Difference Between Solid Liquid and Gas

Difference Between Solid Liquid and Gas - Definition with FAQs

Edited By Team Careers360 | Updated on Jul 02, 2025 05:02 PM IST

Anything which occupies space and has a mass is referred to as matter. Everything that we see around us like, water, air, animals, clothes and more, is made up of matter. The state of the matter is also a physical property of matter. Three main forms, namely solid, liquid and gas, may be present for the matter. Some compounds are present as room temperature gases (oxygen, carbon dioxide), and others are available as fluids, such as water and mercury metal at room temperature.

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Solids
Liquids
Gases
Comparison between solids, liquids and gas

At normal temperatures, many metals exist as solids. Every substance exists in any of these forms. A substance can undergo a change from one state to another. The properties of solids, liquids, and gases are different from each other. Mostly due to their different configurations and the cohesive force between the molecules, solids, liquids and gases are distinct. Solid molecules are packaged together closely and their cohesive forces are strong. Solids cannot therefore fluctuate.

Compared to solids, liquid molecules are much further apart. Therefore, fluids also have weaker cohesive forces between fluid molecules, compared to solids. Compared to solid and liquid molecules, gas molecules are far more distant. There are also very lowest cohesive interactions among its molecules. This gives the flow and compression of gases. This article makes a comparison between solids, liquids and gases.

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Solids

The solids are the type of material with a rigid structure that opposes shape and volume changes. The particles in solids are tightly bound and regularly arranged. Its particle vibrates and twists frequently, but does not reveal any movement, as it is tight-knit. Solid is the matter with the highest molecular attraction. Furthermore, it is somewhat difficult to compress because their molecules have fewer gaps. The particles in solids are very close together and can thus not be squeezed or squashed normally.

Attraction forces between the particles keep and hold them together. The solid particles are regularly organized. They only move about a fixed place by vibrating. This provides solids with a stable form and does not fluidize like liquids. The warmer the solid gets, the more rapid the vibration of its particles. This means that when heated, solids expand. Ice is the solid form of water. Even if it is removed from its container, Ice maintains its form when it is frozen. But ice differs from most solids. Its molecules are packaged less tightly than in liquid water. Therefore, Ice floats. Ice floats.

Solids

Examples: Stone, Pencil, chair

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Liquids

Liquids are fluids, they have a continuous volume, no fixed form. Liquids take the form of the container in which they are present. Liquid has a minimum surface area because of the fluid surface tension. The particles in liquids are randomly arranged and closely related to many of their neighbour particles. Some gaps exist, but fluids normally cannot be compressed or crushed.

The liquid particles have sufficient energy to release some of the attraction forces between the particles. So liquid particles can move and move about, allowing liquids to flow and to be poured. The gaseous form or condition of the water is water vapour. Water vapour is invisible, as opposed to ice or water. Whenever we breathe, we exhale water vapour. We cannot see water vapour when we exhale, but we can see the water vapour condensing (which becomes liquid).

Liquids

Examples: Water, kerosine, honey

Gases

Gas is a state that is freely diffused in every direction. Gases thus fill in whatever quantity the whole space available. It comprises no particular shape or volume of the particles. They are loosely held, and they have a lot of space for free and continuous movement between them. Particulate matter in gases is widely separated and organized at random to make it easy to compress. The particles in a gas have sufficient energy to overcome the attractive forces between the particles thus they are free to flow in any direction. They move fast in straight lines, colliding with one another and their container walls.

Gases

Examples: Oxygen, methane, air

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Comparison between solids, liquids and gas

Rigidity

Solids are very rigid in nature. On the other hand, liquids and gases are not rigid.

Fluidity

There is no ability for solids to flow. Liquids can flow from higher to lower levels (concentration). In every direction, gas can flow.

Shape and volume

Because of their hard structure, solids have distinct shapes and volumes. Liquids have a certain volume, but they lack a definite shape and they gain the shape of the container in which they are stored. There is no clear shape or volume of gases.

Intramolecular interaction

Particles in a solid are tightly packaged and can vibrate, but not move. In liquids, intermolecular interaction is considerably weaker than that of solids so that there is sufficient energy for molecules or particles to move. In the case of gases, the intermolecular bond is not significant, so that the gas molecules and particles can travel freely and fast.

Compressibility

It is not possible to compress solids. and liquids are compressible. Gasses can be severely compressed.

Storage

Without a container or vessel solids can be easily stored. Without a vessel or container, liquids cannot be stored. Vessels are required to store gases.

