CHEMISTRY

5/18/2010 - 5/24/2010

Chemistry Final Exam Review

The exam is not comprehensivebut the skills we learned semester one are relevant as the course is cumulative(builds up).

Concepts assumed fromsemester one include: scientific notation, atoms/moles, and naming compounds. These skills will be tested on and used for this examination.

The exam will focus onchapters 7 – 9 and 12.

Topics include:

chemical reactions

balancing equations ex. p.235 #31 - 36

naming “common” compounds(see chapter 4)

solubility and reactions insolution

          predicting reactions

          acid-base

          oxidation-reduction p. 273 #27 - 29

                   synthesis p. 274 #34, 38

                   decomposition p. 274 #35, 39

                   combustion p. 274 #37

          precipitation reactions p. 272 #11 - 13

          stoichiometry pg. 317 #1 - 7

                   grams → moles

                   mole ratio

                   moles → grams

                   mass calculations

                   limiting reactants

                   percent yield

4/30/2010 #40-47

4/29/2010 #27-28 p. 412, #34 - 39

4/28/2010 #17 - 20 p. 311, p. 312 #22 - 24

4/27/2010 Discuss limiting reagants and percent yield

4/26/2010 Read Chapter 9

4/12/2010 Pg. 311 #15 balancing only due; cw do the stoichiometry

4/13/2010 p. 311 #16a due; finish #16 in class

HW p. 311 #21

4/14/2010 4/15/2010 Read 9.3

4.16 p. 312 #29, 30, 34 - 37

3/22/2010 Introduction to Stoichiometry:

1) Warm Up: Write the balanced equation for decomposing water into Hydrogen and Oxygen gases.

How many moles of water do you need to obtain 1 mole of O2 by electrolysis?

2) Discuss Stoichiometry: Moles of Product and Moles of Reactants

3) Ratio of Products to Reactants - solve the warm-up challenge

4) Read and discuss pages 283 - 287 Mole - to - Mole conversions

CW: pg. 287 #4 - 5, Yellow Practice Problems

HW: Page 287 #1 - 3

3/23/2010 Chemistry Test - reactions chapter 8

3/24/2010 Using moles to calculate mass from chemical equations

Collect and discuss HW

Masses of Products -> Moles Products -> Moles Reactants -> Masses of Reactants

Read and discuss 9.2 Calculating Mass from Equations

HW pg. 295 #1 - 6

3/25/2010

Collect and discuss HW

Limiting Reagants

Percent Yield

Discuss/Read 9.3

HW pg. 308 #1 - 5

3/26/2010

How many sandwiches can you make with 20 slices of bread, 8 portions of peanut butter, and 7 portions of jelly

3/15/2010 Finish review of 8.1: Solubility, precipitation reactions, molecular equation, complete ionic equation, net ionic equation

3/16/2010 Review 8.2 Acid-Base Reactions, oxidation-reduction reactions, precipitation reactions

3/17/2010 Post-chapter Overview of the Types of Reactions, Solutions/Solubility

Examples of each common type of chemical reaction

3/18/2010 The Quantum Atom - Preview and Discussion of Chapter 11

Chapter 8: Reactions

YOU MAY USE A NOTE CARD OR NOTEBOOK PAPER WITH COMMON POLYATOMIC ION CHARGES AND SOLUBILITY RULES

3/8/2010    Classifying Reactions      HW     p. 269 #1 - 7

3/1/2010 Acid-Base Rxns

pg 262 #1-3

3/2/2010 Oxidation-Reduction

pg 262 #4 - 6

2/22/2010 8.1 Reactions in Aqueous Solutions

CW p. 253 #1 - 3

HW p. 253 #4 - 6

2/23/2010

CW Discuss HW due today

2/24/2010

CW Activity pg. 253 - Predicting Precipitates

HW Read pages 254-262; answer any 3 questions on pg. 262 chosen from #1 - 6.

CW Discuss acid-base reactions. Volcano with vinegar and baking soda?

CW Discuss oxidation-reduction reactions.

("LEO the lion says GER" - Lose Electrons, Oxidation; Gain Electrons, Reduction)

HW Pg. 262 #1 - 6 all

2/25/2010

Read and discuss pages 263 - 270: Classifying reactions

HW  - p. 269 #1 - 7.

2/26/2010

Discuss HW and begin chapter review.

