Download Work Booklet - Brooks Composite High School

Name: __________________________________
Crowsnest Consolidated High School
Science 10
Unit A Work booklet
Mr. R. Peebles
Science 10 – Unit A
1
Mr. R. Peebles
Name: __________________________________
Unit A—Energy and Matter in Chemical Change
W ORKSHEET
1
Science Laboratory Safety Rules
1.
2.
3.
4.
5.
6.
Read all written instructions carefully before doing an activity.
Listen to all instructions and follow them carefully.
Wash your hands thoroughly after each activity and after handling chemicals.
Wear safety goggles, gloves, or an apron as required.
Think before you touch. Equipment may be hot and substances may be dangerous.
Smell a substance by fanning the smell toward you with your hand. Do not put your nose close to the
substance.
7. Do not taste anything in the lab.
8. Tie back loose hair and roll up loose sleeves.
9. Never pour liquids into containers held in your hand. Place a test tube in a rack before pouring
substances into it.
10. Clean up any spilled substances immediately as instructed by your teacher.
11. Never look into test tubes or containers from the top. Always look through the sides.
12. Never use cracked or broken glassware. Make sure you follow your teacher’s instructions when
getting rid of broken glass.
13. Label any container you put chemicals in.
14. Report all accidents and spills immediately to your teacher.
15. Read the WHMIS (Workplace Hazardous Materials Information System) safety symbols on any
chemical you will be using and make sure you understand all of them. See Student Reference 1 at the
back of Science 10 for more information.
Science 10 – Unit A
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Mr. R. Peebles
Name: __________________________________
MSDS
Unit A—Energy and Matter in Chemical Change
W ORKSHEET
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MATERIAL SAFETY DATA SHEET
12% SODIUM HYPOCHLORITE
Section I: IDENTIFICATION
PRODUCT: sodium hypochlorite (12% solution)
SYNONYMS: sodium hypochlorite (12% available chlorine), Javel water, liquid bleach
CHEMICAL FORMULA: NaOClO
PRODUCT CODE NO.: 17547
Section II: HAZARDOUS INGREDIENTS
COMPOSITION: sodium hypochlorite solution 10–15 %
HAZARDS: oxidizer, corrosive
Section III: EMERGENCY OVERVIEW
Warning! Harmful if swallowed or inhaled. Causes irritation to eyes and respiratory tract. Causes
substantial but temporary eye injury.
Section IV: POTENTIAL HEALTH EFFECTS & FIRST AID MEASURES
INHALATION: Poisonous vapour. Increasing doses may cause irritation of nose and throat, coughing,
headaches, breathing difficulty, pulmonary edema, and lung injury. Remove patient to fresh air. Have
patient rest and keep warm. Seek medical attention if symptoms are severe.
INGESTION: Poisonous. Causes burns, abdominal cramps, nausea, vomiting, lowered blood pressure,
diarrhea, and shock. If patient is conscious, give 1–2 glasses of milk. Do not induce vomiting. Seek
medical attention.
EYE CONTACT: Burns, irritation. Rinse with water for at least 15 minutes. Seek medical attention.
SKIN CONTACT: Burns, irritation. Rinse with plenty of water. Wash contaminated clothing before reuse.
Section V: PHYSICAL DATA
BOILING POINT: 101oC, starts decomposing to NaCl and NaClO3 at 40oC
FREEZING/MELTING POINT: −25°C
VAPOUR DENSITY (AIR=1): 1.3
VAPOUR PRESSURE: 17.5 mm Hg at 20°C
SOLUBILITY IN WATER: fully miscible
SPECIAL FIRE FIGHTING PROCEDURES & PRECAUTIONS: Wear self-contained breathing
apparatus.
UNUSUAL FIRE & EXPLOSION HAZARDS: May release chlorine gas
Section VI: REACTIVITY
STABILITY: Inherently unstable; slowly decomposes liberating Cl 2; unstable above 40°C
CONDITIONS & MATERIALS TO AVOID: Temperatures above 40 oC, direct sunlight, acids, metals,
ammonia, oxidizable materials, urea
HAZARDOUS DECOMPOSITION PRODUCTS: Cl2
Science 10 – Unit A
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Mr. R. Peebles
Name: __________________________________
continued...
Section VII: EMPLOYEE PROTECTION
CONTROL MEASURES: Use with adequate ventilation.
RESPIRATORY PROTECTION: Use chlorine gas respirator.
PROTECTIVE CLOTHING: Neoprene, rubber or plastic gloves, use plastic sleeves, apron and boots if
handling large quantity.
EYE PROTECTION: Safety goggles
Section VIII: ENVIRONMENTAL PROTECTION
ENVIRONMENTAL PRECAUTIONS: Local exhaust acceptable
SPILL OR LEAK PRECAUTIONS: Wear gloves, boots, apron and goggles during clean-up.
WASTE DISPOSAL: Small spills: mop up with water and run to waste. Large spills: transfer to salvage
container and consult with professional disposal company. Inform local authorities if liquid has entered
surface drains or sewers.
Section IX: REGULATORY CONTROLS
DEPT. OF TRANSPORTATION: Regulated under Transport of Dangerous Goods
DOT CLASSIFICATION: Class 8 (9.2) UN: 1791 PG: III
DOT PROPER SHIPPING NAME: Hypochlorite solutions
OTHER DOT INFORMATION: N/A
WHMIS CLASSIFICATION: C, E, F
OTHER REGULATORY REQUIREMENT: none
Section X: PRECAUTIONS: HANDLING, STORAGE, AND USAGE
Store in cool, dry place away from acids. Do not store in metal containers. Use in well-ventilated area.
Science 10 – Unit A
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Mr. R. Peebles
Name: __________________________________
SAFETY
Unit A—Energy and Matter in Chemical Change
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WHMIS and Hazardous Household Product Symbols
Goal  Review the meanings of warning labels in the science classroom and at home.
Think About It
Throughout Canada, standard symbols are used to identify
dangerous materials


