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  Q1 : Week 7  – 10/12 – 10/16

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Please Make sure Your read all instructions for all assignments.    

LAB 6 – Metal Foil Lab is  Late!

LAB 7 – Percent by Mass of an hydrate is Due 10/13

LAB 8 – Empirical Formula of a Hydrate is Due 10/13

  _________________________________________                                                                                                                                   10/12 – Monday – Columbus Day – “Indigenous People Day”

Columbus discovered America?  But he only made landfall in the Bahamas and Cuba?  Wait didn’t the Vikings make the voyage before he did?  Wait the Chinese mapped out the America’s 70 years before the Viking voyage?  Wait, didn’t native american Indian’s “discover” the America’s first?  Wait wasn’t the America’s already here?

 ____________________________________________                                                                                       Jump to:  Tuesday Homework / top       10/13 – Tuesday – B Day – 1,2B

Main focus – 
 

a)  To determine the empirical formula of copper iodine (Lab 9).

                                  

Period 1,2:   

1.  Lab 7 explanation and note-taking

2.  Complete the Lab 7 – Empirical Formula of copper iodide – adding mass lab

a) Begin/complete the data collection of the Lab 9                                                                                                       b) Start the calculations/write-up of the Lab 9                                                                                                                 c) TEACH % yield, balanced reaction and stoichiometry                                                                                             d) Begin conclusion                                                                                                                                                                                   

We will complete all of your calculations from Lab 9 that lead to your                      

                       a) Mass of copper reacted
                       b) Mass of Iodine reacted
                       c) Mass of product (salt of copper and iodine)
                       d) empirical formula of copper and iodine 
                       e) Balanced chemical reaction of the synthesis of copper and iodine.
                       f) Calculate the Theoretical grams of the product produced.
                       g) Percent Yield.   
 

% Yield  =  experimental  x 100                                                                   theoretical

 

   

____________________________________________________________

Lab 9- Synthesis of Copper Iodide                                                                                                                             (and determination of the empirical Formula of copper iodide)

Lab 9 – Synthesis of Copper Iodide.pdf
View Download

Objectives:   

                         1. To determine the empirical formula of the salt (product).

             2. To calculate the Theoretical amount of grams of the salt through stoichiometry.

             3. To determine the percent yield of the salt.

 

In this lab a salt (ionic compound) will be synthesized from elements in a redox reaction. 

     Cu (s)  +  I2 (g)  —>  Cu? I?  

 The goal is to determine the empirical formula of the salt using the particle and mole concept. Empirical formulas can only be obtained through our current experiments but when it comes to salts or ionic compounds the empirical formula is the formula of compound because the formula is the lowest ratio of the crystal of ions.

We now know that Copper has 2 oxidation states, thus we are trying to identify if Cu lost 1 electron or 2 electrons?

Lab 9 review –  This might help with your calculations!

 

Lab 9 : Synthesis of Copper Iodide

_____________________________________________________                                                                                                             jump to:  top  10/13 – Tuesday’s Homework: – 

1. Please complete the Combustion analysis – 2006 FRQ.pdf worksheet and review with the key.

 

Combustion Analysis – 2006 FRQ.pdf
View Download

Combustion Analysis – 2006 FRQ Key.pdf
View Download

2. Please complete the Stoichiometry 1 – 2009 FRQ adapted worksheet with the video posted below.

Stoichiometry 1  – 2009 FRQ adapted.pdf
View Download

Stoichiometry 1  – 2009 FRQ adapted.pdf Key.pdf
View Download

                                                                                                      

Stoichiometry 1 – 2009 FRQ adapted Video Review:

 

 _______________________________________________________________________                             Jump to:  Wednesday Homework / top    10/14 – Wednesday – A Day – 1AB

Main focus – 
   
a)  To complete the Particle /Mole Concept History Lesson – mole concept finish
b) Review Combustion analysis, molecular formula, empirical formula

Period 1:

1.  Complete / Review the Mole Concept 

a) mole song – Mike Offut

b) Mole concept lesson – diagram, conversions

c) Why we need a mole notes:  H + Cl –> HCl 
     Why we need to balance chemical reactions!!!!
       We can use a scale to count!     

         – Scanning Tunneling Microscopy
          – pizo electric crystals 

Guy – Lussac —> mole concept/particle concept—> smallest movie   

—————1800————————1803—————————————––1831—————————-—--1860———–———–1905

                Voltaic Pile                        Humphrey Davis                                                    Michael Faraday’s                                 Mole Concept                         Atoms                                    created!                               electrolysis of water                                           Laws of electrolysis                                  created.                                 accepted!