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Frequently Asked Questions (FAQs)

1. What is the difference between various states of matter?

The solid substance consists of densely packed particles. A solid retains its form and the particles can't circulate freely. Liquid matter consists of particles that are loosely packaged. The gaseous matter is made of so loosely packed particles that it has no definable shape or volume.

2. What are the properties of liquids, solids, and gases?

Solids - reasonably rigid, distinct size and form. The atoms and molecules in a solid are fixed to one another. Ex: Ice

Liquids - a certain volume but capable of changing form through flow. The atoms and molecules are loosely linked in a liquid. Ex: Water

Gasses - no specific shape or volume. Ex: Hydrogen

3. Write the difference between solid and liquid or solid liquid gas difference.

Solids can diffuse into liquids and have a specific volume. In addition, their compression is insignificant. They have the lowest interparticle spacing and great density. There is a very strong interparticle force of attraction. Moreover, the least kinetic energy is available. The molecules are finally packed in a certain manner. Liquid has medium intermolecular interactions and has a definite volume. Moreover, when compared to solids the diffusion is higher. In addition, the density is moderate. They also flow smoothly since they are less rigid. Indeed, at a particular temperature, the kinetic energy of particles is superior to solids. The intermolecular forces of gases are negligible. They have no definite volume. They can flow smoothly since they have little rigidity. The molecules are poorly packaged, so they fill the container, but they do not have a particular structure and intermolecular space.is very less.

4. Why are solids and liquids incompressible whereas gases are compressible?

The intermolecular space is quite large.in gases. So, gasses are compressible. But solids and liquids are not compressible because of the smaller intermolecular space in solids.

5. What are the different states of water?

Water can exist as solid, liquid and gas. It is solid at low temperatures (under 0°C). Ice is the solid form of water. It is a liquid at "normal" temperatures (from 0°C to 100°C). Water is a gas at temperatures over 100°C (steam). Water vapour is the gaseous form of water. The condition of the water depends on the temperature. Each state has its very special physical features (solid, liquid and gas).

6. What are intermolecular forces in solid liquid and gas?

Intermolecular forces are important as the properties of solids and liquids depend on them. Gas particles have a force called Van Der Waals force.

7. What are the three main states of matter?

The three main states of matter are solid, liquid, and gas. These states differ in their physical properties due to the arrangement and behavior of particles within them.

8. How do particles behave differently in solids, liquids, and gases?

In solids, particles are tightly packed and vibrate in fixed positions. In liquids, particles are close together but can move around each other. In gases, particles are far apart and move freely in all directions.

9. What is the primary factor that determines the state of matter?

The primary factor determining the state of matter is the balance between the kinetic energy of particles and the attractive forces between them. Temperature and pressure play crucial roles in this balance.

10. Can a substance exist in all three states of matter?

Yes, many substances can exist in all three states of matter depending on temperature and pressure conditions. Water is a common example, existing as ice (solid), liquid water, and water vapor (gas).

11. How does the volume of a substance change as it transitions from solid to liquid to gas?

Generally, the volume increases as a substance transitions from solid to liquid to gas. This is due to the increasing space between particles as they gain more kinetic energy.

12. How does the boiling point relate to the transition between liquid and gas states?

The boiling point is the temperature at which a liquid changes to a gas at a given pressure. It marks the transition between the liquid and gas states of matter.

13. What is the main difference in particle movement between liquids and gases?

In liquids, particles can move around each other but remain in close contact. In gases, particles move freely with large spaces between them, allowing the gas to expand to fill its container.

14. What is the process called when a solid changes directly to a gas without passing through the liquid state?

This process is called sublimation. An example is dry ice (solid carbon dioxide) changing directly into carbon dioxide gas at room temperature and pressure.

15. How does the density of a substance typically change between solid, liquid, and gas states?

Density typically decreases from solid to liquid to gas as the particles become less tightly packed. However, there are exceptions, such as water, which is less dense as a solid (ice) than as a liquid.

16. How does pressure affect the state of matter?

Increasing pressure generally favors the more condensed states of matter. For example, high pressure can cause a gas to liquefy or a liquid to solidify by forcing particles closer together.

17. How does surface tension relate to the liquid state of matter?

Surface tension is the tendency of liquid surfaces to shrink into the minimum surface area possible. It results from the cohesive forces between liquid molecules and is responsible for phenomena like water beading on surfaces.

18. What is the melting point, and how does it relate to states of matter?

The melting point is the temperature at which a solid changes to a liquid at a given pressure. It marks the transition between the solid and liquid states of matter.