The Workplace Hazardous Materials Information
System (WHMIS) has produced symbols for such
work places as science laboratories. These are
known as WHMIS symbols.
The Hazardous Household Product Symbols
(HHPS) were developed for people buying and
using materials around the home.
WHMIS
Both sets of symbols provide warnings about the possible
hazards of using certain products, as well as the necessary
precautions to
take.
What to Do
Reinforce your understanding of WHMIS symbols and
HHPS symbols by
 reading “Safety Symbols” on page 455 in your
SCIENCE 10 textbook
 reviewing all the WHMIS symbols and HHPS
symbols
 answering the questions that begin on the next
page
HHPS
continued...
Science 10 – Unit A
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Mr. R. Peebles
Name: __________________________________
1. Briefly explain what kind of hazard each word describes.
(a) toxic
(b) flammable
(c) explosive
(d) reactive
(e) corrosive
2. In the space provided, draw the standard WHMIS symbol for each material.
Corrosive Material
Flammable and
Combustible Material
Compressed Gas
3. Choose two WHMIS symbols you did not use to answer question 2. Describe some precautions you
would take when handling a product labelled with each symbol.
WHMIS symbol
Meaning
Precautions
(a)
(b)
continued...
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
4. Study the display your teacher has provided, showing products that many people use in their homes.
 Look for symbols that are HHPS.
 Read the label on each product to find out how the product is used and decide why it has an HHPS.
 Complete the table below.
HHPS
How product used
Suggested precautions
(a)
(b)
(c)
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
PRACTICE QUESTIONS
Unit A—Energy and Matter in Chemical Change
W ORKSHEET
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Nuclear Notation
Atomic Number and Mass Number
Mass Number
Atomic
Number
Number of
Protons
Number of
Neutrons
carbon-14
14
6
6
8
hydrogen-1
1
1
hydrogen-2
2
1
4
20
2
10
64
29
35
45
7
7
16
16
20
21
Name
carbon-12
oxygen-18
9
10
26
30
53
74
calcium-40
119
50
26
208
33
82
silver-108
mercury-201
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
PRACTICE QUESTIONS
Unit A—Energy and Matter in Chemical Change
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Nuclear Notation
1. State the number of neutrons in each of the following isotopes.
a) 2210 Ne
b) 42 He
c) 4020 Ca
27
d) 13 Al
2. State the number of each of the following subatomic particles in
oxygen-17.
a) protons
b) electrons
c)
neutrons
3. A certain isotope has a mass number of 35. The isotope has 18
neutrons.
a) What is the atomic number of the isotope?
b) What is the atomic symbol of the isotope?
c)
Use nuclear notation to represent the isotope.
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
PRACTICE QUESTIONS
Unit A—Energy and Matter in Chemical Change
W ORKSHEET
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Bohr Models & EELR (Electron Energy Level Representations)
Bohr Models are diagrams used to represent the placement of electrons around the nucleus of an
atom. Electrons are arranged around the nucleus in varying ENERGY LEVELS. We will use rings
around the nucleus to represent where we may find the electrons.
To draw Bohr Models:
1. Draw a nucleus (circle) and write in the number of protons and neutrons for the specific
element. Ex. Carbon - 12
6 p+
6 n0
2. Count which period the element is located. The number of periods represents the number of
energy levels that element contains.
(a) ex. Carbon is in period 2 = 2 energy levels.
(b) draw dashed rings to represent the levels
6 p+
6 n0
3. To add in the electrons (e-) use the atomic number, this is equal to the number of electrons in
the element, to determine how many electrons to add.
(a) Use a dot, ● = e-. Carbon: atomic number = 6 = 6 electrons.
(b) One pair of electrons on each side of the level, 1st level 2 e-, 2nd level 8 e-, 3rd level 8 e-, etc.
