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Welcome to 3.091Lecture 4

September 16, 2009

Matter/Energy Interactions: Atomic Spectra

1

3 4

11 12

19 20 21 22 23 24 25 26 27 28 29 30 31 32

2

5 6 7 8 9 10

13 14 15 16 17 18

33 34 35 36

39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86

37 38

55 56

87 88 89

3.091 Periodic Table Quiz

Name Grade /10

Image by MIT OpenCourseWare.

Rutherford-Geiger-Marsden experiment


Bohr Postulates for the Hydrogen Atom 1. Rutherford atom is correct 2. Classical EM theory not applicable to orbiting e-

3. Newtonian mechanics applicable to orbiting e-

4. Eelectron = Ekinetic + Epotential

5. e- energy quantized through its angular momentum: L = mvr = nh/2π, n = 1, 2, 3,…

6. Planck-Einstein relation applies to e- transitions: ΔE = Ef - Ei = hν = hc/λ

c = νλ

Bohr magneton

Nuclear magneton

Fine structure constant

Inverse fine structure constant

Rydberg constant

Rydberg constant in eV

Bohr radius

Quantum of circulation

Electron specific charge

Electron Compton wavelength

Electron classical radius

Electron magnetic moment`Electron mag. moment anomalyElectron g-factor

Muon mass

Muon magnetic moment

Muon mag. moment anomaly

Muon g-factor

Proton magnetic moment

Proton gyromagnetic ratioNeutron magnetic moment

Stefan-Boltzmann constantFirst radiation constant

Second radiation constant

Electron volt

Atomic mass unit

Standard atmosphere

Standard acceleration of gravity

18

19

20

21

22

23

24

25

26

27

28

293031

32

33

34

35

36

3738

39

4041

42

43

44

45

9.274 015 4(31) X 10_24

5.050 786 6(17) X 10_27

7.297 353 08(33) X 10_3

0.529 177 249(24) X 10_10

3.636 948 07(33) X 10_4

2.426 310 58(22) X 10_12

2.817 940 92(38) X 10_15

928.477 01(31) X 10_26

1.159 652 193(10) X 10_3

1.883 532 7(11) X 10_28

4.490 451 4(15) X 10_26

1.165 923 0(84) X 10_3

1.410 607 61(47) X 10_26

0.966 237 07(40) X 10_26

5.670 51(19) X 10_8

3.741 774 9(22) X 10_16

1.602 177 33(49) X 10_19

1.660 540 2(10) X 10_27

26 752.212 8(81) X 104

2.002 331 846(17)

0.014 387 69(12)

101 325

9.806 65

-1.758 819 62(53) X 1011

137.035 989 5(61)

2.002 319 304 386(20)

10 973 731.534(13)

13.605 698 1(40)

0.34

0.34

0.045

0.045

0.0012

0.30

0.045

0.089

0.30

0.089

0.13

0.340.00860.00001

0.61

0.33

7.2

0.0084

0.34

0.300.41

34

0.608.4

0.30

0.59

exact

exact

J T_1

J T_1

m_1

m2 s_1

T_1 s

_1

W m_2 K

_4

C kg_1

J T_1

J T_1

J T_1

J T_1

m s_2

W m2

m K

J

kg

Pa

eV

m

m

kg

m

α = µ0ce2/2h

h/2me

-e/me

µe

1/α

R∞ = mecα2/2h

R∞ hc/{e}a0 = α/4πR∞

λC = h/mec

re = α2a0

gn

atm

u

eV = (e/C)J = {e}J

c2 = hc/kc1 = 2πhc2

µn

γp

µp

mµ

µµ

ae = µe/µB _ 1

ge = 2(1 + ae)

gµ = 2(1 + aµ)

µΒ = eh/2me

µΝ = eh/2mp

aµ = [µµ/eh/2mµ)] -1

σ = ( π2/ 60)k4/h3c2

C = A s F = (C/V) = m_2 kg_1 s4 A2 Pa = N m_2 = m_1 kg s _ 2 T = kg s_2 A_1 W = J s_1 = m2 kg s_3

J T_1 = m2 AT s = kg s_1 A_1 Wb = V s = m2 kg s_2 A_1 Fm_1 = (C/V) m_1 = m_3 kg_1 s4 A2

1.602 177 33(49) X 10_19 C means (1.602 177 33 + (0.000 000 49) X 10

_19 C Notation :


Figure 6.9Prism Spectrograph A.A. Ångström (1853)


