# Simulation: Probabilistic Interpretation of Atomic Orbitals (Dry Lab)

- Page ID
- 65240

\( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)

\( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)

\( \newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\)

( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\)

\( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\)

\( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\)

\( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\)

\( \newcommand{\Span}{\mathrm{span}}\)

\( \newcommand{\id}{\mathrm{id}}\)

\( \newcommand{\Span}{\mathrm{span}}\)

\( \newcommand{\kernel}{\mathrm{null}\,}\)

\( \newcommand{\range}{\mathrm{range}\,}\)

\( \newcommand{\RealPart}{\mathrm{Re}}\)

\( \newcommand{\ImaginaryPart}{\mathrm{Im}}\)

\( \newcommand{\Argument}{\mathrm{Arg}}\)

\( \newcommand{\norm}[1]{\| #1 \|}\)

\( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\)

\( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\AA}{\unicode[.8,0]{x212B}}\)

\( \newcommand{\vectorA}[1]{\vec{#1}} % arrow\)

\( \newcommand{\vectorAt}[1]{\vec{\text{#1}}} % arrow\)

\( \newcommand{\vectorB}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)

\( \newcommand{\vectorC}[1]{\textbf{#1}} \)

\( \newcommand{\vectorD}[1]{\overrightarrow{#1}} \)

\( \newcommand{\vectorDt}[1]{\overrightarrow{\text{#1}}} \)

\( \newcommand{\vectE}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{\mathbf {#1}}}} \)

\( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)

\( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)

Name: ______________________________

Section: _____________________________

Student ID#:__________________________

The purpose of this exercise is to increase your familiarity with the wavefunctions of the hydrogen atom and how they relate to the probability function and electronic distribution. Modern quantum theory does not treat electrons as particles at all, but rather as waves (or more specifically, their probability distributions behave as waves). In the computer simulations of this worksheet, hydrogen-like orbitals are used, because these are the only atomic wavefunctions which can be exactly calculated. We will use two simulators in this worksheet:

- Simulation 1: Histograms: "http://chem.Libretexts.org/Bird/Sim%3A_At...tal_Histograms"
- Simulation 2: Analytical Results: "http://chem.Libretexts.org/Bird/Sim%3A_Atomic_Orbitals"

## Simulation 1: Constructing and Interpreting Histograms

When you link above for simulation 1, a new tab will open. This simulation is based on the following hypothetical experiment, and represents one of two interpretations of the quantity (\(ψ^2\)). This interpretation treats the electron as a localized particle, moving somewhat randomly, but more likely to be found in certain regions of space than others according to the wave function describing it. The histogram, a particular type of graph showing distributions, which is shown to the right of the diagram of the electron sightings, plots the number of these sightings as a function of distance from the nucleus in small increments.

Select orbitals by clicking on their buttons. (Please note that the labels on the buttons are correctly written, for example 2p_{x} is written with the "x" shown as a subscript. In your table, you too should write them correctly!) Also note that some of the orbitals show nothing if you try to view them: think about why!

You can start to work on a new orbital whenever you like by making another choice. Initially, by default, a sighting will be recorded each time you click on the "Shutter" button. Clicking in the "Auto" box makes the program run automatically, marking sightings as quickly as the program can generate them. You can stop this any time you like by clicking on the "Shutter" button. Allow the diagrams to develop for several minutes until you are sure of their appearance.

**Sketch the electron scatter diagram and the histogram for each orbital (on extra sheets) and hand them in with your worksheet. Also, describe them in words distinguishing between those features which are significant and will be common to repeated runs on the same orbital, and those which are not.****Fill in the following table with the information can get from this simulation; keep in mind that you may not see all modes due to the perspective down from the z-axis.**

Orbital |
\(n\) |
\(l\) |
\(m_l\)* |
# radial nodes |
# angular nodes |
Most probable radius |
least probable radii |
---|---|---|---|---|---|---|---|

\(1s\) |
|||||||

\(2s\) | |||||||

\(2p_x\) | |||||||

\(2p_y\) | |||||||

\(2p_z\) | |||||||

\(3s\) | |||||||

\(3p_x\) | |||||||

\(3p_y\) | |||||||

\(3p_z\) | |||||||

\(3d_{xy}\) | |||||||

\(3d_{xz}\) | |||||||

\(3d_{yz}\) | |||||||

\(3d_{x^2-y^2}\) | |||||||

\(3d_{z^2}\) |

*remember that you cannot always assign a specific \(m_l\) value to each orbital. See here for more details.

