Chemistry with Mrs. Foley

Chapter 13 -Large Quiz- Monday

Review problems at end of chapter – (1,7, 9,15,17,23,27,31,35,40,48,53,55,59)

Ch13_Outline

Welcome to 2nd semester!!

Please work on the following items Wed/Thur nights:

Please complete the Solubility of a Salt Lab by answering questions at end of lab using the textbook as a reference.

Complete the solution calculation worksheet you started in class.

And read Chapter 13.

We have discussed sections 13.1-13.4  Refer to another teacher’s podcast on these topics here:

http://podcasting.jessamine.kyschools.us/groups/jctcstamper/weblog/7b315/Solution_composition__Molarity__Molality__Mole_fraction____by_mass__Energies_of_solution_formation__Solubility_of_gases.html

We will look at sections 13.5 and 13.6 in class this week.

There will be a quiz on Chapter 13 on Monday 2/6.

Here is the answer key to reaction writing:

http://fc.bryanisd.org/~eeike/APChem_ChemEquations%20sol’n.pdf

Other worksheet answers:

Ca+2  +  2OH-  –> Co(OH)2

SrO  +  H2O  –>  Sr+2  +  2OH-

MgCO3  –>  MgO  +  CO2

2Mg  +  O2  –>  2MgO

3Zn  +  2Fe+3  –>  3Zn+2  +  2Fe

Practice problems: AP Chemistry Midterm Practice Problems

Answers: (***Note made answer key quickly while entertaining kids – potential for mistake on my part)

1.  +/- round to left most place value (  23.00 cm + 1.2 cm = 24.2 cm)   x/÷ round to least number of sig figs (52.65 g / 2.3 ml = 23 g/mL)

6. Ti   1s2 2s2 2p6  3s2 3p6 4s2 3d2            Ti+2 1s2 2s2 2p6  3s2 3p6 3d2

Cl-1  1s2 2s2 2p6 3s2 3p6                                 Cu+2  1s2 2s2 2p6 3s2 3p6 3d9

10 a. CΞN    b. C-N  c. sp3, sp, sp2

11. H-H    O=O    F-F    Br-Br   I-I    NΞN    Cl-Cl

16. FeCO3* 2H2O   0.659 moles Fe: 0.658 moles C  ( 1Fe: 1C)  4 moles H: 1 mole Fe   2 moles H2O: 1 mole FeCO3

17. electrolyte – ionic solution  conducts electricity    nonelectrolyte- molecular solution

18.   81.1% yield

19. a. 40.9% C 4.6% H 54.5% O                       b. C3H4O3                c. C6H8O6

20. a. 413kJ            b. 7.39 kJ                 c.    34.4 kJ

21. -233 kJ

22. a. radius of ion is smaller, Ca lost 2 e, 4th energy level lost, greater proton:electron ratio

b. greater charge ions, smaller size ions allow for greater attractive force between ions and greater l.e.

c. K has 1 v.e and Ca has 2 v.e.  K’s 2nd i.e. is much greater than Ca 2nd electron i s lower complete shell

d.  Al has greater effective nuclear charge than Mg

26. a. Xe has more electrons will larger electron cloud, more polarizable than Ne

b. Cu has metallic bonding with delocalized electrons between Cu cations.  CuCl2 is ionic, as a solid the + and – ions are in lattice structure

c. SiO2 has network covalent – atoms bond covalently, without simple molecules. CO2 is a nonpolar molecule with weak intermolecular attractions. 

d. NF3 has lone pair on N resulting in trigonal pyramidal nonsymmetrical shape. The F atoms are not distributed evenly around the N making the atom polar.  BF3 does not have a lone pair on B, as an exception to the octet rule resulting in trigonal planar, a symmetrical shape, allowing for the F atoms to be evenly spaces and nonpolar.

