Kinetic molecular model of liquids and solids

• Temperature is a measure of average kinetic energy per particle.
• Increasing temperature increases the average kinetic energy, which causes an increase in motion.
• The greater the intermolecular forces between particles, the more difficult it is to overcome them and separate the particles from one another.
• The higher the temperature, the greater the average kinetic energy of particles.
• Intermolecular forces are responsible for the behavior of matter at different temperatures.
• At high temperatures, particles have enough thermal energy to overcome intermolecular forces and move freely through the liquid or gas phase.
• As temperature decreases, the average kinetic energy also decreases, causing particles to move slower and have less ability to overcome intermolecular forces.
• At high temperatures, the average kinetic energy of particles can be great enough to overcome the attractive forces holding molecules together.
• As temperature decreases, particles lose some of their thermal energy and become more likely to form bonds with neighboring molecules.
• Stronger intermolecular forces lead to higher boiling points and melting points.
• Stronger intermolecular forces lead to stronger cohesion among molecules, resulting in higher boiling points and melting points.
• At low enough temperatures, all substances will eventually solidify into a crystalline structure due to their strong intermolecular forces.
• As temperature decreases, particles lose some of their thermal energy and become less able to overcome intermolecular forces.
• As temperature decreases, the average kinetic energy of particles also decreases.
• When the average kinetic energy becomes low enough, particles can no longer overcome intermolecular forces and become trapped in their positions relative to other particles.
• Solidification occurs when the average kinetic energy becomes too small to allow particles to vibrate past each other.
• Weaker intermolecular forces result in lower boiling points and melting points.
• When the temperature reaches the melting point, there is not enough thermal energy to overcome all of the intermolecular forces, causing the substance to solidify.
• When the average kinetic energy becomes less than the strength of the intermolecular forces, the substance will condense into a liquid or solid state.
• Increasing pressure increases the number of collisions between particles, leading to stronger intermolecular forces and increased density.