Aboriginal Peoples and Chemistry
List 5 ways Aboriginal peoples used chemicals:
Safety
List 5 pieces of info provided on a MSDS
What are the 3 ways in which WHMIS informs workers about chemicals?
Classification of Matter
Chemical and Physical Properties
Matter
Mixtures
Heterogeneous Homogeneous
Pure Substances
Compounds Elements
Chemical Properties
• describe reactivity of a substance
•
Physical Properties
• describe physical appearance of a substance
Color and Label the periodic table…
Metals and Non-Metals
State Appearance Conductivity Malleability and
ductility
Metals
Non-metals
Metalloids
Developing Atomic Theories
Dalton’s Atom
Theory
Gas Discharge Tube
Describe:
How did they use gas discharge tubes to provide evidence of electrons (JJ Thompson)?
Kelvin / Thompson Model
Describe:
Rutherford’s Experiment
Describe:
Restate Rutherford’s logic in developing his view of the atom
↓
↓
↓
↓
Define:
Nucleus:
Electron:
Empty Space:
Discuss Rutherford’s reasoning for the NEUTRON…
What is an isotope?
What did Niels Bohr mean by “energy levels” for
electrons?
A Working Model of the Atom
Subatomic Particle Relative Charge Symbol Mass (g) Radius (m)
How can the number of neutrons be calculated in different isotopes of the same element?
Electron Dot Diagram
Draw each diagram….
B F S
Name: _____________________________________
Atomic Number and Mass Number
Name Mass Number Atomic
Number
Number of
Protons
Number of
Neutrons
carbon-14 14 6 6 8
hydrogen-1 1 1
hydrogen-2 2 1
carbon-12
oxygen-18
4 2
20 10
64 29
35 45
7 7
16 16
20 21
9 10
26 30
53 74
calcium-40
119 50
26 33
208 82
silver-108
mercury-201
Unit A—Energy and Matter in Chemical Change Unit Support
L ine Master 4
Define:
ION-
Cation-
Anion-
What is a stable octet?
Unit A—Energy and Matter in Chemical Change Unit Support
L ine Master 6
Name: _____________________________________
Atoms and Ions I
Symbol Number of
Protons
Number of
Electrons
Electric Charge
Li+ 3 2 1+
C 6 6 0
F− 9 10 1−
Mg2+
K+
Li
S2−
He
18 0
8 2−
17 1−
11 0
Ca2+
18
Fe3+
23
Fe2+
24
78 1+
78 2+
82 78
30 30
Unit A—Energy and Matter in Chemical Change Unit Support
L ine Master 7
Name: _____________________________________
Atoms and Ions II
Name Symbol Mass
Number
Atomic
Number
Protons Neutrons Electrons Electric
Charge
fluorine atom F 19 9 9 10 9 0
nitride ion N3−
15 7 7 8 10 3−
boron atom 11
carbon atom 14
aluminium
ion
14 3+
gold ion 116 1+
40 19 0
79 35 35
19 18 1−
16 16 2−
Ag 110
cesium ion 77 1+
I− 125
Forming Compounds
Descibe:
Forming Ionic Compounds
Properties of
Ionic Compounds
Naming Ionic Compounds
1.
2.
3.
How to write an ionic compound formula
1.
2.
3.
4.
5.
Unit A—Energy and Matter in Chemical Change Unit Support
L ine Master 8
Name: _____________________________________
Ionic Compounds—Univalent Metal Ions
1. If the following pairs of elements were mixed and heated, they would combine into solid ionic
compounds. Write the name and formula of each compound formed.
Name Formula
a) silver and iodine silver iodide AgI(s)
b) magnesium and oxygen
c) magnesium and bromine
d) calcium and nitrogen
e) zinc and selenium
f) sodium and sulfur
g) barium and phosphorus
h) aluminium and fluorine
i) potassium and chlorine
j) silver and oxygen
continued...
Unit A—Energy and Matter in Chemical Change
2. Write the correct names for each of the following compounds.
a) MgCI2
b) Ag3N
c) CsF
d) CdO
e) MgBr2
f) Al2O3
g) NaI
h) K2S
i) BaS
j) Li3P
Ionic Compounds Worksheet Name: ______________
A. Write the name of each of the following ionic compounds:
1. LiCl(s) ________________ 2. KBr(s) ______________
3. CaCl2(s) ________________ 4. MgO(s) ______________
5. KF(s) ________________ 6. K2O(s) ______________
7. CaO(s) ________________ 8. BeF2(s) ______________
9. AlI3(s) ________________ 10. SrS(s) ______________
11. Rb3P(s) ________________ 12. Fr2O(s) ______________
13. MgCl2(s) ________________ 14. CaF2(s) ______________
B. Write the chemical formula for each of the following ionic compounds:
1. sodium fluoride ___________ 2. barium bromide _________
3. magnesium fluoride __________ 4. aluminum chloride _______
5. lithium bromide _________ 6. potassium nitride ________
7. magnesium sulfide ___________ 8. strontium sulfide ________
9. calcium iodide ___________ 10. cesium fluoride _________
11. lithium phosphide __________ 12. aluminum oxide _________
AND: Complete practice problem 1 on page 43
Multivalent Ionic Compounds
1.
