_____3. I can draw particle diagrams to represent an atom, an element, a molecule, a compound, a mixture Atom Element Molecule Compound Mixture of 2 compounds Mixture of an element and a compound _____4. I can classify substances as a pure substance (element or compound) or as a mixture. Put each of the following examples into the correct column. Examples: C12H22O11, NaCl, Fe, salt water, air, CO2, H2, Ar, soda Element Compound Mixture _____5. I can define homogeneous mixture and heterogeneous mixture in terms of particle distribution. Definitions: homogeneous mixture heterogeneous mixture _____6. I can give an example of homogeneous and heterogeneous mixtures. Two examples of homogeneous mixtures: a. b.
_____18. I can state the 5 parts of the Kinetic Molecular Theory. The five parts of the Kinetic Molecular Theory are: a. b. c. d. e. _____19. I can define an ideal gas. Definition: ideal gas _____20. I can state the conditions of pressure and temperature under which a gas will act “ideally”. A gas will act most “ideally” under the conditions of ___________ pressure and ____________ temperature. _____21. I can state the two elements that act ideally most of the time. The two elements that act ideally most of the time are _____________ & _______________. _____22. I can explain how pressure is created by a gas. What causes gas molecules to create pressure? _____23. I can state the relationship between pressure and volume for gases (assuming constant temperature) and I can represent it graphically. At constant temperature, as the pressure on a gas increases, the volume ____________________. _____24. I can state the relationship between temperature and volume for gases (assuming constant pressure) and I can represent it graphically.. At constant pressure, as the temperature on a gas increases, the volume ____________________. _____25. I can state the relationship between temperature and pressure for gases (assuming constant volume) and I can represent it graphically.. In a fixed container (AKA “has constant volume), as the temperature on a gas increases, the pressure____________________.
_____19. I can explain and apply the meaning of SNAP as it applies to determining molecule polarity. SNAP means______________________________________________________ Why is a molecule of CH4 nonpolar even though the bonds between the carbon and hydrogen are polar? A) The shape of the CH4 molecule is symmetrical. B) The shape of the CH4 molecule is asymmetrical. C) The CH4 molecule has an excess of electrons. D) The CH4 molecule has a deficiency of electrons. Explain, in terms of charge distribution, why a molecule of water (H2O) is polar. _____20. I can determine if a molecular is polar or nonpolar. Determine which molecules are polar and which are nonpolar. Justify your answer. H2O CO2 I2 CH4 _____21. I can explain and apply the expression “like dissolves like” and give an example. “Like dissolves like” means An example of “like dissolving like” is __________________________________ ________________________________________________________________ Explain, in terms of molecular polarity, why ammonia is more soluble than methane in water at 20oC at standard pressure. _____22. I can define intramolecular forces. Definition: Intramolecular forces