Energy levels can only hold a max. of 8 electrons (except for the 1 st), this referred to the
Octet Rule.
6 p+
6 n0
ASSIGNMENT: On loose-leaf paper, divide the sheet into 3 columns (see example table)
Complete the table for elements 1-20 from the periodic table (leave EELR column blank)
Element
Hydrogen
# protons =
# electrons=
# neutrons=
Bohr Model
EELR
Will be completed at a later
time
helium# protons =
# electrons=
# neutrons
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
PRACTICE QUESTIONS
Unit A—Energy and Matter in Chemical Change
W ORKSHEET
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Electron Dot Diagrams
Goal  Demonstrate your understanding of energy levels, and practice drawing electron dot diagrams.
What to Do
Answer each question in the space provided.
1. Complete the following table.
Name of element
Period number
hydrogen
Group number
Number of
energy levels
Number of valence
electrons
3
3
1
2
6
strontium
14
6
3
2
2. Complete the following table by drawing both the energy level diagram and electron dot diagram for
each element. The first row is completed as an example.
Energy level diagram
Electron dot diagram
Name of element
carbon
oxygen
lithium
Science 10 - Unit A
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Mr. R. Peebles
Energy level diagram
Name: __________________________________
Electron dot diagram
Name of element
chlorine
magnesium
phosphorus
3. Draw the missing electron dot diagrams in the following table. Refer to the periodic table as necessary.
4. What feature of helium’s energy levels justifies placing its two valence electrons in a pair? (See the table
above.)
5. Draw an electron dot diagram for an atom of each of the following elements.
selenium (Se)
bromine (Br)
strontium (Sr)
radon (Rn)
francium (Fr)
6. Explain how you decided on the number and placement of the dots.
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
PRACTICE QUESTIONS
Unit A—Energy and Matter in Chemical Change
W ORKSHEET
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Ions and Isotopes
What to Do
Answer each question in the space provided.
1. Complete the following table by filling in the missing information about ions.
Symbol
Number of protons
Number of electrons
Ion charge
Li+
3
2
1+
19
18
1+
Name of ion
lithium ion
Mg2+
chloride ion
9
1–
O2–
I–
scandium ion
18
2–
Se2–
7
10
Al3+
10
4–
calcium ion
phosphide ion
continue…
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
2. Complete the following table by drawing the EELR. The first row is completed as an example.
Ion
Symbol
Lithium
ion
EELR Diagram
Ion
Symbol
EELR Diagram
Aluminum
ion
+
Li
Oxide ion
Calcium ion
Iodide ion
Chloride ion
Sodium
ion
Beryllium ion
3. What is a common feature in all of the EELR diagrams in question 2? (Hint: think “levels”)
_______________________________________________________________________________________________
_______________________________________________________________________________________________
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
PRACTICE QUESTIONS
Unit A—Energy and Matter in Chemical Change
W ORKSHEET
9
Ionic Compounds
Part 1: Modelling Ionic Bonds
Model the formation of of the following ionic compounds using electron dot diagrams. Write the electron dot diagram
for each element in the name. Show the transfer of electrons and the formation of the ionic compound.
1. lithium hydride
4. sodium fluoride
continue…
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
5. calcium oxide
6. magnesium chloride
7. aluminium oxide
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
PRACTICE QUESTIONS
Unit A—Energy and Matter in Chemical Change
W ORKSHEET
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Ionic Compounds
1. Complete the following table.
Element
Anion
Name
Symbol
Name
Symbol
fluorine
F
fluoride
F–
chloride
bromide
oxide
sulfide
nitride
2. Complete the following table.
Formula
Total charge on
cation(s)
Total charge on
anion(s)
Correct () or
incorrect (X)
formula?
Correct formula and
