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Nomenclature involving Polyatomic Ions
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Working Backwards
For each of the following compounds identify whether it is ionic or molecular. If the compound is
ionic, write the name and formula of the ions that make up the compound.
Compound
Ionic or
Cation Formula
Anion Formula
Molecular
and Name
and Name
2+
21
CaSO4(s)
ionic
Ca (calcium ion) SO4 (sulfate ion)
2
H2O(l)
3
Fe2O3(s)
4
Na3PO4(s)
5
MnO2(s)
6
NH3(g)
7
K2Te(s)
8
(NH4)2S2O3(s)
9
Al2(SO3)3(s)
10
Pb(CN)4(s)
11
SnCO3(s)
12
Hg3BO3(s)
13
CuHCO3(s)
14
NH4Br
15
Ga2Se3(s)
16
C3H8(g)
17
Fe(ClO3)2(s)
18
Sc(MnO4)3(s)
19
Rb2Cr2O7(s)
Describe three differences in the properties of ionic and molecular compounds.
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Acids and Bases
Name the following :
1.
HBr (g) ____________________
2.
HNO3 (aq) ____________________
3.
HI(aq)
____________________
4.
HCN(g) ____________________
5.
H3PO4(aq) __________________
6.
HOOCCOOH(aq)
7.
HIO3(aq) ___________________
8.
HNO2(aq) ___________________
9.
HClO3(aq)___________________
10. H2SO3(aq)____________________
11. KOH(aq) ____________________
12. Ba(OH)2(aq)___________________
13. Sr(OH)2 (aq)___________________
14. LiOH (aq) ____________________
_____________
Write the formula for each of the following:
1.
nitric acid ____________________
2.
hydrofluoric acid________________
3.
ammonia ____________________
4.
sodium hydroxide_______________
5.
hypochlorous acid__________________
6.
iron(II) hydroxide_______________
7.
sulfuric acid___________________
8.
hydrogen acetate________________
9.
hydrosulfuric acid_______________
10. calcium carbonate________________
List three (3) properties of acids.
List three (3) properties of bases.
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Mid Unit Review
Atomic Structure
Subatomic particles
1. Identify the three major subatomic particles and their charges.
2. Calculate the number of each particle for the following:
a. beryllium atom
b. bromine atom
c. sulfide ion
d. barium ion
e. tungsten atom
f. nitride ion
Theories
1. identify the theories and their authors represented by the following:
a. atom looks like this
b. atom looks like a planetary system
c. the electrons move around the nucleus in an unknown path.
d. key was the “Gold foil experiment”.
Ions
1. Why do ions form?
2. Draw the Bohr diagram for the atom and the ion for each of the following:
a. lithium
b. oxygen
c. carbon
d. chlorine
e. calcium
f. argon
Compounds
Binary Ionic
1. consist of a metal and a nonmetal (cation and an anion)
2. charges must balance in the final formula to form a neutral compound
3. List the characteristics of an ionic compound.
4. Write the formula for the following:
a. lithium chloride
b. magnesium fluoride
c. scandium sulfide
d. calcium nitride
e. aluminum phosphide
5. Name the following:
a. KBr(s)
b. BaI2(s)
c. Ga2S3(s)
d. MgO(s)
e. GeSe2(s)
Multivalent Metals
1. metals that can form more than one value of ionic charge
2. named using the Stock system or the Classical system
a. describe each naming system
3. Write the formula for the following:
a. copper (I) oxide
b. nickel (III) sulfide
c. manganese (IV) oxide
d. yttrium (III) chloride
e. titanium (III) nitride
4. Name the following:
a. FeO(s)
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b. CoF2(s)
c. V3N5(s)
d. Cr3P2(s)
e. MgS(s)
Polyatomic Ions
1. groups of atoms that remain together in a chemical reaction and contain a charge
2. names usually end in ‘ate’ or ‘ite’
3. Write the formula for the following:
a. sodium nitrate
b. iron (II) hydroxide
c. barium sulfate
d. cuprous chlorate
e. ammonium silicate
4. Name the following:
a. KClO3(s)
b. Ca(OH)2(s)
c. Fe2(CrO4)3(s)
d. Mn5(P3O10)2 (s)
e. NaC6H5COO (s)
Molecular Compounds
1. Composed of only nonmetals.
2. Use the prefixes to indicate the number of atoms present in the molecule.
3. Name the following:
a) N2O (g)
b) P2O6 (g)
c) PCl5 (s)
4. Write the formula for each of the following:
a) carbon monoxide
b) sulfur dibromide
c) triphosphorus heptaoxide
5. Write the formula and name the common molecular compounds given in
class.
