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Simple Ions: complete the following table
Ion Name
1
chloride
2
fluoride
Number of
Protons
Number of
Electrons
Cl-
17
18
1 gained
9
10
Ca2 +
3
4
Ion Symbol
Number of
Electrons
gained or
lost
lost 1
5
16
none
21
36
53
nitride
12
56
13
15
54
gains 3
Al3 +
14
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xenon
K+
10
15
18
selenide
9
11
18
H+
7
8
Argon
20
rubidium
6
Electron
Structure same
as which Noble
gas
oxide
10
page 1
Ionic Compounds- complete the following table
Ionic Charges
e.g. Ba2 + , Cl1.
Chemical
Formula
BaCl2 (s)
Name of
Compound
barium chloride
CaCl2(s)
2.
magnesium chloride
3.
potassium fluoride
4.
NaCl (s)
5.
CdS (s)
lithium nitride
6.
7.
GeBr4 (s)
8.
K3N(s)
9.
strontium phosphide
10.
magnesium arsenide
11.
12.
In2O3
(s)
Ba3As2 (s)
13.
scandium oxide
14.
calcium oxide
15.
Al2O3(s)
16.
ZnO (s)
17.
silver sulfide
18
beryllium hydride
19.
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Ga2Se3
(s)
page 2
Multivalent Ionic Compounds- complete the following table
Ionic Charges
e.g. Cr2 + , Cl1.
Chemical
Formula
CrCl2(s)
Name of
Compound
chromium (II) chloride
CuCl2(s)
2.
manganese (IV) chloride
3.
titanium (III) fluoride
4.
SnO2(s)
5.
FeS(s)
6.
copper (I) nitride
7.
MoBr6(s)
8.
PbO2(s)
9.
vanadium (IV) phosphide
platinum (II) arsenide
10.
11.
Hg2O(s)
12.
Ni3As2(s)
13.
stannic oxide
14.
mercurous oxide
15.
Fe2O3(s)
16.
Cu3P2(s)
17.
gold (III) sulfide
18.
tin (II) chloride
19.
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Co2Se3(s)
page 3
Nomenclature involving Polyatomic Ions
Chemical Formula
1
2
3
Name of Compound
K2CO3(s)
(NH4)2S(s)
calcium hydroxide
magnesium silicate
4
5
Cr(NO3)3 (s)
iron (II) chlorate
6
7
8
Sr(NO3)2 (s)
NaNO2 (s)
9
ammonium sulfate
sodium bicarbonate
10
11
12
K3PO4 (s)
(NH4)3PO4 (s)
calcium sulphite
13
14
KMnO4 (s)
15
sodium thiosulfate
16
barium chlorate
17
sodium hydrogen sulfide
18
Ca(HS)2 (s)
potassium cyanide
19
20
NH4H2PO4(s)
sodium thiocynate
21
22
platinum (IV) sulfate
zinc iodate
23
mercurous nitrate
24
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page 4
Naming Molecular Compounds
Molecular Formula
1
CCl4(l)
2
CO2(g)
3
NO2(g)
4
NO(g)
5
SO3(g)
6
P4O10
Name
argon
7
8
CH4(g)
sucrose
9
10
H2O(l)
11
HCl(g)
12
sulfur
13
methanol
14
hydrogen peroxide
15
ammonia
16
ethanol
17
ozone
diphosphorus decaoxide
18
trinitrogen heptachloride
19
20
chlorine
21
phosphorus
22
dinitrogen tetrabromide
23
nitrogen
tetraphosphorus hexachloride
24
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page 5
Name the following :
Acids and Bases
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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page 6
Science 10 Chemistry
Write the following formulas.
