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Picture of the Atom Picture of the Atom Electromagnetic radiation and Atomic Spectra The Nature of Electron and Atomic Orbitals Many-electron atoms Atomic properties and Periodicity Nuclear chemistry

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3.1.1 Atomic concept, 3.1.1 Atomic concept, 3.1.2 Subatomic particles, 3.1.3 Atomic structure: first ideas

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The classical picture of the atom

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J.J. Thomson’s Cathode Tube Charge-to-mass ratio

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The Atom : J. J. Thomson (1856-1940)

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The Atom based on Thomson’s experiment

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Mass of electron

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Rutherford Experiment Ernest Rutherford – 1911 With Thomson Model : a particles should travel through the atom without deflection.

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Rutherford Experiment

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The Nucleus

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Modern View

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3.2. Electromagnetic Radiation and Quantization 3.2.1: Electromagnetic Radiation 3.2.2: Quantization 3.2.3: The Atomic Spectrum of Hydrogen

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Spectrum

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Electromagnetic radiation

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Electromagnetic Radiation

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ELECTROMAGNETIC RADIATION

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Electromagnetic Radiation - Characteristics

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Radio in the 909kHz. What wavelength does it correspond to?

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Nature of Matter

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Photoelectric effect When UV radiation hits a metal surface, electrons are ejected – photoelectric effect. (in 1905 explained by Albert Einstein using a quantum approach) h =  + EKE  - work function – minimum energy required to remove the electron EKE – kinetic energy of the ejected electron

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Dual Nature of Light

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De Broglie 1924

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$Diffraction$

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Diffraction

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How to test the wave properties of an electron?

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How to test the wave properties of an electron?

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$Diffraction$

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Diffraction

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Conclusion

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Atomic Spectrum of Hydrogen

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Table 3.4. The atomic spectrum of hydrogen

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Atomic Spectrum of Hydrogen

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3.3.2: The Bohr Model

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The Bohr Model

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The Bohr Model

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Wave Function and Atomic Orbitals

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De Broglie

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2.2 SChRONDINGER EQUATION Enter

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Quantum Mechanical Description of the Atom

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The Schrödinger equation

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Schrodinger Wave Equation

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Cartesian and Spherical Coordinate

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The wavefunction

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Homework-2 Please solve problems ; Chapter 3 6, 9, 10, 12, 14, 16 and 17 Due on Wednesday. Recitation time

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Wave Equation for the Hydrogen Atom

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Quantum numbers :

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Radial and Angular Wave Function for 1s derived from Schrodinger Equation

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s orbitals

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Physical Meaning of Orbitals

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p orbitals

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d orbitals

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f orbitals

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Schrödinger Equation

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Heisenberg uncertainty principle

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The Hydrogen Atom : summary

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Polyelectronic Model

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Self-Consistent Field Method

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Many Electron Atoms

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Electron Spin and Pauli Principle

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History of the Periodic Table

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The Aufbau Principle

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Valence electrons

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Rules

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Rules

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Rules

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Rules

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Hund’s Rule

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Penetration Effect

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Penetration Effect

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Slater’s Rules The rules were devised semi-empirically by John C. Slater and published in 1930 Identify Zeff (as a measure of attraction) for any electron Z* = Z – S Where Z = nuclear charge S = shielding constant

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Slater’s Rules The rules were devised semi-empirically by John C. Slater and published in 1930 Rules for determining S S = shielding constant

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Slater’s Rules for determining S for a specific electron The shielding constant (S) ns and np valence electrons: 3a) Each electron in the same (ns, np) group contributes 0.35 to the value of S for each other electron in the group. Except. A 1s electron contributes 0.30 to S of another 1s electron. EXAMPLE: 2s2p5, in a particular 2p electron has 6 other electron in (2s, 2p) group. Each of these contribute 0.35 to the value of S, for a total contribution to S of 60.35=2.10

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Slater’s Rules for determining S for a specific electron Rule -3b: Each electron in n-1 group contribute 0.85 to S Rule -3c: Each electron in n-2 group or lower shells contribute 1.00 to S EXAMPLE: 3s electrons of sodium (1s22s2p63S1) , there are 8 electrons in n-1 (2s, 2p) group, each of these contribute 0.85 to the value of S, for a total contribution to S of 80.85=6.80. There are two electrons in n-2(1S) 2 1 = 2, S = 8.80

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Slater’s Rules for determining S for a specific electron Rule -4a: Each electron in nd and nf valence Each electron in the same group (nd) or (nf) group contribute 0.35 to the value of S to each other electron in the group (same rule as 3a) Rule -4b: Each electron in groups to the left contribute 1 to the value of S.

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Solution Rule-1 : the electron configuration is written using slater’s groupings: (1s2)(2s2, 2p6)(3s2, 3p6)(3d8)(4s2) To calculate S for 3d valence electron: Rule 4a : each electron in the group(3d8) contributes 0.35 to S. Total contribution = 70.35=2.45 Rule 4b : each electron in the group to the left of (3d8) Contribute 1 to S. Total contribution = 181=18.00 Total S = 2.45 +18.00= 20.45 The effective nuclear charge Z*=28-20.45=7.55

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Solution Rule-1 : the electron configuration is written using slater’s groupings: (1s2)(2s2, 2p6)(3s2, 3p6)(3d8) (4s2) To calculate S for 4s valence electron: Rule 3a : each electron in the 4s group contribute 0.35 1 0.35 Rule 3b : each electron in the n-1 group contribute 0.85 (0.85.16) = 13.60 Rule 3c : each electron on the left of n-1 Contribute 1 to S. Total contribution = 101=10.00 Total S = 0.35 + 13.60 + 10.00= 23.95 The effective nuclear charge Z*=28-23.95=4.05

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Comparison of The effective nuclear charge 3d electrons The effective nuclear charge Z*=28-20.45=7.55 4s electrons Z*=28-23.95=4.05 Ni : [Ar]3d8 All transition Metals loose ns electrons more readily than (n-1) d electrons