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Transcript
Unit Objectives- States of Matter
Chemistry Level 4
1. Explain how the Kinetic Molecular Theory describes the behavior of gases
(diffusion, effusion, compressibility, expansion, fluidity, low density).
2. Explain the relationship between temperature and average kinetic energy,
and justify why the Kelvin temperature scale is used to describe gases.
3. Compare and contrast an ideal and a real gas.
4. Identify real gases that behave like ideal gases under specific conditions.
5. Explain the relationship between the pressure, volume, and temperature of a
gas (Boyle’s, Charles’, & Gay-Lussac’s Laws), supported by the kinetic
molecular theory.
6. Explain Avogadro’s hypothesis and use it to solve problems involving gas
stoichiometry.
7. Perform calculations using the combined and ideal gas laws to solve for
pressure, volume, temperature, number of moles of a gas, density, and molar
mass.
8. Explain Dalton’s Law of Partial Pressures and be able to calculate partial
pressures.
9. Explain Graham’s Law of Effusion and justify with calculations.
10. Explain the difference between a solution, colloid, and a suspension.
11. Define a solute, a solvent, and a solution.
12. Describe the process by which solutes dissolve in solvents.
13. Determine if a solute will be able to dissolve in a particular solvent.
14. Describe different factors that affect the rate of dissolution.
15. Identify electrolytes and non-electrolytes and explain why they are classified
as so.
16. Explain the different levels of saturation in a solution.
17. Interpret a solubility curve and use it to determine saturation values of
solutes at different temperatures.
18. Calculate the concentration of a solution in terms of molarity and molality.
19. Calculate the new concentration of a dilute solution.
20. Explain how the boiling point, freezing point, and vapor pressure of a
solution differ from those of the pure solvent.
21. Calculate the new freezing point and boiling point of a solution.
22. Perform stoichiometric calculations given the molarity of the reactants.
23. Write net ionic equations.