51. Sodium dichromate
52. Iron metal
53. Hydrogen nitrate
54. Nitrogen gas
55. Magnesium bisulphate
56. Cobalt (II) chlorate
57. Mercury(II) chloride
58. Silicon dioxide
59. Sodium chlorate
60. Hydrogen sulfate
61. Fluorine gas
62. Sodium hydrogen phosphate
63. Aluminum sulfide
64. Chromic oxalate
65. Rubidium nitrite
66. Hydrogen iodide
67. Ammonium hydrogen sulfite
68. Beryllium borate
69. Barium phosphate
70. Xenon gas
71. Carbon tetrachloride
72. Calcium acetate
73. Lithium hydrogen carbonate
74. Water
75. Copper(I) thiocyanate
76. Mercury(I) acetate
77. Silver thiocyanate
78. Sodium oxide
79. Iron(III) carbonate
80. Magnesium hydride
81. Potassium oxalate
82. Gold(III) nitrate
83. Lithium dihydrogen phosphate
84. Iron(III) oxalate
85. Iron(II) hydroxide
86. Helium gas
87. Ammonia
88. Cadmium acetate
89. Nickel metal
90. Selenium tetrafluoride
91. Hydrogen carbonate
92. Boron trihydride
93. Manganese(II) iodate
94. Strontium sulfite
95. Neon gas
96. Iron(III) cyanide
97. Lithium hydride
98. Ammonium carbonate
99. Xenon hexafluoride
1. Silver chloride
2. Cupric iodide
3. Zinc sulphate
4. Ammonia
5. Strontium fluoride
6. Potassium cyanide
7. Aluminum nitrate
8. Mercury(I) sulphide
9. Sulphur
10. Potassium chromate
11. Potassium nitrite
12. Silver hydroxide
13. Lead (II) nitrate
14. Iron(III) hydroxide
15. Oxygen gas
16. Sulphur trioxide
17. Sodium iodate
18. Aluminum nitrite
19. Sodium hydride
20. Tin(II) bicarbonate
21. Iron (III) sulphate
22. Sodium thiocyanate
23. Cesium borate
24. Mercury
25. Zinc fluoride
26. Barium hydrogen carbonate
27. Tin(IV) sulphate
28. Strontium borate
29. Hydrogen peroxide
30. Nitrogen dioxide
31. Aluminum hydrogen sulfite
32. methane
33. Potassium chlorate
34. Zinc phosphate
35. Lead(IV) iodate
36. Ammonium chlorate
37. Chromium(II) oxide
38. Mercury(I) cyanide
39. Calcium nitrate
40. Bromine liquid
41. Tin(IV) permangante
42. Aluminum oxide
43. Calcium sulphide
44. Iron(III) iodide
45. Magnesium hydroxide
46. Sodium iodate
47. Calcium silicate
48. Glucose
49. Magnesium cyanide
50. Sodium metal
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page 7
Write the name for each of the following.
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
AgI(s)
CCl4(l)
CuSO4(s)
MgO(s)
NaCN(s)
PCl5(s)
Fe(NO3)2(s)
(NH4)2SO4(s)
SO2(s)
Cu2SO4(s)
Fe(NO3)3(s)
NaBr(s)
K2OOCCOO(s)
RbSCN(s)
AlPO4(s)
K2CO3(s)
Na3PO4(s)
SnSO4(s)
Na2CrO4(s)
Pb(NO3)2(s)
Sn(SO4)2(s)
WF6(s)
SO3(g)
K2Cr2O7(s)
Pb(CO3)2(s)
Na2HPO4(s)
Al2(CO3)3(s)
Au(CN)3(s)
KMnO4(s)
SrH2(s)
KHCO3(s)
Al2S3(s)
Cu(CH3COO)2(s)
Ba(SCN)2(s)
NaClO3(s)
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36.
37.
38.
39.
40.
41.
42.
43
44.
45.
46.
47.
48.
49.
50.
51.
52.
53.
54.
55.
56.
57.
58.
59.
60.
61.
62.
63.
64.
65.
66.
67.
68.
69.
70.
Fe(OH)2(s)
Na3BO3(s)
C8H18(l)
V2S5(s)
Fe(OH)2(s)
SnF2(s)
CH3OH(l)
Zn(NO2)2(s)
Ag2CrO4(s)
KCH3COO(s)
NH4OH(s)
O3(g)
Cu2S(s)
HgCr2O7(s)
RbI(s)
NH4IO3(s)
MoCl6(s)
NaHS(s)
CsH2PO4(s)
NaOH(s)
Ni(SCN)2(s)
Pb(HSO4)4(s)
Hg(NO3)2(s)
Na2O(s)
RbH(s)
C6H12O6(s)
NI3
MnS2(s)
Li2CrO4(s)
Li2O(s)
Na2SO3(s)
Zn(CH3COO)2(s)
H2S(g)
C4H10(s)
CsHCO3(s)
page 8
71.
72.
73.
74.
75.
76.
77.
78.
79.
80.
81.
82.
83.
84.
85.
86.
87.
88.
89.
90.
91.
92.
93.
94.
95.
96.
97.
98.
