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Chapter 4-2 The Quantum Model of the Atom By: Astrid Rodriguez Ray Franco Randy Cooper Grace Martinez Rick Perez Electrons as Waves In 1924 Louis de Broglie found that electrons could have dual wave particle nature. Broglie suggested that electrons be considered waves confined to the space around an atomic nucleus. Electrons can have electron waves only at specific frequencies. Diffraction refers to the bending of a wave as it passes by the edge of an object, such as the edge of an atom in a crystal. Interference between electron beings occur when waves over lap. It results in the reduction of energy in some areas and the increase in others. The Heisenberg Uncertainty Principle Proposed by German theoretical physicist Werner Heisenberg in 1927. Principal states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle. It is one of the fundamental principles of our present understanding of light and matter. The Schrödinger Wave Equation Austrian physicist Erwin Schrödinger developed an equation that treated electrons in atoms as waves. With the Heisenberg Uncertainty Principle, the Schrödinger Wave Equation laid the foundation for quantum theory. Quantum theory describes mathematically the wave properties of electrons and other very small particles. Orbitals is a three-dimensional region around the nucleus that indicates the probable location of an Electron. Erwin Schrödinger Atomic Orbitals and Quantum Numbers Quantum numbers specify the properties of atomic orbitals and the properties of electrons in orbitals. Principal quantum number, symbolized by n,indicates the main energy level occupied by the electrons. As the energy level increases the distance from the nucleus increases Angular momentum quantum number, symbolized by l indicates the shape of the orbital. Magnetic quantum number, symbolized by m, indicates the orientation of an orbital around the nucleus. Spin quantum number, has only two possible values (+1/2, 1/2) which indicates the two fundamental spin states of an electron. Quantum Number Relationships in Atomic Structure Main energy level (n) Sublevels in main energy level Number of orbital per sublevel Number of electrons Number of electrons per sublevel in energy level 1 s 1 2 2 2 s p 1 3 2 6 8 3 s p d 1 3 5 2 6 8 18 4 s p d f 1 3 5 7 2 6 8 10 14 32 Bibliography Modern Chemistry Book printed 2005 Published by Holt, Rinehart and Winston Area printed Dallas, Texas Britannica Online. Encyclopedia Britannica Inc. November 6, 2007