Week 7 – 10/11 – 10/14
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10/11 – Monday – Columbus Day –
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10/12 – Tuesday – B Day – 2, 3b/4 Lab
a) Test 2 – Voltaic/Electrolytic Cells/Cubic cell calculations/alloys – Review
b) To Continue with particle and mole theory – 2/3a,4
a) Test 1 – makeup – Review.
b) Particle/mole continues – Modern Atomic Theory – John Dalton!
– John Dalton – Gay – Lussac – Amadeo Avogadro
Particle / Mole Theory Presentation:
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10/12 – Tuesday Homework: –
1: Complete the Mole Concept Lecture (if I did not finish in class) This will probably be for Period 2 who only had 1 period today. I will post what time you can start as the lecture below starts from the G(r) eeks!
Please Start the video below at the 20:00 mark to the end to finish what I did with the other class.
2: Complete the worksheet below by using the lecture below on the Law of Combining volumes and use the Law of Combining volumes tutorial below. Review with the key or lecture.
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Mole Concept Lecture :
Law of Combining Volumed Tutorial :
End Of Tuesday!
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10/13 – Wednesday – A Day – 2/3a Lab, 4
a) Psat today!
I will miss the 2 period day for my 2/3 students 🙁 so do not worry I will review the mole concept ideas that you viewed in my lecture (last night) in class Thursday.
We will however begin the type of calculations and labs that began after the Solvay Conference in 1860 when Canazzaro linked the work of Avogadro and Gay-Lussac to describe the chemical formulas and chemical reactions in the boxes. Chemistry began and everyone was trying to figure out the chemical formulas of compounds using what we now call Analytical Chemistry.
Law of Definite Proportions = the same compound will always have the same percentage of different elements in it.
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10/13 – Wednesday Homework: –
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1: AP Lecture : Calculating chemical formulas from percent by masses (that are obtained through labs).
End of Wednesday..
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10/14 – Thursday – B Day – 2, 3b/4 Lab
a) Complete the particle and mole concept in class for period 2 –
Dalton –> Gay Lussac –>Amedeo Avogadro (Canazarro)
b) Determining the percent by mass of compound (hydrate) experimentally. Our homework has been based on starting with % by masses to determine the chemical formula (fixed ratio of how many atoms). We will perform the type of experiment that was done after the Solvay conference which was first step to determining the chemical formulas.
This is the beginning of Analytical Chemistry.
Law of Definite Proportions = the same compound will always have the same percentage of different elements in it.
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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. |
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10/14 – Thursday Homework: –
1. Please watch lecture 0a ( I model question 3) and complete question 4 on
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1: AP Lecture 0a : Calculating chemical formulas from Combustion analysis (that are obtained through labs).
End of Thursday..
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10/15 – Friday – A Day – 2/3a Lab, 4
a) Determining the percent by mass of compound (hydrate) experimentally. Our homework has been based on starting with % by masses to determine the chemical formula (fixed ratio of how many atoms) or we had to get the % by mass through combustion analysis. We will perform the type of experiment that was done after the Solvay conference which was first step to determining the chemical formulas.
b) To perform Lab 5 and Lab 6 in determining the percent by mass or the empirical formula (in hydrates).
This is Analytical Chemistry.
1. Today we will either be performing Lab 5 & 6 – period 2/3
Lab 6 – period 4
2. While we collect data we complete the following worksheet:
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2/3a, 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. |
![]() |
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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10/15 – Friday Homework: – Lab 5 & 6 we will complete in class Monday!
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3: AP Lecture 1.3 : Stoichiometry and percent yield
End of week 7!