Chemistry with Mrs. Foley

Your final exam for the class starts on Monday with the Multiple Choice Section. The Free Response section A and B will be taken Tuesday, Wednesday, and Thursday.

Work on multiple choice from old tests given in class.  Remember: no calculator and 75 questions in 90 minutes.

Work on packet of released free response given in class.

Check answers here: (you need to click on the year of the test scoring guidelines and find the question by number.)

http://www.collegeboard.com/student/testing/ap/chemistry/samp.html

Some other helpful websites:

Stuff I should know WS:page 1: http://www.chemmybear.com/stuff.pdf

page 2: http://www.chemmybear.com/stuff2.pdf

Test taking strategies: http://www.education.com/study-help/article/how-approach-question-type-ap-chemistry-exam/?page=2

Interactive Review by topic: http://www.sciencegeek.net/APchemistry/APtaters/directory.shtml

List of concepts to review: http://www.adriandingleschemistrypages.com/apguide.html

Even more problems, by topic: http://www.ugdsb.on.ca/ccvisci/APChemma/SampExQu.pdf

Don’t have an AP prep book, here’s a free one online: http://www.aeturnalus.com/upload/prep/AP/master_ap_chemistry.pdf

Study notes: http://www.chemmybear.com/stdycrds.html

http://www.myteacherpages.com/webpages/RStepien/files/AP%20Quick%20Review.pdf

Stay away from the energy drinks, work on as many problems as you can, eat healthy and get some sleep!

The hard work you put in from Sept -April will pay off.

Chapter 21-Nuclear Chem QUIZ -Wednesday

Work on review problems (1,3,5,7,11,19,23,29,31,33,37,39) at the end of the chapter.

Thur – Quiz – Reaction Writing – work on practice reaction writing, study solubility rules, ions formulas and charges

Answer Key:

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

Tomorrow is the test for Chapter 20. 

You have an answer key to problems at the end of the chapter.

Doing the problems in the book are better to prepare for the test than the packet given last week.

Problems to work on for review are:

3, 7, 9a,b,c, 14, 21, 23, 27, 35, 39, 49, 53, 57 a, 60, 73, 76, 79

Some things to focus on:

• Determine the oxidation number of any element.
• Identify for any element in a reaction whether it is gaining or losing electrons (LeO GeR).
• Explain that when oxidation occurs, reduction must also occur (RedOx).
• Correctly apply the terms oxidizing agent and reducing agent to a redox reaction.
• Know and be able to calculate the relationship between Ecell for a redox reaction, delta G and Keq.
• Use delta G = -nFE   and Ecell =Ecell (st) -0.0592/n log Q
• use K= e-deltaG/RT or log K= nE/0.0592
• There are two big topics in electrochemistry, (1) Electrolysis—in which electricity (moving electrons) causes chemical change, and (2) Electrochemical Cells—in which chemical changes cause a flow of electrons (electricity).

 Electrolysis

• During electrolysis, electricity applied to a solution causes ions to migrate to the electrodes.
• An electrode is the part of the conductor that touches the solution.
• Reduction always occurs at the cathode (red cat).
• Oxidation always occurs at the anode (an ox).
• Write equations for the reactions that occur at the electrodes when water undergoes electrolysis.
  (-) cathode: 2 H₂O(l) + 2 e^- ® H₂(g) + 2 OH^-
  (+) anode:    2 H₂O(l) ® O₂(g) + 4 H⁺ + 4 e^-
• Explain that during the electrolysis of an ionic solution, either the + ion can be reduced or water can be reduced.  In the same way, either the – ion can be oxidized or water can be oxidized.
• Use a reduction potential chart to determine which of two substances is more likely to be reduced or oxidized.
• State that electrical current is measured in Coulombs and 1 Coulomb = 1 amp·1 sec.
• State that 1 Faraday (F) = 1 mole of electrons = 96,500 Coulombs.
• Use the Faraday, amps and seconds to quantify electrolysis problems.

 Electrochemical Cells

(Voltaic Cells & Galvanic Cells)

• Oxidization always occurs at the anode and reduction always occurs at the cathode.
• Draw a simple electrochemical cell.
• Use the reduction potential chart to determine which chemical is the anode (smaller E°) and which chemical is the cathode (larger E°).
• State that standard conditions are 25°C, solutions are 1 M, and gases are 1 atm.
• Calculate the voltage of a standard cell as the difference in the two E° values.
• State that the anode is the (-) electrode because the chemicals are being oxidized (losing e^-’s).
• State that for non-standard cells, changes that drive the reaction forward increase the voltage. (The Nernst equation allows you to calculate this voltage for a non-standard cell.)

