Chemistry 120 - Cascadia College



Chemistry 161 section -05 Fall ‘16

Unit 1

Study technique recommendations:

• Check the outcomes for the class ahead of time.

• Skim the text sections before class, paying close attention to blue print vocabulary terms, and the figures. This should take no more than 20 minutes and should prepare you for daily quizzes.

• Read the assigned text sections as soon as possible after class.

• Compare the outcomes to your class notes, taking care to review material not covered in class.

• Learn actively by explaining concepts and relationships to someone else.

• Learn collaboratively by solving recommended exercises in a study group.

Please note that there is a set of text corrections for chapters 1 – 7 at the end of this document.

Most of Chapters 1 and 2 is covered in Preparatory or High School Chemistry (which are prerequisites). Please conduct a thorough review on your own; new or collaborative content will be covered in class.

9/27 Outcomes: (Notes for this class are attached; notes for other dates will be on Canvas.)

1. To know the procedures, outcomes, and expectations for success in this course and your personal goals.

2. To use the vocabulary by which pure substances are described: atom, element, molecule, compound, composition, and that a molecule has a definable boundary (not in book).

3. To review definitions of physical and chemical properties and changes and what a reaction is.

4. To use the vocabulary by which mixtures are described: heterogeneous, homogeneous, solution.

5. To give examples of the physical process of separation.

6. To have an overview of the scientific method and the specific role of a hypothesis.

7. To know and use units of mass, length, time, the abbreviations g, m, s, the metric prefixes k, c, m, μ and n, and how to combine prefixes with measurements.

8. To be able to convert between powers of 10 with ease in your head and with a calculator.

9. To be able to convert among F, C, and K temperature scales using equations.

10. To prepare for lab on 9/29.

Assignments:

Read §1.1 through 1.4, 1.7; Appendix section A1.1. (Reading quizzes start 9/30.)

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

9/29 Laboratory (CC1-330):

• Please purchase safety goggles and lab manual from the bookstore before coming to lab. If the bookstore is temporarily out of lab manuals, let them know, and then access the preliminary information and the first experiment from Canvas (only the first experiment will be on Canvas).

• Lab will begin with a safety and waste handling discussion. The safety protocol form (p. 6 of lab manual) must be signed, by a parent if you are under 18 years of age.

• You will carry out “An Introduction to the Visible Spectrophotometer” from the lab manual, page 26.

• The Prelaboratory Assignment (page 34) is due at the start of lab.

• The written report pages from the lab manual are due at the start of class the second class session after your lab (due 10/4).

9/30 Outcomes:

1. To review key aspects of lab.

2. To use the derived units volume and density, and to solve problems using density with equations.

3. To build and use conversion factors from definitions and measurement-based values, and use units as algebraic quantities.

4. To learn how density can be used as a conversion factor, and to use it to solve problems.

5. To learn the source of “uncertainty” in measured quantities, and to relate examples both from personal experience and laboratory measurements.

6. To know the difference between exact numbers (integers, definitions) and measurement-based numbers that contain uncertainty.

7. To assign and communicate uncertainty using absolute and relative “errors”, confidence intervals, and know when you are communicating accuracy vs. precision.

8. To use uncertainties to assign significant figures and use significant figures in calculations and communications.

9. To grasp how “significant figures” are a useful short-cut for communication of uncertainty.

Assignments:

Read §1.5 through 1.6; lab manual Appendix pp. 70 – 78.

Reading quiz on blue / bold print in sections 1.5 through 1.6.

Recommended exercises: From sections 1.4 through 1.6, all in-chapter Exercise and Practice problems, and select chapter-end problems referred to by the Practice problems.

10/4 Outcomes:

1. To review the Law of Conservation of Mass and understand how it applies to chemical changes.

2. To appreciate the historical implications of the laws of definite composition and multiple proportions, Dalton’s Atomic Theory, and how the Law of Combining Volumes led to the concept of molecules.

3. To know the three principal types of radioactivity (alpha, beta, gamma particles).

4. To know details of experiments that led to the hypothesis and evidence for the electron, the nucleus, the proton, and the neutron, and the modern understanding of the nuclear atom’s structure.

5. To know the number of protons in an atom determines what element it is and defines its atomic number (Z).

6. To know how and why an atom differs from an ion and how ions are symbolized.

7. To know that neutrons determine what isotope of an element an atom is, and the definition of mass number (A). To use isotope notation when necessary to communicate this.

8. To know the modern technique by which mass numbers are determined, and to use atomic mass units.

9. To prepare for lab on 10/6.

Assignments:

Read §2.1 through 2.5. Reading quiz on blue / bold print in sections 2.1 through 2.5.

Recommended exercises: From sections 2.1 through 2.4, all in-chapter Exercise and Practice problems, and select chapter-end problems referred to by the Practice problems.

Lab report due: pages 12 – 16 from lab manual.

Graded Homework exercises due at start of class:

Chapter 1 problems (pp 39 – 43) #12, 18, 40, 44, 46, 86, 92f, g, 94f, g.

10/6 Laboratory: “Measurement and Error…” (p. 35)

Prelaboratory assignment (p.47) due at start of lab; report is due at the start of class on 10/11.