name of compound
(a) LiO
(b) MgO
(c) K2S
(d) AlBr3
(e) NaN3
continue…
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
3. Complete the following table to write the formula of each compound.
Name of compound
Cation
Anion
Formula
(a) beryllium fluoride
(b) sodium nitride
(c) calcium sulfide
(d) aluminum chloride
(e) lithium oxide
(f) magnesium nitride
(g) gallium sulfide
(h) barium bromide
4. Write the chemical formula of the following. Include the state.
a) lithium hydride
f) magnesium chloride
b) silver chloride
g) aluminum hydride
c) sodium oxide
h) barium sulfide
d) calcium phosphide
i) strontium phosphide
e) sodium iodide
j) potassium phosphide
continue…
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
5. Write the proper chemical name of the following:
a) NaCl(s)
f) ScCl3(s)
b) Al2S3(s)
g) AlF3(s)
c) MgI2(s)
h) LiBr(s)
d) Zn3As2(s)
i) Na2S(s)
e) CsF(s)
j) BaI2(s)
6. Complete the following table to find the charge on the cation in these compounds. Decide if your answers
are reasonable before you move on to question 7.
Compound
Charge on cation
(a) Cu2S
(b) Cr2O3
(c) PbO2
(d) NiCl2
(e) CrN
(f) HgO
7. Complete the following table by adding the missing Stock system names.
Formula
Ion
Name
FeCl3
Fe3+
iron(III) chloride
FeO
Fe2+
Cu2S
Cu +
PbO 2
Pb 4+
continue…
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
8. Complete the following table to write the chemical formula for each compound.
Name of compound
Cation
Anion
Chemical formula
(a) copper(I) oxide
(b) lead(IV) bromide
(c) iron(III) sulfide
(d) nickel(III) fluoride
(e) manganese(IV) sulfide
9. Write the chemical formula of the following (Remember: Stock System). Include the state.
a) chromium(II) oxide
f) vanadium(V) oxide
b) tin(II) iodide
g) copper(I) bromide
c) copper(II) selenide
h) lead(IV) oxide
d) iron(III) chloride
i) chromium (III) phosphide
e) mercury(I) sulfide
j) bismuth(III)selenide
10. Write the proper chemical name of the following: (Remember: Stock System).
a) MnCl4(s)
h) SnCl4(s)
b) CuBr2(s)
i) Hg2S (s)
c) FeO (s)
j) Ni2S3(s)
continue…
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
d) CoCl2(s)
k) FeBr3(s)
e) Hg3P2(s)
l) CuCl2(s)
f) Fe2O3(s)
m) BiF5(s)
g) TiO2(s)
n) SnS2(s)
Analyze
1. Explain why you must use the Stock system to name ionic compounds containing transition metals. In
which cases do you not need to use the Stock system to name an ionic compound? Explain your answer.
2. There is something wrong with the name written beside each of the following compounds. In each case,
explain why the name is wrong, and then write the correct name.
Formula
Incorrect name
(a) Ti2O3
dititanium trioxide
(b) NaCl
sodium(I) chloride
(c) CuCl2
copper chloride
(d) NO2
nitrogen(IV) oxide
Science 10 - Unit A
Explanation
21
Correct name
Mr. R. Peebles
Name: __________________________________
PRACTICE QUESTIONS
Unit A—Energy and Matter in Chemical Change
W ORKSHEET
11
Polyatomic Ionic Compounds
1. Write the chemical formula of the following. Include the state.
a) mercury(II) borate
m) calcium hydrogen carbonate
b) zinc dihydrogen phosphate
n) barium chromate
c) calcium sulfite
o) silver dichromate
d) iron(III) nitrate
p) lead(IV) carbonate
e) chromium(III) iodate
q) tin(II) oxalate
f) sodium borate
r) sodium silicate
g) zinc sulfate
s) barium cyanide
h) strontium acetate
t) sodium silicate
i)
antimony (V) iodate
u) cobalt(II) nitrate
j)
zinc phosphate
v) hydrogen hypochlorite
k) cesium borate
w) silver acetate
continue…
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
2. Write the proper chemical name of the following:
a) K3PO4(s)
k) Al2(SO4)3(s)
b) PbCr2O7(s)
l) CuMnO4(s)
c) Co3(PO4)2(s)
m) Hg(NO3)2(s)
d) Fe2(CO3)3(s)
n) Pb(CrO4)2(s)
e) Sn(HSO 4)2(s)
o) NiCO3(s)
f) Cu3PO4(s)
p) Ag2SO 4(s)
g) Fe(HCO3)3(s)
q) PbSO 4(s)
h) Cr2(CO3)3(s)
r) Ni3(PO4)2(s)
i)
Sr(IO3)2(s)
s) CuSO4(s)
j)
Hg(ClO3)2(s)
t) Sb2(HPO4)3
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
PRACTICE QUESTIONS
Unit A—Energy and Matter in Chemical Change