Figure 6.9b


1.00794-259.34-252.870.08992.2013.5981s1

Hydrogen

6.941180.513420.5340.985.392[He]2s1

Lithium

9.012182128724711.84771.579.322[He]2s2

Beryllium

22.98976897.728830.970.935.139[Ne]3s1

Sodium

24.305065010901.741.317.646[Ne]3s2

Magnesium

1

H1

3

Li1

11

Na1

12

Mg2

4

Be2

2IIAIIA

1IAIA


Bohr magneton

Nuclear magneton

Fine structure constant

Inverse fine structure constant

Rydberg constant

Rydberg constant in eV

Bohr radius

Quantum of circulation

Electron specific charge

Electron Compton wavelength

Electron classical radius

Electron magnetic moment`Electron mag. moment anomalyElectron g-factor

Muon mass

Muon magnetic moment

Muon mag. moment anomaly

Muon g-factor

Proton magnetic moment

Proton gyromagnetic ratioNeutron magnetic moment

Stefan-Boltzmann constantFirst radiation constant

Second radiation constant

Electron volt

Atomic mass unit

Standard atmosphere

Standard acceleration of gravity

18

19

20

21

22

23

24

25

26

27

28

293031

32

33

34

35

36

3738

39

4041

42

43

44

45

9.274 015 4(31) X 10_24

5.050 786 6(17) X 10_27

7.297 353 08(33) X 10_3

0.529 177 249(24) X 10_10

3.636 948 07(33) X 10_4

2.426 310 58(22) X 10_12

2.817 940 92(38) X 10_15

928.477 01(31) X 10_26

1.159 652 193(10) X 10_3

1.883 532 7(11) X 10_28

4.490 451 4(15) X 10_26

1.165 923 0(84) X 10_3

1.410 607 61(47) X 10_26

0.966 237 07(40) X 10_26

5.670 51(19) X 10_8

3.741 774 9(22) X 10_16

1.602 177 33(49) X 10_19

1.660 540 2(10) X 10_27

26 752.212 8(81) X 104

2.002 331 846(17)

0.014 387 69(12)

101 325

9.806 65

-1.758 819 62(53) X 1011

137.035 989 5(61)

2.002 319 304 386(20)

10 973 731.534(13)

13.605 698 1(40)

0.34

0.34

0.045

0.045

0.0012

0.30

0.045

0.089

0.30

0.089

0.13

0.340.00860.00001

0.61

0.33

7.2

0.0084

0.34

0.300.41

34

0.608.4

0.30

0.59

exact

exact

J T_1

J T_1

m_1

m2 s_1

T_1 s

_1

W m_2 K

_4

C kg_1

J T_1

J T_1

J T_1

J T_1

m s_2

W m2

m K

J

kg

Pa

eV

m

m

kg

m

α = µ0ce2/2h

h/2me

-e/me

µe

1/α

R∞ = mecα2/2h

R∞ hc/{e}a0 = α/4πR∞

λC = h/mec

re = α2a0

gn

atm

u

eV = (e/C)J = {e}J

c2 = hc/kc1 = 2πhc2

µn

γp

µp

mµ

µµ

ae = µe/µB _ 1

ge = 2(1 + ae)

gµ = 2(1 + aµ)

µΒ = eh/2me

µΝ = eh/2mp

aµ = [µµ/eh/2mµ)] -1

σ = ( π2/ 60)k4/h3c2

C = A s F = (C/V) = m_2 kg_1 s4 A2 Pa = N m_2 = m_1 kg s _ 2 T = kg s_2 A_1 W = J s_1 = m2 kg s_3

J T_1 = m2 AT s = kg s_1 A_1 Wb = V s = m2 kg s_2 A_1 Fm_1 = (C/V) m_1 = m_3 kg_1 s4 A2

1.602 177 33(49) X 10_19 C means (1.602 177 33 + (0.000 000 49) X 10

_19 C Notation :


Figure 6.11a

Electronic emission transition

Higher-Energy Orbit

Lower-Energy Orbit

Photon

e-

e-


Bohr Postulates for the Hydrogen Atom 1. Rutherford atom is correct 2. Classical EM theory not applicable to orbiting e-

3. Newtonian mechanics applicable to orbiting e-

4. Eelectron = Ekinetic + Epotential

5. e- energy quantized through its angular momentum: L = mvr = nh/2π, n = 1, 2, 3,…

6. Planck-Einstein relation applies to e- transitions: ΔE = Ef - Ei = hν = hc/λ

c = νλ

Figure 6.11


486 nm

434 nm

410 nm

656 nm

n = 3

n = 2

n = 4n = 5 n = 6

(a) Balmer Series Transitions (b) Electronic emission transition

Higher-Energy Orbit

Lower-Energy Orbit

Photon

e-

e-

Figure 6.4a

400 450 500 550 600 650 700

Vio

let

Blu

e

Gre

en

Yello

w

Ora

nge

Red

Wavelength , λ (nm)

Wavelength , λ (m)

Frequency , ν (Hz)

10-12

1020 1019 1018 1017 1016 1014 1013 1012 1011 1010 109 108

10-11 10-10 10-9 10-8 10-7 10-6 10-5 10-4 10-3 10-2 10-1 100 101

Gamma X ray Ultraviolet Infrared Microwave Radio

1015

Visible Spectrum

(b)

(a)


Figure 6.12

Lyman Series

Balmer Series

Paschen Series

Brackett Series

Pfund Series

n = 1

n = 2

n = 3

n = 4

n = 5

n = 6


Cecilia Payne (1900-1979)

1st woman graduate student in Astronomy at Harvard

1st Ph.D. in Astronomy at Harvard

1st woman to receive tenure at Harvard

1st woman to chair the Faculty of Arts and Sciences at Harvard

awarded tenure in 1938 but denied a professorship for 18 years

forced to recant her findings that the sun is not dominantly iron but rather hydrogen

Figure 6.9b

lines characteristic of atomic HImage by MIT OpenCourseWare.

Figure removed due to copyright restriction.

MIT OpenCourseWarehttp://ocw.mit.edu

3.091SC Introduction to Solid State ChemistryFall 2009

For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms.

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welcome to 3 · 2009. 9. 16. · bohr postulates for the hydrogen atom 1. rutherford atom is...

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