true
they have no volume and their molecular force of attraction is negligible
Ideal gases are gases with negligible intermolecular forces and molecular volumes. Real gases have intermolecular forces and have definite volumes at room temperature and pressure (RTP).
Real gases have non-zero volume and experience intermolecular forces, which contradict the assumptions of kinetic-molecular theory that gases consist of point particles with no volume and that there are no intermolecular forces present. Real gases also deviate from ideal behavior at high pressures and low temperatures, which is not accounted for in the kinetic-molecular theory.
Gases are in the gaseous state at room temperature. They have weak intermolecular forces and take the shape and volume of their container.
The intermolecular forces in gases are very weak.
Gases have neither a definite shape nor a definite volume. Liquids do not have a definite shape, but they DO have a definite volume. Gases have no or little intermolecular forces holding them together, whereas liquids do have substantial intermolecular forces.
they have no volume and their molecular force of attraction is negligible
The gas molecules interact with one another
Intermolecular forces in argon involve London dispersion forces, which are weak attractive forces caused by temporary fluctuations in electron distribution. These forces are the primary intermolecular force in noble gases like argon, given their lack of permanent dipoles.
Solids and gases are both states of matter, however they differ in their shape, volume, and intermolecular forces. A solid has a fixed shape and volume with strong intermolecular forces holding the particles closely together, while a gas has no fixed shape or volume and weak intermolecular forces allowing the particles to move freely.
Ideal gases are gases with negligible intermolecular forces and molecular volumes. Real gases have intermolecular forces and have definite volumes at room temperature and pressure (RTP).
Gases have a low boiling point because they have weak intermolecular forces that allow them to easily overcome attractive forces and transition to the gaseous phase at relatively low temperatures.
Real gases have non-zero volume and experience intermolecular forces, which contradict the assumptions of kinetic-molecular theory that gases consist of point particles with no volume and that there are no intermolecular forces present. Real gases also deviate from ideal behavior at high pressures and low temperatures, which is not accounted for in the kinetic-molecular theory.
Solids have a fixed shape and volume, liquids have a fixed volume but take the shape of their container, and gases have neither a fixed shape nor volume. These differences in structure affect their properties and behaviors. Solids have strong intermolecular forces, making them rigid and maintaining their shape. Liquids have weaker intermolecular forces, allowing them to flow and take the shape of their container. Gases have very weak intermolecular forces, allowing them to expand to fill their container and move freely.
Gases are in the gaseous state at room temperature. They have weak intermolecular forces and take the shape and volume of their container.
The intermolecular forces in gases are very weak.
Fluids and gases have weak intermolecular forces that allow particles to move past each other, enabling flow. In contrast, solids have stronger intermolecular forces that hold particles in fixed positions, preventing flow. This difference in intermolecular forces allows fluids and gases to flow easily, while solids maintain their rigid structure.