27.    -129.1 kJ

Here is a website with an interactive practice midterm:

http://chemmybear.com/groves/midterm.htm

Here is a website where you can select what area to be quized on:

http://www.sciencegeek.net/APchemistry/APtaters/directory.shtml

***Extra help review session for midterm exam – Monday, Jan 23

Lab notebooks – due Mon Jan 23

Test – Chapter 10 – Thursday

Complete practice problems and multiple choice worksheet

Answers to MC:

1. C

2. A

3. C

4. A

5. A

6. A

7. B

8. C

9. C

10. B

11. B

12. B

13. B

14. D

15. D

16. B

17. C

Lab Report – due Tuesday

Test – Chapter 10 – Thursday

Work on problems     1, 4, 9, 15, 17, 19, 21, 24, 29, 31, 37, 39, 41, 47, 49, 51, 55, 59, 65, 69, 72, 73, 77

Some websites to practice:

http://wps.prenhall.com/esm_brown_chemistry_9/2/668/171122.cw/index.html

http://www.sciencegeek.net/APchemistry/APtaters/chap05rev.htm

Another Teacher’s Podcast on gases

http://podcasting.jessamine.kyschools.us/groups/jctcstamper/wiki/e89a5/Gases.html

Please work on problems 51, 67, 70, 71 at the end of chapter 10.

Formal Lab Report – due Tuesday

Test- Chapter 10 – Thursday

Additional Chapter 10 Review Problems- due Wednesday

Molar Volume Lab due next Tuesday.

Chapter 10 test next Thursday.

Read and take notes 10.7-10.8 for Thursday.

Here’s a fun opportunity – check it out and see if its for you! Brain Bee at Trinity College Sun 2/19 at 3:00 Brain Bee flyer[2]

Chem Club – schedule has been modified slightly:

Jan. 12 – ALL Members – Additional topic of study Estimated time – 60 minutes

Jan. 19 – ALL Members – Practice on old Olympiad Tests Estimated time – 75 minutes (good review for midterm)

Jan. 26 – Exam week – No meeting

Feb. 2 – ALL Members – Additional topic of study Estimated time – 60 minutes

Feb. 9 – ALL Members – Additional topic of study Estimated time – 60 minutes

Feb. 16 – ALL Members – In House Competition to select team members for Hall Olympiad Team Estimated Time – 75 minutes

Feb. 23 – Optional – Practice Olympiad – Estimated time – 60 minutes

March 1 – Olympiad Participants – Practice Olympiad – Estimated time – 60 minutes

March 8 – Olympiad Participants – Practice Olympiad

****Thursday, March 15 is Chemistry Olympiad day at UCONN (8-12 Hall Students will participate in full day field trip)

Please complete problems 8, 9, 10 from Gas Law Worksheet and show work completely on a separate piece of paper to be turned in tomorrow.

If you want to check answers on 1-7 on worksheet, this is what Evangelista and his barometer got.

1. 1800 L

2. 3.85 atm

3. 32 g/mol

4. 1.21 L

5. 2.4 L

6. 3.46 atm

7. 1.96 g/L

Complete problems 1-7 on the worksheet “Chemistry Chpt 10 HW)

Show work out neat and organized.  Read and take notes on sections 10.1-1.5.

After this you can start reading and taking notes on sections 10.6-10.8.

You will have a lab report to work on next week.  Remember to be working on your lab notebook – due Mon 1/23.

Here is the powerpoint on Chapter 10.Ch10_Outline

Happy New Year!

See below to review organic nomenclature.  Test – Thursday

Lab Notebook is due Monday January 23. You will have one more lab this semester. You should be working on this now. See prior post for assignment.

Exam Schedule as of right now:

1/26 periods 8 & 7

1/27 periods 6 & 5

1/30 periods 4 & 3

1/31 periods 2 & 1

Chapter 25 (1-6)

25.1 Organic molecules – know hybridization learned earlier C can be sp4 sp3 sp2, stability of C-C, C-H bonds, properties (solubility, acids/bases)

