The 2p_x, 2p_y, and 2p_z orbitals of an atom have identical shapes but differ in their spatial orientations. These orbitals belong to the same principal energy level (n=2) and are part of the p orbital set, which means they have the same shape, characterized by a dumbbell-like structure. However, each of the orbitals is oriented along a different axis in three-dimensional space:

• The 2p_x orbital is oriented along the x-axis.
• The 2p_y orbital is oriented along the y-axis.
• The 2p_z orbital is oriented along the z-axis.

This orientation difference is crucial for understanding how electrons can occupy these orbitals and how they can overlap with orbitals from other atoms to form chemical bonds. Despite their different orientations, all three 2p orbitals have the same energy level, making them degenerate orbitals in the absence of an external electric or magnetic field.