Acids and Bases
1. List the characteristics of an acid.
2. List the characteristics of a base.
3. Write the formula for the following:
a) hydrochloric acid
b) phosphoric acid
c) carbonous acid
d) hydrofluoric acid
e) nitric acid
4. Write the name for each of the following:
a) H3N (aq)
b) HClO4 (aq)
c) HNO2 (aq)
d) H2Se (aq)
e) C6H5COOH (aq)
GOOD LUCK ON THE EXAM
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Calculating Molar Mass
In each of the following determine the molar mass of the compound given. Your answer should
be to two decimal points.
1.
FeSO4 (s) {151.91 g}
2.
magnesium sulfate
3.
MgSiO3 (s)
4.
sodium hypochlorite
5.
Al(OH)3 (s) {78.01 g}
6.
sodium chloride
7.
calcium carbonate
8.
dinitrogen monoxide
9.
NH4H2PO4 (s) {115.04 g}
10.
Ca(HCO3)2 (s) {162.12 g}
11.
ammonium acetate
12.
lead (II) nitrate
13.
mercury (II) permanganate
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{120.37 g}
{100.40 g}
{74.44 g}
{58.44 g}
{100.09 g}
{44.02 g}
{77.10 g}
{331.21 g}
{438.47 g}
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Calculating Mass to Moles
In each of the following determine the number of moles for the quantity of the compound given. Your answer
should be to the correct number of significant digits.
Remember to determine the amount of one mole of the compound and then use the formula
n= m
to determine the number of moles
M
1.
120 g of sodium phosphate {163.94 g/mole, 0.732 moles}
2.
5.00 g of NaHCO3 (s) {84.01 g/mole, 0.0595 moles}
3.
85.0 g of calcium carbonate {100.09 g/mole, 0.849 moles}
4.
1600 g of carbon dioxide {44.01 g/mole, 36.36 moles}
5.
3.00 kg of water {18.02 g/mole, 166 moles}
6.
78.6 g of methane gas {16.05 g/mole, 4.90 moles}
7.
123 g of sulfuric acid {98.08 g/mole, 1.25 moles}
8.
964 g of ferrous chromate {171.85 g/mole, 5.61 moles}
9.
456 g of mercury (I) borate {660.58 g/mole, 0.690 moles}
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Introduction to Balancing Chemical Reactions
For each of the following count the number of moles of atoms of each element on each side of
the yield( -->) sign, if they balance fine, if not, put in the correct numbers of moles required.
Example : Rocket fuel is burned in a Saturn rocket.
2H2(g) + O2 (g) ---> 2H2O(g)
#H = 4 , #O = 2
-->
1. CH4 (g) +
2O2(g)
#C = , #H =
,#O =
2. H2(g)
Cl2(g)
+
---> CO2(g)
,#O =
2HCl(g)
--->
+ 3H2(g)
+ 2H2O(g)
---> #C = , #H =
--->
#H = , #Cl =
3. N2(g)
#H = 4 , #O = 2
#H = , #Cl =
---> 2NH3(g)
#N = , #H =
--->
#N = , #H =
Try to balance these.
4. ___H2O2(l)
--->
#O = , #H =
---> #O = , #H =
5. ___NO (g)
+
#O = , #N =
6. ___Zn (s)
#Zn = , #S =
___H2O(g)
___O2 (g)
+
___O2(g)
---> ___NO2 (g)
---> #O = , #N =
+ ___S8 (s) ---> ___ZnS
(s)
---> #Zn = , #S =
Formation & Decomposition Reactions
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Balance the following formation reactions by filling in the blanks.
1.
____ C (s) + ____ O2(g) ----> _____ CO2(g)
2.
____ Ba (s) + ____ N2 (g) ----> _____ Ba3N2 (s)
3.
____ Ga (s) + ____ As (s) ----> ____ GaAs (s)
4.