2/8/2010 page 235 #33 - 36

2/9/2010 Balancing Equations Quiz

2/10/2010 Read chapter 8

2/11/2010 Read chapter 8

2/12/2010 Acid-Base reaction: Baking Soda in Vinegar

Balancing Equations: Week of 2/1/2010 - Handout #1 - 30

01/25/2010 Page 237 #1 - 12 With partners

01/26/2010 p. 234 #1 - 10

01/27/2010 p. 235 #31 - 36

01/28/2010 p. 234 #11 - 19

01/29/2010 Quiz - Balancing Equations - chapter 7

Week of 01/21/2010 Read and discuss chapter 7: chemical reactions

12/14/09 - 12/17/09 Review for Test on Percent Composition, Empirical Formula, Molecular Formula. Test Thursday 12/17/09. Your list of missing assignments will be available on 12/17 to work on over the break.

12/07/09 - 12/11/09 Empirical vs. Molecular Formulas

11.30.09 Read pages 185 - 194: percent composition by mass. HW p. 195 #1 - 6

11/30-12/01 HW p. 208 #1 - 6; percent composition exercises and handouts

12/02 - 12/03 HW Read pages 185 - 194; molecular formula vs. empirical formula

Chemistry Monday 8.24.09

Warm-Up: Copy this page of notes.

Collect and discuss HW 2.1 & 2.2.

Mixture: Made out of more than one pure substance, has a variable composition. 

Examples: Air, wood, soda, orange juice, wet sand.

Example 2: Air is mostly made out of:

        Nitrogen                        N₂

        Oxygen                  O₂

        Water                     H2O

        Argon                      Ar

        Carbon Dioxide         CO₂

        Neon                      Ne

        Helium                   He

1.   Helium, Neon, and Argon are noble gases and relatively non-reactive, or inert.

2.   Nitrogen is relatively inert but causes trouble for deep divers if they rise to fast and don’t decompress properly.

3.   Water is a substance made of two hydrogen atoms and one oxygen atom.

4.   Carbon Dioxide is exhaled after we inhale oxygen; plants turn CO₂ into O₂ during photosynthesis.

Example 3: Gold

24K = pure gold

        18K = 56% gold, 20% silver, 24% copper

        14K = 36% gold, 25% silver, 37% copper

Example 4: Salt water and sand

        Salt water and sand can be separated by filtration.

        A mixture of salt and water can be separated by distillation, boiling away the water.

Homogeneous mixtures:

have uniform composition.

Examples:        Soda, Shaken pulp-free orange juice, salt water, air, sugar water, coffee, gold

Heterogeneous mixtures:

have variable compositions.

Examples:         Wood, a sandwich, a mixture of sand and salt water with the sand settling to the bottom, tin foil floating around in a salt water solution.

Read pages 35 – 44.

Homework: p. 43 #1-7

Begin Chapter 2 Review

Page 47 #1 – 12.

Warm Up Tuesday:

Start pp. 45 – 46 #1 – 29.

Review Chapter 2:

Do pp. 45 – 46 with partners, then students present the solutions.

Chapter two test Wednesday.

Wednesday: Chapter 2 test.

New Seating Chart.

Homework: p. 49 #1 – 5.

Read pages 49 – 54.

Thursday:

Assign 24 elements on pg. 24 to partners, who will make small periodic table posters for each.  Hang the posters on the wall in their correct relative positions on the periodic table.

Homework: p. 55 #1-6.

Warm Up: Copy

Dalton’s Atomic Theory: Early 1800’s

1.                        Elements are made of tiny particles called atoms.

2.                        All atoms of a given substance are identical.

3.                        Atoms of different elements are different.

4.                        Atoms of different elements can form compounds together.  A given compound always has the same ratio of the types of atoms.

5.                        Atoms are chemically indivisible particles; atoms cannot be broken or changed during a reaction, but the way that atoms are grouped together can change during a chemical reaction.

Read pages 56 – 59.

HW: Page 59 #1 – 6.

Friday Warm-Up: Copy the following:

1890’s JJ Thompson discovers the electron

He created a stream of negatively charged particles using a cathode tube. 

The particles were repelled by negative electrical fields, so he reasoned they were negatively charged. 

He reasoned that the atom must also contain positive particles, because atoms did not seem to be negatively charged.

Plum Pudding Model: A positively charged spherical cloud holds the electrons.

Rutherford Smashes Plum Pudding Model:

Rutherford found a positively charged particle about 7500 times the mass of the electron.

