Week – 10/18 – 10/22
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10/18 – Monday – B Day – 2, 3b/4 Lab
a) To perform Lab 5 and Lab 6 in determining the percent by mass or the empirical formula (in hydrates).
b) To complete the error analysis of the hydrate labs
c) Complete Mole / Particular concept presentation
Period 2:
1. HW review – connected the problem concepts with stoichiometry of compounds and stoichiometry of chemical reactions
empiri&molec ditto hydrate combination KEY p.pdf
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Stiochiometry 1 – balance yield key.pdf
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2. Mole concept lesson – diagram, conversions
4. Small movie / STM
Period 3/4
1. Same as above plus
2. Complete Lab 5 and 6, conclusion questions.
Particle / Mole Theory Presentation:
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3b/4 Lab – Lab 5 – Percent mass of water in a Hydrate
LAB 5 – copper sulfate pentahydrate lab.pdf
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This image was build by X-ray imaging of salt. |
Now it is more complex than the crystal above for NaCl because we have a polyatomic ion in the crystal. The Yellow is the Sulfur attached to 4 oxygens (red). The brown color (i think its brown) is the copper. Notice regular repeating pattern. Its hard but if look inside the crystal there is one Cu per sulfate ion. |
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Notice the Dot between anhydrate and water. This dot means “WITH” and not to multiple. Thus there are exactly 5 water molecules for every 1 Cu+2 and 1 SO4-2 in the crystal. |
You will notice that water (it has 2 white hydrogen atoms) molecules are situated inside the crystals at particular regions in the crystal in exact ratios. This is a fixed ratio (stoichiometric ratio). It is hard but you can see the 5 water molecules per 1 copper ion and 1 sulfate ion. What makes it hard is that the crystal repeats in all directions. The water can be removed from the salt by heating it. |
*Determine the chemical formula of a hydrate:
LAB 6 – Empirical Formula analysis of Hydrate.pdf

Because of the conservation of mass by Antoine Levassuer, the mass of water that is released from the crystal (hydrate) is the same mass that was is in the crystal. THus the moles of water lost is the water that are in the crystal (in the formula ) .
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10/18 – Monday Homework: – Lab 5 & 6 are due!
a) Lecture 1.1 : Molarity of ions
b) Lecture 1.2 : Preciptation analysis
End of Monday..
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10/19 – Tuesday – A Day – 2/3a Lab, 4
a) To complete Hydrate Labs and the error analysis of the hydrate labs
b) To begin the conservation of mass presentation – balancing chemical reactions, Stoichiometry of chemical reactions using the mole ratios that we get from balancing
Period 2/3:
1. HW review – Stoichiometry of ions, precipitation analysis
Analytical Chemistry II KEY NEW – Mol,Dilution, precipitation analysis.pdf
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A. Flaming Flask Demo:
This means 2 H2 molecules per 1 O2 is needed to maximize the reaction and thus maximize the energy released. If this ratios in the reaction are not 2 to 1 then the reaction will be less efficient with some unreacted reactants and a lower amount of energy released. Sometime the reaction will not even run at all if the ratios are poor.
Period 4
1. Same as above except will complete the LGI Hydrogen demo tomorrow
Conservation of Mass Presentation:
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10/19 – Tuesday Homework: –
2. Please complete the take-home quiz ( Analytic Chemistry Quiz 1 )ON the worksheet that was given out today or posted below:
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End Of Tuesday!
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10/20 – Wednesday – B Day – 2, 3b/4 Lab
b) To begin the conservation of mass presentation – balancing chemical reactions, Stoichiometry of chemical reactions using the mole ratios that we get from balancing
Period 2:
1. HW review – Form Review
Analytical quiz 1 – Hydrate, precipitation, and Stoich KEY.pdf
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4. Flaming Flask demo
5. Hydrogen balloon analysis from yesterday. When did we make GOOD CAKE?
A. Flaming Flask Demo:
This means 2 H2 molecules per 1 O2 is needed to maximize the reaction and thus maximize the energy released. If this ratios in the reaction are not 2 to 1 then the reaction will be less efficient with some unreacted reactants and a lower amount of energy released. Sometime the reaction will not even run at all if the ratios are poor.
Period 4
1. Same as above except will complete the LGI Hydrogen demo.
2. Complete the Conservation of Mass Presentation
3. Lab 7 – Collect data
Conservation of Mass Presentation:
Period 2 : Hydrogen Balloon Explosion Comparison:
2 H2 (g) + O2 (g) —> 2 H20 + Energy
Period 4 : Hydrogen Balloon Explosion Comparison:
2 H2 (g) + O2 (g) —> 2 H20 + Energy
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3b/4 Lab – Lab 7 – Synthesis of Copper Iodide (and determination of the empirical Formula of copper iodide)
Lab 7 – Synthesis of Copper Iodide.pdf
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This Lab will be our first formal lab. I am giving out a data worksheet to keep you organized in your data collection but it will not be handed in. You will write a data section and calculation section in your formal lab write-up that will be in a google doc that will be shared to you in next couple of days.
