Download Nomenclature and Formula Writing A. Write the formula for the

Nomenclature and Formula Writing
Name:
A. Write the formula for the following compounds.
1. silver chloride
3. cupric iodide
5. strontium fluoride
7. aluminium nitrate
9. manganese dioxide
11. potassium nitrite
13. lead (II) nitrate
15. dioxygen (gas)
17. hydrochloric acid
19. sodium hydride
21. iron (III) sulfate
23. cesium perbromate
25. zinc fluoride
27. stannic sulfate
29. hydrogen peroxide
31. aluminium hydrogen sulfite
33. potassium chlorite
35. lead (IV) iodite
37. chromium (II) oxide
39. calcium hypobromite
41. stannic permanganate
43. calcium sulfide
45. magnesium hydroxide
47. potassium peroxide
49. magnesium cyanide
51. sodium dichromate
53. nitric acid
55. magnesium bisulfate
57. mercuric chloride
59. sodium chlorite
61. difluorine (gaz)
63. aluminium sulfide
65. rubidium nitrite
67. ammonium hydrogen sulphate
69. hydroiodic acid
71. carbon tetraiodide
73. dihydrogen oxide
75. cuprous thiocyanate
77. silver thiocyanate
79. ferric carbonate
81. magnesium hydride
83. lithium dihydrogen phosphate
85. ferrous hydroxide
87. hydrogen sulfide
89. nickel
91. carbonic acid
93. manganese (II) iodate
95. neon (gas)
97. lithium hydride
99. xenon hexafluoride
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2. zinc sulfate
4. ammonia
6. potassium cyanide
8. mercurous sulfide
10. potassium chromate
12. silver hydroxide
14. ferric hydroxide
16. sulfur trioxide
18. aluminium nitrite
20. barium bicarbonate
22. sodium thiocyanate
24. phosphoric acid
26. stannic hydrogen carbonate
28. strontium bromate
30. nitrogen dioxide
32. nitrous acid
34. zinc phosphate
36. ammonium perchlorate
38. mercury(I) ferricyanide
40. dibromine (gaz)
42. aluminium oxide
44. ferric iodide
46. sodium hypoiodite
48. hydrobromic acid
50. sodium
52. iron
54. dinitrogen (gas)
56. cobalt (II) permanganate
58. silicon dioxide
60. sulfuric acid
62. sodium biphosphate
64. chromium (III) oxalate
66. hydrogen iodide
68. beryllium bromite
70. xenon (gas)
