Unit 6 Vocabulary Preview
Prefixes/Suffixes/Roots
SubSuperPolyAnBiPreMonoDi
TriTetraPentaHexaHeptaOctaNonaDeca-
Below
Above
Many
Negative/Against
Two
Before
One
Two
Three
Four
Five
Six
Seven
Eight
Nine
Ten
Key Vocab
1. Ionic Bond
2. Covalent Bond
3. Metallic Bond
4. Multivalent
5. Polyatomic Ion
6. Oxidation Number
7. Compound
8. Cation
9. Anion
10. Binary
11. Avogadro’s Number
12. Mole
13. Molecule
14. Molar Mass
15. Percent Composition
16. Empirical Formula
17. Molecular Formula
CALCULATION OF PERCENT HYDRATION FROM THE CHEMICAL FORMULA
The percent hydration (percent water) can be calculated from the formula of the hydrate by dividing the mass of
water in one mole of the hydrate by the molar mass of the hydrate and multiplying this fraction by 100.
EXAMPLE: What is the percent water in copper(II) sulfate pentahydrate, CuSO4 ·5 H2O?
1. Calculate the formula mass. When determining the formula mass for a hydrate, the waters of hydration must
be included.
1 Cu @ 63.55 g = 63.55 g
1 S @ 32.07 g = 32.07 g
4 O @ 16.00 g = 64.00 g
159.62 g/mol
2 H @ 1.01 = 2.02 g
1 O @ 16.00 = 16.00 g
18.02 g/mol
Formula Mass = 159.62 + 5(18.02) = 249.72 g/mol
2. Divide the mass of water in one mole of the hydrate (5 x 18.02 = 90.10) by the molar mass of the hydrate
(249.72) and multiply this fraction by 100.
Percent hydration = (90.10 g /249.72 g)(100) = 36.08%
Worksheet 1
Review/Pre-assessment
1. How many elements make up the following compounds?
a) C12H22O11
C__________ H___________ O___________
b) Ca(HCO3)2
Ca_______ H_________ C__________ O_________
c) C7H5(NO3)3
C______ H________ N__________ O__________
d) Al (OH)3
Al _________ O____________ H_____________
2. Classify as ionic (I) or covalent (C):
a) H2SO4 ___________________
e) BaI2 ____________________
b) MgCl2 ___________________
f) CuNO3 __________________
c) CO2 _____________________
g) H2O ____________________
d) KOH ___________________
h) LiBr2 ___________________
3. Indicate the most likely charges (oxidation number) on the following elements when
they become ions:
a) O ______________
f) Cr_____________
b) H ______________
g) P ____________
c) Br ______________
h) S _____________
d) K ______________
I) Na ____________
e) Ba ______________
j ) C ____________
4. For the multivalent elements below, indicate their possible charges:
a) Fe ________________
b) Pb _______________
c) Sn _______________
d) Cu _______________
e) Ag _______________
f) Ni ________________
5. Write formulas for the following polyatomic ions:
a) phosphate _____________________
b) nitrate ________________________
c) carbonate _____________________
d) hydroxide ______________________
e) sulfate _________________________
f) ammonium ____________________
g) acetate ________________________
h) chromate ______________________
i) dichromate ____________________
j) permaganate __________________
k) oxalate ________________________
6. Using table 9.2 on p. 255 of your textbook, write the names for each multivalent metal
ion.
a) Cu +1 __________________________
b) Fe+3 __________________________
c) Co+2 __________________________
d) Hg+2 __________________________
e) Pb+4 __________________________
f) Cr+3 ___________________________
g) Sn+2 ___________________________
Name: _____________________
Chamberlain
Class: ________
Ionic Compound Puzzles
Directions: With a partner, use the puzzle pieces in the baggie to make ten different compounds. To make a
compound, the charges have to cancel (the puzzle has to make a rectangle). List the metal ion (+), the nonmetal
ion (-) and then write the formula by adding subscripts to represent the number of that ion that there are in the
compound. After the notes, you will be able to go back and name your compounds. You must do a minimum
of 5 compounds in which the metal and nonmetal do not have the same charge.
