Chemistry (Inorganic) Chapter 1 - Atoms: Structure and Function
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The document discusses principles of physical science, focusing on atomic structure, including the Bohr model and quantum mechanics. It explores concepts such as isotopes, mass spectrometry, and the Schrödinger equation, explaining electron behavior and energy levels in atoms. Additional topics include atomic orbitals, electron configurations, and measurements related to atomic and ionic radii.
Chemistry (Inorganic) Chapter 1 - Atoms: Structure and Function
- 1. Physical Science for the Masses With Doctor Bones (Don R. Mueller, Ph.D.) Scientist Educator Entertainer J U G G L E R
- 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
- 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
- 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, 4r2 R(r)2 , for the 1s, 2s and 3s atomic orbitals of the hydrogen atom.
- 38. Radial distribution functions, 4r2 R(r)2 , for the 1s, 2s and 2p atomic orbitals of the hydrogen atom.
- 39. Radial distribution functions, 4r2 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
- 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.