Inorganic Chemistry

1
Lecture 1Sections 2-1, 2-2-1

• Introduction
• History of Periodic Table
• Quantum-mechanics basis of the Periodic Table
• Schrödingers equation
• The particle in a box

2
(No Transcript)
3
Abundance of the Elements
4
Molybdenum Nitrogenase
NH3
N2
Fe protein
MoFe protein
Fe protein
65 Å
190 Å
5
The Scope of Inorganic Chemistry
6
A Partial Sequence of the Elements (1867)
7
Periodic Table as Formulated by Mendeleev in 1871
eka-B Sc 1879
eka-Si Ge 1886
eka-Al Ga 1875
Elements placed according to the value of their
atomic weights present a clear periodicity of
properties. (Mendeleev, 1869)
8
The Modern Periodic TableFigure 2-1, Miessler
and Tarr
9
The Quantum Mechanics Basis of the Periodic Table

• 1926, 1927 Schrodinger and Heisenberg describe
  the wave properties of the electron
• Electrons are treated as waves and can be
  described by a mathematical function ?.
• Using this function ?, the probability to find
  the electron in a given place in space can be
  calculated.
• The area of space where the electron is most
  likely located is called orbital.
• Schrodinger formulated a differential equation
  that can be used to determine the wave function
  of the electron
• H ? E ?
• H is a Hamiltonian operator or in short
  Hamiltonian.
• A Hamiltonian is a function that has as argument
  another function.

10
Quiz Concepts for Recitation on January 17

• Form of Schrodinger equation HYEY Definition of
  H,E, Y (slide 9 of Power Point class notes)
• Math memo (see Blackboard course site)
• -
• - values of x for which sin(x) 0,1 or
  cos(x) 0,1