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Week 10  – 11/1 – 11/5

                                                                                                                                                                                        Jump toTuesday,   Wednesday,  Thursday,   Friday                                                                                                                              ______________________________________________________________

11/1 – Monday – B Day – 2, 3b/4 Lab

Main focus –                                                                                                                                                         
                                                  

     a) To perform the analysis of carbonates (lab 9) .

     b) To continue with part 1 one of Test 2.

 Period 2: 

1. Continue with part 1 of test 2.                                                                                                                     

Period 3/4: 

1.   Lab 9 – Analysis of Carbonates Complete all calculations and hand in (No conclusion).   

2.  Lab 8 & Lab 9 salt visual comparisons. Can we determine differences in the macro based on the micro.

3.  Continue with Test 2.  You will be able to continue at home with part 2 of the test.   

                                                                                                                    

Friday’s Stoichiometry:

 

Pumpkin Stoichiometry:

 

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3b/4  Lab – Lab 9 – Analysis of Sodium Carbonate and Sodium Hydrogen Carbonate 

Lab 9 – Determine the identity of the carbonate by reacting the 2 salts with HCl to produce NaCl.  How much NaCl is made will determine the identity of the salt.   
 
                               The salts are either:          Na2CO3     –   sodium carbonate –  washing soda   
                                                                                     NaHCO3    –   sodium hydrogen carbonate –  baking soda                                                                                                                                                                                                                                                                               This a NOT a precipitation analysis lab but it an Analytical Lab as we will use stoichiometry to identify the starting salts by using how much NaCl is produced by reacting them with HCl.                                                                                                                                                
     Data gathering for Lab:
    a) mass out unknown carbonates A or B in an evaporating dish
    b) add excess HCl till the reaction reaches completion.
    c) place the evaporating dish on a hot plate under the fume hood (evaporating off the water to recover NaCl)
    d) Mass OUT dried NaCl    

Lab 9 review:

 

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11/1 – Monday Homework: – 

1.  Please complete all Labs ( labs 4 – 9). They are all due tomorrow.Lab 6 and Lab 9 do not have conclusions.   

2:  Please work on Test question  #1 (of part 2) which will be due in class. This page is the 1st question of part 2.

Test 2 – Part 2 – Question 1 – .pdf
View Download

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11/2 – Tuesday – A Day – 2/3a Lab, 4 

Main focus –                                                                                                                                                         
                                                  

     a) To Complete Part 1 of Test 2

     b) To begin Part 2 of Test 3

Period 2/3: 

1.  Collect part 2 – question 1

2.  Complete Part 1 of Test 2 

3. Gave back both precipitation quizzes. (The best out of the 2 went into Power School)                                                                                                Reviewed 2nd quiz (2nd one after the Golden Arches Quiz)

Stoichiometry 4c – Precipitation – limiting reagent key p .pdf
View Download

Golden Arches Quiz:
Stoichiometry 4a – Precipitation – limiting reagent Key p .pdf
View Download

4. Begin Part 2 of Test 2                                                                                                         

Period 4: 

1. Collect part 2 – question 1                                                                                                         

2. Complete Part 1 of Test 2
  
                                                                                                                      

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11/2 – Tuesday Homework: – 

1. Please work on Test question  #3 – #7 (of part 2) which will be due in class. 

 

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11/3 – Wednesday – B Day – 2, 3b/4 Lab 

Main focus –                                                                                                                                                         
                                                  

     a) To complete the Part 2 of the test

     b) To Review Concepts of Keq value and law of mass action

Period 2: – After today you will have one more class period for the test (you may come in the rest of the week on your time to complete.)

1.  Continue with test 2, question 3 begins.                                                                                                                

Period 3/4: – Last day to work on the test in class. 