Metal Ion
Nonmetal
Ion
Chemical
Formula
Compound Name
Mrs. C
O.K.
Ba+2
P-3
Ba3P2
Barium phosphide

Analysis & Results:
1. What do you think it means if a compound is binary?
2. What does the oxidation number tell you about the number of valence electrons the ion has?
3. Why can’t two negative ions or two positive ions bond together?
4. What is the sum of the charges each time you made a compound?
5. What do the subscripts tell you in the formula?
6. Reflect on the activity that you just did. In what ways did it help you?
Compound
1. Magnesium fluoride
2. Copper (II) phosphate
3. Zinc acetate
4. Silver carbonate
5. Iron (III) sulfite
6. Aluminum hydroxide
7. Sodium sulfate
8. Calcium nitrate
9. Rubidium dichromate
10. Ammonium oxalate
11. Potassium peroxide
12. Chromium (III) sulfate
13. Tin (IV) oxide
14. Lead (II) cyanide
15. Aluminum hydrogen carbonate
16. Ammonium chlorate
17. Magnesium iodate
18. Sodium hydroxide
19. Phosphoric acid
20. Hydrochloric acid
21. Sodium chlorate
22. Lead (II) oxide
23. Calcium carbonate
24. Copper (I) chloride
25. Silver Nitrate
Write positive ion
with charge as
superscript
Write negative ion
with charge as
superscript
Write formula with
correct subscripts (no +
or – signs!)
Name These:
1. Rb2O
2. CoF2
3. NiCO3
4. K3PO4
5. H2SO4
6. Al(NO3)3
7. HgSO4
8. Zn(OH)2
9. Ba(ClO3)2
10.Mg(C2H3O2)2
11. AgCN
12. NaHCO3
13. HNO3
14. KOH
15. Cu2CrO4
16. Sr(NO2)2
17. HC2H3O2
18. LiMnO4
19. BaBr2
20. CaCl2
21. AgNO3
22. KI
23. LiOH
24. CuSO4
25. HCl
Full Name
Write Molecular Formulas for:
1. Carbon tetrachloride
2. Dihydrogen monoxide
3. Dinitrogen trioxide
4. Triphophorous tetrabromide
5. Dicarbon hexachloride
6. Carbon monoxide
7. Trinitrogen octasulfur pentachloride
8. Dihydrogen dioxide
9. Carbon dioxide
10. Tetracarbon octaoxide
Try these ionic compounds &
acids (WS#2)
11. Calcium oxide
12. Aluminum oxide
13. Lithium nitride
14. Sodium fluoride
15. Sodium phosphate
16. Nitric Acid
17. Acetic Acid
18. Silver Nitrate
Mixed Review
Compound
19. Copper (II) Sulfate
20. Tricarbon nonachloride
21. Ammonium carbonate
22. Carbon monoxide
23. Iron (III) oxide
Ionic or Covalent
Formula
Write Molecular Names for:
Remember to use prefixes to indicate how many of each type of
atom there are. Do not use “mono” in front of the first element
1. NH3
2. P4O10
3. S2O3
4. CCl5
5. CO4
6. C3H6O3
7. PO3
8. CO
9.
