Chemistry 161-01, -03Unit 2Fall ‘10

10/18, 19 Laboratory: Analysis of Orthophosphate

10/18 (10/19) Outcomes:

  1. To review and practice skills of determining formulas from percent composition and the reverse.
  2. To know and use the terms that relate components of chemical equations: reactants, products, coefficients, balanced, and other notations that communicate information from chemical equations in several styles.
  3. To explain and use the equalities between masses of reactants and products, moles of reactants and products, atoms of reactants and products, and molecules of reactants and products.
  4. To use “guess-and-check” skills to obtain balanced chemical equations given known reactants and products.
  5. To build and use stoichiometric (mole) ratios to obtain moles and masses of reactants and products.
  6. To define and identify the limiting reagent from two techniques: how much of a substance is needed, or which reactant predicts the smallest amount of product.
  7. To use limiting reagent to determine theoretical yield, and data from experiments to determine percentage yield.

Assignments:

Read §3.5 through 3.7 (Reading quiz)

Recommended exercises: From the above sections, all in-chapter Exercise and Practice problems, and select chapter-end problems referred to by the Practice problems.

10/20, 21, 22 Outcomes:

  1. To know and use the terms that describe components of a solution.
  2. To review the structure and polarity of the water molecule, and how its properties make it a good solvent.
  3. To contrast strong electrolytes from weak and non-electrolytes (and distinguish these from concentration).
  4. To show weak electrolytes and related ions in chemical equations that do not go to completion.
  5. To refer to and use concentration in moles per liter units (molarity), and be able to convert among moles, volumes, and molarity with ease.
  6. To refer to and use concentration in parts per million (ppm), and be able to convert among mass, volume, and ppm (and related units) with ease using appropriate approximations.
  7. To know that a dilution does not change moles, and use the dilution formula to solve problems.
  8. To know how to use molarity and volume to calculate quantities of chemicals present in reactions and analyses.
  9. To use terms that refer to the process of titration, and be able to perform titration calculations.

Assignments:

Read §4.1 through 4.3 and 4.8. (Reading Quiz)

Recommended exercises: From the above sections, all in-chapter Exercise and Practice problems, and select chapter-end problems referred to by the Practice problems.

Lab report due 10/21, 10/22

10/25 (10/26) Laboratory: Reactions in Aqueous Solutions

10/25 (10/26) Outcomes:

  1. To be able to write and interpret reactions involving ionic substances in three formats: molecular (or whole-formula) equations, complete (or total) ionic equations, and net ionic equations.
  2. To know and use the terms describing precipitation reactions.
  3. To memorize a set of solubility rules to predict solubilities and when precipitation reactions should occur.
  4. To review from prior learning definitions of acids and bases and recognize neutralization reactions.
  5. To know that strong acids and bases are strong electrolytes (and these terms do not describe concentration), and that weak acids and bases do not dissociate completely in water.
  6. To memorize that HCl, HBr, HNO3, and H2SO4 (first H+) are strong acids.
  7. To memorize that group I metal-hydroxides are strong bases.
  8. To use prior learning to determine stoichiometry of neutralization reactions.
  9. To recognize oxidation-reduction (“redox”) reactions through the gain / loss of electrons, or the gain / loss of H, or by the presence of elements, or by changes in monatomic ions’ charges.
  10. To understand how “half-reactions” are used in communicating and interpreting redox equations.
  11. To use oxidation numbers as a communication tool, and assign them in elements and monatomic ions.

Assignments:

Read §4.4 through 4.7 (Reading Quiz)

Recommended exercises: From the above sections, all in-chapter Exercise and Practice problems, and select chapter-end problems referred to by the Practice problems.

Graded Homework, end of Chapter 3: 18, 26, 38c, 38d, 58 end of Chapter 4: 24, 40c

10/27, 28, 29 Outcomes:

  1. To view thermochemistry as the study of energy changes and exchanges in chemical processes.
  2. To know how and why to differentiate among the system (what we study), the surroundings (what the system exchanges energy with), and the rest of the universe (note differences from text).
  3. To have a qualitative understanding of how adding energy to a system differs from release of energy by a system, what types of changes produce each, and how the conservation of energy applies.
  4. To view and interpret energy changes in chemical reactions through reaction profile diagrams, and use the terms exothermic, endothermic, and activation energy.
  5. To describe and calculate work as a change in energy in pressure-volume changes.
  6. To view the conservation of energy through Internal Energy change, the interplay of heat and work.
  7. To be able to convert among various energy units and know settings where each is appropriate.
  8. To know and use (in equations) specific heat capacity, heat capacity, and how calorimeters quantify heat changes. To perform calculations for calorimetry experiments.

Assignments:

Read §5.1 through 5.3 (reading Quiz 10/27, 28)

Recommended exercises: From the above sections, all in-chapter Exercise and Practice problems, and select chapter-end problems referred to by the Practice problems.

Lab report due 10/28, 10/29

Graded Homework, due 10/28 (-03) or 29 (-01) end of Chapter 4: 46, 50 (“KHP” is 204.2 g/mole), 56, 70, 78

11/1, 11/2 Laboratory: Sodium Hydroxide Solutions

11/1 (11/2) Outcomes:

  1. To know that enthalpy is defined for convenience as heat when pressure is constant, and its formal definition.
  2. To know and identify how the sign of an enthalpy change corresponds to endo- and exothermic reactions, and how enthalpy changes are indicated in chemical reaction equations.
  3. Know what conditions a standard enthalpy (heat) of reaction refers to, and the difference between it and a standard enthalpy (heat) of formation.
  4. To know properties of state functions and examples of several.
  5. To use enthalpy as a state function to figure out heat changes for reactions we do not perform: from enthalpies of reactions, or from standard enthalpies of formation.

Assignments:

Read §5.4 through 5.6 (Reading Quiz)

Recommended exercises: From the above sections, all in-chapter Exercise and Practice problems, and select chapter-end problems referred to by the Practice problems.

11/3 (Section –01): Chapter 5 Problem-solving session(No reading quiz)

11/4 (Section –03): Chapter 5 Problem-solving session; start Ch. 6, Unit 3(No reading quiz)

Lab report due.

Laboratory Notebooks Due: Notebooks will be returned at the start of the next lab (11/8) with time to copy any required information from the Prelab.

11/5 (Section -01) Group Sheet 2.

Lab report due.

Laboratory Notebooks Due: Notebooks will be returned atthe start of the next lab (11/9) with time to copy any required information from the Prelab.

11/8, 11/9 Laboratory: Thermochemistry

11/8 (Section -01) Outcomes: Success on an hour exam! Content from the above learning outcomes.

Start Ch. 6, Unit 3 (No reading quiz).

11/9 (Section -03) Outcomes:

Group Sheet 2

Success on an hour exam! Content from the above learning outcomes.

11/11 Holiday, no classes

11/12 Non-Instructional Day (College open, no classes)