Ca(ClO4)2(s)
NH4ClO(s)
CrO(s)
CsCN(s)
H2(g)
S8(s)
MnO(s)
Ca(OH)2(s)
CoCl2(s)
Zn(IO3)2(s)
PtCl4(s)
Hg(NO2)2(s)
HCl(g)
Cr2O3(s)
Al(OH)3(s)
(NH4)3BO3(s)
NaCl(s)
KrF4(g)
BaCr2O7(s)
Sr3(PO4)2(s)
Fe2O3(s)
(NH4)2HPO4(s)
NaCH3COO(s)
Fe(CH3COO)2(s)
PbCO3(s)
BeSiO3(s)
XeO2(g)
Hg(NO3)(s)
A.
B. Classification of Matter
Types of Matter
1. Identify and define the types of pure substances.
2. Identify and define the two main types of mixtures.
Chemical vs Physical Properties
1. Identify the difference between a chemical and a physical change.
Periodic Table
Patterns
1. Identify the four basic patterns found on the periodic table.
a. Classify silicon,rubidium and krypton according to these
patterns.
2. Which group numbers are alkali metals, noble gases and halogens?
3. Why is silicon called a metalloid?
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
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page 9
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)
b. CoF2(s)
c. V3N5(s)
d. Cr3P2(s)
e. MgS(s)
Complex 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)
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page 10
5. Use the variations of complex ions.
a. NO3- = nitrate, NO2- = nitrite , NO- = hyponitrite ,
NO4- = pernitrate
b. Name the following:
i) NaNO2 (s)
ii) KClO4 (s)
iii) Ca(IO)2 (s)
c. Write the formula for the following:
i) barium phosphite
ii) chromium (II) percarbonate
iii) iron (III) hypobromite
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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page 11
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)
#H = 4 , #O = 2
---> CO2(g)
+ 2H2O(g)
#C = , #H = ,#O =
---> #C = , #H = ,#O =
2. H2(g)
--->
+
Cl2(g)
2HCl(g)
#H = , #Cl =
---> #H = , #Cl =
3. N2(g)
---> 2NH3(g)
+ 3H2(g)
#N = , #H =
--->
#N = , #H =
Try to balance these.
4. ___H2O2(l) --->
#O = , #H =
5. ___NO (g)
#O = , #N =
___H2O(g)
+
___O2(g)
---> #O = , #H =
+
___O2 (g)
---> ___NO2 (g)
---> #O = , #N =
6. ___Zn (s)
+ ___S8 (s) ---> ___ZnS (s)
#Zn = , #S =
---> #Zn = , #S =
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page 12
Formation & Decomposition Reactions
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)
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page 13
Write and balance the following equations.
1.
Aluminum metal plus chlorine gas produces aluminum chloride
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.
10.
Sucrose decomposes to its elements.
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page 14
Fill in the blanks and balance the following formatiom and decomposition reactions. The
word equation is on top and the chemical equation is underneath it.
1.
nickel metal
___
2.
+ _________
_____
+ ____
sodium oxide
nitric acid
S8 (s)
---->____ Ni2S3 (s)
----> sodium
____ ________
3.
----> ___________________
+ ______
---->____ _____
----> hydrogen
chromium metal
6.
N2 (g)
+ ___
O2 (g)
+ ____
_______
----> ____ ____________
manganese (IV) chloride
----> _________
+ ___________
____
----> ___
+ ____
_____________
____________________ ----->
___
7.
+ ___
+ __________
+ white phosphorous ----> chromium (III) phosphide
____ ________
5.
O2(g)
+ _________
____ _________ ---->___ H2 (g)
4.
+ ___
Pb3N4 (s)
----> ___
Mn (s)
lead metal
Cl 2(g)
+ ________
________
+ ___
N2 (g)
lead metal
+ ____________________ ----> plumbous selenide
___ ________
+
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____ Se (s)
----> ____ ___________
page 15
8.
gold
+
sulfur
---->
____________
____ ______ + ____ _____ ----> ____
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 ----> ________ + _________
____ ________
15.
-----> ___ ______ + ____ _____
methane gas ----> _______________ + ______________
____CH4(g)
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----> ____C(s) + ____ H2 (g)
page 16
Single Replacement Reactions
Balance the following equations by writting 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:
3. _____ Al(s) + _____ Fe2O3(s) -----> _____ Fe(s) + _____ Al2O3(s)
word equation:
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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page 17
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
+ _____ _________ ----> _____ HgNO3(aq) + _____ Ga(s)
+
mercury
---> ______________
+ ___________
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 + ________
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page 18
Balancing Double Replacement Reactions
For the following reactions include the formulas, balancing, and phases for all reactions. Balancing using the
simplest whole number coefficients.