____ K (s) + ____ S8 (s) ----> ____ K2S (s)
5.
____ Na (s) + ____ Cl 2(g) ----> ____ NaCl (s)
Balance the following decomposition reactions by filling in the blanks.
1.
_____H2O (l) ----> ____H2 (g) + ____ O2 (g)
2.
_____ Li3N (s) ----> ____ Li (s) + ____ N2 (g)
3.
_____ CO2 (g) ----> ____ C (s) + ____ O2 (g)
4.
_____ HCl (aq) ----> ____ H2 (g) + ____ Cl2 (g)
5.
_____ TiI4 (s) ----> _____ Ti (s) + ____ I2 (g)
Write and balance the following equations.
1.
Aluminum metal plus chlorine gas produces aluminum chloride
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2.
Magnesium metal plus oxygen gas produces magnesium oxide
3.
Sulfur plus oxygen gas produces sulfur dioxide
4.
Copper metal reacts with sulfur to form copper (II) sulfide
5.
Nitrogen gas reacts with hydrogen gas to form ammonia
6.
Methane gas decomposes to its elements
7.
Iron (II) bromide decomposes to its elements.
8.
Mercury (I) sulfide decomposes to its elements.
9.
Tetraphosphorous decaoxide decomposes to its elements.
Fill in the blanks and balance the following formation and decomposition
reactions. The word equation is on top and the chemical equation is underneath it.
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1.
nickel metal
___
2.
+ _________
_____
+ ____
sodium oxide
nitric acid
---->____ Ni2S3 (s)
----> sodium
____ ________
3.
S8 (s)
----> ___________________
+ ______
---->____ _____
----> hydrogen
chromium metal
+
____ ________
5.
6.
8.
+ ___
O2 (g)
phosphorous ----> chromium (III) phosphide
_______
----> _________
____
----> ___
____________________ ----->
Pb3N4 (s)
+ __________
N2 (g)
manganese (IV) chloride
___
7.
+ ___
+ ____
_____________
O2(g)
+ _________
____ _________ ---->___ H2 (g)
4.
+ ___
----> ___
----> ____ ____________
+ ___________
Mn (s)
+ ____
lead metal
________
Cl 2(g)
+ ________
+ ___
N2 (g)
lead metal
+ ____________________ ----> plumbous selenide
___ ________
+
gold
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+
sulfur
____ Se (s)
---->
----> ____ ___________
____________
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____ ______ + ____ _____ ----> ____
9.
silver chloride ----> silver metal
____ ________ ---->____
10.
11.
_____
Au2S (s)
+ chlorine gas
+ ____
______
carbon +
chlorine gas ----> ____________________
____ ____
+ ____
__________
_______ ---->____ CCl4 (l)
----> iron metal + nitrogen gas + oxygen gas
____Fe(NO3)3 (s) ---->____ ____ + ____ _______ + ____ ________
12.
silver metal + iodine solid -----> ________________
____ ________ +____ _______ ----> _____ AgI (s)
13.
__________ +
sulfur
---->
_____________
____Cu (s) +____ ______ -----> _____ Cu2S (s)
14.
xenon hexafluoride ----> ________ + _________
____ ________
-----> ___ ______ + ____ _____
Single Replacement Reactions
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Balance the following equations by writing in the SIMPLEST WHOLE NUMBER coefficients in
the space provided. Give the word equation for each (names of elements and compounds
involved).
1. _____ K(s) + _____ HNO3(aq) -------> _____ H2(g) + _____ KNO3(aq)
word equation:
2.
_____ Na(s) + _____ HOH(l) -----> _____ H2(g) + _____ NaOH(aq)
word equation:
_____ Al(s) + _____ Fe2O3(s) -----> _____ Fe(s) + _____ Al2O3(s)
word equation:
3.