Test Tomorrow-Chapter 19

Were you missing the answer key to the last few problems, here it is:

answer key

Here is the powerpoint on Chapter 20:

Ch20_Outline

Chapter 19 Test – Thursday

Powerpoints used in Class:

Free Energy PPT

Chpt 19 review

Ch19_Outline

Work on problems at the end of Chapter 19, answer key given in class(1, 3, 5, 21-37 odds, 41, 43(a&d), 47-57odds, 61-69odds)

Also complete Free Response Problems.  Answer keys found here:

http://apcentral.collegeboard.com/apc/members/repository/ap06_chemistry_samples_q2.pdf

http://apcentral.collegeboard.com/apc/public/repository/ap11_chemistry_form_b_q3.pdf

Are you looking for a summer opportunity in the science field? Great way to get involved in research, meet new friends, live on college campus. 

Here is one at UCONN:

http://chemistry.uconn.edu/secret.htm

 Here is a website where you can search for summer programs by topic and location.

http://www.pathwaystoscience.org/programs.asp?u=HighSchool_High

Please work on Chapter 19 sample and practice exercises within the chapter.

For Thursday: Problems 19. 5, 19.6, 19.7, 19.8

For Friday: Problems 19. 9, 19.10, 19.11, 19.12

Also due Friday is the completed Qualitative Analysis of cation and anion lab.

Tomorrow is the quiz on Ksp.

Here are answer keys to free response questions.

I think these are videos on solving these problems.

http://www.edutube.org/en/video/ap-chemistry-solving-solubility-equilibrium-problems-ksp-part-i

http://www.edutube.org/en/video/ap-chemistry-solubility-equilibrium

Check answer key to Ksp worksheet in prior post.

HW- more Ksp problems WS found here:

http://apchemistrynmsi.wikispaces.com/file/view/Solubility+Equilibrium+FR+worksheet.pdf

Quiz Ksp problems -Wed

Also, be reading and taking notes on Chapter 19.

Make sure you have read 17. 4, 17.5, 17.6 and worked on sample problems 17.9, 17.10, 17.11, 17.12, 17.13, 17.15 and 17.16.

Then complete worksheet on Ksp given in class:

http://chemistryconnections.com/equilibrium/solubility4.pdf

An answer key to this will be posted later in the weekend.

Please also start to read chapter 19 and take notes.

Please work on Buffer problems – 2 worksheets – one given out other day, answer key given in class.

2nd – past AP exam question 1 – given in class found here: http://apcentral.collegeboard.com/apc/public/repository/ap09_frq_chemistry.pdf

answer key – http://apcentral.collegeboard.com/apc/public/repository/ap09_chemistry_sgs.pdf

Also read through lab for tomorrow and complete prelab, was given out in class.

copy found here – quals_lab[1]

Please work on the write-up for the titration labs.

Note-When working on calculations for titration of the standardization of NaOH, use the Ka of HP- as 3.9 x 10-6 and this is not perfect, you don’t know exact volume of initial acid, it called for about 5omL, for the sake of doing the calculations, assume the initial volume of acid is 50 mL.  Please show equations with ICE tables for finding initial pH and equivalence point pH.

Please write calculations very neatly and type up tables, explanations!

This is due Wed as well as 17.4-17-5 reading.

Tonight’s homework – Please read 17-3 on titrations and take notes.

Below is a link to the handout in class.

http://apchemistrynmsi.wikispaces.com/file/view/15+BUFFERS+MADE+EASY.pdf

On the link below, there is a video that goes to the handout on buffers.  This is helpful if you are absent or need extra help. Scroll down to acid/base equilibrium and click on companion video for Buffers Made Easy.

http://apchemistrynmsi.wikispaces.com/AP+Chemistry+Class+Lecture+Notes+AND+instructional+videos

Please work on past problems assigned and review section 16-10.