72. lithium hydrogen carbonate
74. calcium acetate
76. mercurous acetate
78. sodium oxide
80. potassium hydrogen-oxalate
82. gold (III) nitrate
84. iron (III) binoxalate
86. hydrazine
88. cadmium (II) acetate
90. uranium tetrafluoride
92. boron trihydroxide
94. strontium sulfite
96. ferric cyanide
98. ammonium carbonate
100. barium pyrophosphate
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1
B. Name the following compounds.
1. AgI
3. CuSO4
5. NaCN
7. Fe(NO3)2
9. SO2
11. Fe(NO3)3
13. K2C2O4
15. AlPO4
17. Na3PO4
19. Na2CrO4
21. Sn(SO4)2
23. SO3
25. Pb(C2O4)2
27. Al2(CO3)3
29. KMnO4
31. KHCO3
33. Cu(C2H3O2)2
35. NaClO3
37. NaBrO
39. V2S5
41. SnF2
43. Zn(NO2)2
45. KCH3COO
47. H2SO4(aq)
49. HgCr2O7
51. NH4IO
53. NaHS
55. NaOH
57. Pb(HSO4)4
59. Na2O2
61. H3PO4
63. MnS2
65. Li2O
67. Zn2P2O7
69. H2SO3(aq)
71. Ca(ClO4)2
73. CrFe(CN)6
75. HF
77. MnO
79. AsH3
81. PtCl4
83. HCl(aq)
85. Al(OH)3
87. HClO4(aq)
89. BaCr2O7
91. Fe2O3
93. CH3COONa
95. Be(BrO2)2
97. AlI3
99. Na4Fe(CN)6
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2. CCl4
4. MgO
6. PCl5
8. (NH4)2SO4
10. Cu2SO4
12. NaBr
14. RbSCN
16. K2CO3
18. SnSO4
20. Pb(NO3)2
22. WF6
24. K2Cr2O7
26. Na2HPO4
28. Au(CN)3
30. SrH2
32. Al2S3
34. Ba(SCN)2
36. Fe(OH)2
38. HNO2(aq)
40. Fe(ClO)2
42. HBr(aq)
44. Ag2OOCCOO
46. NH4OH
48. Cu2S
50. RbI
52. MoCl5
54. CsH2PO4
56. Ni(SCN)2
58. Hg(NO3)2
60. RbH
62. NI3
64. Li2CrO4
66. Na2SO3
68. H2S(aq)
70. CsHCO3
72. NH4ClO2
74. CsCN
76. HNO3(aq)
78. CaS2O8
80. Zn(IO2)2
82. H3OHC2O4
84. PH3
86. NH4BrO3
88. KrF4
90. Sr3(PO4)2
92. (NH4)2HPO4
94. PbCO3
96. XeO2
98. HCl(aq)
100. FIN
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2
Balancing Chemical Equations
1.
__ CaCO3 
__ CaO + __ CO2
2.
__ Fe3O4 +
__ H2 
3.
__ Fe2O3 +
__ C 
4.
__ P4 +
__ O2 
5.
__ Ga +
__ H2SO4 
6.
__ Ca(OH)2 +
7.
__ Zn +
__ HCl 
__ ZnCl2 +
__ H2
8.
__ Mg +
__ CO2 
__ MgO +
__ C
9.
__ Al2O3 +
__ HCl 
14. __ Cr +
__ O2 
__ H2O
__ O2 
__ CrBr3 
20. __ Al2(SO4)3 +
21. __ SiO2 +
__ CaCl2 +
__ H2O
__ H2O
__ O2 + __ NaF +
__ H2O +
__ H2O
__ NO
__ Br2 + __ CrCl3
__ SrI2 +
22. __ CH4 + __ O2 
__ H2O
__ AlCl3 +
__ Sb2O3 + __ SO2
__ NH3 +
__ Al 
__ HNO3
__ Ca(NO3)2 +
__ O2  __ CO2 +
19. __ Sr(IO3)2 
__ H2O
__ Cr2O3
__ NaOH 
17. __ NH3 +
18. __ Cl2 +
__ Al +
__ HCl 
__ Sb2S3 
15. __ C2H6 +
__ CaCl2 +
__ H2S  __ CuS +
13. __ O2 +
16. __ F2 +
__ H2 + __ Ga2(SO4)3
__ HNO3 
12. __ Ca(AlO2)2 +
__ H2O
__ CO
__ P2O5
__ H2 
10. __ Cu(NO3)2 +
11. __ CaO +
__ Fe +
__ Fe +
__ O2
__ H2O 
__ Si +
__ Al(OH)3 +
__ (NH4)2SO4
__ Al2O3
__ CO2 +
__ H2O
23. __ C4H8 +
__ O2 
__ CO2 +
__ H2O
24. __ C6H6 +
__ O2 
__ CO2 +
__ H2O
25. __ C4H2 +
__ O2 
__ CO2 +
__ H2O
26. __ C5H12 +
__ O2  __ CO2 +
__ H2O
Writing and Balancing Chemical Equations
 Complete the following synthesis reactions.
a. gallium and oxygen 
b. nitrogen and oxygen 
(producing dinitrogen pentoxide)
 Complete the following decomposition reactions.