4. _____ K(s) + _____ AlCl3(s) -----> _____ Al(s) + _____ KCl(s)
word equation:
5. _____ Cl2(g) + _____ MgBr2(aq) -----> _____ Br2(l) + _____ MgCl2(aq)
word equation:
6. _____ H2S(g) + _____ Ag(s) ----> _____ Ag2S(s) + _____ H2(g)
word equation:
7. _____ Ca(s) + _____ Ag2SO4(aq) ----> _____ CaSO4(s)
word equation:
+
_____ Ag(s)
8. _____ Al(s) + _____ Pb(NO3)2(aq) ----> _____ Al(NO3)3(aq) + _____ Pb(s)
word equation:
9. _____ Zn(s) + _____ Cu(NO3)2(aq) ----> _____ Zn(NO3)2(aq) + _____ Cu(s)
word equation:
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10. _____ Cl2(g) + _____ NaI(aq) ----> _____ NaCl(aq) + _____ I2(s)
word equation:
11. _____ Cu(s) + _____ HNO3(aq) ----> _____ Cu(NO3)2(aq) + _____ H2(g)
word equation:
12. _____ K(s) + _____ H3PO4(aq) ----> _____ H2(g) + _____ K3PO4(aq)
word equation:
13. _____ Mg(s) + _____ Zn3(PO4)2(aq) ---->_____ Zn(s) + _____ Mg3(PO4)2(aq)
word equation:
14. _____ Cr2(SO4)3(aq) + _____ Pt(s) ----> _____ Cr(s) + _____ Pt(SO4)2(aq)
word equation:
15. _____ __________
word equation:
gallium nitrate
+ _____ _________
+
mercury
----> _____ HgNO3(aq) + _____ Ga(s)
---> ______________
+ ___________
16. _____ __________ + _____ ________---->_____ (NH4) 2S(aq)+_____ P4(s)
word equation:
ammonium phosphide solution +
sulphur ----> ____________
+
____________
17. _____ Sc(MnO4)3(aq) + _____ ________-----> _____ _______________+_____ Sc(s)
word equation:
___________ +
nickel
---->nickel (II) permanganate + ________
Balancing Double Replacement Reactions
For the following reactions include the formulas, balancing, and phases for all reactions.
Balancing using the simplest whole number coefficients.
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1. _____ CuCl2(aq) + _____ K2S(aq) ---> _____ KCl(aq) +
word equation:
_____ CuS(s)
2. _____ MnCl4(aq) + _____ NiBr3(aq) ---> _____ MnBr4(aq) + _____ NiCl3(aq)
word equation:
3. _____ Au2S3(aq) +
word equation:
4. _____ InI3(aq)
word equation:
+
_____ MgF2(aq) ---> _____ AuF3(aq) +
_____ FeO(aq) ---> _____ FeI2(aq) +
5. _____ PuN2(aq) +
word equation:
_____ MgS(s)
_____ In2O3(aq)
_____ VAt5(aq) ---> _____ PuAt6(aq) +
_____ V3N5(aq)
6. _____ _____________+ _____ ______________---> _____ ________+ _____ ______
Word equation:
magnesium phosphide (aq) + cobalt (II) sulfide solution ---> magnesium sulfide solid + cobalt
(II) phosphide solution
7. _____ ____________+ _____
_____
_______________---> _____ __________+ _____
Word equation:
copper (II) bromide (aq) + gold (III) arsenide solution ---> copper (II)arsenide solution + gold
(III) bromide (aq)
8. _____ NH4Br(aq) + _____ Hg3N(aq) ---> _____ (NH4)3N(aq) + _____ HgBr(s)
Word equation:
9. _____ HgS(aq) + _____ NH4OH(aq) ---> _____ Hg(OH)2(s) +
Word equation:
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_____ (NH4)2S(aq)
workbook
10. __ Zn(CH3COO)2(aq) + __ NH4OH(aq) ---> __Zn(OH)2(s) + __ NH4CH3COO(aq)
Word equation:
11. __ Co(IO3)3(aq) +
Word equation:
__ Na2SO4(aq) ---> __ Co2(SO4)3(aq) +
__ NaIO3(aq)
12. __ _______________+ __ ___________---> __ ________+ __ _________
Word equation:
solution of lead (IV) nitrate + solution of gold (III) chloride---> aqueous gold (III) nitrate +
aqueous lead (IV) chloride
13. __ _______+ __ ________---> __ ________+ ___ _________
Word equation:
hydrochloric acid poured into aqueous lead (IV) nitrate to produce aqueous lead (IV) chloride
and nitric acid
14. __ ________+ __ _________---> ___ ________+ ___ _________
Word equation:
magnesium hydrogen phosphate solution reacts with aqueous sodium iodide to yield