2.
3.
4.
Unit A—Energy and Matter in Chemical Change Unit Support
L ine Master 9
Name: _____________________________________
Ionic Compounds—Multivalent Metal Ions
1. If the following pairs of elements were mixed and heated, they would combine into solid ionic
compounds. In this worksheet, use the most common ionic form of the multivalent metal ion.
The most common form is listed first in the periodic table. For example, iron exists as both 2+
and 3+ ions, with iron(III) being the most common.
Name Formula
a) iron and sulfur iron(III) sulfide Fe2S3(s)
b) copper and oxygen
c) manganese and fluorine
d) gold and nitrogen
e) chromium and chlorine
f) platinum and
phosphorus
g) nickel and oxygen
h) cobalt and bromine
i) tungsten and iodine
j) manganese and sulfur
continued...
Unit A—Energy and Matter in Chemical Change
2. Write the correct name for each of the following compounds. The charge on the multivalent
ion is not given by the periodic table. It is determined by the charge of the non-metal and the
subscripts that appear in the formula.
a) FeCl2(s) iron(II) chloride
b) FeBr3(s)
c) CrS(s)
d) SnO2(s)
e) Pb3N2(s)
f) HgI2(s)
g) CrO3(s)
h) MnF4(s)
i) Cu2O(s)
j) AuI3(s)
Polyatomic Ionic Compounds
1.
2.
3.
Unit A—Energy and Matter in Chemical Change Unit Support
L ine Master 10
Name: _____________________________________
Ionic Compounds—Polyatomic Ions
The names and charges of polyatomic ions can be found in lists and need not be memorized. It is a
good idea, however, to get to know the more common ones introduced in the practice below.
Remember to form the name by combining the positive and negative ion:
name = positive ion + negative ion
COMBINE IONS FORMULA NAME
iron(II) & nitrate Fe2+
NO3− Fe(NO3)2(s) iron(II) nitrate
aluminium & nitrate Al3+
NO3− Al(NO3)3(s) aluminium nitrate
sodium & sulfate
lead(IV) & sulfate
magnesium &
carbonate
gold(III) & sulfite
zinc &
hydrogencarbonate
ammonium & nitrate
copper(I) & phosphate
silver & hydroxide
aluminium &
hydroxide
lead(II) & phosphate
potassium & acetate
manganese(V) &
sulfate
Polyatomic Ionic Compounds Worksheet Name: ______________
A. Write the name of each of the following compounds:
1. CuCO3(s) ________________ 2. Cu2CO3(s) _____________
3. NaNO3(s) ________________ 4. CuHCO3(s) _____________
5. CaSO4(s) ________________ 6. Mg(OH)2(s) ____________
7. Sr(ClO2)2(s) ______________ 8. Na2Cr2O7(s) ___________
9. Ba(CH3COO)2(s) ___________ 10. KSCN(s) ______________
11. LiNO2(s) ________________ 12. LiNO3(s) ______________
13. FeSO4(s) ________________ 14. NaOH(s) ______________
B. Write the chemical formula for each of the following compounds:
1. magnesium sulfate __________ 2. ammonium hydroxide __________
3. sodium phosphate __________ 4. copper (II) nitrate ___________
5. ammonium chloride __________ 6. calcium sulfite _______________
7. sodium hydrogensulfite ________ 8. nickel (II) phosphate __________
9. barium hydroxide ___________ 10. iron (III) carbonate __________
11. copper (I) permanganate ______ 12. iron (II) carbonate __________
All Ionic Compounds Worksheet
Write the chemical formula Name each compound
for each compound
1. calcium carbonate a. IrO2
2. beryllium oxide b. RaS
3. lithium fluoride c. MgO
4. nickel (ll) bromide d. CaCl2
5. lead (ll) chloride e. SnBr2
6. ammonium hydroxide f. KOH
7. silver phosphate g. Al2O3
8. magnesium acetate h. Ti(NO3)4
9. rubidium sulfide i. AgClO4
10. potassium permanganate j. Sr3(PO4)2
11. barium nitride k. PtO
12. strontium sulfate l. CuI
13. strontium sulfite m. Cu2CO3
14. lithium hydroxide n. AgCH3COO
15. iron (lll) oxide o. NaNO3
16. titanium (lV) iodide p. Cr2(OOCCOO)3
Unit A—Energy and Matter in Chemical Change Unit Support
L ine Master 11
Name: _____________________________________
All Ionic Compounds
I. Write the formula for each compound.
1) calcium acetate
2) potassium chloride
3) ammonium carbonate
4) sodium nitride
5) titanium(IV) hypochlorite
6) iron(III) sulfide
7) zinc dichromate
8) platinum(IV) oxide
9) aluminium hydroxide
10) mercury(II) nitrate
11) strontium fluoride
12) tin(IV) hydrogenoxalate
13) calcium peroxide
14) gold(I) sulfate
15) lead(IV) thiocyanate
16) nickel(III) sulfide
continued...
Unit A—Energy and Matter in Chemical Change
II. Write the name of each compound.
17) CsI(s)
18) SnCl4(s)
19) Cr(NO3)3(s)
20) (NH4)3PO4(s)
21) Cu2SO4(s)
22) Mg(H2PO4)2(s)
23) Na2S2O3(s)
24) AgClO3(s)
25) Zn(OH)2(s)
Solubility
Properties of acids and bases
Very Soluble
Slightly Soluble
Properties of Acids Identifying Acids
Classical Naming of Acids IUPAC Naming of Acids
Acids
Neutralization Reactions
Properties of Bases Identifying Bases
Naming Bases
Bases
Ionic Compounds, Acids, & Bases Worksheet
Chemical Name Chemical Formula Ionic, Acid, or Base
rubidium oxide
strontium hydroxide
HNO2(aq)
iron (II) iodide
NaOH(aq)
CrO(s)
Pb(NO3)4(aq)
aqueous hydrogen
sulfate
Ag3PO4(s)
potassium hydroxide
HCl(g)
HCl(aq)
lithium fluoride
aluminum phosphide
acetic acid
beryllium sulphide
CuF(s)
Au2Se(s)
Ti(OH)3(aq)
hydroiodic acid
SnO2(s)
C6H5COOH(aq)
lithium hydroxide
ZnBr2(s)
platinum (IV) chlorate
Describe
Forming Molecular
Compounds
Properties of
Molecular Compounds
Molecular Prefixes
Molecular Prefixes
Common Hydrogen
Compounds
diatomic & polyatomic
molecular elements
Unit A—Energy and Matter in Chemical Change Unit Support
L ine Master 12
Name: _____________________________________
Binary Molecular Compounds
A. Write the correct name for each compound below. Use prefixes to indicate the number of atoms of
each element in the name of the molecular compound. (Remember: The prefix “mono-” is not used
with the name of the first element.)
1 atom: mono- 3 atoms: tri- 5 atoms: penta- 7 atoms: hepta 9 atoms: nona-
2 atoms: di- 4 atoms: tetra- 6 atoms: hexa 8 atoms: octa- 10 atoms: deca-
1) BrCl3
2) BN
3) N2O3
4) NI3
5) SF6
6) XeF4
7) PCl3
8) CH4
9) PCl5
10) P2O5
11) S2Cl2
12) ICl2
13) NH3
14) P4O10
15) H2O
16) OF2
continued...
Unit A—Energy and Matter in Chemical Change
B. Write the correct formula for each compound below. Use subscripts to indicate the number of
atoms of each element in the formula (never reduce).
1) chlorine monoxide
2) sulfur hexachloride
3) dinitrogen monoxide
4) nitrogen trifluoride
5) sulfur tetrachloride
6) xenon trioxide
7) carbon dioxide
8) boron trichloride
9) diphosphorus pentoxide
10) phosphorus trichloride
11) sulfur dioxide
12) bromine pentafluoride
13) disulfur dichloride
14) boron trifluoride
15) tetraarsenic decoxide
16) silicon tetrachloride
Ionic and Molecular Compounds Worksheet Name: ______________
A. Write the name of each of the following compounds and state if it is ionic or
molecular. If ionic, state the solubility:
1. MgBr2 ________________ 2. KHSO4 __________________
3. CF4 ________________ 4. Ca(OH)2 __________________
5. N2Br4 ________________ 6. P2O5 __________________
7. NH3 ________________ 8. (NH4)3PO4 _________________
9. SO3 ________________ 10. NaOH __________________
11. CuSO4 ________________ 12. PCl3 __________________
13. CH4 ________________ 14. FeI3 __________________
B. Write the formula of each of the following compounds and state if it is ionic or
molecular. If ionic, state the solubility:
1. sulfur hexafluoride ___________ 2. silver phosphate ____________
3. phosphorus pentachloride ________ 4. sodium iodide _______________
5. manganese (II) chloride _________ 6. nitrogen trifluoride ___________
7. sodium perchlorate ___________ 8. methanol ______________
9. cobalt (II) permanganate ___________ 10. silicon tetrafluoride __________
11. ammonia _____________ 12. aluminum oxide _________
What is a chemical reaction?