19. How does the kinetic molecular theory explain the behavior of particles in different states of matter?

The kinetic molecular theory states that particles are in constant motion. In solids, they vibrate; in liquids, they move and collide with nearby particles; in gases, they move rapidly and collide with container walls and other particles.

20. What is viscosity, and how does it differ among the states of matter?

Viscosity is a measure of a fluid's resistance to flow. Gases have very low viscosity, liquids have higher viscosity, and solids (which don't flow) have infinite viscosity.

21. What is diffusion, and how does it differ in solids, liquids, and gases?

Diffusion is the movement of particles from an area of high concentration to an area of low concentration. It occurs fastest in gases, slower in liquids, and very slowly in solids due to differences in particle mobility.

22. How does the arrangement of particles differ between crystalline and amorphous solids?

In crystalline solids, particles are arranged in a regular, repeating pattern. In amorphous solids, particles are arranged randomly without a definite pattern.

23. How do intermolecular forces affect the state of matter?

Stronger intermolecular forces tend to keep particles closer together, favoring solid and liquid states. Weaker forces allow particles to separate more easily, favoring the gas state.

24. How does the concept of cohesion differ between solids, liquids, and gases?

Cohesion, the attraction between like molecules, is strongest in solids, weaker in liquids, and very weak in gases. This difference contributes to the distinct properties of each state of matter.

25. What is the triple point of a substance?

The triple point is the unique combination of temperature and pressure at which a substance can exist simultaneously in all three states of matter: solid, liquid, and gas.

26. How does the concept of latent heat relate to changes in states of matter?

Latent heat is the energy absorbed or released by a substance during a change in state without a change in temperature. It's crucial in phase transitions like melting (fusion) and vaporization.

27. How do quantum mechanical effects influence the behavior of matter at extremely low temperatures, leading to states like Bose-Einstein condensates?

At extremely low temperatures, quantum mechanical effects become dominant, leading to exotic states of matter like Bose-Einstein condensates. In these states, particles behave more like waves and can occupy the same quantum state, exhibiting properties distinct from classical solids, liquids, or gases.

28. Why do gases easily compress while liquids and solids do not?

Gases are easily compressible because there is a lot of empty space between their particles. Liquids and solids have particles much closer together, leaving little room for compression.

29. What is the difference between evaporation and boiling?

Evaporation occurs at the surface of a liquid at any temperature, while boiling occurs throughout the liquid when the vapor pressure equals the atmospheric pressure at the boiling point.

30. What is plasma, and how does it relate to the three main states of matter?

Plasma is often considered the fourth state of matter. It's an ionized gas where electrons are stripped from atoms, creating a mixture of charged particles. It has properties distinct from solids, liquids, and gases.

31. How does the concept of vapor pressure relate to the liquid and gas states?

Vapor pressure is the pressure exerted by a vapor in equilibrium with its liquid phase at a given temperature. It increases with temperature and plays a crucial role in phase transitions between liquid and gas states.

32. What is supercritical fluid, and how does it blur the line between liquid and gas states?

A supercritical fluid is a substance at a temperature and pressure above its critical point, where distinct liquid and gas phases do not exist. It can expand like a gas but has a density similar to a liquid.

33. What is the difference between an exothermic and endothermic phase change?

An exothermic phase change releases heat to the surroundings (e.g., condensation), while an endothermic phase change absorbs heat from the surroundings (e.g., evaporation).

34. How does the ideal gas law relate to the behavior of gases?

The ideal gas law (PV = nRT) describes the relationship between pressure, volume, amount, and temperature of an ideal gas. It's based on assumptions about gas particle behavior and is most accurate for gases at low pressures and high temperatures.

35. What is Brownian motion, and how does it relate to particles in liquids and gases?

Brownian motion is the random movement of particles suspended in a fluid, resulting from collisions with fast-moving molecules of the fluid. It's more pronounced in gases than in liquids due to greater particle mobility.

36. What is the difference between melting and freezing in terms of energy transfer?

Melting (solid to liquid) absorbs energy from the surroundings, while freezing (liquid to solid) releases energy to the surroundings. Both occur at the same temperature for a given substance at a specific pressure.

37. How does atmospheric pressure affect the boiling point of liquids?

Higher atmospheric pressure increases the boiling point of liquids by exerting more force on the surface, requiring more energy for vapor bubbles to form. Lower pressure decreases the boiling point.

38. What is the difference between intensive and extensive properties of matter, and how do they relate to states of matter?

Intensive properties (like melting point and density) don't depend on the amount of substance and are often used to characterize states of matter. Extensive properties (like mass and volume) depend on the amount of substance present.