C7F9
Try these ionic compounds
& acids (WS#2)
10. CuSO4
11. KMnO4
12. SnF2
13. (NH4)3PO4
14. HgCrO4
15. AgNO3
16. H3PO4
17. Pb(NO3)4
18. H2CO3
Mixed Review
Compound
19. CO2
20. Co(CN)3
21. OF2
22. Zn(OH)2
23. Ni2CO3
Ionic or Covalent
Name
1. Convert to moles:
a. 32.9 g neon
1.63 moles
b. 0.00823 g molybdenum
8.58 x 10-5
moles
c. 6.16 g calcium nitrate
0.0376 moles
d. 6.4 x 10-4 g aluminum phosphate
5.2 x 10-6
moles
e. 7.12 x 1023 molecules silicon tetrafluoride
1.18 moles
f. 4.87 x 1017 atoms arsenic
8.09 x 10-7
moles
g. 0.98 L of N2O
0.044 moles
2. Convert to grams:
a. 0.112 moles tungsten
20.6 g
b. 2.48 x 10-3 moles carbon
0.0298 g
c. 51.6 moles nickel (II) oxide
3.85 x 103 g
d. 1.09 moles zinc hydroxide
108 g
3. Convert to molecules:
a. 6.72 moles sodium chloride
4.05 x 1024
molecules
b. 102 moles chromium (III) bromide
6.14 x 1025
molecules
c. 47.9 g cobalt (II) oxalate
1.96 x 1022
molecules
d. 16.2 g diphosphorus pentoxide
6.87 x 1022
molecules
e. 4.61 L of H2O
1.24x 1023
molecules
4. Convert to grams:
a. 1.06 x 1027 atoms copper
1.12 x 105 g
b. 7.39 x 1023 molecules tin (II) chromate
288 g
c. 8.27 x 1024 molecules potassium dichromate
4040 g
d. 4.52 x 1021 molecules barium sulfate
1.75 g
e. 5.78 L of N2
7.23 g N2
5. Convert to Liters:
a. 6.54 moles H2
b. 3.98 g O2
146 Liters
2.79 Liters
1. Determine the percentage composition of each of the following compounds:
a) sodium oxalate, Na2C2O4 (33% Na, 20% C, 47% O)
b) ethanol, C2H5OH (52% C, 13% H, 35% O)
c) aluminum oxide, Al2O3 (53% Al, 47% O)
d) potassium sulfate, K2SO4 (44.87% K, 18.40% S, 36.72% O)
2. Calculate the mass of the given element in each of the following compounds:
a) bromine in 50.0 g potassium bromine, KBr (33.5 g)
b) chromium in 1.00 kg sodium dichromate, Na2Cr2O7 (0.397 kg)
c) nitrogen in 85.0 mg of lysine, C6H14N2O2 (16.3 mg)
d) cobalt in 2.84 g cobalt (II) acetate, Co(C2H3O2)2 (0.947 g Co)
3. A sample of Ag2S has a mass of 62.4g. What mass of each element could be obtained by decomposing
this sample? (54.35 g Ag, 8.05 g S)
4. Calculate the mass of zinc in a 30.00 g sample of zinc nitrate, Zn(NO3)2 (10.36 g Zn)
5. Calculate the mass of oxygen in 4.00 g of manganese dioxide, MnO2. (1.47 g O)
6. Calculate the mass of gold in 0.780 g of Au2Se3. (0.487 g Au)
1. Complete the table by writing the molecular formula for each of the following substances:
Compound
Molecular Formula
Water
H2 O
Hydrogen Peroxide
H2O2
Glucose
C6H12O6
Methane
CH4
Ethane
C2H6
Octane
C8H18
Empirical Formula
2. Determine the molecular formula of each of the following unknown substances:
 empirical formula CH2
 experimental molar mass 28 g/mol
(C2H4)


empirical formula C6H8O
experimental molar mass 290 g/mol
(C18H24O3)
3. Determine the empirical formula for compounds that have the following analyses: 57.6% strontium, 13.8%
phosphorus, and 28.6% oxygen. (Sr3P2O8)
4. Determine the empirical formula for compounds that have the following analyses: a 0.858 g sample of an
unknown substance is composed of 0.537 of copper and 0.321 g of fluorine. (CuF2)
5. A 10.64 g sample of a lead compound is analyzed and found to be made up of 9.65 g of lead and 0.99 g of
oxygen. The molecular mass of the unknown compound is 1,370 grams/mole. Determine the molecular
formula for this compound. (Pb6O8)
6. Determine the molecular formula for a compound that is 36.2% aluminum and 63.8% sulfur and has a
molecular mass of 1,893 g/ mole. (Al6S9)