Mrs. Cook's Blog

AP Chemistry: Week of Feb 1st

College Board Course Description

III. Reactions

A. Reaction types

1. Acid-base reactions; concepts of Arrhenius, Brønsted-Lowry, and Lewis; coordination complexes; amphoterism

    2. Precipitation reactions

    3. Oxidation-reduction reactions (Oxidation number)

B. Stoichiometry

1. Ionic and molecular species present in chemical systems: net ionic equations

2. Balancing of equations

IV. Descriptive Chemistry

    1. Chemical reactivity and products of chemical reactions

2. Relationships in the periodic table: horizontal, vertical, and diagonal with examples from alkali metals, alkaline earth metals, halogens, and the first series of transition elements

3. Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties)

 

Reaction Set Due Dates: F = 2/1, G = 2/2, H = 2/3, I = 2/4, J = 2/5, K= 2/8

Redox Quiz (Common oxidizers and reducers) = 2/9

1^st Reaction Test = 2/10

 

 

College Board Course Description

III. Reactions

A. Reaction types

3. Oxidation-reduction reactions

a. Oxidation number

b. The role of the electron in oxidation-reduction

c. Electrochemistry: electrolytic and galvanic cells; Faraday’s laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions

 

Monday, 2/1:  Review Section 4.4.  Start read-behind of Chapter 20.  And page 889, #87, 91a

Tuesday and Wednesday, 2/2 and 2/3: Page 885, #25 and write line notation, 33, 35, 37, 39, 41

Thursday, 2/4:  Page 886, #49, 51, 59, 61, 65.  Read sections 20.7 & 20.8.  Prelab 22.  AP Problems Worksheet

Friday, 2/8:  Work day.  Work on all of above in class.

 

Looking ahead: 

Lab 22 and AP Problem set due on Friday, 2/12

Electrochemistry Test on Tuesday, 2/16

AP Chemistry: Electrochemistry Notes and Assignments

Students should review section 4.4 and read Chapter 2O.

Electrochemistry - Chapter 20 (Students should read behind.) - Study of the interchange of chemical and electrical energy.  Focus on chemical changes that occur when electric current flows. (Redox reactions)

Need mobile ions – solution (electrolytes), molten

Electrons flow from the anode (negative terminal) to the cathode (positive terminal) 

Mnemonic: a to c (alphabetical order)

Anode    

Physics people = negative (Actually electrodes are neutral!)

attracts anions

anion donates e- (oxidation)

anion is oxidized (ox# increases)

anode is reduced

Cathode

Physics people =  positive

attracts cations

cation gain e- (reduction)

cation is reduced (ox# decreases)

cathode is oxidized

Electrical measures: 

coulomb (C) = measure of the charge (defined SI base unit)

1 faraday (F) = charge on one mole of e-'s = 96,485 C

1 ampere (A, old = amp) = measure of current (charge/unit time) = 1 C/s

Sample 20.14 on page 878 and practice

Homework  Page 889, #87, 91a.  Assigned: 1/21/09

Define:

electrolytic cell (2 electrodes, one solution)

half cell - metal electrode (strip) in solution of ions of the metal

galvanic/voltaic cell (2 half cells joined by salt bridge or porous disk)

Note: If a half-reaction does not include a metal, use Pt(s) for the electrode.

Line notation:(note alphabetical order:  anode || cathode)

Sample 20.4, page 853.    So:  Pt(s) | I^-(aq) || Cr₂O₇^2-(aq), H⁺(aq) | Pt(s)

Practice Problem on page 854:  Zn(s) | Zn²⁺(aq)|| ClO^3-(aq), Cl^-(aq), H⁺(aq) | Pt(s)

Homework: Page 885, #25 and write line notation  Assigned 1/23/09

Students should read about electrode potentials (page 855)

    Electrical potential = potential energy (energy to move electrons)

    (Script E or emf: electromotive force)

V (volt)    1V = 1J/C    The higher potential = more work can be done

Standard potential - 25 oC, 1M solutions, gas at 1 bar pressure, pure solids and liquids

    Read “Standard Reduction Potentials) on page 856.

Reported as compared to standard hydrogen electrode (platinum electrode, contact with 1 M H+ and bathed in H2 gas)

Eo = sum of half cells:  See chart on page 857, Appendix E on page 1117, AP handout

Always run spontaneously in the direction of positive cell potential.    Not 100% efficient.