W ORKSHEET
12
Molecular Compounds
Part 2: Modelling Covalent Bonds
Model the formation of of the following molecular compounds using electron dot diagrams. Write the electron dot
diagram for each element in the name. Show the sharing of electrons and the formation of the molecular compound.
1. molecular hydrogen
2. water, H2O
3. methane, CH4
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
4. molecular oxygen
5. molecular nitrogen
6. carbon disulfide
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
PRACTICE QUESTIONS
Unit A—Energy and Matter in Chemical Change
W ORKSHEET
13
Naming Molecular Compounds
1. Write the chemical formula of the following:
a)
sulfur hexafluoride
g) dinitrogen hexabromide
b)
carbon dioxide
h) sulfur dioxide
c)
dinitrogen monoxide
i) carbon monoxide
d)
arsenic tribromide
j) tetraphosphorous decaoxide
e)
tetranitrogen hexahydride
k) dinitrogen pentachloride
f)
disulfur hexafluoride
l) carbon tetrachloride
2. Write the proper chemical name of the following:
a)
P2Cl5
g) SiS2
b)
NCl3
h) OCl2
c)
CS2
i) NO2(g)
d)
ClBr2
j) P2O5
e)
NO(g)
k) SF6
f)
N2O4
l) PBr5
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
PRACTICE QUESTIONS
Unit A—Energy and Matter in Chemical Change
W ORKSHEET
14
Review: Naming Ionic and Molecular Compounds
Complete the following table.
Chemical formula
Ionic or molecular?
Name of compound
NH4Cl
potassium sulfide
CI4
calcium oxide
ammonium chloride
Li3N
Mg(OH)2
zinc oxide
CuNO 3
silicon dioxide
oxygen dichloride
CuCl
FeCl2
calcium sulfide
calcium hydrogencarbonate
P2O5
silicon tetrabromide
aluminium bromate
Ca(HS)2
ammonium nitrite
AgCH3COO
calcium chromate
N2O5
iron(III) carbonate
HgS
silver hydrogensulfate
continue…
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
Chemical formula
Ionic or molecular?
Name of compound
KMnO 4
Mg(OH)2
AlPO4
carbon disulfide
potassium sulfate
SnF2
K2Cr2O 7
HgS
sodium tetraborate
vanadium(V) oxide
(NH4)2Cr2O7
bismuth(V) phosphate
Na2SiO 3
Co3(PO 4)2
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
PRACTICE QUESTIONS
Unit A—Energy and Matter in Chemical Change
W ORKSHEET
15
Solubility Table
Goal  Predict solubility using a solubility table.
What to Do
Use the following solubility table to complete the tables below.
NH4+
NO3–
CH3COO–
Cl–
SO 42–
S2–
OH–
CO32–
Ions
all
ClO3–
Br–
PO43–
ClO4–
I–
SO32–
all
most
most
most
group 1
group 1
group 1
group 2
NH4+
NH4+
NH4+
Sr2+
High
solubility
Ba2+
Tl+
none
none
Ag+
Ag+
Ag+
Hg+
Pb 2+
Pb 2+
Cu+
Ca2+
Hg+
Ba2+
Tl+
Sr2+
most
most
most
Low
solubility
Ra2+
1. Complete the following table.
Cation
Anion
Na+
Cl–
High or low
solubility?
Name
Formula
sodium chloride
NaCl
lithium iodide
Mg(ClO3)2
strontium hydroxide
BaCO3
continue…
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
2. Complete the following table.
Name
Formula
High or low
solubility?
Al(OH)3
ammonium chloride
K2S
molybdenum(V) chlorate
Pb(CH3COO)2
copper(II) iodide
FeCO3
calcium sulfite
Ba3(PO4)2 (s)
palladium(II) bromide
HgI
strontium sulfate
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
Unit A—Energy and Matter in Chemical Change
Activity
Water’s Purpose in a Reaction
W ORKSHEET
16
1) Purpose: To examine some of the basic principles of chemical reactions and to make
qualitative observations of chemical reactions
2) Design: Two solid substances will be mixed in order to produce a chemical reaction.
3) Materials:
a) lead (II) nitrate
b) potassium iodide
c) Cream of tartar (potassium
bitartrate)
d) Baking soda (sodium bicarbonate)
e)
f)
g)
h)
10 weighing dishes
4 x 30mL beakers
Glass stirring rod
Scopula
4) CAUTION: LEAD (II) NITRATE AND SODIUM IODIDE ARE STRONG OXIDIZING AGENTS
AND MAY IRRITATE OR BURN YOUR SKIN. GLOVES AND GOGGLES ARE MADITORY!
FOLLOW ALL PROCEDURES AND DISPOSAL PROCEDURES!
5) Part 1: Lead (II) nitrate and sodium iodide
a) A balanced chemical reaction for the mixing of lead (II) nitrate and sodium iodide is
provided as followed. Label each compound correctly.
(reactants)
Pb(NO3)2 (s)
+2 KI (s)
(products)