25.2 Hydrocarbons – alkane (saturated) , alkene, alkyne, aromatic

25.3 Alkanes – be familiar with condensed structural formulas of alkanes, isomers, naming

Naming compounds is important – see website http://www.chemguide.co.uk/basicorg/conventions/names.html

http://www.sciencegeek.net/APchemistry/organic/ochem.shtml

practice naming http://chemistry.boisestate.edu/people/richardbanks/organic/nomenclature/alkanenomenclature1.htm

quia practice quiz http://www.quia.com/quiz/3439898.html

25.4 Unsaturated – naming

Organic Reactions – p. 997 addition reactions – alkene and halogen – double bond (pi) breaks and forms bonds with halogen atoms                                                 p. 1000 substitution reations – aromatic and molecule – an atom or atoms of molecule replaces an H                                                                           p.1007 Esterification reactions – carboxylic acid and alcohol form an ester and water (condensation rxn)                                                                                               p. 1007 Saponification reaction – ester(triglyceride-fat)  and base form salts of  fat and alcohol

p.998-999 – don’t worry about now, will learn later

Functional Groups – study table 25.4 – you need to be able to identify a functional group (matching!)

p.1000-1009         alcohols, ethers, aldehydes, ketones, carboxylic acids, esters, amines, amides – learn a property of each.  You do not need to name compounds of these.

Outline of chapter:  Chpt 25 outline

Powerpoint for Chapter 25: I didn’t have it to upload. Click on the google search below and you can download from first website.

https://www.google.com/search?sourceid=navclient&aq=f&oq=brown+lemay+chapter+25+powerpoint&ie=UTF-8&rlz=1T4ADFA_enUS396US397&q=brown+lemay+chapter+25+powerpoint&gs_upl=0l0l0l240358lllllllllll0

textbook website with multiple choice questions

http://wps.prenhall.com/esm_brown_chemistry_9/2/681/174467.cw/index.html

Lab Notebook Assignment AP Chemistry Lab Notebook

Past lab assignments not yet returned to you (if you want to work on reflections for lab notebook)

alkaline earth lab

The Halogens

Bring in a new toy or gently used children’s book (any age) to donate to FBLA drive for local hospital.  Great cause.  If everyone brings in one item that will give 35 children something to smile about.  The drive ends tomorrow, please bring in item to class. 

Study your ions for ion quiz on Monday!http://www.chemmybear.com/stuff.pdf

Try going here for flashcards on ions.  http://www.quia.com/profiles/jfoley144

Work on reading Chapter 11 and completing problems. You should do at least half of below for Monday. Test is on Thursday. 

Here is the powerpoint for this chapter. Ch11_Outline

11-1 Solids, Liquids, Gases p.442 (1,3,5) What are the differences between solids, liquids and gases?

11-2 IMF p. 442 -443 (7-21 odds) The type of interparticle attraction affects if a substance is a solid, liquid or a gas at room temperature, as well as its boiling and melting points and other properties.  Particles are held together by electrostatic forces.  Ions are held together tightly because there is a complete positive and negative charge.  Ionic compounds are always solids and have high melting points which vary because of charge of ion and size of ion.  Metals are positive cations with mobile electrons.  These ions are also held together tightly because of a complete charge.  They are solids (except Hg) and have high melting points.  Covalent compounds have intermolecular forces.  Molecules are neutral particles that can have partial positive and negative ends (dipoles) because of motion of electrons.  Because there is no complete charge in molecules, intermolecular forces are weaker than between ions seen in ionic and metallic substances.  The IMF vary depending on polarity, total number of electrons, and even shape of molecule.  Be able to compare boiling points of substances given their formulas. 

***Chemists have recently considered changing the definition of the hydrogen bond.  It is thought that it acts more like a covalent bond (sharing of electrons) than an electrostatic force. Read about this here.  This is a great example that science is changing and a lot of what we learn are theories that get modified.   http://blogs.nature.com/news/2010/11/chemists_redefine_hydrogen_bon.html

11-3 Properties of Liquids p. 443 (23, 25) The properties of liquids depend on the IMF.  What are viscosity, surface tension, cohesive and adhesive forces and how are they related to IMF?