Cu (s) + I2 (g) —> Cu? I?
Objectives: 1. To determine the empirical formula of the salt (product).
2. To determine the percent yield of the salt.
We will take notes on how to perform this lab.
Lab 7 : Synthesis of Copper Iodide
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10/20 – Wednesday Homework: –
Lecture 1.5 : Molarity Stiochiometry
End of Wednesday..
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10/21 – Thursday – A Day – 2/3a Lab, 4
a) To complete the conservation of mass presentation – balancing chemical reactions, Stoichiometry of chemical reactions using the mole ratios that we get from balancing – applications to Challenger and Hindenburg
b) To perform an “adding mass lab” – Lab 7
Period 2/3:
1. Complete the Challenger and Hindenburg discussion.
2. Flaming Flask demo and review of the balloon demos from the video below.
Period 4:
1. Complete the Challenger and Hindenburg discussion.
2. Review of the balloon demos from the video of both classes.
3. Lab 7 – Note-taking setup –
A. Flaming Flask Demo:
This means 2 H2 molecules per 1 O2 is needed to maximize the reaction and thus maximize the energy released. If this ratios in the reaction are not 2 to 1 then the reaction will be less efficient with some unreacted reactants and a lower amount of energy released. Sometime the reaction will not even run at all if the ratios are poor.
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2/3a Lab/4 – Lab 7 – Synthesis of Copper Iodide (and determination of the empirical Formula of copper iodide)
Lab 7 – Synthesis of Copper Iodide.pdf
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This Lab will be our first formal lab. I am giving out a data worksheet to keep you organized in your data collection but it will not be handed in. You will write a data section and calculation section in your formal lab write-up that will be in a google doc that will be shared to you in next couple of days.
Cu (s) + I2 (g) —> Cu? I?
Objectives: 1. To determine the empirical formula of the salt (product).
2. To determine the percent yield of the salt.
We will take notes on how to perform this lab.
Lab 7 : Synthesis of Copper Iodide
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10/21 – Thursday Homework: –
What is the Limiting Reagent in this demo? Why isn’t the flame coming out of the tube and burning my room into oblivion?
2. Please view the Limiting reagent Lecture that teaches the chart method of calculating the limiting reagent. Complete side one with me. How could this method made last night’s homework easier?
1 : The Flaming Tube Demo – for the lecture below!
2 : Limiting Reagent Lecture – Teaches the chart method!
End of Thursday..
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10/22 – Friday – B Day – 2, 3b/4 Lab
a) To introduce Limiting Reagent concept in class and review the “chart method”.
b) To perform an “adding mass lab” – Lab 7 – Synthesis of copper iodide
Period 2:
1. We will review the concept of limiting reagent through the chart method, using a previous homework problem that Liam said was hard.
2. Flaming tube demo.
3. Lab 7 discussion of the write-up requirements.
Period 3/4:
1. Same as as number 1. and 2.
2. Lab 7 note-taking and perform experiment.
Classwork today:
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2, 3b/4 Lab – Lab 7 – Synthesis of Copper Iodide (and determination of the empirical Formula of copper iodide)
Lab 7 – Synthesis of Copper Iodide.pdf
View Download
This Lab will be our first formal lab. I am giving out a data worksheet to keep you organized in your data collection but it will not be handed in. You will write a data section and calculation section in your formal lab write-up that will be in a google doc that will be shared to you in next couple of days.
Cu (s) + I2 (g) —> Cu? I?
Objectives: 1. To determine the empirical formula of the salt (product).
2. To determine the percent yield of the salt.
We will take notes on how to perform this lab.
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10/22 – Friday Homework: –
1. Complete the backside of the Limiting reagent intro demo new worksheet.pdf (questions 3 and 4 ONLY) that was homework (front side) from Thursday night using the video posted below. You could try these 2 questions on your own first and then view the video if you are feeling adventurous!
2. Complete the Short Form from a Tall Teacher below: This form is based on a recent free response question. You have 3 submissions to this form. Use the ICE Chart!
3. Complete the Lab 7 calculations on the handout I gave you.
If you need help with Lab 7 I have posted a review video below the weekends form.
You should be able to calculate or determine the following:
a) Mass of the copper reacted
b) Mass of the iodine reacted
c) Mass of the product
d) empirical formula for the salt
e) Calculate the theoretical amount of product (salt) using the empirical formula (that you found).
f) Calculate a percent yield.
1 : Side 2 of Thursday nights homework – Teaches the chart method!
End of Thursday..
3 : Lab 7 review – This might help with your calculations!
End of week 8!