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) +
_____ MgS(s)
_____ In2O3(aq)
5. _____ PuN2(aq) + _____ VAt5(aq) ---> _____ PuAt6(aq) +
word equation:
_____ 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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page 19
_____ (NH4)2S(aq)
10. __ Zn(CH3COO)2(aq) + __ NH4OH(aq) ---> __Zn(OH)2(s)
Word equation:
11. __ Co(IO3)3(aq) +
Word equation:
__ Na2SO4(aq) ---> __ Co2(SO4)3(aq) +
+ __ NH4CH3COO(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. __ __________+ __ __________---> __ ___________+ ___ ___________
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 ( gasline 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. ___Al(s) + __NH4ClO4(s)--> __Al2O3(s) + __AlCl3(s) + __NO(g) + __HOH(l)
Reaction type _____
13. ___NO2 (g) + ____HOH(l) --> ____HNO3(aq) + ____NO(g)
Reaction type _____
14. ___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 (aq) + ___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 (l) --->
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) --->
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page 23
Still More Practice
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 is reacted with sulfuric acid to produce sodium sulfate and hydrochloric acid.
Equation:
Type:
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page 24
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.
Bread dough rises because carbon dioxide is produced when cream of tartar (KHC4H4O6) reacts with
sodium bicarbonate (baking soda). Other products are water and KNaC4H4O6.
Equation:
Type:
15.
A deadly gas (hydrogen cyanide) is produced when hydrochloric acid is added to a potassium cyanide
solution.
Equation:
Type:
16.
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:
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page 25
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)
2.
magnesium sulfate
3.
MgSiO3 (s)
4.
sodium hypochlorite
5.
Al(OH)3 (s)
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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{151.91 g}
{120.37 g}
{100.40 g}
{74.44 g}
{78.01 g}
{58.44 g}
{100.09 g}
{44.02 g}
{77.10 g}
{331.21 g}
{438.47 g}
page 26
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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page 27
Marvin says, “Show all of your work when
completing the open boxes. Remember to watch
for significant digits!”
formula
1.
C12H22O11
2.
NaOH(s)
5.
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molar mass
given mass
number of moles
1000 g
0.641 mol
ammonium
phosphate
3.
4.
name of substance
10.0 kg
CO2
(s)
5.00 mol
sulfuric acid
5000 g
page 28
Marvin says, “If you smell an odorless gas, it is
probably carbon monoxide!”
formula
6.
name of substance
given mass
CaCO3 (s)
aluminum oxide
8.
ethanol
9.
NaHSO3 (s)
10.
Mg(OH)2
(s)
number of moles
2.378 mol
7.
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molar mass
6.0 g
30.48 mol
250 mol
15 g
page 29
Marvin says, “Water is composed of two gins,
oxygin and hydrogin. Oxygin is pure gin and
hydrogin is gin and water”
formula
name of substance
molar mass
ammonium
benzoate
11.
given mass
350 g
phosphoric acid
50 mol
12.
13.
14.
15.
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number of moles
Al2(HPO4)3
(s)
10 g
ammonium carbonate
0.50 g
magnesium
dichromate
5.00 mol
page 30
Chemistry Final Review
Fill in the following blanks to BEST complete the statement.
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 ____________________ 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
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page 31
“____________________” 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.
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.
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page 32
u) A mole represents ____________________particles and this number is credited to the Scientist
____________________.
Fill in the following chart.
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page 33
a, i, or m
Formula
Name
silver bromide
magnesium nitrate
hydrochloric acid
tin (IV) chloride
sucrose
methanol
ammonium sulphide
cobalt (II) nitrate
acetic acid
ammonium sulphate
Co(OH)2(s)
P4Br6(s)
Ni3(PO4)2(s)
Pb(NO2)2(s)
H2O2(l)
NH3(g)
AgSCN(s)
Mn(HPO4)2(s)
CH4(g)
List the differences between the following:
1. metals and nonmetals.(4)
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2. Atoms and Ions. (3)
page 34
3. molecular and ionic bonds.(3)
4. acids and bases.(2)
Balance the following reactions. Include the phases and the type of reaction.
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. White phosphorus and vanadium combine in a synthesis reaction.
Complete the following chart.
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page 35
Formula
Name of Substance
Molar Mass
glucose
Mass
10.5 g
(NH4)2CO3(s)
357 g
calcium benzoate
0.389 moles
carbonic acid
5.07 moles
potassium
157 g
dichromate
Good Luck on the Final!
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Moles
page 36