Physical Science for the Masses: http://science-for-the-masses.blogspot.com Chapter 1 - Atoms with Doctor Bones aka Don R. Mueller, Ph.D.

1. Physical Science for the Masses
With Doctor Bones (Don R. Mueller, Ph.D.)
Scientist
Educator
Entertainer
J
U
G
G
L
E
R

2. Chapter 1
AtomsAtoms

3. Planetary Model of the Atom
Where are the Croutons?

4. X = Na
A = 23
Z = 11
N = A – Z = 12
Na – Natrium
(Sodium)

6. 1 proton 1 proton
1 neutron
1 proton
2 neutrons

7. Boron (B) has two isotopes:
10B (20% = 0.20) and 11B (80% = 0.8)
Mass = 0.20 × 10.0 amu + 0.80 × 11.0 amu = 10.8 amu

8. The World’s Greatest
Combination of Atoms

10. Mass spectrometric traces for (a) atomic Ru and (b) molecular S8;
the mass:charge ratio is m/z and in these traces z = 1.
(c) The molecular structure of S8.
atomic Ru
molecular S8
S8

11. (ChemCards) http://www.hcc.mnscu.edu/chem/chemstacks.html
Ne (g)

12. (ChemCards) http://www.hcc.mnscu.edu/chem/chemstacks.html
Neon isotopes

16. A schematic representation of part of the emission spectrum of
hydrogen showing the Lyman, Balmer and Paschen series of
emission lines. The photograph shows the predominant lines in the
observed, visible part of the spectrum of hydrogen which appear at
656.3 (red), 486.1 (cyan) and 434.0 nm (blue). Other fainter lines
are not visible in this photograph.
Lyman Balmer Paschen
656.3
434.0
486.1

17. Several transitions within the Lyman and Balmer
series in the emission spectrum of atomic hydrogen.
Lyman series
Balmer series
Ionization
continuum
n = 1n > 1
n > 2 n = 2
n = 1
n = 2
n = 3
n = 4
n = 5
n = ∞ n = ∞

19. Emission Series for
the Hydrogen atom
n = 1
n = 2
n = 3
n = 4
n = 5

20. Electron orbits assume discrete energy states also known as
quantized states. As a consequence, only certain photon energies
are allowed when, for example, an electron jumps from a higher to
a lower energy level, thus producing an emission line. The Bohr
model predicts these energies for the hydrogen atom.
The Bohr Model of the Atom
Bohr’s model of the
H-atom assumes a
circular orbit of the
electron about the
hydrogen nucleus.

21. H-atom emission lines
With the electron in the ground state,
it cannot radiate further.

22. http://hyperphysics.phy-astr.gsu.edu/hbase/bohr.html
Bohr model: FCentripetal = FElectrostatic

23. http://hyperphysics.phy-astr.gsu.edu/hbase/bohr.html
Bohr postulated that the angular momentum L of the
hydrogen atom’s electron was quantized:
Having employed the de Broglie relationship λ = h/mv
and the standing wave condition: 2 π r = n λn

24. http://hyperphysics.phy-astr.gsu.edu/hbase/bohr.html
L = mvr = nh/2π r

25. 2
0
22
42
εh8n
meZ
E 
2
0
22
emπZ
εhn
r 
Bohr Energies (E)
Bohr radii (r)

26. Ms. Wave
Mr. Particle:
Beware, the Dual Nature of Light: A headache for the Director?
Is it a wave, or is it a particle? Interestingly, this is also true of
electrons and other such particles.

27. Classical Mechanics Quantum Mechanics
So along comes the Quantum Gang:
Albert Einstein (Photoelectric Effect)
Louis de Broglie (Wave-Particle Duality)
Werner Heisenberg (Uncertainty Principle)
Erwin Schrödinger (Wave Mechanics) and more…
The Transition of Wave Mechanics into Quantum Mechanics:
The wave function ψ, which describes the electron as it varies
with position (r) and time (t) satisfies the differential equation
first constructed by physicist Erwin Schrödinger:
The Schrödinger Equation used in
non-relativistic quantum mechanics

28. You too can become a
Quantum Mechanic.
I’m glad I did!
Just wish my pencil
would stop making
so many mistakes…

29. Examining the Schrodinger Equation
Solving the Schrödinger equation for an electron orbiting the
atomic nucleus, leads to discrete energy levels for the electron.