a. rubidium carbonate 
b. strontium chlorate 
c. aluminum oxide 
d. magnesium hydroxide 
(carbonates tend to produce CO2 and metal oxides)
(chlorates tend to produce O2 and metal chlorides)
(hydroxides tend to produce H2O and metal oxides)
 Complete the following single displacement reactions.
a. chlorine and gold (III) bromide 
b. zinc and hydrochloric acid 
c. magnesium and water 
d. aluminum and iron (III) sulfate 
3
 Complete the following double displacement reactions.
a. copper (II) nitrate and potassium sulfide 
b. calcium hydroxide and phosphoric acid 
c. sodium sulfite and hydroiodic acid 
 Complete the following combustion reactions
a. for the complete combustion of octane (C8H18)
b. for the incomplete combustion of methane (CH4)
The mole and Avogadro’s Number
 How many atoms in 3.78 mol of silver?
 How many molecules in 0.45 mol of oxalic acid, H2OOCCOO?
 Calculate the number of moles present in 7.45 x 1022 molecules of C6H12O6.
 Based on you’re the values from questions # , how many oxygen atoms are present?
 Given 2.67 x 1022 atoms of radon, determine the number of moles.
 Determine the molar mass ammonium sulfate, (NH4)2SO4.
 Calculate the number of moles present in 56.8 g of phosphorous hexachloride.
 How many grams in 0.422 mol of tin (II) chloride?
 How many grams in 2.00 x 1025 atoms of neon?
 Determine the amount of atoms of hydrogen in 6.25 g of calcium hydroxide, Ca(OH)2.
Calculate the mass in milligrams of all of the hydrogen in 5.34 x 10 24 molecules of calcium stearate and 3.54 x 1023
molecules of water.
Mass-mass and Limiting Reactant
Mass-mass problems
 When iron (II) hydroxide is mixed with phosphoric acid, iron (II) phosphate precipitate results.
a. Balance the following equation: Fe(OH)2 (aq) + H3PO4 (aq)  Fe3(PO4)2 (s) + H2O (l)
b. If 3.20 g of Fe(OH)2 is treated with an excess of phosphoric acid, how many grams of Fe3(PO4)2 precipitate can be
formed?
 If 120. g of propane, C3H8, is completely combusted in excess oxygen, how many grams of water are formed? (Do not
forget a balanced chemical equation!)
 For the following reaction: 4 FeCr2O7 + 8 K2CO3 + O2  2 Fe2O3 + 8 K2CrO4 + 8 CO2
Complete one of the following:
a. How many grams of FeCr2O7 are required to pruduce 44.0 g of CO2?
b. How many g of Fe2O3 will be produced from 300.0 g of FeCr2O7?
c. How many grams of K2CrO4 are formed per gram of K2CO3 used?
Limiting Reactant Problems
 Arcylonitrile, C3H3N, is the starting material for the production of a kind of synthetic fiber (acrylics) and can be made
from propylene, C3H6, by reaction with nitric oxide, NO, as follows:
4 C3H6 (g) + 6 NO (g)  4 C3H3N (s) + 6 H2O (l) + N2 (g)
What mass of C3H3N can be made when 21.6 g of C3H6 react with 21.6 g of nitric oxide?
 One of the components of the fuel mixture on the Apollo lunar module involved a reaction with hydrazine, N 2H4, and
dinitrogen tetraoxide, N2O4. If the balanced equation for this reaction is:
2 N2H4 (l) + N2O4 (g)  3 N2 (g) + 4 H2O (g),
what volume of N2 gas (measured at STP) would result from the reaction of 1500 kg of hydrazine and 1000 kg of N 2O4?
Indicate as well, the limiting reactant.
 If 90.0 g of FeCl3 reacts with 52.0 g of H2S, what is the limiting reactant? What is the mass of HCl produced? What
mass of excess reactant remains after the reaction?
2 FeCl3(aq) + 3 H2S(aq)  6 HCl(aq) + Fe2S3(s)
4