magnesium iodide solution and aqueous sodium hydrogen phosphate
15. __ __________+ __ _________---> __ __________+ __ ____________
Word equation:
aqueous zinc sulphate is mixed with a solution of ammonium phosphate to produce ammonium
sulfate solution and zinc phosphate precipitate
16. __ __________+ __ _________---> __ _________+ ___ ___________
Word equation:
solid sodium carbonate is stirred into a solution of iron (III) nitrate to yield sodium nitrate solution
and iron (III) carbonate precipitate
17. __ __________+ __ __________---> __ ___________+ ___ ___________
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Word equation:
aluminum sulphate solution is poured into a barium hydroxide solution to yield two solids: barium
sulphate and aluminum hydroxide
18. __ _____________+ __ ____________---> __ __________+ __ ____________
Word equation:
solution of ammonium borate reacts with solid palladium (IV) dihydrogen phosphate to produce
ammonium dihydrogen phosphate solution and palladium (IV) borate
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Hydrocarbon Combustion
Hydrocarbons are compounds that contain carbon, hydrogen and sometimes oxygen. When
they combust (burn) they are reacting with oxygen and they always produce carbon dioxide gas
and water vapour. Balanace in the order of carbons, hydrogens and finally oxygens (CHO).
ex.
methane is combusted.
___CH4 (g) + ___O2 (g) ---> ___CO2 (g) + ___H2O (g)
1.
Propane reacts with oxygen in a barbeque.
2.
Butane is combusted in a disposable lighter.
3.
Pentane (C5H12) is burned.
4.
C6H10 (hexyne) + O2 (g) --->
5.
Methanol is burned as part of automobile fuel ( gasoline antifreeze )
6.
Ethanol is part of Mohawk gasoline and is combusted in your automobile engine.
7.
C3H7OH (g) (propanol) + O2 (g) --->
8.
C4H9OH (g) (butanol) + O2 (g) --->
9.
Benzene (C6H6) reacts with oxygen.
10.
Glucose is metabolized (burned) in the body. Note: The water that is produced will
usually
be liquid in the body.
11.
Sucrose is combusted. Note: The water that is produced will usually
be liquid in the body.
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Balancing Equations : All Types
Balance the following equations and indicate the type of reaction.
1. __Ca(OH)2 (aq) + __H3PO4 (aq) --> __HOH(l) + __Ca3(PO4)2 (s)
Reaction type _____
2. ___Al(OH)3 (s) + __HCl (aq) --> __AlCl3 (aq) + __HOH(l)
Reaction type _____
3. ___AgNO3 (aq) + __H2SO4 (aq) --> __Ag2SO4 (s) + __HNO3 (aq)
Reaction type _____
4. ___Cr (s) + __S8 (s) --> __Cr2S3(s)
Reaction type _____
5. ___KClO3 (s) --> __KCl(s) +___O2(g)
Reaction type _____
6. ___Zn(s) + __HCl(aq) --> __ZnCl2(aq) + __H2 (g)
Reaction type _____
7. ___Au2S3 (aq) + __H2(g) --> __Au(s) + __H2S(aq)
Reaction type _____
8. ___Ca(s) + __HOH(l) --> __Ca(OH)2 (aq) + __H2 (g)
Reaction type _____
9. ___Pb(NO3)2(aq) + __H3AsO4(aq) --> __PbHAsO4 (s) +__HNO3(aq)
Reaction type _____
10. ___NaCl (aq) + __HOH (l) --> __Cl2(g) + __H2(g) + __NaOH(aq)
Reaction type _____
11. ___Fe2O3 (s) + ___Al(s) --> ___Fe (s) + ___Al2O3 (s)
Reaction type _____
12. ___NO2 (g) + ____HOH(l) --> ____HNO3(aq) + ____NO(g)
Reaction type _____
13. ___Ca3(PO4)2 (s) +____ H2SO4 (aq) --> ___CaSO4 (s) +__ H3PO4 (aq)
Reaction type _____
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More Practice on Balancing Equations
Balance the following equations by filling the simplest whole number coefficient in the space
provided. Identify the reaction type as formation (f), decomposition (d), single replacement (sr),
double replacement (dr), hydrocarbon combustion (hc) or other (o).