1.  Continue with test 2, question 3 begins.

2.  Quick review of the precipitation quizzes.

Stoichiometry 4c – Precipitation – limiting reagent key p .pdf
View Download

Golden Arches Quiz:
Stoichiometry 4a – Precipitation – limiting reagent Key p .pdf
View Download                                                                                                        

                                                                                                                    

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11/3 – Wednesday Homework: – 

Stoichiometry 4d – Equilibrium and Stoichiometry worksheet (3 pages) completed correctly is worth                   5 EXTRA Credit Points for Test 2.  It needs to be in your test (folder of fun) by Friday afternoon.  Question 8 has aspects to it that this worksheet reviews/or teaches with the corresponding video below.                   

  1. Please view the lecture below on the Reaction Completion and Equilibrium basics.

  2.  Follow along with me with the lecture to complete the worksheet below and/or review with the key:

Stoichiometry 4d – Equilibrium and Stoichiometry .pdf
View Download

Stoichiometry 4d – Equilibrium and Stoichiometry key .pdf
View Download

 3. Please work on Test question  #8 – #9 (of part 2) which will be due in class. 

Test 2 – Part 2 – Complete .pdf
View Download
 

1 :Reaction completion AND Equilibrium basics

End of Wednesday..

 

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11/4 – Thursday – A Day – 2/3a Lab, 4

Main focus –                                                                                                                                                         
                                                  

     a) To begin our discussion of acid/base chemistry –

     b) To identify strong acids, weak acids, strong bases, and weak bases and relate these strengths             with Coulombs Law

Period 2/3: 

1.  Complete the last period of in class testing of Test 2. Place everything in your folders of fun.

2.  Acid/Basics intro lesson – We will continue our tour of Stoichiometry through acid/base chemistry                                                                                                              

Period 4: 

1.  Acid/Basics intro lesson – We will continue our tour of Stoichiometry through acid/base chemistry   

Acid/Basics intro lesson notes:

Acid/Base basics (no pun intended…ok maybe) – Stoichiometry through Acid/Base reactions.
 
                Demos – magnesium hydroxide, electrolyte 
                                        a) Strong Bases – weak bases Table F
                                             Coulombs Law!
 
                                        b) Acid and base definition introduction
                                                Why acids are dangerous? – what is the action of H+
                                                Why bases are dangerous?  – What is the action of OH
                                                Neutralization reaction –  example :  OH- from Mg(OH)2
                                        c) Conductivity of metals – mobile electrons
 
                                        d) Electrolyte definitions – mobile ions
                                                Strong ACids and Bases are strongest electrolytes
                                                Salts that are soluble are electrolytes in (aq) and (l) phases only
                                                Stiochiometry is with Strong Acids or Strong Bases – (completion reactions)
                                                Weak acids/Weak bases do not completely dissociate.
                                                Vinegar (organic acid) weak acid = structure
 
                                          e)   Strong Acids – from Halogens – why HF is weak and why HCl, HBr, HI are strong?
                                                Coulombs LAW!!!!       
 
                                        Milk of Magnesia = Mg(OH)2                                                                   Drano = NaOH
Both produce OH- ions but one is dangerous why?

                  NaCl (s)

 Ionic solids  – NOT Electrolytes!

(positive and negative ions locked in a crystal)

  They are never electrolytes because the do not conduct electricity in solution or as a  liquid.  The ions ARE NOT FREE and thus cannot move.  It is the movement of ions that will enable them to conduct a charge.  All ionic compounds are a solid at STP due to STRONG COULOMBIC Attractions between the positive and negative ions.  Each ion is actually surrounded by 6 other oppositely charged ions that keep the ions in a very stable (low energy) structure.

THUS IONIC Compounds in a solid state NEVER conduct a charge!

  Ionic liquids – Electrolytes

 These liquids require very high temperatures to occur as the ions would want to attract to each to form a crystal at lower temperature BUT at these high temperatures these liquids (of negative and positive ions) can conduct because the ions are free to move!

