphics/sp

ectrum.gif• http://www.soc.soton.ac.uk/JRD/SCHOOL/eq/eq001b_emspec01.html•

Documents

2 Periodic Table 21 01 09 [Kompatibilitätsmodus]neutron/download/lehre/chemistry/old... · 2.4.1.1 Pauli‘s Rule • Within one atom electrons can not be equal in all 4 quantum