39. How does the concept of entropy relate to the different states of matter?

Entropy, a measure of disorder, generally increases as matter changes from solid to liquid to gas. Gases have the highest entropy due to their particles' greater freedom of movement.

40. What is the significance of critical temperature and pressure in understanding states of matter?

The critical temperature is the highest temperature at which a substance can exist as a liquid. Above this temperature, no amount of pressure can liquefy the gas. The critical pressure is the pressure required to liquefy a gas at its critical temperature.

41. How do phase diagrams help in understanding the relationships between states of matter?

Phase diagrams visually represent how temperature, pressure, and physical state are related for a given substance. They show phase boundaries and help predict state changes under various conditions.

42. What is supersaturation, and how does it relate to the stability of different states of matter?

Supersaturation is a state where a solution contains more dissolved material than could be dissolved under normal circumstances. It's an unstable state that can lead to rapid crystallization, demonstrating the delicate balance between dissolved and solid states.

43. How does the concept of partial pressure apply to gases in mixtures?

Partial pressure is the pressure exerted by a particular gas in a mixture. The total pressure of a gas mixture is the sum of the partial pressures of its components, as described by Dalton's law of partial pressures.

44. What is the difference between elastic and inelastic collisions in gases, and how do they affect gas behavior?

In elastic collisions, kinetic energy is conserved, while in inelastic collisions, some kinetic energy is converted to other forms. Most gas particle collisions are nearly elastic, contributing to the uniform distribution of gas particles in a container.

45. How does the concept of mean free path differ for particles in solids, liquids, and gases?

Mean free path is the average distance a particle travels between collisions. It's very short in solids, slightly longer in liquids, and much longer in gases due to the increasing space between particles in each state.

46. What is the relationship between temperature and the average kinetic energy of particles in different states of matter?

Temperature is directly proportional to the average kinetic energy of particles in all states of matter. Higher temperatures mean higher average kinetic energy, regardless of the state.

47. How does the concept of vapor pressure curve help in understanding phase transitions?

The vapor pressure curve on a phase diagram shows the relationship between vapor pressure and temperature for a substance. It helps predict at what conditions phase transitions will occur and whether a substance will exist as a solid, liquid, or gas under given conditions.

48. What is supercooling, and how does it challenge our understanding of phase transitions?

Supercooling occurs when a liquid is cooled below its freezing point without solidifying. This metastable state challenges the simple view of phase transitions and demonstrates the importance of nucleation in the freezing process.

49. How do intermolecular forces affect the boiling points of different substances?

Stronger intermolecular forces result in higher boiling points because more energy is required to overcome these forces and separate the molecules into the gas phase.

50. What is the difference between evaporation and sublimation in terms of energy changes?

Both evaporation and sublimation involve the transition to the gas phase, but evaporation occurs from the liquid state while sublimation occurs directly from the solid state. Sublimation typically requires more energy as it involves breaking stronger intermolecular bonds.

51. How does the concept of dynamic equilibrium apply to phase transitions?

Dynamic equilibrium in phase transitions refers to a state where the rate of particles leaving one phase equals the rate of particles returning to that phase. This concept is crucial in understanding processes like evaporation and condensation at the molecular level.

52. What is the significance of the heat of vaporization, and how does it relate to intermolecular forces?

The heat of vaporization is the energy required to vaporize a unit quantity of a liquid at its boiling point. It's directly related to the strength of intermolecular forces

53. How does pressure affect the spacing and movement of particles in different states of matter?

Increased pressure generally decreases the spacing between particles and restricts their movement. This effect is most pronounced in gases, less so in liquids, and least in solids due to their different compressibilities.

54. What is the relationship between molecular structure and the state of matter a substance typically exists in at room temperature?

Molecular structure influences intermolecular forces, which in turn affect the state of matter. Generally, substances with stronger intermolecular forces (like those with hydrogen bonding or larger molecules) tend to be liquids or solids at room temperature, while those with weaker forces tend to be gases.

55. How does the concept of surface area to volume ratio relate to the behavior of matter in different states?

The surface area to volume ratio is highest for gases, lower for liquids, and lowest for solids. This ratio affects properties like reaction rates, evaporation rates, and heat transfer, which are generally faster or more efficient for substances with higher surface area to volume ratios.

56. What is the role of nucleation in phase transitions, particularly in the formation of solids from liquids?

Nucleation is the initial process in the formation of a new thermodynamic phase or structure. In the transition from liquid to solid, nucleation sites serve as starting points for crystal growth. Understanding nucleation is crucial for explaining phenomena like supercooling and the formation of crystalline structures.