11-4 Phase Changes p. 443-444 (27-35 odds) What are the names of the phase changes? How is energy involved in changing phase?  Remember the lab that we did in freezing and melting water and how temperature remains constant during a phase change.  Interpret heating and cooling curves.  Use molar heat of fusion, vaporization, and sublimation to solve energy calculations (same as heat of reaction) How much energy is needed to melt a certain number of grams of ice?  Know what critical temperature and pressure are.

11-5 Vapor Pressure p. 444 (37-45 odds) Know what vapor pressure for a liquid means and how IMF and temperature affects it.  Know the diagram (figure 11.23) that shows average distribution of k.e.of molecules for a liquid at room temp to show that evaporation can occur at room temperature. 

11-6 Phase Diagrams Be able to intepret a phase diagram for a substance.  Know how the phase diagram for H2O and CO2 vary. 

11-7, 11-8 Solids Know the difference between amporphous and crystalline solid.  Know that different unit cells form for crystals.  Compare simple cubic, body-centered, and face-centered cubic.  Understand close packing of solids and coordination number. Compare the four types of solids, how they form and their properties (table 11.7). Describe the difference in carbon bonding seen in diamond and graphite.

The network covalent bonds carbon atoms can be altered.  This is seen in the study of nanotechnology. Here are some video clips on this topic.  http://www.vega.org.uk/video/programmeset/12

Here is a great video that summarizes hybridization and sigma and pi bonds.

http://www.youtube.com/watch?v=d1E18tBTlBg&feature=related

Here is animation that shows pi and sigma bonds:

http://www.mhhe.com/physsci/chemistry/animations/chang_7e_esp/bom5s2_6.swf

Links that show VSEPR shapes:

http://intro.chem.okstate.edu/1314F97/Chapter9/VSEPR.html

http://www.youtube.com/watch?v=i3FCHVlSZc4

Below are links to animations for different concepts seen in chapter 8 and 9.

http://wps.prenhall.com/esm_brown_chemistry_9/2/666/170666.cw/index.html

http://wps.prenhall.com/esm_brown_chemistry_9/2/667/170888.cw/index.html

Below are links to multiple choice questions from chapter 8 and 9.

http://wps.prenhall.com/esm_brown_chemistry_9/2/666/170666.cw/index.html

http://wps.prenhall.com/esm_brown_chemistry_9/2/667/170888.cw/index.html

Read sections 9.4, 9,5 for Thur and 9.6 for Fri  and Worksheet/Textbook problems for Mon

Test – Chapters 8 & 9 – Tuesday

Powerpoints: Ch08_Outline  Ch09_Outline

9.1 – Molecular shapes intro

9.2 – VSEPR Model - Know the names and structure of the different molecular shapes.  Be able to estimate shape and bond angle of central atoms in a large molecule.  Know that a lone pair and multiple bonds repel more than single bonds.  Study table you completed in class of shapes.

9.3 – Molecular Polarity – molecules with symmetry can be nonpolar

9.4 + 9.5 – Orbital Overlaps and hybridization

9.6 – Multiple bonds

Complete bond enthalpy problem p. 310 (63) for Tue

Read and take notes on Chapter 9 sections 1 & 2 for Wed

Please read chapter 8, take notes and complete practice exercises.

Suggested order and practice problems:

Start with 8.5 – Be able to draw lewis dot diagrams for molecules and polyatomic ions. Use formal charge to support best possible diagram.  p. 309 (43, 45)

 8.6- Know when resonance can occur and what that means. Be familiar with benzene as an example. p. 309 (49, 51)

8.7 – Know the three types of exceptions to the octet rules.  p. 309 (57, 59)

8.8 – Use bond enthalpies to calculate ΔH (This is another way to find heat of reaction. ΔH = Σbroken bonds – Σformed bonds          Know what factors affect bond length        p. 310 (61)

8.1 -so easy! 

8.2 -Know the factors that affect lattice energy. Read A closer Look on p. 280 about the Born-Haber Cycle. p. 308 (13, 17, 19, 21)

8.3 – so easy!

