Recall: Each subshell has a unique shape based on it's angular momentum quantum number (L).
For dx2−y2: For the d subshell, L = 2, which means the orbital shape is a four-leaf clover. x2–y2 tells us that it's oriented along the x and y axis. The boundary surface for a dx2−y2 orbital would look like this:
Sketch the boundary surface of a dx2−y2 and a py orbital. Be sure to show and label the axes.
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