If you increase water vapor why does the partial pressure of other atmospheric gases decreases?

I know that the atmospheric pressure depends on altitude. But wouldn't it make sense that if you increase water vapor its partial pressure would increase and therefore the total atmospheric pressure would, instead of taking away the partial pressure of other solutions. And does this mean when it is more humid or hot there are less atmospheric gases for us to breathe in?

Answer:
Think of a closed cup with hot water in it. If you increase the water vapor inside the cup, this would only increase the vapor pressure inside the cup. Remember what makes up vapor pressure? The concentrations and energy of particles. As you increase water vapor, the pressure will increase. If you are at standard conditions such as 101.31 kPa, you would be able to increase the vapor pressure inside the cup only to a certain extent before dynamic equilibrium occurs, that is where there would be a fixed amount of liquid molecules evaporating as there are gas molcules condensing. The place where this could work is at a high altitude where atmospheric pressure is low and now you can get the vapor pressure to be higher than that of the atmospheric pressure. I hope this made sense. :)

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If you increase water vapor why does the partial pressure of other atmospheric gases decreases?

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