Rutherford created an alpha particle beam of positively charged particles, some of which get deflected by the air.  Curious, Rutherford sets up an experiment in which he shoots alpha particles at a thin metal foil and builds a circular detector around it.  Most of the particles go straight through the foil, but some are scattered or even bounced backwards! 

He concludes the plum pudding model is false, because ALL the particles would go through the foil like cannonballs through paper.  Therefore, he concluded that the center off an atom had a small, dense positively charged nucleus. 

Rutherford created the nuclear model of the atom, in which a small, dense positively charged center of the atom has moving electrons scattered around it.

1932 Rutherford discovers the NEUTRON, a negatively charged particle slightly heavier than the proton.

HW: Read pages 60 – 67.  DO p. 67 #1 – 3

_______________________________________________________________

Chemistry with Mr. Kalafus

Week of 08/17/2009

Monday: 1.1 and Introductions

Focus Questions: What is the nature and use of mathematics?  How should you comport yourself in class?  What are the procedures?

1)      Warm-Up: Index cards with parental contact info, last science class/teacher, student strengths and weaknesses

2)      Introductions and ice-breaker: 2 truths and a lie

3)      Procedures:

a.      Entering and starting class – sharpen pencil, straight to seat, check agenda for do-now (warm-up)

b.      Bathroom – extreme emergency only as per school rules,

go during passing periods

c.      HW – expect HW nightly Monday through Thursday with some weekend readings or short assignments

d.      HW is an essential component of practice.  Don’t fall behind.

e.      Bring your book and supplies every day

f.        Keep an ORGANIZED notebook with notes, HW, tests, quizzes, and handouts.

g.      SHOW WORK ALWAYS – USE A PENCIL – NO CALCULATORS

h.      Class rules

4)      Pre-reading questions p. 3

5)      Read pp. 3 – 8

HW 1: Signed syllabus

HW 2: p. 8 #1 – 5

Tuesday 8/18/09 1.2 Using Science

Concept question – How do scientists approach problem-solving?

1)      Warm-Up: Explain the scientific method.   Name the parts of a science lab.

2)      Collect and discuss HW

3)      Read pages 9 – 14.

4)      CW #1: p. 14 #1 - 4

5)      Read pages 15 – 18.

6)      CW #2 p. 17 #1 – 3.

7)      HW 3: p. 14 #4 - 6, p. 15 #11 – 13, p. 21 #1 - 10 

Wednesday:  2.1 Nature of Matter

Focus Questions: What is an atom? Element? Compound? Molecule? What are the most common states of matter?

1)      Warm-Up:  Is water a solid, liquid or gas?  What elements form water?

2)      Collect and discuss HW.

3)      Vocabulary:

a.      Matter – the “stuff” which the universe is made of

b.      Atoms – all matter is composed of timy particles called atoms (which in turn are made of electrons, neutrons, and protons; which are made of “quarks”)

c.      Elements – types of atoms

d.      Compounds – made by two or more different kinds of atoms stuck together

                                                               i.      H₂O

e.      Molecules – two or more atoms stuck together

                                                               i.      O₂

f.        States of matter:

                                                               i.      Solid

                                                             ii.      Liquid

                                                            iii.      Gas

4)      Read pages 24 – 29

5)      Lab p. 30?

6)      HW 4: P. 30 #1 – 3

7)      HW: Study for quiz Thursday on 1.1 – 2.1 see p. 18 (all) and p. 44 (2.1 only)

Thursday: 1.5 Solving Equations

1)      Warm-up: What is the differences between a solid and a gas?  Compare and contrast molecules and compounds.

2)      Physical change vs. chemical change

a.      Physical change

                                                              i.      State change (solid, liqud, gas)

                                                            ii.      Characteristics of compounds

                                                          iii.      Odor

                                                          iv.      Color

                                                            v.      Volume

                                                          vi.      Shape

                                                        vii.      Density

                                                      viii.      Melting point

                                                          ix.      Boiling point

                                                            x.      Solubility

1.      Ability to dissolve in various liquids, esp. water

b.      Chemical change

                                                              i.      A change in the chemical composition of matter

                                                            ii.      Ability to form new substances

1.      Burning something

2.      Hydrogen Peroxide breaks up into water and oxygen when exposed to light

3.      Rusting

4.      Digestion

5.      Rusting

3)      Quiz 1.1 – 1.3, 2.1

4)      Read pages 31 – 34.