What is the difference between three states of matter
Objectives Differentiate between the three main states of matter. Describe different properties of matter. Describe the properties of a solid, a liquid, and a gas. Describe the properties of a solid and a liquid.
Describe the properties of gases and liquids. Understand the transitions between states of matter. Understand how matter changes from one state to another and what affects the change. Describe the processes of evaporation and condensation. Describe the processes of melting and solidification. Describe the processes of freezing and melting.
Explain cohesion. How many different phases of matter are there? What are the phases of matter? Question ea. Question So in this question, we have to distinguish between solids liquids and gases on the basis of the The molecule or let's look at this one by one as I know in solids the molecules here.
They are very tightly packed. I'm a stereotype chick back. There is no all we can say very less intermolecular space. So intermolecular space is very less and there is a high force of attraction.
That is we can say intermolecular force of cohesion is very high and that is why the molecules do not move. That is the only way Rick along about the mean position and the solid has a definite shape and volume. Let's look at the next one in liquids in liquids.
The molecules are less tightly packed. As we compare it with the solid in comparison to the solid are less likely back so they have less.
Income water cooler force of attraction and intermolecular distances here in case of Liquids then that in solids so they do not have a definite shape. No definite shape, but yes, they acquire the shape of the container in which they have they are contained so they have a definite volume.
Adam given temperature. Let's move on to the gases gases the molecules of so far apart. Its volume is usually greater than that of its corresponding solid water is a well-known exception to this rule.
The highest temperature at which a particular liquid can exist is called its critical temperature. This process of a liquid changing to a gas is called evaporation. Gas molecules have either very weak bonds or no bonds at all, so they can move freely and quickly. Because of this, not only will a gas conform to the shape of its container, it will also expand to completely fill the container.
Gas molecules have enough kinetic energy that the effect of intermolecular forces is small or zero, for an ideal gas , and they are spaced very far apart from each other; the typical distance between neighboring molecules is much greater than the size of the molecules themselves.
A gas at a temperature below its critical temperature can also be called a vapor. A vapor can be liquefied through compression without cooling. It can also exist in equilibrium with a liquid or solid , in which case the gas pressure equals the vapor pressure of the liquid or solid. A supercritical fluid SCF is a gas whose temperature and pressure are greater than the critical temperature and critical pressure.
In this state, the distinction between liquid and gas disappears. A supercritical fluid has the physical properties of a gas, but its high density lends it the properties of a solvent in some cases. This can be useful in several applications.