30. How about a getting a Schrodinger Equation Tattoo?

31. The polar coordinates (r, , ) for a point on the surface; r is the
radial coordinate,  and  are angular coordinates measured in
radians (rad). The Cartesian axes (x, y and z) are also shown.
Using polar coordinates to
construct wave functions

33. Solutions of the Schrödinger equation for the hydrogen atom: The
1s, 2s and 2p atomic orbitals. For these forms of the solutions, the
distance r from the nucleus is measured in atomic units.
1s
2s
2px
2pz
2py

34. Plots of the radial parts of the wavefunction, R(r), versus distance,
r, from the nucleus for (a) the 1s and (b) the 2s atomic orbitals of
the hydrogen atom; the nucleus is at r = 0. The vertical scales for
the two plots are different but the horizontal scales are the same.

35. Plots of radial parts of the wavefunction R(r) against r for the 2p,
3p, 4p and 3d atomic orbitals; the nucleus is at r = 0.

37. Radial distribution functions, 4r2
R(r)2
, for the 1s, 2s and 3s atomic
orbitals of the hydrogen atom.

38. Radial distribution functions, 4r2
R(r)2
, for the 1s, 2s and 2p atomic
orbitals of the hydrogen atom.

39. Radial distribution functions, 4r2
R(r)2
, for the 3s, 3p and 3d atomic
orbitals of the hydrogen atom.

42. Boundary surfaces for the angular parts of the 1s and 2p atomic
orbitals of the hydrogen atom. The nodal plane shown in grey for
the 2pz atomic orbital lies in the xy plane.

43. Representations of
an s orbital
A set of 3 degenerate p orbitals.
The px orbital’s lobes pass into and out of the plane of the paper.
in-plane in-planeout-of-plane

44. A set of three degenerate p orbitals.

45. Cross-sections through atomic orbitals of hydrogen: (a) 1s - zero
radial nodes, (b) 2s - one radial node, (c) 3s - two radial nodes,
(d) 2p - zero radial nodes and (e) 3p - one radial node.
1s
2s
3s
2p
3p

46. Representations of a set of five degenerate d atomic orbitals.
dyz dxy dxz
dz2
dx2-y2

47. Set of five degenerate d atomic orbitals.

48. Set of seven degenerate f atomic orbitals.

49. Ground state electronic configurations of the elements up to Z = 103.

57. Periodic table of the Elements
s - block d - block p - block

58. f - block

59. (ChemCards) http://www.hcc.mnscu.edu/chem/chemstacks.html

60. (ChemCards) http://www.hcc.mnscu.edu/chem/chemstacks.html

62. (ChemCards) http://www.hcc.mnscu.edu/chem/chemstacks.html

63. (ChemCards) http://www.hcc.mnscu.edu/chem/chemstacks.html

64. (ChemCards) http://www.hcc.mnscu.edu/chem/chemstacks.html

65. Measuring Atomic Radii
(a) Metallic Radii
(b) Covalent Radii
(c) Ionic Radii

66. Atomic radii for selected elements in picometers (pm)

68. Ionic radii for selected elements in picometers (pm)

69. Ionic radii for selected elements in picometers (pm)

70. First, second and third (some fourth) ionization energies (kJ/mol).

71. First, second and third ionization energies (kJ/mol).

72. The first ionization energy values in kJ/mol
for elements up to Rn (Z = 86).

73. The first ionization energy values in eV for
elements up to Rn (Z = 86).

74. First electron affinities (kJ/mol) for the main group elements.

75. Pauling, Mulliken and Allred-Rochow electronegativities (χ).

76. Pauling, Mulliken and Allred-Rochow electronegativities (χ).

78. Diagrams for the ground state electron configurations of O and Si.
The complete configurations are shown here, but it is common to
simply indicate the valence electrons. For O, this consists of the 2s
and 2p levels and for Si, the 3s and 3p levels.

79. Energy level diagrams for electronic transitions.

80. Approximate enthalpy changes DEAH(298 K) associated with the
attachment of an electron to an atom or anion.