 –Seeing atoms – Scanning Tunneling Electron Microscopy – (pizo electric crystal)

The need for a particle theory and mole theory.  They are deeply intertwined.
   

Richard Feynman said in Volume One of his Lectures on Physics:

If, in some cataclysm, all of scientific knowledge were to be destroyed, and only one sentence passed on to the next generation of creatures, what statement would contain the most information in the fewest words? I believe it is the atomic hypothesis that all things are made of atoms — little particles that move around in perpetual motion, attracting each other when they are a little distance apart, but repelling upon being squeezed into one another.

2. Review the analytical homework from last week and Tuesday. 

Percent by mass, empirical formula, molecular formula, combustion analysis.

Analytical Chemistry I KEY- determining chemical formulas.pdf
View Download

Combustion Analysis – 2006 FRQ Key.pdf
View Download

Stoichiometry 1  – 2009 FRQ adapted.pdf Key.pdf
View Download

                                                                                                                  

______________________________________________________                                                                                                                    

Mole Concept Diagram Lesson:
 
A mole is an abbreviated NUMBER that helps chemistry quantify the actual number of particles (atoms, ions, electrons, molecules, etc.) needed to DO chemistry. 
 
We need an abbreviated number because these microscopic particles ARE SO SMALL that we need a TREMENDOUS amount of them to have a significant amount of matter that we can measure with in the microscopic world.  Think how many atoms a mole of Al atoms stacked on each other would be?  (Lab 4!) It was over a 100 trillion meters even though each Al atom has 0.286 nm diameter!!  Light travels at about 10000 trillion meters per second so this distance would extend way beyond our solar system!
 
Please remember that the mole is a “how many quantity” that helps us actually Do Chemistry!!! From the mole concept we are able to:
 
1. Determine the atomic mass of elements (This is how we determined how elements  differed initially!!!).
2: Determine chemical formulas of compounds.
3: Determine the chemical equations of chemical reaction.
4: Predicting quantities like how much of product will we produce given a certain amount of reactants in a chemical reaction.
5:  Predicting quantities like how much of a reactant is needed to make certain amount of product.
6: Determining the quantities (V, P, T, n)  of a gas under changing conditions.
7:  Solve Electrolytic Problems (Amperage, how much metal is deposited on cathode, etc.)
8: Determine a concentration (Molarity = mole / Liter of solution) of a solution of ions etc.
9: Finding a quantity that is directly related to the mole.

The key is here is that we are able to use this How many Number not by counting particles which would be impossible but by USING A SCALE!   Because we decided to make the Relative Atomic Mass the equivalent in grams that 1 MOLE of every element would measure we can use a GRAM Balance or Scale to measure mass AND THEM convert to moles or vice versa.  
 
*OUR WINDOW INTO THE WORLD OF HOW MANY Particle IS THROUGH MASS or volume if a gas.
 
Using moles to answer how many is called Stoichiometry!!!
 
Stoichiometry works because of the Law of Conservation of Mass.
Because of Antoine Lavoisier and the Modern Atomic Theory by John Dalton, atoms are neither created nor destroyed in chemical reactions and are just rearranged into different ratios of elements in compounds.  These ratios are a How Many Value!
 
Stiochiometry also works because of the Law of definite proportions.
Because of Joseph Proust and the Modern Atomic Theory, each compound has its own unique arrangement of atoms called a chemical formula which results in each unique compound having a unique percent by mass of each type of atom (element) in its molecule.  This is due to compound having a unique ratio of atoms in their chemical formulas.  Chemical formulas are a How many Value!
 
Since chemical reactions are a result of atoms, molecules, and ions colliding as individual particles then to calculate the outcomes of reactions we must consider the moles (THE HOW MANY VALUE) of the chemical species. 

 

 

Particle / Mole Theory Presentation:

Scanning Tunneling Microscopy (STM):

 

____________________________________________________________                                                                    jump to:  top               10/14 – Wednesday’s Homework: –

 
1.  The lab is NOT due yet. I will review errors in lab tomorrow.
 

2.  Please complete the Stoichiometry 2 – Mole Concept Practice.pdf worksheet and review with the key or the video below.

