What is the Difference Between Px Py and Pz Orbitals?

The difference between Px, Py, and Pz orbitals lies in their orientation in space. All three orbitals are part of the P subshell and have a dumbbell shape. However, they are oriented along different axes:

1. Px Orbital: This orbital is oriented along the x-axis, meaning it has lobes that lie along the x-axis.
2. Py Orbital: This orbital is oriented along the y-axis, with lobes lying along the y-axis.
3. Pz Orbital: This orbital is oriented along the z-axis, with lobes lying along the z-axis.

The Px, Py, and Pz orbitals have similar shapes and sizes, and their sizes change with the increase of the n value. The key difference between these orbitals is their orientation in space, which affects the type of bond they form. For example, Px and Py orbitals tend to form pi bonds, while Pz orbitals form sigma bonds.

Comparative Table: Px Py vs Pz Orbitals

The key difference between Px, Py, and Pz orbitals lies in their orientation in space. All three orbitals have a dumbbell shape and contain two lobes, but they are oriented along different axes. Here is a table summarizing their differences:

These orbitals are part of the p subshell, which consists of three orbitals: Px, Py, and Pz. The p subshell can hold a total of 6 electrons.