PbI2
+ 2 KNO3
_____________ +______________  _______________ +________________
b) Are the reactants molecular or ionic substances? How do you know?
_______________________________________________________________________________________________
______________________________________________________________________________________________
c) Gather approximately 2 x 0.5 g of each reactant in labelled weighing dishes and return to
your work table. CAUTION! Record your observations of the reactants:
_______________________________________________________________________________________________
______________________________________________________________________________________________
d) Combine 0.5 g of each reactant into a separate weighing dish and mix together using a
glass stirring rod. Record your observations.
_______________________________________________________________________________________________
______________________________________________________________________________________________
e) In separate 30 mL beakers, dissolve the remaining 0.5 g of each solid in approximately 5
mL of water. Record your observations.
_______________________________________________________________________________________________
______________________________________________________________________________________________
continue…
Science 10 - Unit A
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Mr. R. Peebles
Name: __________________________________
f) Pour the potassium iodide solution into the lead (II) nitrate solution and record your
observations.
_______________________________________________________________________________________________
______________________________________________________________________________________________
g) Dispose of all liquids and solid waste into the appropriate containers.
DO NOT POUR WASTE DOWN THE DRAIN OR PLACE IN THE GARBAGE.
6) Part 2: Baking soda and cream of tartar
a) The following balanced reaction is provided for you: name the missing reactants and
products.
NaHCO3(s) + KHC4H4O6(s)  NaKC4H4O6 (aq) + CO2(g) + H2O(l)
_______________+potassium bitartrate
sodium potassium tartrate + ________________+ ____________
b) Are the reactants molecular or ionic substances? How do you know?
_______________________________________________________________________________________________
______________________________________________________________________________________________
c) Based on the chemical equation, what do you expect to see when you mix the reactants
provided?
___________________________________________________________________
d) Gather approximately 2 x 0.5 g of each reactant in labelled weighing dishes and return to
your work table. Record your observations of the reactants:
_______________________________________________________________________________________________
______________________________________________________________________________________________
e) Combine 0.5 g of each reactant into a separate weighing dish and mix together using a
glass stirring rod. Record your observations.
_______________________________________________________________________________________________
______________________________________________________________________________________________
f) In separate 30 mL beakers, dissolve the remaining 0.5 g of each solid in approximately 5
mL of distilled water. Record your observations.
_______________________________________________________________________________________________
______________________________________________________________________________________________
g) Pour the sodium bicarbonate solution into the potassium bitartrate solution and record your
observations.
_______________________________________________________________________________________________
______________________________________________________________________________________________
h) For Part 2 ONLY, all waste may be thrown in the garbage and/or down the drain.
continue…
Science 10 - Unit A
32
Mr. R. Peebles
Name: __________________________________
7) Between your partner and you, devise a scientific theory for why the solid mixtures not react
until you dissolved them in water as you observed in Parts 1 and 2.
____________________________________________________________________________________________
____________________________________________________________________________________________
____________________________________________________________________________________________
____________________________________________________________________________________________
____________________________________________________________________________________________
____________________________________________________________________________________________
____________________________________________________________________________________________
8) Based on how the reaction actually occurred, copy and rewrite the chemical equations with the
appropriate states for each reactant and product as they where in the reaction.
a) Part 1: (you will need to use your solubility table to determine which product formed the
solid)
b) Part 2:
Science 10 - Unit A
33
Mr. R. Peebles
Name: __________________________________
Unit A—Energy and Matter in Chemical Change
Activity
Physical or Chemical Reactions?
W ORKSHEET
17
What to Do
Classify each change in the following table as either chemical or physical. Explain your classification.
Chemical or physical?
Explanation
Change
A sheet of paper is crumpled into a ball.
A sheet of paper is set on fire and burns
to ashes.
Steel wool is placed in a glass of salty
water. The steel wool rusts.
A sheet of flexible, colourless plastic is
left outside, in bright sunlight, and
becomes yellow and brittle over time.
A teaspoon of white sugar (sucrose)
dissolves in a glass of warm water.
Vinegar is poured over a teaspoon of
baking soda. The white powdered
baking soda fizzes, and bubbles form.
A red-hot nail is inserted into a large
block of ice. Steam is formed as the nail
contacts the block, and water flows
away from the nail.
Science 10 - Unit A
34
Mr. R. Peebles
Name: __________________________________
Unit A—Energy and Matter in Chemical Change
Activity
Chemical Reactions
W ORKSHEET
18
1. Complete the following tables writing the complete skeleton equation for each question.
- Ensure to include:
o Proper chemical formulas (remember: Ionic vs. Molecular)
o States for each compound or element (refer to periodic table and solubility table)
Word
equation
iron + sulfur → iron(II) sulfide
Skeleton
equation
2.
calcium + oxygen gas → calcium oxide
Word
equation
Skeleton
equation
3.
Word
equation
calcium oxide + carbon dioxide → calcium carbonate
Skeleton
equation
4.
copper(II) oxide → copper + oxygen gas
Word
equation
Skeleton
equation
5.
Word
equation
water → hydrogen gas + oxygen gas
Skeleton
equation
continue…
Science 10 - Unit A
35
Mr. R. Peebles
Name: __________________________________
6.
potassium + water → potassium hydroxide + hydrogen gas
Word
equation
Skeleton
equation
7.
Word
equation
zinc + tin(II) chloride → zinc chloride + tin
Skeleton
equation
8.
Word
equation
copper + silver nitrate → copper(II) nitrate + silver
Skeleton
equation
9.
Word
equation
potassium iodide + lead(II) nitrate → potassium nitrate + lead(II) iodide
Skeleton
equation
10.
Word
equation
sodium chloride + silver nitrate → sodium nitrate + silver chloride
Skeleton
equation
11.
Word
equation
barium chloride + potassium sulfate → barium sulfate + potassium chloride
Skeleton
equation
continue…
Science 10 - Unit A
36
Mr. R. Peebles
Name: __________________________________
12. Refer back to your chemical reactions, 1-11. What do the reactions in each group have in
common?
Reactions
Similarities among reactions
1, 2, and 3
4 and 5
6, 7, and 8
9, 10, and 11
13.
Develop a classification system for the chemical reactions you observed in this activity.
continue…
Science 10 - Unit A
37
Mr. R. Peebles
Name: __________________________________
14.
Write the skeleton equations 1-11 on the following page. Using the pipe cleaners to assist
you, devise a method to ensure that the Law of Conservation of Matter (the number of
atoms in the reactants must equal the number of atoms in the products) remains true for
each equation.
Equation #
Skeleton Equation
1
Fe (s)
+
S8 (s)