Samples 20.5 – 20.6   Homework:  Page 885, #33

Sample 20.7   Homework:  Page 885, #35,37,39

Sample 20.8   Homework:  Page 885, #41

Sample 20.9

DGo = - n F Eo = - RT ln K = -2.303 RT log K

    log K = nEo (96485)/(2.303*8.31*298) = nEo/0.0592

       F ln(10)  R   T

Sample 20.10 on page 864 and practice

Homework: pg 886, #49, 51

Nernst Equation:  Derived on page 865:  E = Eo - (0.0592/n) log Q

        Sample 20.11 on page 866 and practice

Homework: Page 887 #59, 61, 65

	D G	Q -v- K	E
forward reaction favored (spontaneous)	negative < 0	Q < K	positive > 0
at equilibrium	= 0	Q = K	= 0
reverse reaction favored	positive > 0	Q > K	negative < 0

Homework: Read about batteries, fuel cells, corrosion (Sec20.7 & 20.8)

And Prelab 22: Electrochemical Cells

And AP problem set

Lab22: 

Lab Report: Identifiers (Name, date of data collection, lab partner, period), Title, Purpose, Procedure, Data (what you actually measured…not anything you calculated).  Calculations and Analysis (includes two tables listed in your lab book as data – but they are NOT data you measured), Post-lab Questions, Error Analysis (Parts 2 & 3)

Honors Chemistry: Week of Feb 1

GPS:

SCSh3. Students will identify and investigate problems scientifically.

c. Collect, organize and record appropriate data.

e. Develop reasonable conclusions based on data collected.

f. Evaluate whether conclusions are reasonable by reviewing the process and checking against other available information.

SCSh5. Students will demonstrate the computation and estimation skills necessary for analyzing data and developing reasonable scientific explanations.

d. Express appropriate numbers of significant figures for calculated data, using scientific notation where appropriate.

e. Solve scientific problems by substituting quantitative values, using dimensional analysis and/or simple algebraic formulas as appropriate.

SC2 Students will relate how the Law of Conservation of Matter is used to determine chemical composition in compounds and chemical reactions.

c. Apply concepts of the mole and Avogadro’s number to conceptualize and calculate

• Empirical/molecular formulas,

• Mass, moles and molecules relationships,

 

 

Monday, Feb1: Attempt lab calculations and Worksheet #82-93

Tuesday,  Feb 2: Complete empirical formula lab report and Mole project

Wednesday, Feb 3: Hydrate and combustion problems on assignment sheet (due Friday) and hydrate prelab (due Thursday)

Thursday, Feb4: Complete hydrate lab report (due Monday)

Friday, Feb 5:  Review Assignment (due Monday)

Monday, Feb 8:  Study for Chapter 6 Test

Tuesday, Feb 9: Chapter 6 test

 

Wednesday, March 17:  Book project due

Honors Chemistry: Week of January 25

GPS:

SCSh3. Students will identify and investigate problems scientifically.

a. Suggest reasonable hypotheses for identified problems.

b. Develop procedures for solving scientific problems.

c. Collect, organize and record appropriate data.

e. Develop reasonable conclusions based on data collected.

f. Evaluate whether conclusions are reasonable by reviewing the process and checking against other available information.

SCSh5. Students will demonstrate the computation and estimation skills necessary for analyzing data and developing reasonable scientific explanations.

d. Express appropriate numbers of significant figures for calculated data, using scientific notation where appropriate.

e. Solve scientific problems by substituting quantitative values, using dimensional analysis and/or simple algebraic formulas as appropriate.

SC2 Students will relate how the Law of Conservation of Matter is used to determine chemical composition in compounds and chemical reactions.

c. Apply concepts of the mole and Avogadro’s number to conceptualize and calculate

• Empirical/molecular formulas,

• Mass, moles and molecules relationships,

 

 

Monday, Jan 25:  Mole lab due today.  Chalk lab in class.

Tuesday, Jan 26:  Review assignment is due today.  Study for tomorrow’s Mole Test.

Wednesday, Jan 27: Mole Test today.  Homework:  Worksheet #56-65

Thursday, Jan 28: Worksheet #69-78 to nearest 0.1%

Friday, Jan 29:  Due Monday:  Empirical Formula Prelab.  Due Tuesday: Worksheet #90-93.  Due Wednesday: Empirical Formula Lab Report includes prelab, data, calculations, questions

 

Honors Chemistry: Chapter 6 (Part two) Notes and Assignments

Percent Composition

    1. Calculate formula mass

    2. Divide component mass by formula mass

    3. Multiply by 100 to get %

    4. Check: Sum = 100% ⁺/- 0.1

 

Part of formula from element   x 100
formula weight

 

(# of atoms)(atomic weight) x 100
   formula weight

 

Sample on page 192.  Sample 6.9 on page 193.  Practice on page 194

Homework: Worksheet #69-78 to nearest 0.1%

 

Recall: empirical formula = Smallest whole number ratio of elements/ions in a compound.

