CH 8 HOMEWORK
Assign oxidation numbers to the following:
+1 –1
+2 -1
+4 –2
NaCl
MgBr2
SO2
+1 +3 –2
+1 –3
+2 +5 –2
Na3BO3
Na3N
Fe(NO3)2
0
Al
+4 –1
CBr4
+3 –2
NO2-1
+1 +7 –2
CuClO4
+5 -2
PO4-3
-3 +1
NH4+1
1. Distinguish between binary and ternary acids and give two examples of each.
Binary contain hydrogen and a nonmetal; ternary contain hydrogen and a polyatomic
ion.
2. What are monatomic ions?
A single atom with a charge.
3. In naming and writing formulas, what determines the order in which the elements
appear? Positive ions come first; elements are written from least electronegative to
most electronegative with some exceptions.
4. What are oxidation numbers?
Number that show the distribution of electrons in a
compound. These are NOT IONS!
1
Monatomic Ions:
O-2
Sulfide
S-2
Mg+2 magnesium ion
Tin (II) ion
Sn+2
Fe+3
iron (III) ion
Barium ion
Ba+2
N-3
nitride
Fluoride
F-1
Ag+1
silver ion
Copper (I) ion Cu+1
oxide
Binary Molecular:
N2F2
dinitrogen difluoride
Dinitrogen Monoxide
N2 O
CI4
carbon tetraiodide
Phosphorous Trichloride
PCl3
NO2
nitrogen dioxide
Pentabromine Dioxide
Br5O2
P3O4
triphosphorous tetraoxide
Sulfur Mononitride
SN
SCl2
sulfur dichloride
Carbon Disulfide
CS2
MgCl2 magnesium chloride
Nickel (II) Chloride
NiCl2
W2O3 tungsten (III) oxide
Vanadium (III) Phosphide
VP
ZnS
zinc sulfide
Silver Sulfide
Ag2S
AlF3
aluminum fluoride
Potassium Chloride
KCl
Cd3P2 cadmium phosphide
Calcium Selenide
CaSe
FeN
Molybdenum (VI) Fluoride
MoF6
Cs2 S cesium sulfide
Cadmium Bromide
CdBr2
Y2O3 yttrium oxide
Manganese (II) Nitride
Mn3N2
SnI4
Gold (I) Oxide
Au2O
Titanium (IV) Sulfide
TiS2
Binary Ionic:
iron (III) nitride
tin (IV) iodide
Cu3P2 copper (II) phosphide
2
Polyatomic Ionic:
NaNO3
sodium nitrate
Magnesium Borate
Mg3(BO3)2
W PO4
tungsten (III) phosphate
Tin (IV) Sulfate
Sn(SO4)2
K2SO3
potassium sulfite
Calcium Bicarbonate Ca(HCO3)2
Mg(C2H3O2)2 magnesium acetate
Hydrogen Peroxide
H2O2
Fe(BrO3)2
iron (II) bromate
Sodium Azide
NaN3
KMnO4
potassium permanganate
Lead (II) Tartrate
PbC4H4O6
ZnCr2O7
zinc dichromate
Al2(CO3)3
aluminum carbonate
Copper (II) Ortho-Silicate
Cu2SiO4
Hydrogen Cyanide HCN
cadmium ferricyanide
silver hypochlorite
Iridium (VI) Hydroxide
Ir(OH)6
Barium Nitrate
Ba(NO3)2
Cd3[Fe(CN)6]2
AgClO
Acids:
HCl
hydrochloric acid
Sulfuric Acid
H2SO4
HIO3 iodic acid
Hydrofluoric Acid
HF
H2CO3 carbonic acid
Nitric Acid
HNO3
HBr
Oxalic Acid
H2C2O4
hydrobromic acid
3
Formula Writing:
potassium chlorate
KClO3
potassium chloride
KCl
nickel (II) phosphide Ni3P2
tin (IV) nitrite
Sn(NO2)4
aluminum borate
AlBO3
cobalt (III) sulfate
Co2(SO4)3
cadmium sulfate
CdSO4
ammonium carbonate (NH4)2CO3
magnesium hydroxide Mg(OH)2
aluminum sulfite
Al2(SO3)3
sodium bromide
NaBr
silver acetate
AgC2H3O2
zinc nitrate
Zn(NO3)2
sulfur dioxide
SO2
phosphoric acid
H3PO4
ammonium chlorate NH4ClO3
zinc sulfide
ZnS
potassium nitride
K3N
gold (I) dichromate
Au2Cr2O7
lead (IV) phosphate
Pb3(PO4)4
lead (II) iodate
Pb(IO3)2
calcium acetate
Ca(C2H3O2)2
copper (II) phosphate Cu3(PO4)2
lithium dichromate
Li2Cr2O7
aluminum oxide
Al2O3
potassium oxide
K2O
hydrobromic acid
HBr
ammonium hydroxideNH4OH
barium hydroxide
Ba(OH)2
magnesium borate
Mg3(BO3)2
carbon tetrachloride CCl4
sodium dichromate
Na2Cr2O7
nitrogen dioxide
NO2
barium chlorate
Ba(ClO3)2
sodium bicarbonate
NaHCO3
carbonic acid
H2CO3
calcium permanganateCa(MnO4)2
citric acid
H3C6H5O7
lithium nitrite
zinc iodate
Zn(IO3)2
cadmium perchlorate Cd(ClO4)2
barium chlorite
Ba(ClO2)2
manganese (II) oxide MnO
magnesium nitride
Mg3N2
lithium borate
Li3BO3
cobalt (II) bisulfate
Co(HSO4)2
hydroiodic acid
HI
iron (II) phosphate
Fe3(PO4)2
carbon disulfide
CS2
LiNO2
dinitrogen pentoxide N2O5
4
Naming:
Pb3(PO4)2
lead (II) phosphate
CoSO4
cobalt (II) sulfate
CuSO4
copper (II) sulfate
CuSO3
copper (II) sulfite
Pb(ClO3)4
lead (IV) chlorate
H2SO4
sulfuric acid
Fe(N3)3
iron (III) azide
Fe2(SO4)3
iron (III) sulfate
Cr(OH)2 chromium (II) hydroxide KBrO3
potassium bromate
Cd(IO3)2
cadmium iodate
FeCO3
iron (II) carbonate
CaCr2O7
calcium dichromate
Ba(NO3)2
barium nitrate
KNO3
potassium nitrate
NH4C2H3O2
ammonium acetate
Pb3N2
lead (II) nitride
Ba3P2
barium phosphide
HCl
hydrochloric acid
SO3
sulfur trioxide
Mg(NO3)2
magnesium nitrate
HNO3
nitric acid
Li2SO4
lithium sulfate
(NH4)2CO3
ammonium carbonate
CuCrO4
copper (II) chromate NaHCO3
sodium bicarbonate
Ca(ClO2)2
calcium chlorite
Ba(NO2)2
barium nitrite
Ag2CrO4
silver chromate
Sn3(PO4)2
tin (II) phosphate
HC7H5O2
benzoic acid
CaH2
calcium hydride
AuClO4
gold (I) perchlorate
Mg(OH)2
magnesium hydroxide
KHSO4
potassium bisulphate SrCl2
strontium chloride
MnS
manganese (II) sulfideAgNO3
silver nitrate
P2O5
diphosphorous pentoxide FeHPO4
PCl5
phosphorous pentachloride HC2H3O2
H3PO4
phosphoric acid
N2O
iron (II) hydrogen phosphate
acetic acid
dinitrogen monoxide
5
Make a correction, if necessary, and then provide the name/formula.