What is combined?
What is formed?
5 pieces of evidence?
Reactants
Exothermic Reaction
Products
Endothermic Reaction
Conservation of Mass
Word Equation Chemical Equation
Balancing Equations
Rules
Steps
Balanced
Coefficients
States
Tips and Examples
Tips
Unit A—Energy and Matter in Chemical Change Unit Support
L ine Master 17
Name: _____________________________________
Balancing Formula Equations 1
Balance the following chemical equations:
a) _____ Na(s) + _____ O2(g) _____ Na2O(s)
b) _____ Al(s) + _____ Cl2(g) _____ AlCl3(s)
c) _____ N2(g) + _____ O2(g) _____ NO2(g)
d) _____ HI(g) _____ H2(g) + _____ I2(s)
e) _____ NH3(g) _____ H2(g) + _____ N2(g)
f) _____ Al2S3(s) _____ Al(s) + _____ S8(s)
g) _____ BN(s) + _____ Cl2(g) _____ BCl3(g) + _____ N2(g)
h) _____ SnF4(aq) + _____ Cr(s) _____ CrF3(aq) + _____ Sn(s)
i) _____ Mg(s) + _____ HCl(aq) _____ MgCl2(aq) + _____ H2(g)
j) _____ (NH4)3PO4(aq) + _____ CaBr2(aq) _____ Ca3(PO4)2(s) + _____ NH4Br(aq)
k) _____ Pb(NO3)4(aq) + _____ K2Cr2O7(aq) _____ Pb(Cr2O7)2(s) + _____ KNO3(aq)
l) _____ AgClO4(aq) + _____ Na3PO4(aq) _____ NaClO4(aq) + _____ Ag3PO4(s)
m) _____ HCl(aq) + _____ Ca(OH)2(s) _____ CaCl2(aq) + _____ H2O(l)
n) _____ CH3COOH(aq) + _____ Ba(OH)2(aq) _____ Ba(CH3COO)2(aq) + _____ H2O(l)
o) _____ C3H8(g) + _____ O2(g) _____ CO2(g) + _____ H2O(g)
p) _____ C6H14(l) + _____ O2(g) _____ CO2(g) + _____ H2O(g)
q) _____ C3H6OS2(s) + _____ O2(g) _____ CO2(g) + _____ H2O(g) + _____ SO2(g)
Unit A—Energy and Matter in Chemical Change Unit Support
L ine Master 18
Name: _____________________________________
Balancing Formula Equations 2
Balance the following chemical equations:
a) _____ Pb(s) + _____ O2(g) _____ PbO(s)
b) _____ N2(g) + _____ H2(g) _____ NH3(g)
c) _____ Na(s) + _____ H2O(l) _____ NaOH(aq) + _____ H2(g)
d) _____ C4H10(g) + _____ O2(g) _____ CO2(g) + _____ H2O(g)
e) _____ H3PO4(aq) + _____ KOH(aq) _____ K3PO4(aq) + _____ H2O(l)
f) _____ C5H12(l) + _____ O2(g) _____ CO2(g) + _____ H2O(g)
g) _____ Zn3N2(s) + _____ H2O(l) _____ Zn(OH)2(aq) + _____ NH3(g)
h) _____ Fe3O4(s) + _____ H2(g) _____ Fe(s) + _____ H2O(l)
i) _____ Al(s) + _____ H2SO4(aq) _____ H2(g) + _____ Al2(SO4)3(aq)
j) _____ CrS(s) + _____ O2(g) _____ CrO(s) + _____ SO2(g)
k) _____ HClO3(aq) + _____ HCl(aq) _____ H2O(l) + _____ Cl2(g)
l) _____ CaC2(s) + _____ AsBr3(aq) _____ C(s) + _____ As(s) + _____ CaBr2(aq)
m) _____ 4 NH3(g) + _____ 5 O2(g) _____ 4 NO(g) + _____ 6 H2O(l)
n) _____ HNO3(aq) + _____ NO(g) _____ NO2(g) + _____ H2O(l)
o) _____ Al(NO3)3(aq) + _____ NaOH(aq) _____ NaNO3(aq) + _____ Al(OH)3(s)
p) _____ C2H5OH(l) + _____ O2(g) _____ CO2(g) + _____ H2O(g)
q) _____ NaIO3(s) _____ NaI(s) + _____ O2(g)
Unit A—Energy and Matter in Chemical Change Unit Support
L ine Master 16
Name: _____________________________________
Writing Formula Equations from Word Equations
In the following exercises, recall that many of the non-metal elements exist as molecules, such as
H2(g) or S8(s). Refer to Table A2.9 on page 48 of Science 10 for the chemical formulas of molecular
elements.