Example 6.10 on page 198

 

empirical formula from percent composition data

1. Divide the mass or mass percentage
  by the atomic weight of the element
    = moles

2. Divide by the smallest number.

3. Adjust ratios to simplest whole
  number ratio.
    a) multiply to whole numbers
    b) least common denominator

 

Example 6.11 on page 199.  Example 6.12 on page 202.  Example 6.13 on page 203,  Practice on page 203, 204

 

Homework: Worksheet #82-88

 

Molecular formula = (empirical formula)factor

factor = whole number

factor = molar mass / empirical formula mass)

 

Example 6.15 on page 206. Practice on page 207

 

Homework: Empirical Formula Prelab (Lab report = prelab, data,calculations, questions)

Homework: Worksheet # 90-93

 

A closer look at hydrates

Homework:  Hydrate Prelab (Formal lab report) and problems on assignment sheet

 

Combustion Analysis

What are the products of the combustion of a hydrocarbon?  CO₂ + H₂O

All of the carbon in the reactant shows up in the CO₂.

All of the hydrogen in the reactant shows up in the H₂O

Homework:  Combustion analysis problems on assignment sheet

 

Homework: Review Assignment

AP Chemistry: Week of January 25

College Board Course Description

III. Reactions

A. Reaction types

1. Acid-base reactions; concepts of Arrhenius, Brønsted-Lowry, and Lewis; coordination complexes; amphoterism

    2. Precipitation reactions

    3. Oxidation-reduction reactions (Oxidation number)

B. Stoichiometry

1. Ionic and molecular species present in chemical systems: net ionic equations

2. Balancing of equations

IV. Descriptive Chemistry

    1. Chemical reactivity and products of chemical reactions

2. Relationships in the periodic table: horizontal, vertical, and diagonal with examples from alkali metals, alkaline earth metals, halogens, and the first series of transition elements

3. Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties)

V. Laboratory: The AP Chemistry Exam includes some questions based on experiences and skills students acquire in the laboratory:

    • making observations of chemical reactions and substances

    • recording data

 

 

Instructional Activity:  Continuing Lab 19 – due February 1^st.

 

Reaction Set D due Wednesday, 1/27

Reaction Set E due Friday, 1/29 (Last day to work on lab in class.)

Reaction Set F due Monday, 2/1

Honors Chemistry: Week of 1/19

Chapter 6

GPS: SC2 Students will relate how the Law of Conservation of Matter is used to determine chemical composition in compounds and chemical reactions.

c. Apply concepts of the mole and Avogadro’s number to conceptualize and calculate: Mass, moles and molecules relationships

 

1/19

Read Page 179:

Defining the mole and Avogadro's number

See blue box on page 180

Example 6.3 on page 182.  Example 6.4 on page 183.  Practice on page 184

Homework: Page 184,  #4,5

 

 

1/20

Calculate molar mass of a compound.

See sample on page 185.  Example 6.5 on page 186 and Ba(OH)₂.  Practice Problem (pg 187)

See NaCl example on page 187

Example 6.6 on page 187.  Example 6.7 on page 189.  Practice on pag e188

Example 6.8 on page 190.  Practice on page 191

Homework: Page 195, #1,2,3,5

 

 

1/21

Mixed practice.  Assign mole project.(Due 2/3)  Start work on Review assignment:  Page 210, #14bdg, 15bh, 16bg, 20bd, 22bd, 24be, 25bd, 26bd

 

 

1/22

Mole Quiz

and MOLE, MASS, PARTICLE, AND VOLUME RELATIONSHIPS worksheet lab

 

 

1/25: Chalk Lab

 

1/26: Review is due

 

1/27:  Test Chapter 6, Part One – THE MOLE

AP Chemistry: January 19-29

College Board Course Description

III. Reactions

A. Reaction types

1. Acid-base reactions; concepts of Arrhenius, Brønsted-Lowry, and Lewis; coordination complexes; amphoterism

B. Stoichiometry

1. Ionic and molecular species present in chemical systems: net ionic equations

2. Balancing of equations

IV. Descriptive Chemistry

    1. Chemical reactivity and products of chemical reactions

2. Relationships in the periodic table: horizontal, vertical, and diagonal with examples from alkali metals, alkaline earth metals, halogens, and the first series of transition elements

3. Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties)

V. Laboratory: The AP Chemistry Exam includes some questions based on experiences and skills students acquire in the laboratory:

    • making observations of chemical reactions and substances

    • recording data

 

 

Instructional Activity:  Lab 19 – due February 1^st.

AP Chemistry: Due on Friday, January 15

Redox Balancing Worksheet

Reaction Set A

Prelab 19 (Turn this one in at beginning of period.)

Honors Chemistry: Sigfig quiz

Wednesday, 1/12