Preparation for your Semester 1 Exam
Your exam will be in 2 parts:
Part I – Current Unit – Chemical Reactions and Balancing Equations – Open Response
 You may ONLY use the gold packet on this part of the test.
Part II – Former Units – Moles, Matter, Measurement, Candles – Multiple Choice
 You may use your comp book, your calculator, and the gold packet on this part of the
test.
Unit 5 – Chemical Reactions and Equations - Learning Targets
1.
Write a balanced chemical equation for a chemical reaction
a)
Identify common vocabulary used in chemical equations: reactant, product, word
equation, formula equation, subscript, coefficient, state symbols for solids, liquids,
gases, +, 
b) Write accurate formulas for chemical elements and compounds
c) Use coefficients to balance a skeleton equation.
d) Use atom inventory to check that an equation is balanced.
e) Convert a word equation into a balanced chemical equation
2.
Classify a reaction by type (synthesis, decomposition, single replacement, double
replacement, combustion)
3.
Predict the product of simple chemical reactions (particularly double replacement
reactions)
a)
Use the reaction type to predict what will be produced if given information about the
reactants.
UNIT 4: The MOLE Learning Targets
1. Define ‘mole’ in multiple ways and explain its importance to chemists.
A. What is molar mass and how is it calculated?
2.
B. What is Avogadro’s number?
C. Why is the mole important to chemists (and chemistry students)?
Use what you know about moles to solve mole problems.
A. How do you convert grams into moles and/or moles into grams?
B.
3.
How do you convert moles into particles and/or particles into moles?
Use what you know about the mole to interpret information related to the formula of a
compound.
A. How do you calculate percentage composition* when given the formula of a
compound or lab information about the mass of its elements? [* % of each element
]
B. How do you determine the empirical formula of a compound when given the %
composition or lab information about the mass of its elements.
C. How do you determine the molecular formula when given the empirical formula and
the molar mass?
Link to Textbook
Section 11.1
Read pp 320-328
(from Chapter 9)
Read pp 324-328 Do
Practice Problems 3-6
Read pp 330-337
Do Practice Problems
13-21
Section 11.2
Read pp 330-337
Do Practice Problems
13-21
Section 11.2 & 11.3
Read pp 337-339 and
344
Read pp 337-339
Link to Textbook
Read 293-296
Do sample 10.4
Read 290-293
Read 287-290
Read 297-299
Do samples 10.5 & 10.6
Read 290-293
Do samples 10.2 & 10.3
Read 305-308
Do samples 10.9 & 10.10
Read 309-310
Do sample 10.11
Read 311-312
Do sample 10.12
4.
5.
Be able to use mole-related vocabulary:
A. What is the difference between an element, an ionic compound, and a covalent
compound? [review]
B. What is the difference between an atom, a molecule, and a formula unit?
C. What is the difference between atomic mass, molecular mass, and formula mass?
D. What is the difference between a molecular formula and an empirical formula?
Use scientific notation to work with large and small measurements. [review]
6.
Use significant figures in mathematical calculations. [review]
Unit 3: Studying Matter - Learning Targets
1. How can we explore chemistry in a safe and effective way?
A. Recognize and demonstrate safe laboratory practices.
B. Identify and safely use common laboratory equipment.
2. How is matter described, organized, and separated?
A. Define matter
B. Categorize a sample of matter as a substance (element or compound) or a mixture
(heterogeneous or homogeneous)
C. Describe how chemical symbols and formulas can be used to determine if matter is
an element, compound, or a mixture.
D. Describe how matter (mixtures, compounds, elements) can be separated
(physically? chemically? via nuclear reactions?)
E. Describe and use several common methods of separating mixtures:
chromatography, distillation, and filtration.
F. Explain how water in third-world countries can be purified for drinking.
3.
Describe why and how atoms combine to form compounds
D. State that atoms combine to achieve greater stability, as evidenced by a complete
outer shell.