Reaction Equation
Reaction Type
1.
___ Al (s) + ___ O2 (g) ---> ___ Al2O3 (s)
____
2.
___HCl (aq) + ___ Ca(OH)2 (aq) ---> ___ HOH(l) + ___CaCl2 (aq)
____
3.
___CH4 (g) + ___O2 (g) ---> ___ CO2 (g) + ___H2O(l)
____
4.
___Zn(s) + ___Pb(CH3COO)2 (aq) ---> ___Pb(s) + ___Zn(CH3COO)2 (aq)
____
5.
___SO3 (g) + ___H2O(l) ---> ___H2SO4 (aq)
____
6.
___HgO(s) ---> ___Hg(s) + ___O2 (g)
____
7.
___CaCO3 (s) ---> ___ CaO(s) + ___CO2 (g)
____
8.
___NaI (aq) + ___Pb(NO3)2 (aq) ---> ___PbI2 (s) + ___ NaNO3 (aq)
____
9.
___Cl2 (g) + ___NaI (aq) ---> ___I2 (aq) + ___ NaCl (aq)
____
10.
___Al2(SO4)3 (aq) + ___Ca(OH)2 (aq) ---> ___Al(OH)3 (s) +___CaSO4 (s)
____
11.
__Al2(SO4)3 + ___Ca(HCO3)2 (aq) ---> __Al(OH)3 (s) + __CaSO4 (s) +__CO2 (g)
____
Predict the Products of the following reactions and balance the equations.
12.
___C8H18 (l) + ___ O2 (g) --->
13.
H2O
14.
___Na(s) + ___ Cl2 (g) --->
15.
___Ca (s) + ___HOH(l) --->
16.
___H2SO4 (aq) + ___Al(OH)3 (s) --->
17.
___Cl2 (aq) + ___KBr (aq) --->
18.
___Na2CO3 (aq) + ___ Ca(OH)2 (aq) --->
(l)
--->
Still More Practice
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Write the balanced equation, including phase symbols, and identify the reaction type for each of
the following.
1.
Hydrosulfuric acid reacts with the iron in pipes to produce iron (II) sulfide and hydrogen
gas.
Equation:
Type:
2.
Iron reacts with the water and oxygen in the air to produce rust (iron (III) hydroxide)
Equation:
Type:
3.
Coal (C9H6) is combusted in a stove.
Equation:
Type:
4.
Iron is added to sulfuric acid to release hydrogen gas and iron (II) sulfate.
Equation:
Type:
5.
Hydrogen is burned as a fuel in experimental vehicles.
Equation:
Type:
6.
Sodium benzoate solution reacts with magnesium sulfate solution to produce sodium
sulfate and magnesium benzoate
Equation:
Type:
7.
Mercury (II) sulfide (cinnabar) is decomposed.
Equation:
Type:
8.
Every year people around the house fall victim to dangerous fumes produced when
products such as Sani-Flush (NaHSO4) and chlorine bleach solution (NaClO) are mixed.
These two react in salt water (NaCl (aq))to produce chlorine gas, sodium sulfate and water.
Equation Type:
9.
Rock salt (sodium chloride) is reacted with sulfuric acid to produce sodium sulfate and
hydrochloric acid.
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Equation:
Type:
10. The sodium sulfate above is reacted with charcoal (carbon) and limestone (calcium
carbonate) to produce sodium carbonate(soda ash), calcium sulfide and carbon dioxide.
Equation:
Type:
11. The soda ash from above is then dissolved and reacted with slaked lime (calcium
hydroxide) to produce caustic soda (sodium hydroxide) and calcium carbonate.
Equation:
Type:
12. Potassium was discovered in 1807 by electrically decomposing potash (potassium
chloride)
Equation:
Type:
13. Boric acid is used in laboratory eye washes to neutralize a sodium hydroxide solution that
was accidentally splashed into an eye.
Equation:
Type:
14. A deadly gas (hydrogen cyanide) is produced when hydrochloric acid is added to a
potassium cyanide solution.
Equation:
Type:
15. Lead was produced by the ancient Romans in two steps.
a) Lead (II) sulfide is found in silver ore. The lead (II) sulfide is heated in air (oxygen) to
produce lead (II) oxide and sulfur dioxide gas.