8.4 Know how a difference in electronegativity affects bond polarity. Know what is meant by a dipole moment and the variables that affect it. p. 308 (35, 37, ) You do not need to calculate dipole moments.

Quiz Tomorrow on Chapter 7

See prior posts for helpful information

Here is the answer key for worksheet due today. PT HW answer

Complete We Are Family Packet and Read Chapter 7 and take notes. 

Here is an outline of the chapter

chpt 7 notes2 (updated)

Here is a powerpoint from this chapter

Ch07_Outline

website companion to our text – click on Student Activities for short videos of important concepts- and Problem Solving for Multiple Choice Quizes on Chapter 7.      http://wps.prenhall.com/esm_brown_chemistry_9/2/665/170446.cw/index.html

Another teacher’s podcast on:

atomic radius, ionization energy, electron affinity: http://podcasting.jessamine.kyschools.us/groups/jctcstamper/weblog/50d04/Periodic_trends__atomic_size__ionization_energy__electron_affinity.html

electronegativityhttp://podcasting.jessamine.kyschools.us/groups/jctcstamper/weblog/c1119/Types_of_bonding__Electronegativity__Bond_polarity__Dipole_moments__Ionic_size.html

Please complete Halogen Lab with flowchart and questions.

Test on Chapter 6 on Tuesday. See helpful items below.

Here are more sample calculations for this section:

light problems                               Bohr/ deBroglie Calc

Textbook Multiple Choice Problems

http://wps.prenhall.com/esm_brown_chemistry_9/2/664/170213.cw/index.html

Powerpoint on new atomic model:

http://preparatorychemistry.com/11Bishop.pdf

Podcast on Bohr’s Model

http://podcasting.jessamine.kyschools.us/groups/jctcstamper/weblog/043fa/Electromagnetic_radiation__Nature_of_matter__Atomic_spectrum_of_hydrogen__Bohr_model.html

Want to know more about Bohr

http://www.nobelprize.org/nobel_prizes/physics/laureates/1922/bohr-bio.html

Chem Club this week (Thur) is Chem B Chem Club 2011-12

Work on Chapter 6 problems (3,5,7,9,11,13,17,21,25,27,33) due Thur

Here are some helpful items:

video we watched on Dr. Quantum http://www.teachertube.com/viewVideo.php?title=Dr__Quantum&video_id=235180

Lecture Notes Chapter 6   Lecture Notes Chapter 6

Chapter 6 Powerpoint Ch06_Outline

Work on Chapter 6:

Read the following sections and complete sample/practice exercises.

6.1, 6.2,6.3 (S+P 6.1-6.4)

6.4,6.5,6.6 (S+P 6.5-6.6)

6.7, 6.8, 6.9 (S+P 6.7-6.9)

“Chapter 5 Problems” Answer Key

1.  exo       exo

     endo     exo

     exo       endo

     endo     endo

     exo       endo

2.  a) 45.9  J/K

     b) 0.917  J/g K

3.  9.02 J

4.  50,000 kJ

8.  -891 kJ

9.  -75 kJ

10.  -47 kJ

11.  26.2 kJ/mole

12.  -746.95 kJ

13.  -3,245.2 kJ

14.  -2,569.8 kJ

 Hess’s Law

1.   -1630 kJ

2.   -486 kJ

3.   +256 kJ

Heat of Formation

a) -134 kJ

b) -566.0 kJ

c) -890 kJ

d) -1120 kJ

e) -113 kJ

“NChO Ch 6 Thermochemistry” Answer Key

1999

27.  B

1998

22.  C

24.  A

25.  C

26.  A

1997

19.  C

24.  A

25.  A

1996

22.  D

23.  C

1995

21.  D

22.  B

23.  A

26.  C

1994

24.  A

27.  C

1993

13.  C

15.  C

click on this website for work to answers for last page:

http://chemmybear.com/groves/apch06_ptap_ans.pdf

a) C2H2 + 2H2 –> C2H6

b) -311.4 kJ

a) -3058 kJ

b) -160.6 kJ

School tomorrow!!!