E. Differentiate between an atom and an ion.
F. Describe that electrons are shared to form covalent bonds and transferred to form
ionic bonds.
G. Identify the type of bonding (covalent, ionic) between two elements given their
location on the periodic table.
H. Use the periodic table to predict the number of valence electrons and likely charge
of elements in the main blocks (far right and far left) of the periodic table.
4. Communicate information about ionic and covalent compounds using formulas and
names
A. Be able to name and write the formulas for ionic compounds – with the help of the
periodic table and a reference sheet.
B. Describe the type of information a formula for an ionic or covalent compound
provides (parenthesis, subscripts, charges of ions)
C. Be able to write the formula and charge for any monoatomic or polyatomic ion with
the help of the periodic table and/or a reference sheet.
D. Be able to name and write the formulas for covalent compounds – with the help of
the periodic table and a reference sheet.
Check glossary
Read 290
See notes
Read 309-312
Review 63, 85 & R56-58
Do sample MH-1
Review 66-72, R59-R61
Do samples 3.1, 3.2, 3,3
and MH-2 & MH-3
Read R80 and R81
Read Sections
2.2: Mixtures
and
2.3 Elements and
Compounds
Do Practice Problems 9,
10, 18, 19
Do Section Assessment
for 2.2 (# 11-17) and 2.3
(# 20-27)
Read Sections
7.1 pp 187-188
7.2 pp 194-196
8.1 pp 213-216
Read Chapter 9, focusing
on Sections
9.1, 9.2, 9.3, 9.5
Try the practice
problems throughout
the chapter. You can
check your answers in
the back of the book.
Unit 2 – Measurement Learning Targets
1. Describe what makes up a quality measurement.
A. What are the components of a quality measurement?
B. What is the difference between accuracy and precision?
C. How is percent error calculated?
D. What causes uncertainty in measurements?
E. What are significant figures and why do we use them?
F. How do you determine the number of significant figures in a
measurement and in a calculated answer?
G. What is scientific notation and why do we use it?
2. Describe and use the International System of Measurements (SI).
A. What are the major SI quantities, units, and instruments used in the
study of chemistry? [identify the correct tool for the particular job]
B. What do the metric prefixes milli-, centi-, kilo-, and nano- represent?
C. What is nanotechnology and why is it important?
3. Accurately use appropriate tools to measure each of the major SI quantities
commonly used in chemistry.
A. What are the best devices to measure length, mass, and volume?
4. Convert one metric unit into another using dimensional analysis and
conversion factors.
A. What is dimensional analysis?
B. What is a conversion factor?
C. How is one SI unit be converted into another using dimensional analysis
and conversion factors?
5.
6.
7.
8.
Determine and analyze density measurements.
A. How is density calculated? What are its units?
B. How is density determined in the laboratory?
… for a ‘regularly shaped’ object?
… for an ‘irregularly shaped’ object?
C. Is density an intensive or extensive property? Explain
Make and analyze observations of a candle.
A. What is the difference between qualitative and quantitative
observations?
B. What is the difference between observations and inferences?
C. What is the difference between physical and chemical properties?
D. What is the difference between intensive and extensive properties?
E. What are the characteristics of quality observations made by scientists?
Describe what constitutes a candle.
A. What are the three parts of a candle… and what makes up each part?
Describe how a candle works
A. How do you start and stop a candle?
B. How does a candle burn? What is required? What is made?
READ Section 3.1 pp. 63-72
DO Practice Problems
# 1-7 (found throughout the
section) and check your answers
on p. R83
READ Section 3.2 pp. 73-79
READ Section 3.3
pp. 80-87
DO Practice Problems
# 32-34 & 36 (found throughout
the section) and check your
answers on p. R83
READ Section 3.3 pp. 89-93
DO Practice Problems
# 46-49 (found throughout the
section) and check your answers
on p. R83
Text book Resources*: Chapter
3
READ Section 3.1
pp. 63-72
DO Practice Problems
# 1-7 (found throughout the
section) and check your answers
on p. R83