L06 - Dr. P. Lucas U of A MSE 110 Electronic structure of...

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Unformatted text preview: Dr. P. Lucas U of A MSE 110 Electronic structure of atoms SUMMARY FROM LAST CLASS Bohrs model provides a rational to the concept of stable orbits however it can not explain all properties of atoms. The three-dimensional standing waves corresponding to the stable orbits of electrons must be described by three quantum numbers n , m , l . Each of these orbitals can host two electrons of opposite spin which are described by a fourth quantum number s . Four quantum numbers are needed to describe each electron in the atom: n : describes the size of the orbital. n=1, 2, 3, 4 l : describes the shape of the orbital. l = 0, 1, 2 (n-1) m : describes the orientation of the orbital. m = -l,0,l s : describes the spin of the electron. s=, s=- Several rules govern the sequence for filling up orbitals: Aufbau : orbitals of low energy gets filled first. Pauli : only two electrons of opposite spin in each orbital. Hund : degenerated orbitals (orbitals of same energy) are filled with unpaired electrons first. Dr. P. Lucas U of A MSE 110 THE PERIODIC TABLE Elements classification: Each element has a specific number of electrons, the atomic number Z. As Z increase, the mass and charge of the nucleus increases correspondingly . These electrons occupy orbitals of increasing energy. What is a sensible way to organize, classify these elements? Dr. P. Lucas U of A MSE 110 Mendeleev THE PERIODIC TABLE 1871: While writing a chemistry textbook, Mendeleev realized that many elements had similar chemical and physical properties (colors, melting point, reactivity with oxygen, chlorine, hydrogen) Br 2 Some elements are gaseous at room temperature.Some elements are gaseous at room temperature....
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This note was uploaded on 11/19/2009 for the course MSE 110 taught by Professor Lucas during the Spring '08 term at University of Arizona- Tucson.

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L06 - Dr. P. Lucas U of A MSE 110 Electronic structure of...

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