Chem102 10.2 - Chemistry 102B Discussion Worksheet #10...

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Chemistry 102B – Discussion Worksheet #10 Electronic Structure of Atoms The Schrödinger equation defines wave equations which describe the distribution of electrons around the nucleus. The wave functions that satisfy the Schrödinger equation are called atomic orbitals . They define the allowed energy states of the electrons. The energy levels are described by quantum numbers . For this class we will only focus on the principal quantum number ( n ). The value of n determines the size of the orbital and the energy of electrons in that orbital. The s orbitals (left) are spherical. They increase in size with increasing values of n. Each s orbital can hold a maximum of 2 electrons. The p orbitals (right) are dumbbell shaped. Each of the three p orbitals is oriented differently in space. All three p orbitals are of the same energy and can each hold a maximum of 2 electrons. The d orbitals (see textbook) are cloverleaf shaped (except d z 2 ). The f orbital shapes are more complex and can be found in the textbook. The importance of these orbitals is apparent when we look at th Periodic Table. Period 1 (H and He) is the n = 1 energy level. This
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This note was uploaded on 02/14/2011 for the course CHEMISTRY 102 taught by Professor Whitt during the Spring '11 term at University of Illinois, Urbana Champaign.

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Chem102 10.2 - Chemistry 102B Discussion Worksheet #10...

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