Following the Text

• atomic size, ionization energy and electron affinity pages 52, 53 & 57
• electronegativity and the bonding continuum pages 70 to 73
• ionic and covalent bonding page 75 & 81
• polar covalent bonds and polar molecules --> geometry page 85 to 91
• balancing equations page 114 to 118

March 3

• types of chemical reactions (main variations)
1. synthesis and decomposition page 119
2. combustion reactions page 123
3. single and double displacement reactions page 126
   activity series of metals page 130
4. neutralization reactions
• Working with the Mole and mass together page 180 to 192

March 7

• Average atomic mass and the periodic table Page 164
• isotopic and relative abundance of isotopes
  calculating average mass page 165
  calculating isotopic abundance page 169
• Avogadros constant and the Mole page 171 to 179
• Stoichiometry == working with the balanced equation page 234 to ....

March 10

• Determining the number of molecules and atoms in a sample given a mass
  Convert mass to moles then moles to number of molecules the times the number of atoms in the molecule for total number of atoms in this sample
  See page 189 for conversion diagram &/or check your note that was written on the board.
  Make sure you do the assigned homework on this topic
• Law of Definite Proportions: definition is found on page 198 and leads to the following
  Percentage Composition and calculations page 202
  empirical formula and calculations page 207, 209
  On page 210 is a list of multipliers that you may encounter so as to convert a decimal fraction into a whole number. You should only see fractions in multiples of halfs or thirds (1/3 or 2/3)

March 21

• Review of material up to this point Pages 165 to 210
• the molecular formula and its calculations page 215, 217
• limiting reagent or reactant page 251
• percentage yield page 260
• Finding Empirical and molecular formulas by experiment Page 219
  Two examples possible to carry out
  1. decomposition of potassium chlorate
  2. dehydration of copper (II) sulfate pentahydrate Page 223

March 24 Test this day

• Start of Stiochiometry: Working with the Balanced Equation Chapter 7 Page 234
1. Mole relationships in the chemical equation. Mole ratios are based on the coefficients from the balanced equation., hence mole:mole ratios
   A system will be taught as to how to work the math solving
2. Different ratios of reactions Page 239
• Test in one week on this material

• working with ratios: the system; no thinking required, just reading.
• Mass relationships Page 241
• Mass Moles it really doesn't matter the mix; system solves the problem Page 247
  We can even thow in number of particles or molecules for your added pleasure.
• The Limiting Reagent Page 251 to 259

This is the end of chapter 7 and Unit 3

• stiochiometry: working with the balanced equation Page 247
  watch the units given in question information.
• Limiting reagent Page 251 to 259

April 4

• More practice with limiting reagent and finding the limiting reagent Page 252
• Limiting eagent in stiochiometric problems Page 256
• Percentage yield Page 260 with the simple formula on page 261
• Applications of percentage yield and purity of product Page 264 & 268

April 7

• Percentage Yield Page 260
  Using percentage yield to deduce the actual yield Page 263
• Percentage purity Page 268
  This is the end of chapter 7
• Solutions and solubility Chapter 8 Page 283
• Types of solution and quantifying terms & definitions relating to solutions Page 284
• Factors that affect the rate of dissolving and solubility Page 290
  Polar and non- Polar solutes and solvents Page 291
• Predicting solubility Page293
• Factors that Affect solubility Page 295 to 299
  1. molecular size
  2. temperature
  3. heat
  4. pressure
• Concentration of solutions Page 302
  Units of concentration Page 302 to 311
• Molar Concentration: the most important of the units Page 313 to 316

April 11

• Test chapter 7 Pages 234 to 270
• Units used in quantifying solutions page 302 to 312
• Molar concentations; working with the numbers Page 313 to 316
• Preparing solutions: how to make a solution to a given or require concentration in mol/L Page 319
• Diluting solutions to needed or required concentrations Page 320

End of Chapter 8

April 13 (Wednesday)

• Concentration of solutions review chapter 8 wrap up
• Solution solubility; make predictions about solubility page 330
• General solubility guidlines page 334
• Reactions of aqueous solutions; double displacement reaction in which the insoluble salt precipitates page 337 to 341
• Identifying ions in solution page 344

April 18

• Stiochometry of solutions Page 348
• Concentrations of ions Page 348
• Mass percent of ions page 350
• Minimum volume to precipitate page 351
• Mass of a precipitated product; will all the salt precipitate from solution (limiting reagent) page 353 to 355
• Aqueous solutions and water quality; a reading exercise page 357 to 364

April 21

• More review of solution stiochiometry
  1. Diluting a solution Page 320
  2. Mass percent of ions Page 350
  3. Finding minimum volume to precipitate Page 351
  4. Find the mass of a precipitated compound Page 353
  5. Finding the mass of a precipitate from mixing solutions of known concentrations Page 354
• Test on chapter 8 & 9 ---> solutions Next Monday.
• Start of acid and bases page 369
• Acid base theories page 370 to 379
  Two theories: Arrhenius & Bronstead-Lowery Summary page 379

This is the end of chapter 10

April 25

• Strong and weak acids and bases page 381 to page 383
• Monoprotic and polyprotic acids page 382 & 383
• Naming acids page 384
• pH and hydogen ion concentration page 385 to 389
• Acid base reactions, introduction to indicators page 395
• The titration page 399 to 401

April 28 ISU day Assignment given out in class or read here
Page 405 Do these questions: 1, 2, 3, 4, 8, 11, 14, 15

May 2

• Continuation with acids and bases
  Conjugate acid-base pairs Page 376
  Strong weak acids Page 381
  Polyprotic acids Page 383
  pH scale with math Page 386
  Neutralizations and the titration (math calculations) Page394
• End of acids and based

This is the start of the Gas Laws Chapter 11 & 12

• Kinetic Molecular Theory page 418 to 423
• Intoduction to pressure and volume of gases
  measurement of pressure and various units page 424 to 428
• relation between pressure and volume: Boyle's Law page 428 to 435
• Temperature: Kelvin scale and absolute zero page 440
• Charles' Law page 440 to 446
• Gay-Lussac's Law page 447 to 451
• Combined gas law calculations page 452 to 457
• Dalton's Law of Partial Pressure page 459 to 460
• Application of gases; just a reading section page 462 to 466

May 5 Test on Acids and Bases

May 9

May 5 Test on Gas Laws Chapter 11