Correction
Name/Formula
Ba3NO3
Ba(NO3)2
barium nitrate
KSO4
K2SO4
potassium sulfate
Mg3(PO4)2
correct
magnesium phosphate
BaCr2O7
correct
barium dichromate
NaC2H3O2
correct
sodium acetate
PbBr2
correct
lead (II) bromide
Ag2(CO3)2
Ag2CO3
silver carbonate
NaHCO3
correct
sodium bicarbonate
HSO4
H2SO4
sulfuric acid
NH4(NO2)2
NH4NO2
ammonium nitrite
Magnesium (II) hydroxide
magnesium hydroxide Mg(OH)2
Dilithium oxide
lithium oxide
Li2O
Fluoric acid
hydrofluoric acid
HF
Calcium bicarbonate
correct
Ca(HCO3)2
Pb(II)SO4
PbSO4
lead (II) sulfate
6
Practice Quiz:
Formula:
Name:
6. S-2
sulfide
2. chromium (III) ion___Cr+3____
7. I-1
iodide
3. yttrium ion ___Y+3____
8. Fe+3
iron (III) ion
4. nitride
___N-3____
9. Ba+2
barium ion
5. chlorine
____Cl2___
10. O-2
oxide
1. silver
___Ag____
Provide Formulas:
11. sodium sulfate
Na2SO4
12. copper (I) oxide
Cu2O
13. potassium chlorite
KClO2
14. calcium phosphate
Ca3(PO4)2
15. aluminum nitride
AlN
16. chromium (III) chloride CrCl3
17. phosphorus trichloride
PCl3
18. oxalic acid
H2C2O4
19. barium phosphide
Ba3P2
20. gold (I) fluoride
AuF
Provide Names:
21. P2O3
diphosphorous trioxide
26. Ni(ClO3)2 nickle (II) chlorate
22. SnCl2
tin (II) chloride
27. Pb3N4
lead (IV) nitride
23. ZnS
zinc sulfide
28. MgSO4
magnesium sulfate
24. NaOH
sodium hydroxide
29. HBr
hydrobromic acid
25. CuBr2
copper (II) bromide
30. K2O
potassium oxide
7
Calculate the Formula Mass of the following:
1. a. H2SO4
98 g/mol
b. NH4NO3
80 g/mol
c. Fe(C2H3O2)2 (SF)
173.933 g/mol
d. CaSO4  2H2O
172 g/mol
2. Determine the formula mass for the following. (SF)
H OH O
| | |
H—C—C—C—O—H
|
H
89.0700 g/mol
3. Calculate the formula mass for acetylsalicylic acid:
180 g/mol
9C/8H/4O
Mole Calculations:
1. Calculate the mass of 2.00 mols of sulfuric acid.
196 g
2. Calculate the number of moles in 60.00 g of potassium carbonate (SF).
FM = 138.2055
.4341 moles
3. Calculate the number of molecules in 2.00 g of carbon dioxide.
2.73 x 1022 molecules
4. Find the number of grams in 7.2434 x 1024 ions of lithium ions.
84 g
5. 3.45 x 1023 “molecules” of barium phosphate would contain how many atoms?
4.485 x 1024 atoms
8
Composition Stoichiometry:
1. 23 g of manganese (III) sulfate would contain how many grams of manganese?
6.4 g Mn
2. 77 g of phosphoric acid would contain how many mols of hydrogen?
2.36 mol H
3. 3.4 mols of zinc sulfite would contain how many grams of zinc?
221 g Zn
4. 2.5 mols of calcium thiosulfate would contain how many mols of calcium?
2.5 mols
5. 56.33 g of barium would be how many mols?
.411 mol Ba
6. 657 g of sodium peroxide would contain how many mols of oxygen? (SF)
77.9783 g Na2O2
16.9 mol O
7. If a sample of iron (III) oxide contained 26 g of iron, what was the mass of the original
sample?
37.14 g Fe2O3
8. 45 g of oxygen would be how many mols?
1.41 mol O
9. 23 g of nitrogen dioxide would contain how many grams of oxygen? (SF)
16 g O 46.0055
10. The average person exhales 500 mols of carbon dioxide in a day. How many grams
of carbon would that be?