10/7 Outcomes

1. To review key aspects of lab.

2. To understand the differences among the mass number, the actual mass of one atom, and the average of all isotopes of an element (average atomic mass).

3. To know the information available in the Periodic Table of the Elements and the nomenclature of its organization: periods, groups, blocks, and metals vs. nonmetals.

4. To know four specific groups by name: alkali metals, alkaline earth metals, halogens, inert gases.

5. To understand and use the Periodic Table group to determine monatomic ion charges.

6. To know that ionic compounds are made from numbers of ions in ratios giving charge balance, and to recognize ionic compounds from their chemical formulas.

7. To know how molecules differ from ionic compounds and from other types of covalent compounds.

8. To use the terms molecular formula, empirical formula, and formula unit (not in book).

9. To give names from formulas, and determine formulas from names for binary covalent compounds, binary ionic compounds, and ionic compounds of polyatomic ions.

10. To know from memory the polyatomic ions ammonium, acetate, nitrate, hydroxide, carbonate, sulfate, and phosphate.

11. To know from memory the binary acids of the halogens, acetic, nitric, sulfuric, and phosphoric acids.

Assignments:

Read §2.6 through 2.10. Reading quiz on these sections.

Recommended exercises: From sections 2.5 through 2.10, all in-chapter Exercise and Practice problems, and select chapter-end problems referred to by the Practice problems.

10/11 Outcomes:

1. To calculate formula masses for molecular and ionic compounds.

2. To convert between mass of a substance and number of molecules or formula units, and understand how Avogadro’s number conveniently accomplishes counting by weighing.

3. To define and use the mole as a counting unit.

4. To convert among molecules (or formula units), moles, and masses with ease.

5. To identify moles of an atom in a mole of a substance and use this skill to determine percent by mass.

6. To use percent by mass data to obtain empirical formulas.

7. To compare empirical formulas to molecular masses to determine molecular formulas.

8. To prepare for lab on 10/13.

Assignments:

Read §3.1 through 3.5. Reading Quiz on these sections.

Recommended exercises: From sections 3.1 through 3.5, all in-chapter Exercise and Practice problems, and select chapter-end problems referred to by the Practice problems.

Lab report due at start of class.

10/13 No In-Laboratory Session: In place of an in-laboratory session there is an exercise on the use of resource materials, both electronic and hard copy. Read the description on p.48 of the lab manual (“Chemical Resource Lab”); the actual assignment will have been handed out in class and posted on Canvas. Due 10/20 at start of lab.

10/14:

Group Sheet 1 (performed and due in class before the start of the exam)

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

Pick up Unit 2

Kelter, 1st ed., errata for chapters 1 - 7

Page 162, problem 25a, answer (page A23, 2.5 ppm): If 1000.0 L is intended, then answer is 2.5 x 10-3 ppm. If 1000.0 mL is intended, then the answer is 2.5 ppm.

Page 190-191 Exercise 5.7: The value -2202 kJ is incorrect. If values of ΔfHo from the Appendix are summed, you get -2222 kJ combusting to liquid water or -2046 kJ to gaseous water. Note that literature values are -2219.2 (Handbook of Chemistry & Physics and most recent NIST entry), -2219.9, -2207, and -2204 (older NIST entries) for gas phase ΔcHo. Note also that p 185 shows -2220.

Page 196, figure 5.24 and subsequent equations: For each ΔH, after multiplying by moles, the units should be kJ, not kJ/mol.

Page 196, paragraph above Exercise 5.9: The value – 5128 kJ/mol is actually per 4 moles, thus -1282 kJ/mol.

Page 197, Exercise 5.9: Same problem as above, units are kJ.

Page 206, problem 5.77b.: The Instructors’ edition and some of the student editions (but not all) have the “g” missing from “100.0 g.”

Page 206, problem 5.78: The subscript (3) is missing in SO3 in the last equation.

Page 244, third paragraph: change “nonradial” to “radial”

Page 245 fig. 6.39, two errata: (1) The values on the Y-axis should be negative. (This was corrected in the Instructors’ Resources on-line where a “ -1 x “ was placed before the y-axis legend “Energy.” (2) The electrons are depicted as all paired in the 2p level for O; there should be one pair and two unpaired.

Page 253, problem 17, answer (page A24): answers are reversed.

Page 261, Figure 7.1 incorrectly shows He as a member of the “p block.” (It is correct in Chapter 6 figures.)

Page 257, problem 106: The order of orbital energies for 4s and 3d reverses for ions compared to atoms. Since this is not presented in this chapter, students would conclude that Zn2+ is [Ar]4s23d8 with 2 unpaired electrons, where it actually is [Ar]3d10 with 0 unpaired electrons. They would also get the incorrect configuration for Fe3+, but in either case they would conclude that it has unpaired electrons.

Page 281, Figure 7.8: Lower part of the figure incorrectly shows He to be larger than Ne. (It is correct in the upper part of the figure.)

Page 863, problem 29: The answer in the appendix, p. A44 should be – 233 kJ.

Page 864, problem 57: The answer in the appendix, p.A44 is correct, but the diagram is wrong.

Page 864, problem 75: The answer in the appendix, p. A44 should be 0.082 A.

Page A11 Appendix 3, duplicate entries for NH4Cl(s) (but the values for So differ).

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