Do you know how to find the pH of a salt solution? Below is a website that works out this problem and #73 in the book (a,b,c) are good practice of this.

http://www.chem.purdue.edu/gchelp/howtosolveit/Equilibrium/Salt_Solutions.htm#phofsalts

Please study section 16-9 and complete problems 66, 72, 74, 76, 78, 79, 100

Here’s a tutorial on pH: http://www.wwnorton.com/college/chemistry/gilbert2/tutorials/interface.asp?chapter=chapter_16&folder=ph_scale

Attention Chemistry Olympiad Participants:  We can take all 13 participants to the local competition next Thur!  I found a great teacher’s website to help you prepare.  It has annotated answers to some of the released exams. Please spend time reviewing these.  Click on one of the local olympiad annoted answers.

  http://www.instruction.greenriver.edu/kmarr/Chem%20163/Exam%20Study%20Guides/Chem163%20Final%20Exam%20Study%20Guide.htm

http://portal.acs.org/portal/PublicWebSite/education/students/highschool/olympiad/CNBP_028637

Please complete the following problems at the end of Chapter 16 for tomorrow:

# 19, 21, 24, 26, 28, 29, 34, 38, 43, and 53

What a fun liquid Nitrogen Day!! 

Please read Chapter 16 and work on practice problems.

Here is the powerpoint.Ch16_Outline

 I will update the blog later in the weekend with other helpful practice problems.

Happy Leap Day!

Please work on reading sections 16.1, 16.2, 16.3 and 16.4

Here are textbook problems to work on. You received the answer key in class.

1, 3, 7, 9, 11, 17, 19, 23, 25, 27, 30, 33, 35, 41, 43, 45, 47

See earlier post for answer keys to worksheets. I have updated them because there were a couple errors.

Chem Club- this thur and next thur are for those participating in the Chemistry Olympiad.

Please continue working on chapter 15.  See earlier post for answer keys and helpful websites.

Test-Chapter 15- Tuesday

Did you google today?

Please read Chapter 15 Equilibrium, work on sample problems within chapter. 

Also complete worksheets given in class. See below for answer keys.

This is the Excel spreadsheet I set up to solve for x in number 9 on the study questions

 Quadratic Equation Solver:

http://www.math.com/students/calculators/source/quadratic.htm

Also check out these tutorials.

Kc vs. Kp:

http://www.wwnorton.com/college/chemistry/gilbert2/tutorials/interface.asp?chapter=chapter_15&folder=equil_gas_phase

Solving Equilibrium Problems:

 http://www.wwnorton.com/college/chemistry/gilbert2/tutorials/interface.asp?chapter=chapter_15&folder=solving_equilibrium’

Le Chatelier’s Principle:

http://www.wwnorton.com/college/chemistry/gilbert2/tutorials/interface.asp?chapter=chapter_15&folder=le_chateliers

test – chpt 14 – tomorrow

Chem Club – competition tomorrow 2:15-3:40

some asked for answers to Arrhenius – can be found on website below – but these get into graphing that does not need to done on test. 

http://apchemistrynmsi.wikispaces.com/file/view/12+Arrehenius+Made+Easy+soltuions.pdf

Sorry, I tried to post earlier and it didn’t work. 

Test – Chapter 14 – Thursday

Review Problems- answer key given in class

3, 6, 11, 13, 19, 21, 23, 25, 29, 31, 33, 37, 40, 43, 45, 47a,49, 51,55,57, 59, 61,65

 Here are some videos of another teacher covering Kinetic concepts. They are long, but really well done and are great if you were absent.

http://vimeo.com/15970385Instantaneous and Relative Rates along with Differential Rate Law Part I

http://vimeo.com/15970471Differential Rate Law Part II

http://vimeo.com/15994920Integrated Rate Law Part I

http://vimeo.com/15995052Part II

http://vimeo.com/15998163mechanisms

http://vimeo.com/16007475Arrhenius equation for calculating activation energy Part I

http://vimeo.com/16007568Part II

Chapter 14 Powerpoint – Ch14_Outline

Read sections 14.1, 14.2, and 14.3 for Wed – take notes and work on practice problems in sections.  Good Tutorial: http://www.wwnorton.com/college/chemistry/gilbert2/tutorials/interface.asp?chapter=chapter_14&folder=reaction_order

for Thur- finish worksheet problems from class 

Thur – kinetics lab

for Fri – read section 14.4 -take notes and work on practice problems

for Mon – read sections 14.5, 14.6, 14.7 – take notes and work on practice problems

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