Stoichiometry 2 – Mole Concept Practice.pdf
View Download
 
Stoichiometry 2 – Mole Concept Practice Key.pdf
View Download 

3. Please view Lecture 1.3 with the worksheet below.

     I will walk you through all questions except number 4.                                                                                                                                                          
4.  Complete Worksheet Stoichiometry 1 – balance yield.pdf (number 4) and review with key below:
 
Stoichiometry 1 – balance yield.pdf
View Download
 
Stoichiometry 1 – balance yield key.pdf
View Download 
                                     

2. Reaction of decomposing salt for Stoichiometry 2 – Mole Concept Practice.pdf

2. Review video for Stoichiometry 2 – Mole Concept Practice.pdf

3: AP Lecture 1.3 : Stoichiometry and percent yield 

 

_____________________________________________________________                                            Jump to:  Thursday Homework / top 10/15 – Thursday – B Day – 1,2B                                 

Main focus –             
 
a) To complete the error analysis of Lab 9.
b) To introduce solution equilibrium and molarity
c)  To introduce precipitation analysis analytical procedure.

  

   Period 1,2:
 

1.  Complete review of the error analysis of Lab 9 – Empirical formula of copper iodide

Please see my notes posted above video.

2.  Molarity and solution analysis introduction using worksheet below: 

We did question 1 from the worksheet below.

Analytical Chemistry II NEW – Mol,Dilution, precipitation analysis.pdf                                                            View Download

Analytical Chemistry II NEW – Mol,Dilution, precipitation analysis KEY Page 1.pdf                                                      View Download

3.  Lab 10 – Precipitation Analysis  

a) Mass out unknown group 1 carbonate
b) Dissolve the salt in water
c) Create a precipitate
d) Collect the precipitate on filter paper and add to oven for tomorrow.

                                                                                                                                

   Lab 9 : Synthesis of Copper Iodide – Error Analysis

Last few minutes I discuss how you can determine what your errors might be.

 

Errors in Lab 9 can be broken down the following way in how we obtained the mass of each element:

Remember to look at your actual ratio and not the rounded one to analyze.

mass of iodine :    copper & iodine product                –       initial mass of copper

 ↑ mass Iodine       (Recrystallization of I2 (s) = ↑ mass)                 –       initial mass of copper

   ↓ mass Iodine     (Loss of flakes while massing (s) = ↓ mass)       –       initial mass of copper

 

mass of copper :   initial mass of copper        –       cleaned copper

  ↑ mass copper:       initial mass of copper      –        (Scrapped some copper atoms off = ↓ mass)                 

 ↓ mass copper:       initial mass of copper      –        (*Did not clean off all of the product= ↑ mass)   

 ↓ mass copper:       initial mass of copper      –        (Did not completely dry = ↑ mass)   

 

_________________________________________________________________________________________                                                                              Lab 10 – Precipitation Analysis of an Alkali carbonate

                                                                                                                                                                                                                                Lab 10 – Gravimetric analysis of a metal carbonate NEW 1920.pdf
View Download
 

Objectives:   

                         1. To identify the formula of a alkali carbonate form by precipitation analysis.

             2. To determine the theoretical mass of the precipitate.

             3. To determine the percent yield of the precipitate.

  

Data gathering for Lab 10 –
     
Measure your data from Lab 10 – Gravimetric analysis of a metal carbonate.
    a) dry out carbonates with microwave.
    b) attain dried mass of unknown carbonate.
    c) Dissolve in water (about 200ml)
    d) Add 125 ml CaCl2  solution
    e) filter precipitate with aspirator and Buchner funnel.
    f) dry out precipitate (put measured filter paper on watch glass) in oven. 
 
                                                                

 

_______________________________________________________                                                                                                   jump to:  top                        10/15 – Thursday Homework: –

 – Lab 9 is due tomorrow – conclusion!

 

1. Please complete the worksheet started in class by completing questions 2 & 3 and review with the key below:

The problem I did in class (question 1) is reviewed by the video below. Please complete questions 2 & 3 after you have reviewed question 1 with the video. For those that were in class, you can go directly to question 2 and 3 ONLY.  The video only covers question 1 that we did in class. Question 2 and 3 are similar to question 1.

Analytical Chemistry II NEW – Mol,Dilution, precipitation analysis.pdf                                                                              View Download

Analytical Chemistry II NEW – Mol,Dilution, precipitation analysis KEY Page 1.pdf                                                      View Download

2. Please complete questions 4 & 5 with me using the Lecture AP 1.2 Precipitation Analysis 2. This is the second side of the worksheet that was handed out today.  

