Final answer:
The gaseous state is characterized by the lowest density and is influenced by temperature and pressure changes. The liquid state has an indefinite shape and a higher density. The solid state has particles that are less free to move around than in the other states.
Step-by-step explanation:
1. This state is characterized by the lowest density of the three states. This describes the gaseous state, as gas particles are spread out and not closely packed together.
2. This state is characterized by an indefinite shape and high density. This refers to the liquid state, which adapts its shape to fit its container but has particles that are still relatively close together, contributing to a higher density than gases.
3. Temperature changes significantly influence the volume of this state. This is typical of the gaseous state, as gases expand or contract significantly with temperature changes according to the Ideal Gas Law.
4. Pressure changes influence the volume of this state more than the other two states. This also pertains to the gaseous state, where pressure changes can lead to notable volume changes, as predicted by the Ideal Gas Law.
5. In this state, constituent particles are less free to move around than in other states. This describes the solid state, where particles are in fixed positions and can only vibrate in place.