Equation:
Type:
b) The lead(II) oxide is then heated with charcoal (carbon) to produce lead and carbon
dioxide.
Equation:
Type:
Chemistry Final Review
Fill in the following blanks to BEST complete the statement.
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a) A __________________ is considered to be consistent throughout. This type of matter can
be of two types ______________ or ________________ of which there are 109 of these on a
______________ table.
b) A mixture can be of two types ____________________ or ____________________.
c) Ice tea in a pitcher is known as a ____________________ because it is dissolved in water.
The ice tea mix is known as the ____________________ the water is called the
____________________ and any mixture dissolved in water is given a symbol of
___________.
d) ____________________ are a combination of two or more elements. The rearrangement of
electrons determines whether they are ionic or molecular. When elements lose electrons they
become ____________________ charged and are called ___________ ; these elements are
____________ which are found on the ________ side of the periodic table. Elements that gain
electrons become __________________charged and are called ______________; these
elements are ____________________which are found on the ________________ side of the
periodic table. The name given to the formula where these two elements combined is called an
____________________ formula.
e) When 2 non-metallic elements ____________________ electrons, the result is a
____________________ compound. The naming of this type of compound uses a
__________________ which determines the number of elements in this compound and a
_____________ which is usually “ide”.
f) The ____________________ refers to the number of this positively charged particle. It is
called a ________ and is found in the____________________ of an atom. The
____________________mass of any element is a combination of ____________________ and
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____________________ only because ____________________ are considered to have no
mass.
g) ____________________ are vertical columns and ____________________ are horizontal
rows on the periodic table.
h) Group number ____________________ the ____________________family consists of the
most reactive metal in existence. That metal is ____________________.
i) Group number ____________________ the ____________________ family is known as the
“____________________” because it combines with group IA and IIA metals to form crystals
called ‘salts’.
k) ____________________ are solid at room temperature with the exception of mercury. Other
properties include ____________________, ____________________, and
___________________
l) Some non-metals exist in pairs. These elements are known as ____________________
molecules and are oxygen, nitrogen and ____________________. Two elements are poly
atomic. They are ____________________ which has a symbol of ____________________ and
____________________ having a symbol of ____________________.
m) ____________________ was responsible for the Orbits model of the Atom. Rutherford was
responsible for ____________________model, Thompson developed the
____________________ model and the currently accepted model is____________________. It
has electrons moving in an unpredictable path around the nucleus.
n) In ____________________ reactions ____________________ is needed in order to burn a
hydrocarbon. When balancing these reactions, balance ____________________ first
____________________second and ____________________ last.
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o) Isotopes occur when ____________________ are lost or gained. The result is a change in
the atomic ____________________ of the substance.
p) ____________________ is a name given to a metal that can have more than one charge.
The charges of the metal are represented by ____________________. This is called the
_______________naming system.
q) In forming an ionic compound it is essential that charges ____________________ to form a
____________________ compound (having no charge).
r) In order for a compound to be an acid the substance must contain a
____________________ion and be ____________________in ____________________
s) Bases usually contain the ____________________ ion.
t) A reaction that releases energy is known as a(n) ____________________ reaction. You
usually can feel the temperature rise because heat is being released. The opposite is a(n)
____________________ reaction. It absorbs ____________________ and the temperature
feels cool.
u) A mole represents ____________________particles and this number is credited to the
Scientist ____________________.
Fill in the following chart.
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List the differences between the following:
1. metals and nonmetals.(4)
2. Atoms and Ions. (3)
3. molecular and ionic bonds.(3)
4. acids and bases.(2)
Balance the following reactions. Include the phases and the type of reaction.
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1. A solution of iron (II) sulphate is combined with solid ammonium hydroxide to produce a
solution of ammonium sulphate and a iron (II) hydroxide precipitate.
2. Carbonic acid is poured on a sheet of aluminum foil. The resulting reaction begins to
release a hydrogen gas and a precipitate of aluminum carbonate.
3. Octane combusts.
4. Titanium (IV) permanganate decomposes into its elements.
5. Phosphorus and vanadium combine in a synthesis reaction.
Complete the following chart.
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Good Luck on the Final!
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