1: QUANTITATIVE CHEMISTRY OBJECTIVES
From the IB Syllabus:
1.1
Fundamentals
Matter: Classification, Properties & Changes
Measurement: Metrics, Uncertainty, Significant Figures, Scientific Notation
Mole Concept and Avagadro’s Constant
1.1.1
Apply the mole concept to substances.
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QUIZ 1
1.1.2
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QUIZ 1
The mole concept applies to all kinds of particles: atoms, molecules, ions, electrons, formula units, and so on.
The amount of substance is measured in moles (mol).
The approximate value of Avogadro’s constant (L), 6.02 × 1023 mol–1, should be known.
Determine the number of particles and the amount of substance (in moles)
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1.2
How well can you address the
stated objective…at this time?
Not at all So-so
I know
this!
Convert between the amount of substance (in moles) and the number of atoms, molecules, ions, electrons and
formula units.
Formulas
1.2.1
1.2.2
Define the terms relative atomic mass (Ar) and relative molecular mass (Mr)
Calculate the mass of one mole of a species from its formula.
1.2.3
Solve problems involving the relationship between the amount of substance in moles, mass, and molar
mass.
Distinguish between the terms empirical formula and molecular formula.
Determine the empirical formula from the percent composition or from other experimental data.
Determine the molecular formula when given both the empirical formula and experimental data.
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The term molar mass (in g mol–1) will be used.
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QUIZ 2
1.2.4
1.2.5
1.3
1.2.6
Chemical Equations
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QUIZ 2
1.4
1.3.1
Deduce chemical equations when all reactants and products are given.
1.3.2
Identify the mole ratios of any two species in a balanced chemical equation.
Apply the state symbols (s), (l), (g), (aq).
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1.3.3
Mass and Gaseous Volume Relationships in Chemical Reactions
1.4.1
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QUIZ 2
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QUIZ 4
Calculate theoretical yields from chemical equations.
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1.4.2
1.4.3
1.4.4
1.4.5
1.4.6
1.5
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QUIZ 2
Students should be aware of the difference between coefficients and subscripts.
Given a chemical equation and the mass or amount (in moles) of one species, calculate the mass or amount of
another species.
Determine the limiting reactant and the reactant in excess when quantities of reacting substances are
given.
Solve problems involving theoretical, experimental and percentage yield.
Apply Avogadro’s law to calculate reacting volumes of gases.
Apply the concept of molar volume at standard temperature and pressure in calculations.
Solve problems involving the relationship between temperature, pressure and volume for a fixed mass of
an ideal gas.
Solve problems using the ideal gas equation, PV = nRT
Analyze graphs relating to the ideal gas equation.
1.4.7
1.4.8
Solutions
1.5.1
1.5.2
Distinguish between the terms solute, solvent, solution, and concentration (g dm -1 and mol dm-1)
Solve problems involving concentration, amount of solute, and volume of solution.
Possible Resources for Review / Practice on Quantitative Chemistry
(1)
(2)
(3)
(4)
(5)
Green and Damjii – Chapter 1: Do Exercises and check your answers.
Green and Damjii – Further Worked Examples – This shows you how to solve a number of different types of
stoichiometry problems. If you are struggling, this may be a good place to go to see how to work problems.
Chang – Chapter 3 – Pretty much the whole chapter is needed 
– Chapter 4 – Focus on Sections 1 and 5; Sections 6 and 7 are interesting
titration applications that might be helpful
– Chapter 5 – Focus on Sections 4 and 5.
Neuss – Chapter 1 with IB Questions – Great way to review a lot of ideas in just a few pages. The questions are either
released items or fashioned after actual IB questions. Mostly multiple choice, but there are a few longer problems. Check
your answers with key.
Other: (If you find a great resource for this unit, please submit information about the resource to your instructor!)
Assgn # Exercise
1
0
1.1
1.2
2
1.2.3
3
1.3
1.3.1
1.4
1.4.1
4
1.2.4
5
1.5
6
1.4.2
1.4.3
7
1.16
8
Further Worked
Examples
Page #
p. 4
p. 5
p. 7
p.7-8
pp. 14-15
p. 17
pp. 19-20
p. 21
pp. 12-13
pp. 28-29
pp. 23-24
p. 25
p.36
pp. 37-46
Assigned Questions
# 1-5
# 1-6 and either 7 or 8
# 1-2 and 3d, e, f
# 1-5
# 1-3, 4(do 5), 5(do 5)
# 1-3, 4(do 5), 5(do 5)
# 1-4
# 1-3
#1-10; 12(a,c); 14; 15; 18(a-c); 20
#1-10
#1-10
#1-10
#1-5
#1-22; 25; 27-29
Due Date
NOTE
1.5.1
1.5.2
pp. 31-32
p. 33
#1-3; 4(a-c); 5(a-c); 8; 10
#1-3
Will be assigned
in acid/base unit
Answer your questions in your chemistry comp book. Be sure to title and date your entry. Number each answer. You do not
have to write the question down… but you may want to include some of the question in your answer… to make it useful for later reference. When you are done
with the work, check your answer against the answer key. Make corrections, as needed, in a different color of pen/pencil. If you don’t understand a question
and/or answer, mark the problem and pursue it! You can bring this ‘problem problems’ up in class, with your classmates, and/or with me individually. [I have Pd
2 and Pd 7 as plan periods… and there is always lunch or after school. Before school is generally NOT an option.] Points for these assignments will be based
on completion and evidence of corrections. This is an important opportunity for you to learn. So do these! Answer your questions in your chemistry comp book.
Be sure to title and date your entry. Number each answer. You do not have to write the question down… but you may want to include some of the question in
your answer… to make it useful for later reference. When you are done with the work, check your answer against the answer key. Make corrections, as
needed, in a different color of pen/pencil. If you don’t understand a question and/or answer, mark the problem and pursue it! You can bring this ‘problem
problems’ up in class, with your classmates, and/or with me individually. [I have Pd 2 and Pd 7 as plan periods… and there is always lunch or after school.
Before school is generally NOT an option.] Points for these assignments will be based on completion and evidence of corrections. This is an important
opportunity for you to learn. So do these!