FeS (s)
2
3
4
5
6
7
8
9
10
11
Science 10 - Unit A
38
Mr. R. Peebles
Name: __________________________________
Unit A—Energy and Matter in Chemical Change
Activity
Balancing Chemical Reactions
W ORKSHEET
19
What to Do
Answer the questions in each section in the space provided.
Balancing Formation Reaction Equations
1. Balance each equation for a formation reaction.
(a)
K(s)
+
O2(g)

K2O (s)
(b)
P4(s)
+
Cl2(g)

PCl5(s)
(c)
Cu(s)
+
S8(s)

CuS(s)
(d)
Mg(s)
+
O2(g)

MgO(s)
(e)
Fe(s)
+
O2(g)

Fe2O3(s)
(f)
P4(s)
+
S8(g)

P2S5(s)
(g)
C(s)
+
O2(g)

CO(g)
(h)
N2(g)
+
O2(g)

NO2(g)
(i)
Li(s)
+
N2(g)

Li3N(s)
(j)
S8(s)
+
O2(g)

SO2(g)
2. Write a balanced chemical equation to represent each reaction described below.
(a) Solid aluminum metal reacts with oxygen gas to form solid aluminum oxide.
(b) Metallic zinc combines with elemental sulfur to form zinc sulfide.
Balancing Decomposition Reaction Equations
3. Balance each equation for a decomposition reaction.
(a)
NaCl(s) 
Na(s)
+ Cl2(g)
(b)
CaBr2(s)

Ca(s)
(c)
CCl4(l) 
C(s)
+ Cl2(g)
(d)
NCl3 (g) 
N2(g)
+ Cl2(g)
+
Br2(l)
continue…
Science 10 - Unit A
39
Mr. R. Peebles
Name: __________________________________
(e)
P4O10(s) 
P4(s)
+ O2(g)
(f)
Ag2O(s) 
Ag(s)
+ O2(g)
(g)
HCl(aq) 
H2(g)
+ Cl2(g)
(h)
KI(s)

K(s)
+ I2(s)
(i)
AlCl3(s) 
Al(s)
+ Cl2(g)
(j)
CuO(s) 
Cu(s)
+ O2(g)
4. Write a balanced chemical equation to represent each reaction described below.
(a) Rubidium oxide decomposes into its elements.
(b) Calcium chloride decomposes into its elements.
Balancing Single Replacement Reaction Equations
5. Balance each equation for a single replacement reaction.
(a) K(s)
+
H3PO4(aq)

K3PO4(aq)
+
H2(g)
(b)
Fe(s)
+
H2S(aq)

Fe2S3(s)
+
H2(g)
(c)
Cl2(g)
+
MgBr2(aq)

MgCl2(aq)
+
Br2(aq)
(d)
Cu(s)
+
Ag2CO3(s)

CuCO3(s)
+
Ag(s)
(e)
Br2(g)
+
KI(aq)

I2(aq)
+
KBr(aq)
(f)
Mg(s)
+
Zn3(PO4)2(s)

Mg3(PO4)2(s)
+
Zn(s)
(g)
K(s)
+
Al(NO3)3(aq)

Al(s)
+
KNO3(aq)
(h)
Ca(s)
+
H2O(l)

Ca(OH)2(s)
+
H2(g)
(i)
Na(s)
+
H2SO4(s)

Na2SO 4(aq)
+
H2(g)
(j)
K(s)
+
H2O(l)

KOH(aq)
+
H2(g)
6. Write a balanced chemical equation to represent each reaction (a & b) described below.
(a) Silver reacts with gold(III) nitrate.
continue…
Science 10 - Unit A
40
Mr. R. Peebles
Name: __________________________________
(b) Copper reacts with lead(II) sulfate.
Balancing Double Replacement Reaction Equations
7. Balance each equation for a double replacement reaction.
(a) Na2SO 4(aq)
+
BaCl2(aq)

BaSO4(s)
+
NaCl(aq)
(b)
HNO3(aq)
+
Ba(OH)2(aq)

H2O(l)
+
Ba(NO3)2(aq)
(c)
Na2CO3(aq)
+
Fe(NO3)3(aq)