Analytical Chemistry II NEW – Mol,Dilution, precipitation analysis.pdf                                                                              View Download

 
3. Please complete question 6 and then review with key below.
 
Analytical Chemistry II NEW – Mol,Dilution, precipitation analysis Complete Key 24-25 p.pdf                              View Download
 

4. Please complete the Analytical quiz 1 – Hydrate, precipitation, and Stoich.pdf worksheet and then enter your answers into the form posted below.  The form will be on auto-grade to grade your responses.  You may submit as many as 4 times as you would like BEFORE Friday morning.  Friday morning I will post a handwritten key and review in class. 

Analytical quiz 1 – Hydrate, precipitation, and Stoich.pdf
View Download

                           

1: AP Lecture 1.2 : Precipitation Analysis 1 – Question 1 review 

 

2: AP Lecture 1.2 : Preciptation Analysis 2 – Question 4 & 5

 

4. Analytic Chemistry Quiz 1 Form:                                                                                                                    

 

End of week 7!

           _______________________________________________                                                                   Jump to:  Friday Homework /top  10/16 – Friday – A Day – 1AB                              

Main focus – 
                                                                                                                                                       
  • a) To identify the mole/particle concept was needed to do       Stoichiometry – RATIO’s.
     b) To Review the past Stoichiometry homework assignments.                     c)  To identify the Law of Conservation of mass in chemical equations that have chemical formulas (that have been determined experimentally) provides us a way to use Ratios of each chemical TO
                                     SOLVE FOR ANOTHER CHEMICAL.
                                     d) To determine the Limiting Reagent in stoichiometry problems.

e) GO Canes!

 

Period 1 :

RATIOS – are ratios of “how many” = moles!!!! Most of what we do mathematically will be using these ratios to answer or verify.

Ratios of atoms in compounds —–> chemical formulas 
 
Ratios of each substance in a chemical reaction = Balanced Chemical Reaction –> Predict                 

Quick Homework Review– connected the problem concepts with stoichiometry of compounds and stoichiometry of chemical reactions

Types of Chemical Analysis we have studied: 

               a)  % by mass – (Hydrate Labs)

               b)  combustion analysis

               c)  precipitation analysis – ( we started this lab Frid)

1. Percent by mass —–> empirical formula/molecular formula

empiri&molec ditto hydrate combination KEY p.pdf
View Download  

2. Combustion analysis —> percent by mass —> empirical/molecular formula

Analytical Chemistry I KEY- determining chemical formulas.pdf
View Download  

3. Stoichiometry of ions, precipitation analysis

Analytical Chemistry II NEW – Mol,Dilution, precipitation analysis Complete Key 24-25 p.pdf                              View Download

4.  Quiz / Form review: (Precipitation analysis Review)

Analytical quiz 1 – Hydrate, precipitation, and Stoich KEY.pdf
View Download   

5.  Flaming Tube Demo – 

a) Which reactant was Limiting the reaction?

c) Calculate the Limiting reagent given the worksheet from homework of Thursday.

d) Use the non-chart method (Stoichiometry table) to solve the same problem and “see” the ratios.

What is the Limiting Reagent in this demo?  Why isn’t the flame coming out of the tube and burning my room into oblivion?

 
Limiting reagent intro demo new worksheet.pdf

                                                                                                                                                                                                                                   

                                                                                                    

1 : The Flaming Tube Demo – for the lecture below!

2 : Limiting Reagent Lecture –  Teaches the nonchart method up to 22:31

 

__________________________________________________                                                                                   jump to:  top                             10/16 – Friday Homework: – 

 

1. Please View the Limiting reagent Lecture posted above that is associated with the tube demo I did in class (start at 10:20). Please complete the worksheet with me in the video since I did not get to complete it in class. You need to view this and learn how to complete a Stoichiometry Table to answer which chemical in the demo was the limiting reagent and who is the excess chemical.
 
Limiting reagent intro demo new worksheet.pdf

  

2. Please View Lecture 1.5 below on Molar stoichiometry.   I will model how to complete the first side of the worksheet and then you will complete the backside on your own and review with the key.
 
 New Skills:  a) Identifying Limiting Reagent
                      b) Using Molarity in stoichiometry problems. 
                      c) calculating the excess chemical 
                                                                                                                               
Stoichiometry 3 – Molarity limiting reagent.pdf
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Stoichiometry 3 – Molarity limiting reagent Key.pdf
View Download 

2: Lecture 1.5 : Molarity Stoichiometry