Below is a worksheet that will be part of a packet I give you tomorrow of additional Chapter 5 problems.  You can get a head start tonight.

Chpt 5 problems

Also, this Thursday’s Chem Club will be open to all AP chem students (all Chem Club students are expected to come). It is a scheduled A day, but we missed a B day last week(that lab will be made up at another time).  It will be a problem session for chapter 5  2:15-3:15.

Here are my answers to the Chapter 5 problems. 

I hope you are all getting by. So no school this week. But guess what – the AP exam will not be postponed.

I don’t have access to updating this regularly. You should have read all of Chapter 5 and completed sample problems.
Also complete:
Problems at the end of chapter 5 (3, 11, 13, 23, 25, 29, 31, 33, 41, 43, 45, 47, 49, 51, 57, 59, 61, 63, 67, 69, 73, 75)
Read and take notes Chapter 6 6.1-6.9 review each sample problem within the sections and try the practice exercises

When we return to school, we will review Chapter 5 quickly and take a test on it and then proceed to chapter 6. The more time you can work on reading and trying problems now, the easier time you will have when we return.

I do not have power or access to the internet, but if I am able I will update this with answer keys.

Stay warm and positive!

Please work on Chapter 5 as follows: (The problems are within the chapter – review the sample exercises and complete the practice exercises)

Tues – 5.1-5.3 read and take notes

Wed- 5.4 read and complete problem 5.5

Thur- 5.5 read and complete problems 5.6 and 5.7

Weekend- 5.6-5.8 read and complete problems 5.9-5.13

Here is the powerpoint for Chapter 5 Ch05_Outline

Chalk Lab – Letter to Ms. Powder – one per lab group – address her questions, include data, calculations- due Monday

Study Sections 4.5 and 4.6- quiz Tuesday

• Molarity
• Making solutions using a volumetric flask
• Molarity of ions in an electrolyte solution (ions dissociate and multiply)
• Dilutions
• Solution Stoichiometry (use molarity use convert volume ->moles)
• Titrations

Complete problems

4.5 problems 53-63 odds

4.6 problems 65, 69, 71, 73

 Here is a video of a teacher solving a solution stoichiometry problem:

http://www.youtube.com/watch?v=n5TaI_XR3y4&feature=related

Please read section 4.5 and study sample problems 4.11, 4.12 and 4.13.

A letter (one per lab group) to Veronica Powder for the making chalk lab is due Mon 10/24.

Test on Chapter 3 sections 3-7 on Tuesday.

Complete problems at the end of chapter 3 (18 a,19a, 23,33,37,45,65,47a,49,55,59,69,71)

Powerpoint on Chapter 3: Ch03_Outline

Your homework is the worksheet given in class on conversions using the mole, mass, and number of particles.  A copy can be found below. This is due on Thursday.

mole conversions2

Today we looked at Percent Composition problems and Empirical Formula problems.  Please complete worksheets given in class. This is in chapter 3 sections 2-6.

 A couple errors on worksheet – 1.b. should ask about iron, not Mg and 5 should aska bout iron, not aluminum!

Please read sections 3.3-3.6.  Take notes on different types of calculations.  Review sample problems and complete practice problems within the sections. These calculations include:

%composition

molar mass

mass ↔ moles ↔ # particles

empirical formula

stoichiometry conversions (mole↔mole, mole↔gram, gram↔mole, gram↔gram)

Finish the Types of Chemical Reactions Lab.

Tomorrow After school 30 minutes 1st Chem Club Meeting Bring: $25 check

The Nobel Prizes were awarded today. The Nobel Prize in Chemistry 2011 was awarded to Dan Shechtman from Israel “for the discovery of quasicrystals”. Read about his story below.

http://www.guardian.co.uk/science/2011/oct/05/nobel-prize-chemistry-work-quasicrystals

Reminder: Chem 4 Kids Meeting Wed
Chem Club Meeting Thur 30 minutes please bring check Hall High School $25

Today we worked on reaction writing in class.

Test on 3.1 3.2 4.1 4.2 4.3 4.4 is Tuesday.