               NaCl (s)     —–>      Na+(aq) + Cl (aq)

 Ionic solutions –  Electrolytes
(dissolved ions) – must be soluble! 

These solutions ARE electrolytes!  The ions although surrounded by water, are free to move and thus charge can be conducted through. the solution.

IF the ionic solid is insoluble then it will not make a solution and the ions will still be locked in a crystal which will result in no charge being conduced         

                                Sucrose (s)

 Molecular compounds – NOT Electrolytes!

Make molecules not ionic crystals

These are made from nonmetals (small atoms) with a high attraction for electrons. These compounds make bonds by fighting for electrons between atoms since they all have high attraction for electrons. Each bond — is a pair of electrons between these atoms.  Because of the “tug of war” for electrons between these compounds, these electrons are not free to move and conduct a charge.  In fact because the electrons are held so tightly these compounds are so poor at conducting we call them insulators.

Molecular compounds NEVER conduct as a solid or in a solution (even if they dissolve).
Molecule compounds NEVER conduct in a solution because they are molecule with NO charge and thus are not electrolytes!
Even if they are dissolved in solution there are no ions as theses are only atoms (Neutral!)

             Metallic compounds – Fe (s)

   Metallic compounds  – NOT electrolytes

 These compounds do conduct in the solid state because they are made of metals (large atoms with a low attraction for their electrons) and thus allow the electrons in their outer most shell to “roam” throughout the crystal.  They unlike molecular compounds have loosely held electrons and thus these electrons are allowed to move freely.  Free moving charges conduct electricity!!

We say that metallic compounds have a sea of mobile electrons in a crystal of positive nuclei.  Do not confuse the positive circles with ions as they are the nuclei of the atoms.

So electrolytes are compounds that conduct electricity as FREE IONS!
 
                    a) IONIC compounds (salts) that are melted (molten)
                    b) IONIC compounds (salts) that are dissolved
                    c) Base solutions – FREE OH–  ions
                 d) Acid solutions – Free H ions
 
NOT Electrolytes:
                     a) Ionic solids in the solid phase 
                     b) Molecular compounds
                     c) Metallic compounds
 
                                                                                                                   

Acid/Base Intro Presentation:

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11/4 – Thursday Homework: – 

                                                                                                                                                                                                                                  1.  Please continue our acid base intro with the lecture 2 video below IF you need a refresher on today’s intro acid and base lesson.

2.  Complete the form below on today’s concepts.You will have 3 graded submissions.                           

1 :Acid Base Intro 1 lesson:

 

1 :Acid Base Intro 2 lesson:

 

 2: Acid base intro Lesson Form

End of Thursday..

Electrolytes Demo (Ernie!):

 

Milk of Magnesia Demo (Weak Base = insoluble salt with a hydroxide):

 

 

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11/5 – Friday – B Day – 2, 3b/4 Lab  

Main focus –                                                                                                                                                         
                                                  

     a) To review concepts of an electrolyte with acid and bases and their relative strengths.

     b) To define and review the ACID /Base guys.

 Classwork:
Acid and Bases Intro packet new.pdf
View Download

Period 2:  – 

1.   A quick review of the electrolyte concepts (free ions), strong and weak base and acid.

2.   Acid/Base definitions – beginning of the acid/base packet       

3.   Weak acid/base equilibria, Conjugate acid, Conjugate base                                                                                       

Period 3/4: – 

1.   A quick review of the electrolyte concepts (free ions), strong and weak base and acid.

2.   Acid/Base definitions – beginning of the acid/base packet       

3.   Weak acid/base equilibria, Conjugate acid, Conjugate base       

Notes for today:

This is the mechanism of how CO2 acts an acid by the the Lewis Definition.

The most complete definition is the Lewis acid base definition because there are acids and bases that DO NOT HAVE protons to donate or possibly accept BUT create acidic conditions or Basic Conditions.
 
