Question

2. For the 1-D particle in a box, compute the wavefunction (?) and the probability density (?²) for the n = 3 case with x = 0, 1/6, 1/3, 1/2, 2/3, 5/6, 1. Assume the normalization factor (A) is the square root of 2 and that a = 1. Draw a plot representing ? and ?². How many nodes are present? 3. Determine the principal quantum numbers l and m? for electrons in (a) the n=4 shell, (b) the n = 5 shell, and (c) the n= 7 shell 4. Draw representations of the general shapes for s, p, and d orbitals. Use a 3-D coordinate and be sure to indicate the sign of the wave function by shading or +/- signs. Indicate the number and location of any angular nodes in each case 5. Give the total number of nodes present in the following orbitals and indicate how many are radial and how many angular: 4p, 5d, 6f, 7g. 6. Draw a cross-sectional representation depicting radial nodes present in 4s and 5d_{x²-y²} orbitals and show how the sign of the wavefunction changes throughout the orbital using shading or +/- signs.

          2. For the 1-D particle in a box, compute the wavefunction (?) and the probability density (?²) for the n = 3 case with x = 0, 1/6, 1/3, 1/2, 2/3, 5/6, 1. Assume the normalization factor (A) is the square root of 2 and that a = 1. Draw a plot representing ? and ?². How many nodes are present?
3. Determine the principal quantum numbers l and m? for electrons in (a) the n=4 shell, (b) the n = 5 shell, and (c) the n= 7 shell
4. Draw representations of the general shapes for s, p, and d orbitals. Use a 3-D coordinate and be sure to indicate the sign of the wave function by shading or +/- signs. Indicate the number and location of any angular nodes in each case
5. Give the total number of nodes present in the following orbitals and indicate how many are radial and how many angular: 4p, 5d, 6f, 7g.
6. Draw a cross-sectional representation depicting radial nodes present in 4s and 5d_{x²-y²} orbitals and show how the sign of the wavefunction changes throughout the orbital using shading or +/- signs.

2. For the 1-D particle in a box, compute the wavefunction (?) and the probability density (?²) for the n = 3 case with x = 0, 1/6, 1/3, 1/2, 2/3, 5/6, 1. Assume the normalization factor (A) is the square root of 2 and that a = 1. Draw a plot representing ? and ?². How many nodes are present?
3. Determine the principal quantum numbers l and m? for electrons in (a) the n=4 shell, (b) the n = 5 shell, and (c) the n= 7 shell
4. Draw representations of the general shapes for s, p, and d orbitals. Use a 3-D coordinate and be sure to indicate the sign of the wave function by shading or +/- signs. Indicate the number and location of any angular nodes in each case
5. Give the total number of nodes present in the following orbitals and indicate how many are radial and how many angular: 4p, 5d, 6f, 7g.
6. Draw a cross-sectional representation depicting radial nodes present in 4s and 5dx²-y² orbitals and show how the sign of the wavefunction changes throughout the orbital using shading or +/- signs.

Added by Erik L.

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