## Using the Atomic Orbital Simulation

- Simulation 2: Analytical Results: "http://Libretexts.org/Bird/Sim%3A_Atomic_Orbitals"I

In this second part of the experiment, you will be examining the wave functions in more detail to reinforce your understanding of material from the text. The applet below allows you to display slices of constant z-coordinate, which you can set, through a number of different orbitals. The image which is displayed illustrates the other way of interpreting the wave function, that is, treating the electron as a delocalized "cloud" whose density is related to ψ. The brightness of the color that you see is related (logarithmically, for practical reasons) to the value of ψ^{2}. The brightest regions correspond to high "electron density". The color used in the different regions is determined by the sign of ψ: red is positive, blue is negative. The nucleus of the atom is shown as a yellow spot. Remember, PLEASE, that this sign is COMPLETELY unrelated to the sign of the charge on the electron.

If you are just experimenting, to get a sense of the three-dimensional shape of an orbital, your choice of z-coordinate(s) should be guided by the scale shown below the image. Imagine the three- dimensional orbitals (which have been scaled to appear a reasonable size) centered in a cube which has faces which are the size of the image. (The questions below give specific values of z to use.)

Once you have displayed the section you want, you can find out ψ, (radial) and (angular) for any point in the section by moving the cursor (mouse pointer) to it and then clicking the left mouse button. The program gives a continuous read-out of the Cartesian and polar coordinates to help you while you are positioning the mouse. You will need a very steady hand to position the cursor on a specific pixel, but there is an alternative. Once you have selected any point with the mouse, a second cursor (a small cross) appears. You can move it independently using the arrow keys: it moves one pixel each time you press a key. To get its position and the related data, press ENTER. (In order to move it quickly, either hold down the appropriate arrow key, or use the mouse again.)

If you scroll the applet off the screen and back again, the panel which shows the mouse position etc may disappear. It will reappear when you select an orbital or a z value. In general, the ψ values shown will not be valid until after you click somewhere on the contour plot.

The relation between the Cartesian and polar coordinate systems is shown in the figure below.

*Diagram showing the polar coordinate system*

## Q3: On the three-dimensional character of the orbitals

Display the section of the 3s orbital at z = 0. Sketch what you see. By using the mouse find and report the radii of the nodes. Now change z by 50 pm intervals up to 500. Where do the nodes go, and why?

## Q4: On the shape of nodal surface of the \(3d_{z^2}\) orbital

Display the section of the 3d_{z2} orbital at z = 0. Sketch and describe what you see. Now change z by 100 pm intervals up to 1000. Find, using the mouse, the approximate theta (q) values for the node. How does this relate to what you know of the three-dimensional shape of the 3d_{z2} orbital.

## Q5: On the shape of nodal surface of the \(3d_{z^2}\) orbital

Display the section of the 3d_{xy} orbital at z = 0. Sketch what you see. By trial and error find and report the coordinates of the maximum and minimum values of ψ. (Just do the antinode in the quadrant with x and y both positive. Figure the other three out from the symmetry of the orbital.)

## Q6: On the three-dimensional shape of the \(3d_{xz}\) orbital and polar coordinates

Investigate a series of sections through the 3d_{xz} orbital. Change z by 50 pm intervals up to 200 and by 100 thereafter up to 1000. Find, by trial and error with the mouse, the coordinates of the maximum value of ψ on each section. Determine r for the overall maximum from a graph of ψ vs r. Compare it with the value from question 5 - why should it be the same?

## Q7: From Simulated Histogram

Why when you selected the 2p_{z}, 3d_{xz} or 3d_{yz }orbitals in the histogram simulation, nothing showed up?

## Q8: On the Radial Probability Functions

Select the 2p_{x} orbital with z = 0. Sketch what you see. Using the mouse to read off the values from the diagram keeping y = 0 and varying x, plot a graph of 4.p.r^{2}.ψ^{2} vs r. What is the relation of this graph to the histogram for the same orbital from the first part of the dry lab?

## Q9: On the radial and angular parts of the ψ functions

Repeat the procedure in Exercise 8 but read off ψ values along the line x = y (ie at 45^{o}) between the axes. Compare this plot to the one you got from Exercise 8, in particular, where are the maxima and how do the values relate in general to those you found for question 8. Are your results consistent with the functions for the radial and angular parts of ψ as illustrated in the text?