Note: This is "stuff" you already know. There was an ALEKS requirement to get into this course. ALL of this fundamentals stuff is really what was tested in ALEKS - so you should have this stuff down. If not, get busy learning it (again).
Students will be able too...
| Outcome Topic | Dr. McCord COMMENTS... | |
|---|---|---|
| 1 | Name simple ionic compounds based on the names of the cation and anion. | |
| 2 | Name the general/common cations, anions, and polyatomic ions used in this course. | |
| 3 | Name simple binary covalent compounds using proper prefixes. | |
| 4 | Provide both the chemical formula and name for the first 10 alkanes (hydrocarbons). | |
| 1 | Write a complete chemical formula, including if necessary hydrates of water. | |
| 2 | Calculate the molar mass of a given compound (chemical formula). | |
| 3 | Calculate the percent composition of a chemical compound. | |
| 4 | Explain the difference in atoms, molecules, and formula units for a given compound. | |
| 5 | Calculate microscopic amounts (molecules and atoms) contained within macroscopic amounts (grams or pounds). | |
| 6 | Determine the empirical formula for a compound from percent composition data. | |
| 1 | Write, balance, and label a chemical reaction using whole number coefficients. | balance any equation - supply the correct coefficients |
| 2 | Explain the role of the stoichiometric coefficients. | |
| 3 | Explain the difference in the two terms "limiting reactant" and "reactant in excess". | |
| 4 | Correctly identify the limiting reactant of a given reaction. | |
| 5 | Calculate the yield (both absolute and percentage) of a product in a chemical reaction. | Figure (calculate) all the amounts of products made using the limiting reactant. |
| 6 | Calculate the excess amount of the reactant that is in excess for a chemical reaction. | When a limiting reaction is run, HOW much of the excess reactant(s) still remains? aka what are the leftovers? |
| 7 | Qualitatively (microscopic illustrations, chemical reactions) and quantitatively express the conservation of mass and conservation of atoms for chemical processes. | |
| Numbers 7 and 8 below were brought in from the Gases Outcomes (it is still stoichiometry) | ||
| 7 | Apply the concept of the gas laws to gas phase reactions. | When we say - calculate "amounts" amounts can be moles, grams, kg, lbs, liters, pressure, etc... "AMOUNT" manifest themselves in varioius ways. FOR GASES... moles of gas can be stated in pressure and/or volume units as well. |
| 8 | Perform stoichiometric calculations using gas properties, masses, moles, limiting reagents, and percent yield. | |
Students will be able too...
| Outcome Topic | Directly Relates To... | 1 | Describe pressure from a macroscopic and microscopic perspective. | Know the PHYSICAL way in which pressure is defined and calculated. (force/area) |
|---|---|---|
| 2 | Relate Boyles, Charles', and Avogadro's gas laws to observations of gas behavior. | Know all the gas laws and how the 4 state functions of amount in moles (n,), pressure (P), volume (V), and temperature (T) interrelate. "Knowing" means you will do many calculations using these state function variables. |
| 3 | Calculate the values for state functions (n, V, T, P) using the ideal gas equation. | |
| 4 | Define the conditions of STP and SATP. | Know the actual values for STP and SATP |
| 5 | Relate the number density and mass density for a given gas, including quantitative calculations such as mass, molecular weight, and density. | density of gases is though of in 2 ways (1) number density (mol/L) and (2) mass density (g/L). Know the difference and how to calculate either one. |
| 6 | Relate partial pressures and the total pressure as described by Dalton’s Law of Partial Pressure. | Be able to calculate the total pressure from all the partial pressures for a mixture of gases. Also get the mole fraction for each gas as well. \(P_{\rm total} = P_{\rm A} + P_{\rm B} + P_{\rm C} + \cdots \) \(\hskip24pt X_{\rm A} = P_{\rm A}/P_{\rm total} \) |
| 9 | Relate kinetic energy to the temperature of a gas. | What is the formula for calculating the kinetic energy of an ideal gas? \(E_{\rm k} = 3/2RT \) Remember to use 8.314 J/mol·K for R and that the answer is in J/mol. If you need answer for a specific amount of gas (moles) then multiply by n to scale the value and get just J (joules) for then answer. |
| 10 | Relate temperature, molar mass, and gas velocity. | What is the formula for calculating the rms velocity of a gas? (T and M to give v) \( v_{\rm rms} = \sqrt{3RT\over M}\) Once again,remember to use 8.314 J/mol·K for R. Also change your molar mass for the gas into kg/mol. For example, N2 has M = 0.028 kg/mol. The velocity units will be m/s. |
| 11 | Describe the effect of molar mass and temperature on the Maxwell-Boltzmann gas velocity distribution. | Know how to fully interpret a velocity distribution diagram (plot). How does T effect the plot? How does molar mass effect the plot? |
| 12 | Apply kinetic molecular theory to a variety of gas phenomena including diffusion and effusion. | |
| 13 | Calculate relative effusion and diffusion rates using Graham’s Law. | Relative rates means you'll be getting v1/v2 or how much faster is gas A than gas B? Both diffusion and effusion are STILL proportional to the rms velocity of the gases. |
| 14 | Explain the quantitative relationship between state functions (n, T, V, and P) as described by kinetic molecular theory. | All those laws (if this goes up, then this goes down, etc...) and effects are explained by fully realizing the ENERGETICS of the particles themselves (kinetic molecular theory). Know how and why each effect is realized. |
| 15 | Describe macroscopic gas behavior using a small particle model of a gas. | |
| 16 | State when the ideal gas model fails to predict the behavior of gases observed in nature and in the laboratory. | Know how and why our "perfect world" view (ideal view!) of a gas does NOT work very well at all under cetain "tough" conditions. Ultimately there is ONE answer as to why all gases are ultimately NOT ideal. What is that one thing? (Answer: gases are REAL, not imaginary). |
| 17 | Explain what the breakdown of the ideal gas law reveals about the assumptions of kinetic molecular theory. | If you are REAL... (Fact 1) you take up real space and volume, and (Fact 2) you always have SOME attractive and repulsive forces between you and others. |
| 18 | Explain the general principles of the hard sphere model and van der Waal's model of gas. | The Hard Sphere model will adjust to "Fact 1" above by subtracting the volume of the actual molecules (\(nb\)) to give the actual "empty space" that the molecules move within. \( P(V - nb) = nRT \) The VDW model matches the hard sphere model and goes "one better" by also adjusting for attractive forces between the molecules (Fact 2). \( \left(P + {an^2\over V^2}\right)(V - nb) = nRT \) Both models keep the framework of the ideal gas law - they just add or subtract from parts of it to better model REAL behavior of gases at extreme conditions. |
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