Why don't we take into consideration the rotation and vibration of gas molecules on the pressure of the gas?

"Ideal gas" is jargon for "mathematical model involving point particles with mass and collisions," so it kind of defines away your question as "not askable," but that's an unsatisfying answer.

For a real gas, you get to include other stuff, like the volume of the particles, or (for a molecular gas) rotations and vibrations. Those count as additional "degrees of freedom" in statistical mechanics, and can be considered independently of the components of the velocity along the x, y, and z axes.

For molecular gasses, as you add energy, temperature increases (and along with it, the velocity of the molecules), and at certain temperatures, those rotational or vibrational modes become important.

Here's a graph of the specific heat* (i.e., change in temperature when you add energy) of diatomic hydrogen:

Source

Note that, at low temperatures, rotational and vibrational modes are not important, and the ideal gas law works surprisingly well (especially if you modify it a bit for the volume of the hydrogen). At higher temperatures, the ideal gas law will lead you astray. The surprising thing is how well it works at low temperatures.

* Technically the specific heat at constant volume