Here are the answer keys to the worksheets that you should be working on.  Work through them first and then check answers.  (Click on them to enlarge.) You should have also completed the textbook problems and check answers with answer key given in class. 

Two simple animations of precipitation reactions:

http://www.wisc-online.com/objects/ViewObject.aspx?ID=GCH2904

http://www.mhhe.com/physsci/chemistry/animations/chang_7e_esp/crm3s2_3.swf

Today we took a quiz on formula writing.  You should have read the textbook and be working on the textbook questions (see earlier post) for 3.1, 3.2, 4.1-4.4  Test on this section will be on Tuesday. Study the different types of reactions, writing equations, balancing reactions and solubility rules.

Check out these great(?) solubility rules videos:

http://www.youtube.com/watch?v=yf9wzB_fUkQ

http://www.youtube.com/watch?v=VJoKQ3ULCVs&feature=related

http://www.youtube.com/watch?v=3-3g36nzj-g&feature=related

http://www.youtube.com/watch?v=SnOZxLnJnF0&feature=related

http://www.youtube.com/watch?v=aLrXaSSW1zI&feature=related

Also: Have you tried any of the links to the right?  Try these:

Videos by chemistry teachers on writing reactions:

http://podcasting.jessamine.kyschools.us/groups/jctcstamper/weblog/962a5/Precipitation_rxn__Acid_Base_rxn__oxide_rxn__decomposition_rxn__coordination_compounds.html

http://vimeo.com/15032138

Today we went over the different types of reactions.

You should continue to read and take notes on 3.1, 3.2 and 4.1, 4.2,4.3, and 4.4. This reading should be done by Tue.

And then work on the textbook problems for these sections Chpt. 3 (3-13 odds) and Chpt. 4 (1-47 odds). 

Also, spend time on making corrections to your Chapter 2 test.  You will have a quiz on formula writing for ionic, covalent, and acids on Wednesday.  Study ions and charges. 

So in class earlier, we found out that electrons travel at just 1% of the speed of light and that nothing theoretically should travel faster than the speed of light. Check out this news article and audio on neutrinos that might actually travel faster!http://www.npr.org/2011/09/23/140745856/new-data-put-cosmic-speed-limit-to-the-test

(From Wikipedia:)A neutrino is an electrically neutral, weakly interacting elementary subatomic particle with a small but non-zero mass. Being electrically neutral, it is able to pass through ordinary matter almost unaffected, “like a bullet passing through a bank of fog”. The neutrino (meaning “small neutral one”) is denoted by the Greek letter ν (nu).

Neutrinos do not carry electric charge, which means that they are not affected by the electromagnetic forces that act on electrons. Neutrinos are affected only by the weak sub-atomic force, of much shorter range than electromagnetism, and are therefore able to travel great distances through matter without being affected by it. Neutrinos also interact gravitationally with other particles.

Neutrinos are created as a result of certain types of radioactive decay, or nuclear reactions such as those that take place in the Sun, in nuclear reactors, or when cosmic rays hit atoms. There are three types, or “flavors“, of neutrinos: electron neutrinos, muon neutrinos and tau neutrinos. Each type also has a corresponding antiparticle, called an antineutrino. Electron neutrinos (or antineutrinos) result when protons decay, through beta decay, to neutrons, or vice versa. Interactions involving neutrinos are mediated by the weak interaction.

Most neutrinos passing through the Earth emanate from the Sun. About 65 billion (6.5×10¹⁰) solar neutrinos per second pass through every square centimeter perpendicular to the direction of the Sun in the region of the Earth.

Today we took the test on Chapter 2.

Please complete the Metallic Bully Lab for Monday.  This includes a separate piece of paper writing out the full reactions, oxidation and reduction half reactions and the net ionic equations for each of the reactions that you observed.  Also complete the questions on the worksheet.  So which metal is the biggest bully (oxidizes easiest)? What is a metal that would be an even bigger bully – more reactive than Magnesium?

Please read and take notes on sections 3.1 3.2 4.1 and 4.4 for Monday.