1. Rewrite the following word equations as formula equations and then balance them:
a) solid sodium metal reacts with chlorine gas to produce solid sodium chloride
b) solid potassium metal reacts with oxygen gas to produce solid potassium oxide
c) hydrogen gas reacts with oxygen gas to produce liquid water
d) solid potassium chlorate decomposes into oxygen gas and solid potassium chloride
e) solid aluminium oxide is decomposed into solid aluminium and oxygen gas
f) mercury(II) sulfide is decomposed into liquid mercury and solid sulfur
g) aqueous cobalt(III) nitrate reacts with solid zinc to produce aqueous zinc nitrate and solid
cobalt
continued...
Unit A—Energy and Matter in Chemical Change
h) fluorine gas reacts with aqueous lead(IV) iodide to produce aqueous lead(IV) fluoride and
solid iodine
i) aqueous gold(III) bromide reacts with solid silver metal to produce solid silver bromide
and solid gold metal
j) aqueous sodium sulfate reacts with aqueous strontium hydroxide to produce aqueous
sodium hydroxide and solid strontium sulfate
k) aqueous thallium(I) hydroxide reacts with aqueous magnesium bromide to produce solid
magnesium hydroxide and solid thallium bromide
l) methane gas reacts with oxygen gas to produce carbon dioxide gas and water vapour
Types of Reactions
Formation
Decomposition
Combustion
Single Replacement
Double Replacement
Unit A—Energy and Matter in Chemical Change Unit Support
L ine Master 19
Name: _____________________________________
Classifying and Balancing Chemical Equations
A. Classify the following reactions as: formation, decomposition, single replacement, double
replacement, or combustion.
1. 2 KClO3(s) 2 KCl(s) + 3 O2(g)
2. 3 ZnCl2(aq) + 2 K3PO4(aq) 6 KCl(aq) + Zn3(PO4)2(s)
3. Mg(s) + 2 HCl(aq) MgCl2(aq) + H2(g)
4. 2 H2(g) + O2(g) 2 H2O(g)
5. Al(s) + 3 NiBr2(aq) 2 AlBr3(aq) + 3 Ni(s)
6. 4 Al(s) + 3 O2(g) 2 Al2O3(s)
7. 2 NaCl(s) 2 Na(s) + Cl2(g)
8. CaCl2(s) + F2(g) CaF2(s) + Cl2(g)
9. AgNO3(aq) + KCl(aq) AgCl(s) + KNO3(aq)
10. 2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g)
11. N2(g) + 3 H2(g) 2 NH3(g)
12. 2 H2O2(aq) 2 H2O(l) + O2(g)
13. (NH4)2SO4(aq) + Ba(NO3)2(aq) BaSO4(s) + 2 NH4NO3(aq)
14. MgI2(aq) + Br2(l) MgBr2(aq) + I2(s)
15. SO3(g) + H2O(l) H2SO4(aq)
continued...
Unit A—Energy and Matter in Chemical Change
B. Balance and classify each chemical equation below.
1. ____ CH4(g) + ____O2(g) ____CO2(g) + ___H2O(g)
2. ____ Na(s) + ____I2(s) ____NaI(s)
3. ____ NaOH(aq) + ____H2SO4(aq) ____Na2SO4(aq) + ____ H2O(l)
4. ____ Fe(s) + ____O2(g) ____Fe2O3(s)
5. ____ Pb(NO3)2(aq) + ____K2CrO4(aq) __ PbCrO4(s) + __KNO3(aq)
6. ____ S8(s) + ____O2(g) ____SO3(g)
7. ____ C3H5(NO3)3(s) __CO2(g) + ____N2(g) + __H2O(l) + ___O2(g)
8. ____ Fe(s) + ____CuCl2(aq) ____FeCl2(aq) + ____Cu(s)
9. ____ C3H8(g) + ____ O2(g) ____CO2(g) + ____H2O(g)
10. ____ CaSO4(aq) + ___AlBr3(aq) ___CaBr2(aq) + ___Al2(SO4)3(s)
Mole
Specific Heat Capacity
Phase Changes