Worksheet 11

# Worksheet 11 - Worksheet 11 - Electronic Structure of Atoms...

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Worksheet 11 - Electronic Structure of Atoms The Schroedinger equation defines wave equations which describe the distribution of electrons around the nucleus. The wave functions that satisfy the Schroedinger equation are called atomic orbitals . They define the allowed energy states of the electrons. The energy levels are described by three quantum numbers , n , l and m l . n is the principal quantum number and has values of 1, 2, 3, . .. The value of n determines the size of the orbital and the energy of electrons in that orbital. l is the angular momentum quantum number as has values of 0 through n -1. The value of l determines the shape of the orbital. m l is the magnetic quantum number and has values of - l through + l and determines the orientation of the orbital. 1. Complete the first two columns of the chart shown below for n = 1 through n = 4. n l m l orbital name # e - total e - in level n 1 0 0 1s 2 2 0 2 1 -1, 0, 1 6 3 0 3d 4 The l = 0 orbitals are called s orbitals . The l = 1 orbitals are called p orbitals . For l = 2, 3 and 4, they are called d , f and g orbitals. Each orbital can contain a maximum of 2 electrons . 2. Fill in the orbital names and the number of electrons per orbital and per energy level in the chart. 3. How many orbitals are present in each of the principal levels? n = 1 n = 2 n = 3 n = 4 n = 5

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The s orbitals are spherical . They increase in size with increasing values of n . The p orbitals are dumbbell shaped. Each of the three p orbitals is oriented differently in space, as shown below. Again, size of these orbitals increases with
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## This note was uploaded on 12/05/2011 for the course CHEM 231 taught by Professor Beck during the Spring '11 term at Indiana.

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Worksheet 11 - Worksheet 11 - Electronic Structure of Atoms...

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