Chem Unit 11 - Liquids

Unit 11 - Liquids

A liquid can be described as a form of matter that has a definite volume and takes the shape of its container.

• The attractive forces between particles in a liquid are more effective than those between particles in a gas.

• This attraction is explained by intermolecular forces (dipole-dipole, London dispersion, and hydrogen bonding).

Properties of Liquids and the Kinetic-Molecular Theory

• Like gases, particles in a liquid are in constant motion.

• Liquids are more ordered than gases because of the stronger intermolecular forces and lower mobility of particles.

Properties of Liquids and the Kinetic-Molecular Theory Continued

• Relatively High Density – At normal atmospheric pressure, most substances are hundreds of times denser in a liquid state than in a gaseous state.

  • Due to the close arrangement of liquid particles.

• Relative Incompressibility – Liquids are much less compressible than gases because liquid particles are more closely packed together.

Densities and Compressibility

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• Ability to Diffuse – Any liquid gradually diffuses throughout any other liquid in which in can dissolve.

  • The constant, random motion of particles causes diffusion in liquids.

Diffusion of Liquids

• Diffusion is much slower in liquids than in gases because liquid particles are close together.

  • Also attractive forces between the particles slows their movement.

  • As temperature increases, diffusion increases.

Diffusion of Liquids Continued

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Surface Tension – A property common to all liquids is surface tension, a force that tends to pull adjacent parts of a liquid’s surface together, thereby decreasing surface area to the smallest possible size.

• The higher the force of attraction, the higher the surface tension.

Surface Tension

• Capillary action is the attraction of the surface of a liquid to the surface of a solid.

  • This attraction tends to pull the liquid molecules upward along the surface and against the pull of gravity.

Capillary Action

• Vaporization – The process by which a liquid or solid changes to a gas is vaporization.

• Evaporation is a form of vaporization.

  • Evaporation is the process by which particles escape from the surface of a nonboiling liquid and enter the gas state.

  • Evaporation occurs because the particles of a liquid have different kinetic energies.

Vaporization and Evaporation

1. ​Particles with higher kinetic energy move faster and can overcome intermolecular forces.

2. Evaporation occurs at the surface of a liquid.

Boiling is the change of a liquid to bubbles of vapor.

• Boiling occurs throughout the liquid.

Boiling

The physical change of a liquid to a solid by removal of energy as heat is called freezing or solidification.

• When a liquid is cooled, the average kinetic energy of its particles decreases.

• When energy is low enough, attractive forces pull the particles in a more orderly arrangement.

Freezing