Textbook questions for this section include in chapter 3: (3-13 odds) and in chapter 4 (1-9 odds and 35-47 odds). Please complete these by Tuesday.

This reaction demonstrates two different “types” of reactions. What are they?

What type of reaction does the following cartoon personify?

Answers to formula writing worksheet given in class:

CaCl₂  P₃O₅  SO₂  CCl₄  Na₂CrO₄  HBr  MgBr₂  Fe₃(PO₄)₂  Al₂(SO₄)₃  Ag₃N  Sn(HCO₃)₄  H₂SO₃

 Ferric sulfide, calcium sulfate, dinitrogen tetroxide, phosphorus trichloride, potassium chloride, stannic oxide, carbon monobromide, tetrasulfur decoxide, carbonic acid

 Carbon disulfide, stannic hydroxide, potassium oxide, acetic acid, ammonium dichromate, sulfur monoxide

 AgNO₃, HBr, BF₃, FeSO₄, H₂CrO₄, N₃I₇

 Cd(ClO₄)₂   (should be cadmium perchlorate)

Today we looked at the answer keys to the formula writing worksheets, how the mass spectrometer measures atomic weights, that angstroms are used to measure diameter of an atom and the charactertics that elements have based on location of element on periodic table.  Please work on the textbook problems listed on prior post tonight.  The test on Chapter 2 is on Friday. STUDY THE IONS!!!!

Here is the powerpoint on Chapter 2. Ch02_Outline

Here’s a teacher’s website from a different school that summarizes nomenclature and gives practice quizes. http://chemistry.alanearhart.org/Old/Tutorials/Nomen/index.html

Here’s another teacher’s videos on formula writing. http://www.kentchemistry.com/moviesfiles/chemguy/advanced/ChemguyCompounds.htm

Also, did you check out the textbook’s -The Central Science- website —> found under AP Chem links –> It has tutorial info and practice quizes to study Chapter 2.

Please read and take notes on Chapter 2 for Monday.

Complete problems by Wednesday.

(11, 17, 19, 21, 23, 25, 26, 27, 29, 31, 33, 35, 37, 45, 47, 49, 63, 65, 70, 86)

You will need to memorize ions and their charges for the next test. 

Find the formula and charge for the following ions:

acetate
ammonium
bicarbonate (hydrogen carbonate)
carbonate
chlorate

chromate
hydroxide
nitrate
phosphate
sulfate
sulfite

Today we completed looking at Chapter 1 (Test tomorrow) and the expectations to the Chromatography Lab write-up (due Friday).

On Thursday we collected data for the Density Lab. So what were the metals?  Use your slope of each line of best fit to determine.  Complete sheet, data table, and graph for Monday.

Also on Thursday, we discussed significant figure rules. 

On Friday, we reviewed the sig fig worksheet, looked at how you could turn density into a conversion factor, if density = 5 g/mL, then 5 g = 1 mL so you could use   5 g/1 mL    or 1 mL/ 5 g. And we indirectly measured the thickness of aluminum foil and thickness of copper wire. 

Be sure to complete textbook problems (1, 7, 9, 11, 13, 15, 19, 21, 23a.,25a. 27, 31, 33, 35,37,39, 45, 49, 51, 62)

The answers to some of them are in the back of the book. After you work through them, check your answers. 

The test on Chapter 1 will be next Thursday. Here is a powerpoint presentation with notes from Chapter 1 – good to study. Chapter 1 Outline

Today I presented an important problem solving method to be used this year: dimensional analysis. Your homework is the worksheet I gave out in class.  Make sure that you use the method I reviewed.

Homework-

due Friday – Letter to Mrs. Foley – introduce self, strengths/weaknesses in school, past experiences in science, feelings about Chem

due Tuesday- Read Chapter 1

due Tuesday- Quiz on Element Symbols

Homework-

due Friday – Letter to Mrs. Foley – introduce self, strengths/weaknesses in school, past experiences in science, feelings about Chem

due Tuesday- Read Chapter 1

due Tuesday- Quiz on Element Symbols