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SYLLABUS OUTCOMES:
designs and evaluates investigations in order to obtain primary and secondary data and information CH11/12-2
selects and processes appropriate qualitative and quantitative data and information using a range of appropriate media CH11/12-4
solves scientific problems using primary and secondary data, critical thinking skills and scientific processes CH11/12-6
describes, applies and quantitatively analyses the mole concept and stoichiometric relationships CH11-9
Chemists must be able to quantify reactions in order to make predictions about yields and communicate using nomenclature, genres and modes unique to the discipline.
Using the mole concept, you will have the opportunity to select and use appropriate mathematical representations to solve problems, make predictions and calculate the mass of reactants and products, whether solid, liquid or gas. You will further develop understanding of the universal language of chemistry. You will be introduced to the idea that science is a global enterprise that relies on clear communication, international conventions, peer review and reproducibility.
You will focus on designing and evaluating investigations that enable you to obtain quantitative data to help you solve problems related to quantitative chemistry.
Background:
Of some use is the Quantity/Quantity/Ration [QQR] approach: see video https://www.youtube.com/watch?v=Ja4ReSIyb6A&index=3&list=PLeFSFSJ9WqSBlS5riye9fg1b6SlJQ00h4 [Note it should be Intro to Quantitative - not qualitative) 5:30
RESOURCES:
TEXT REFERENCE: CHAPTER 6
Workbook (downloaded below or accessible from https://drive.google.com/open?id=15cs4XxBLvd1Kltokw0XxtEaPpZw93efL )
11C IQC0 Workbook 2018.docxMDQ1 What happens in chemical reactions?
1.1a conduct practical investigations to observe and measure the quantitative relationships of chemical reactions, including but not limited to:
– masses of solids and/or liquids in chemical reactions
All chemical reactions involve solids, liquids and/or gases. Atoms can be recombined as the reaction proceeds. Chemical bonds between atoms are broken, and new bonds are formed.
What else happens in chemical reactions?
Is mass always conserved?
TASK 1.1.1
Metals react with dilute acids to form hydrogen gas.
Bicarb soda (sodium hydrogen carbonate) reacts with vinegar to form carbon dioxide gas.
Hydrogen peroxide can be decomposed into water and oxygen gas.
Copper sulfate and sodium hydroxide solutions form a copper hydroxide precipitate when they are combined.
Select TWO of these reactions and design separate experiments to test whether the mass at the end of each reaction is the same as it was at the start of the reaction.
A chemical reaction involves atoms in the reactants being rearranged to form the products. No material is lost or gained.
During any chemical reaction no particles are created or destroyed: the atoms are simply rearranged from the reactants to the products. The products may have different properties to the reactants.
Mass is never lost or gained in chemical reactions. We say that mass is always conserved. In other words, the total mass of products at the end of the reaction is equal to the total mass of the reactants at the beginning (BBC Bitesize, 2014).
Open and closed systems
Systems can be either open or closed. A closed system is one where a quantity or series of quantities cannot enter or leave the system. In a closed system, the mass of the system cannot change over time.
The opposite of a closed system is an open system. An open system is one where a quantity or series of quantities can enter or leave the system to a significant degree. In an open system, the mass of the system can change over time.
VIDEOS:
Conservation of Mass https://www.youtube.com/watch?v=v2rL7rrk5qk&list=PLeFSFSJ9WqSBlS5riye9fg1b6SlJQ00h4&index=2 6:04
PRACTICAL:
Modelling conservation of mass: making a biopolymer
TASK 1.1.2
1. A solid has a mass of 25g is mixed with 60g of a solution. A chemical reaction takes place and a gas is produced. The final mass of the solid mixture is 75g. What is the mass of the gas released? (Dearborn Schools, 2015)
2. If 100g of a substance reacts with 70g of another substance, what will be the mass of the products after the reaction? (Dearborn Schools, 2015)
3. A student adds 15g of baking soda to 10g of acetic acid in a beaker. A chemical reaction occurs and a gas is given off. After the reaction, the mass of the products remaining in the beaker is 23g. Has the mass been conserved in this reaction? Explain. (Dearborn Schools, 2015)
1.1b conduct practical investigations to observe and measure the quantitative relationships of chemical reactions, including but not limited to:
– volumes of gases in chemical reactions
The volume of gas produced can be used to follow the course of a reaction. Gas volumes can be measured using a gas syringe or an upturned measuring cylinder or burette.
The mass of gas produced can be measured using a sensitive balance.
VIDEOS:
Collecting gases: https://www.youtube.com/watch?v=1Ux1Z3XgRqE&index=1&list=PLeFSFSJ9WqSBlS5riye9fg1b6SlJQ00h4 5:27
1.2a relate stoichiometry to the law of conservation of mass in chemical reactions by investigating:
– balancing chemical equations
11C IQC1 2 Balancing Equations PPT.pptxUsing a balanced chemical equation to calculate amounts of reactants and products is called stoichiometry. It is a super technical-sounding word that simply means the amalgamation of Chemistry and Mathematics (Khan Academy, 2016).
Stoichiometric calculations are based on the law of conservation of mass.
The total mass of all products is equal to the total mass of all reactants in a chemical reaction.
Balancing chemical equations help ensure we have followed the law of conservation of mass.
2H2(g) + O2(g) --> 2H2O(l)
Reactants Products
A chemical equation should be balanced on both sides. A chemical equation shows us the substances involved in a chemical reaction: the substances that react (reactants) and the substances that are produced (products). In general, a chemical equation looks like this:
Reactants --> Products
According to the law of conservation of mass, when a chemical reaction occurs, the mass of the products should be equal to the mass of the reactants. Therefore, the amount of the atoms in each element does not change in the chemical reaction. As a result, the chemical equation that shows the chemical reaction needs to be balanced. A balanced chemical equation occurs when the number of the atoms involved in the reactants side is equal to the number of atoms in the products side (Study, 2016).