In table K they list CO2 an acid but it had no protons to donate?  It is an acid because when we bubble CO2 in water the conditions in water become more acidic.  
 
                    CO2  +   H2O             ——>              intermediate                  ——>             H2CO3
                                                                                                                                                                                      then…..
                                                    H2CO  +   H2O  <——>  H3O+  +   HCO-1
 
CO2 can accept a pair if electrons (JUST LIKE a proton!!!) so the best and most complete definition of acids and bases is the LEWIS acid base definitions! Lewis acids like CO2 are electron acceptors while bases like water in the example are electron donators!!
 
4. Demo with straw and pH probe.

CO2 acts an acid by the the Lewis Definition.

The most complete definition is the Lewis acid base definition because there are acids and bases that DO NOT HAVE protons to donate or possibly accept BUT create acidic conditions or Basic Conditions.
 
In table K they list CO2 an acid but it had no protons to donate?  It is an acid because when we bubble CO2 in water the conditions in water become more acidic.  
Back to the pumpkin Stoichiometry from last week:

C2H2 (g)  +   5/2O(g)    —> 2CO2 (g)   +  H2O (g)

                                                                
                                             0r
 
2C2H(g)  +    5 O(g)    —> 4CO2 (g)   +  2H2O (g)
The chemical reaction that exploded the pumpkin was combustion or redox but the reaction the made fuel, C2Hwas?
What kind reaction is this?
 

                       CaC2 (s)   +   2H2O (l)           —–>                C2H2 (g)    +    Ca(OH)2

The Arrhenius definition although a good start to defining acids and bases is not complete because we have chemicals that do not have any hydroxide ions in their structure (like NaOH) but will create acidic or basic conditions in water.  In the case above,  the hydroxide ion (OH) was produced by the action of the  carbide ion (C2-2).   So the Bronsted-Lowry definition is a more complete definition because it includes those chemical species that Produce the Basic or Acidic conditions by Accepting a proton or donating a proton.                                                                                                                                                                                     
In the case above the carbide ion (C2-2) ion is the Bronsted-Lowry base (the carbide ion accepted the proton.) and the water is the Bronsted- Lowry acid (because water DONATED A PROTON) (
 
*Notice that acids must have electron deficient hydrogen to donate protons (H+).
 *Notice that Bases must have an ability to accept protons (H+).  Having a lone pair of electrons or having a negative           charge helps attract the protons!
 
                  The result of this acid base reaction is that acetylene C2H2 was produced.
 

                                                                                                           

                                                                                                                    

Today’s lecture:

 

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11/5 – Friday Homework: –  Make sure you refresh this page to make sure you have the current version!!!!

1. Please make two more submissions to last nights formMy key was wrong for question 7 and with what we did in class you should be able to complete it to perfection. Thank you Meghan!

Period 3/4 Needs to view reviewing the weak acid – weak base equilibria equation that we left off in class (where we identified the all the acids and bases on each side and the conjugate pairs) –
Please do so viewing the video below from 0:00 to 2:20.

2.  View lecture below (start at 14:40 to 37:50) and Complete Page 2 of the Acid base Intro Packet  and review with the key below (after watching the video): Please skip the Lewis Acid/base definition explanation. I will review that Monday!

Acid and Bases Intro packet new.pdf
View Download
 
Intro Acid Bases Packet Key 1718 p.pdf
View Download
 
3. NOW complete the all three of reactions (or the 2 remaining) on the Conjugate Acid Base Pairs and Complex ions new.pdf 
 and review with the key below:
 
Conjugate Acid Base Pairs and Complex ions new.pdf 
 
Conjugate Acid Base Pairs and Complex ions new key p.pdf
View Download

                                            So everyone should have the first 2 pages of the packet completed (excluding the Lewis definition on front page) AND should have the Conjugate Acid Base Pairs worksheet completed (front side).                                                                                                                                                                                                

Page 2 video for homework starting at 14:40: