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Transcript
Energy levels of various orbitals For hydrogen, energy level depend only on n For multielectron atoms (all others) - energy levels depend on both n and l A diagram which shows the orbital energy levels for both is shown below. MEMORIZE ! Order of orbital energy levels (from low to high energy) for multielectron atoms 1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p <4d < 4f . Questions 1. Identify the shell and subshell of an orbital with the quantum numbers n = 3, l = 1, ml = 1. Ans: 3px (the ml is related to the spatial orientation of the orbital and can have a value of x, y or z (see figure of p n l ml orbitals below) 2. Give the orbital notations for electrons in orbitals with the following set of quantum # (a) n = 2, l = 1, ml = 1 (b) n = 4, l = 3, ml = -2 (c ) n =3, l = 2, ml = -1 Ans 2p 4f 3d 1 5.8 The Shapes of Orbitals The shape of a given orbital is defined by the quantum number l. When l = 0 called a s orbital When l = 1 called a p When l = 2 called a d When l = 3 called a f and so forth s orbitals 1. All s orbitals are spherical 2. 3. Probability of finding an electron depends only on the distance of the electron from the nucleus Differences among s orbitals in different shells are: - size increases in successively higher shells - electron distribution in outer s oribtals have region of max. probability separated by a node (a surface of zero probability) Figure represents (a) 1s (b) 2s and (c) 3s orbitals. Note the nodes of zero probability in 2s and 3s orbitals 3s 2s 1s 2 px orbital py orbital pz orbital d orbitals 1. there are 5 types of d orbitals 2. four are cloverleaf shape where there are 4 lobes of max. electron probability separated by two nodal planes through the nucleus 3. A dz2 orbital similar in shape to a pz orbital f orbitals and beyond There are seven types of f orbitals DO NOT NEED TO KNOW SHAPES Representations of the five 3d orbitals 3 This document was created with Win2PDF available at http://www.daneprairie.com. The unregistered version of Win2PDF is for evaluation or non-commercial use only.