In general, to balance an equation, here are the things we need to do:
Count the atoms of each element in the reactants and the products.
Use coefficients; place them in front of the compounds as needed.
Where possible, leave an element until last as any coefficient placed in from of an element only affects that element (eg 2Li) whereas any coefficient placed in front of a compound affects all atoms in the compound (eg 2NaCl)
The steps are simple, but it is a process of trial and error.
Revisit the POWERPOINT: (downloaded below, or available on https://drive.google.com/open?id=1wgBIwqcwe1uqVd3FTLPxVJkQIuZgDmA8 )
11C IQC 1a Balancing Equations.pptxWORKED EXAMPLES
TASK 1.2.1
1. In the reaction: 4Li(s) + O2(g) → 2Li2O(s)
a. what is the product?
b. what are the reactants?
c. what does the “(s)” after the formula of lithium oxide signify?
d. what is the coefficient of the lithium metal?
REVIEW:
6.1 Review p212
Key Qs p212
1.2b relate stoichiometry to the law of conservation of mass in chemical reactions by investigating:
– solving problems regarding mass changes in chemical reactions
This is where we bring stoichiometry and the law of conservation of mass together. When a chemical reaction is written as an equation, and is balanced, we can get an idea of the relative amounts of each substance present as either reactant(s) or product(s). As we learn more about stoichiometry, we will be able to make direct calculations to demonstrate the conservation of mass in any chemical reaction (Chan, et al., 2018).
Chemical reactions may involve one or more products being in a different state at room temperature to the reactant(s). Chemists need to take into account the different states which may be produced when applying the law of conservation of mass to the reaction. In addition to the balancing of chemical equations, we will also use subscripts to show these states (Chan, et al., 2018).
VIDEOS:
Balancing equations 1 https://www.youtube.com/watch?v=bDiBHbM0Its 7:32
Balancing equations 2 https://www.youtube.com/watch?v=Al5EFBYJf-0 8:55
Stoichiometry https://www.youtube.com/watch?v=UIWMKkWoJPU&index=5&list=PLeFSFSJ9WqSBlS5riye9fg1b6SlJQ00h4 5:54
Mass changes in chemical reactions https://www.youtube.com/watch?v=ClmESFa-5hc&index=4&list=PLeFSFSJ9WqSBlS5riye9fg1b6SlJQ00h4 7:01
TASK:
11C IQC 1a Balancing Equations.docxREVIEW:
6.2 Review p217
Key Qs p217
CHAPTER REVIEW: p218
MDQ2 How are measurements made in Chemistry?
RESOURCES:
TEXT REFERENCE: CHAPTER 7
Background: Significant figures
2.1a explore the concept of the mole and relate this to Avogadro’s constant to describe, calculate and manipulate masses, chemical amounts and numbers of particles in:
– moles of elements and compounds 𝑛=𝑚/𝑀𝑀 (n = chemical amount in moles, m = mass in grams, MM = molar mass in gmol-1)
POWERPOINT:
Downloaded below, or accessible at https://drive.google.com/open?id=1wDpJaX1K_NnZrdeaY5YWyjH92PTvyNEt
11C IQC2 1a Mole Concept PPT.pptxVIDEOS:
Stoichiometry and the mole https://www.youtube.com/watch?v=dUXXaVqnclc&index=6&list=PLeFSFSJ9WqSBlS5riye9fg1b6SlJQ00h4 6:20
One mole of a compound https://www.youtube.com/watch?v=AD-VjZIq4bM&index=8&list=PLeFSFSJ9WqSBlS5riye9fg1b6SlJQ00h4 5:15
REVIEW:
7.1 Review p228
KQs p228
7.2 Review p232
KQs p232
2.1b explore the concept of the mole and relate this to Avogadro’s constant to describe, calculate and manipulate masses, chemical amounts and numbers of particles in:
– percentage composition calculations and empirical formulae
POWERPOINTS:
Downloaded below, or accessible from
11C IQC2 1b Molar Mass PPT.ppt11C IQC2 1c MolarMass Particle PPT.pptVIDEOS:
Empirical formula of a compound https://www.youtube.com/watch?v=in_d7sYAlVA&index=7&list=PLeFSFSJ9WqSBlS5riye9fg1b6SlJQ00h4 6:02
Mole concept https://www.youtube.com/watch?v=XQvB5-aYAj4&index=9&list=PLeFSFSJ9WqSBlS5riye9fg1b6SlJQ00h4 5:23
Percentage composition and empirical formula https://www.youtube.com/watch?v=YZKecuCzq5U&index=17&list=PLeFSFSJ9WqSBlS5riye9fg1b6SlJQ00h4 7:15
REVIEW:
7.3 Review p237
KQs p237
2.1c explore the concept of the mole and relate this to Avogadro’s constant to describe, calculate and manipulate masses, chemical amounts and numbers of particles in:
– limiting reagent reactions
VIDEOS:
TASK:
Downloaded below, or accessible from https://drive.google.com/open?id=1AtzpKTOHiWalYJKn2mxdH6iEcWOd7xE2
11C IQC2 1d Mole Calculations.pdfREVIEW:
7.4 Review p241
KQs p241
7.5 Review p245
KQs p245
2.2 conduct a practical investigation to demonstrate and calculate the molar mass (mass of one mole) of:
– an element
– a compound
2.3 conduct an investigation to determine that chemicals react in simple whole number ratios by moles
CHAPTER REVIEW:
pp246-8
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