Unit 4: State of matter; Gaseous State

4.0 Investigates the behavior of the gaseous state of matter.

4.1 Uses organization of particles in three principal states of matter to explain their typical characteristics

Investigates the organization of particles in the principal states solid, liquid and gas.

Compares the macroscopic properties such as volume, density, shape( under the influence of gravity) and compressibility of solids, liquids and gases in relation to the arrangement of particles and their movement.

4.2 Uses the model of ideal gas as a means of describing the behavioral patterns of real gases.

Defines an ideal gas .

Writes the ideal gas equation and its derivatives with their terms.

Defines the term of a gas equation

States Boyle, Charles and Avogadro laws and show the consistency of the ideal gas equation.

Defines the molar volume of a gas.

Solves problems related to the ideal gas equation and its derivatives.

Determines experimentally the molar volume of oxygen.

Determines the relative atomic mass of magnesium experimentally.

4.3 Uses molecular kinetic theory of gases as a means of explaining the behavior of real gases.

States the assumptions of the molecular kinetic theory of gases.

Describe the factors affecting the pressure of a gas.

Writes expressions for mean speed, mean square speed and root mean square speed.

States the kinetic molecular equation and describes its terms.

Derives (C²)‾= 3RT/M

Describes the information given by Maxwell - Boltzmann curves for gases.

4.4 Uses Dalton law of partial pressures to explain the behavior of a gaseous mixture.

Describes the information given by Maxwell - Boltzmann curves for gases.

Explains the term partial pressure and states Dalton law of partial pressures.

Derives Dalton law of partial pressures from the ideal gas equation.

Solves problems related to Dalton law of partial pressures.

4.5 Analyses amendments to the ideal gas equation for applying it to real gases.

Defines the compressibility factor and graphically presents how this value varies with pressure in real and ideal gases.

Describes the reasons for the deviation of real gases from the behavior of ideal gases by citing assumptions of the molecular kinetic theory.

Presents van der Waals equation as an equation constructed to explain the deviation of real gases from the ideal behavior.

Describes the critical temperature.

Values the idea that scientific concepts are not static but subject to continuous improvements based on facts.