Fe2(CO3)3(s)
+
NaNO3(aq)
(d)
CaCl2(aq)
+
K3PO 4(aq)

Ca3(PO4)2(s)
+
KCl(aq)
(e)
Al2(SO4)3(aq)
+
Ba(OH)2(aq)

Al(OH)3(s)
+
BaSO 4(s)
(f)
NaOH(aq)
+
H2SO 4(aq)

H2O(l)
+
Na2SO4(aq)
(g)
Na3PO 4(aq)
+
Ag2SO4 (s)

Na2SO4(aq)
+
Ag3PO4(s)
(h)
Na2CrO4(aq)
+
Cu(NO 3)2(aq)

NaNO3(aq)
+
CuCrO4(aq)
(i)
H3PO4(aq)
+
KOH(aq)

H2O(l)
+
K3PO 4(aq)
(j)
Na2CO3(aq)
+
HNO3(aq)

H2CO3(aq)
+
NaNO3(aq)
8. Write a balanced chemical equation to represent each reaction described below.
(a) Solutions of sodium hydroxide and hydrochloric acid react.
(b) A silver nitrate solution reacts with a sodium chloride solution.
Balancing Combustion Reaction Equations
9. Balance each equation for a combustion reaction.
(a) C2H6(g)
+
O2(g)

CO2(g)
+
H2O(g)
(b)
C3H8(g)
+
O2(g)

CO2(g)
+
H2O(g)
(c)
C6H14(g)
+
O2(g)

CO2(g)
+
H2O(g)
(d)
C8H18(g)
+
O2(g)

CO2(g)
+
H2O(g)
(e)
C2H2(g)
+
O2(g)

CO2(g)
+
H2O(g)
(f)
C2H4(g)
+
O2(g)

CO2(g)
+
H2O(g)
continue…
Science 10 - Unit A
41
Mr. R. Peebles
Name: __________________________________
(g)
ZnS(s)
+
O2(g)

ZnO(s)
+
SO2(g)
(h)
CH3NO2(l)
+
O2(g)

CO2(g)
+
H2O(g)
(i)
NH3(g)
+
O2(g)

NO2(g)
+
H2O(g)
(j)
C2H5SH(g)
+
O2(g)

CO2(g)
+
H2O(g)
+
NO2(g)
+
SO2(g)
10. Write a balanced chemical equation to represent each reaction described below.
(a) Candle wax, C25H52, is burned to produce carbon dioxide and water.
(b) Sucrose, C12H22O11, is burned to produce carbon dioxide and water.
Classifying and Balancing Equations
11. Classify each reaction as a formation (F), decomposition (D), single replacement (SR), double
replacement (DR), or combustion (C) reaction. Then balance each equation.
Reaction
Classification
Li(s)
+
AlCl3(aq)

Al (s)
NH3(g)

N2(g)
+
H2(g)
K(s)
+
Br2(l)

KBr(s)
C10H22(l)
+
O2(g)

NH4OH (aq)
+
H2CO3(aq)
H2O (l)

Al(s)
Zn(s)
+
LiCl(aq)
CO2(g)
+
H2O(g)

H2O(l)
+
(NH4)2CO 3(aq)
H2(g)
+
O2(g)
+
Cl2(g)

AlCl3(s)
+
SnF4(aq)

Sn(s)
+
ZnF2(aq)
Science 10 - Unit A
42
Mr. R. Peebles
Name: __________________________________
Unit A—Energy and Matter in Chemical Change
Activity
Mole Calculations
W ORKSHEET
20
Find the molar mass of each of the following elements.
1. potassium , K(s)
2. zirconium, Zr(s)
3. chlorine, Cl2(g)
4. oxygen, O 2(g)
Determine the molar mass of each of the following compounds.
5. potassium bromide, KBr(s)
6. methane, CH4(g)
Science 10 - Unit A
43
Mr. R. Peebles
Name: __________________________________
7. sodium sulfate, Na2SO4(s)
8. aluminum nitrate, Al(NO3)3 (s)
Calculate the number of moles in each of the following:
9. 1000 g of NaCl
10. 32.5 g of NaHCO 3(s)
11. 4.69 g of Na2CO3(s)
12. 0.258 g of MgSO 47H2O(s)
Science 10 - Unit A
44
Mr. R. Peebles
Name: __________________________________
13. 550 g of sodium phosphate
14. 6.2 g of carbon dioxide
15. 500 mL of water
Calculate the mass in grams of the following:
16. 0.21 mol of NaCl(s)
17. 55.56 mol of H2O(l)
Science 10 - Unit A
45
Mr. R. Peebles
Name: __________________________________
18. 0.100 mol of KHC4H4O6(s)
19. 1.2 mol of sodium sulphate decahydrate
20. 0.15 mol of phosphorus
21. 0.025 mol of tin (II) fluoride
22. 0.400 mol of calcium sulphate dihydrate
Science 10 - Unit A
46
Mr. R. Peebles