6000 g C
9
Calculate the Percent Composition of the following:
FM = 160
FM = 232
1a. Fe2O3
b. Ag2O
70% Fe 30% O
93% Ag 7% O
2. Determine the percent calcium in calcium phosphate.
38.71%
3. For the compound sodium sulfate decahydrate, calculate the following:
a. %Na
b. %O
c. %H2O
FM = 322
14.3%
70%
56%
4. Calculate the mass of the metal in each of the following:
a. 50 g of MgS
21.42 g Mg
b. 25 g of FeCO3
12.07g Fe
c. 200.00 g of aluminum oxide (SF) 52.92506% Al
105.85 g Al
d. 50 g of lead (II) oxide which is 30% pure 13.92 g Pb
5. The active ingredient in common household liquid bleach is the hypochlorite ion, ClOa) Determine the percent of active ingredient in sodium hypochlorite. 69 %
b) If bleach contains a 5% solution of sodium hypochlorite by mass, calculate the
percentage of hypolchlorite ion in the bleach.
3.45 %
6. A sample of brass contains by mass 28.0% zinc and 72.0% copper. How many
kilograms of brass could be produced from 6.00 kilograms of copper?
8.33 kg
7. A household detergent contains 35% sodium tripolyphosphate, Na5P8O10. This
complex salt keeps the pH of the wash water slightly basic by buffering action. The
tripolyphosphate can also form soluble complexes with hard water ions (Ca+2 and Mn+2)
that would otherwise form insoluble precipitates with detergent molecules. Determine
the percent of phosphorous in the detergent. 16.6 %
10
Empirical and Molecular Formula Determination:
1. Calculate the empirical formula for the following compounds:
a. 63.1% Mn; 36.9% S
MnS
b. 26.6% K; 35.4% Cr; 38.0% O
K2Cr2O7
2. Find the empirical formula for a compound given that a 48.5g sample is found to
contain 1.75g of carbon and 46.75g of bromine.
CBr4
3. The formula mass of a compound is 92g/mol. Analysis shows that there are .608g of
nitrogen and 1.388g of oxygen. What is the molecular formula of the compound?
N2O4
4. Determine the molecular formula of a compound that has a formula mass of 220 and is
56.4% phosphorus and 43.7% oxygen.
P4O6
5. A 13.83 g sample of unknown decomposes when heated, giving CO2 (g) and 6.57g of
solid MgO. What is the empirical formula for the compound?
MgCO3
Practice Quiz 1:
1. What are the empirical and molecular formulas of a compound if 212.1g of the
compound contains 42.4g of hydrogen and 169.7g of carbon. The formula mass of the
compound is 30.0 g/mol.
CH3 / C2H6
2. What is the formula mass of lithium phosphate?
116 g/mol
3. How many grams of chromium are in 20g of chromium (II) chloride?
8.5 g Cr
4. 3.56 x 1023 molecules of carbon dioxide would be how many grams?
26 g CO2
5. 76g of copper (II) oxide would contain how many mols of copper and how many
moles of oxygen?
.96 mol each
11
Practice Quiz 2:
1. Assign oxidation numbers to the following:
+3 –2
+3 +6 -2
-1
A. NO2
B. Fe2(SO4)3
2. Determine the formula mass of #1B.
400 g/mol
3. 4 moles of carbon tetrachloride would contain how many moles of carbon?
4 mol C
4. If a sample of iron (III) oxide contained 2.5 moles of oxygen, then how many grams
of iron would be in it? 93.33 g Fe
5. Find the percent composition of carbon tetrachloride.
8% C 92 % Cl
6. Mass of crucible and contents before heating.
Mass of empty crucible.
Mass of crucible and contents after heating.
21.54g
19.82g
20.94g
Find the percent water in the sample.
34.88%
Practice Quiz 3:
1. Assign oxidation numbers to the following:
+4 –2
+3 -2
A. IrS2
B. C2O4-2
2. What is the formula mass of sodium tetraborate?
202 g/mol
3. 18.46g of copper (II) chloride would contain how many moles of chlorine?
.27 mol Cl
4. Find the percent composition of diphosphorous pentoxide.
43.7 %P, 56.3% O
5. 11 moles of sulfuric acid would be how many grams?
1078 g H2SO4
6. Determine the molecular formula of a compound with a formula mass of 32 g/mol
which is 87.5% nitrogen and 12.5% hydrogen.
N2H4
12