Worksheet #1: Binary Ionic Compounds WS
Write the name of the following binary compounds
KCl
K2O
CaO
MgCl2
ZnS
RbBr
Al2O3
Na3N
Ca2C
KI
MgO
AlCl3
BaS
Al2S3
SrF2
MgI2
CaSe
BaBr2
CsCl
Mg3P2
Write the formula for the following binary compounds
calcium iodide
magnesium fluoride
sodium nitride
rubidium oxide
barium nitride
lithium chloride
silver sulfide
aluminum nitride
magnesium phosphide
sodium chloride
barium oxide
aluminum arsenide
calcium sulfide
sodium iodide
lithium sulfide
magnesium nitride
Write the formula of the following binary compounds
copper (II) iodide
iron (II) sulfide
silver bromide
gold (III) chloride
lead (IV) sulfide
vanadium (V) nitride
gallium (I) iodide
nickel (III) selenide
cobalt (III) oxide
manganese (III) oxide
copper (I) oxide
manganese (IV) oxide
gold (I) sulfide
chromium (VI) oxide
zinc selenide
vanadium (III) chloride
iron (III) bromide
tin (IV) chloride
antimony (V) bromide
titanium (IV) oxide
Write the name of the following binary compounds
FeCl3
FeCl2
V2O5
MnO2
NiF3
CuS
Fe2O3
Au2O
AuCl3
PbO
Pb2S3
ZnBr2
MnCl2
SnF4
Reveiw Module / Chapters 5–8
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Worksheet ##2: Chapter 6 Practice Problems
SECTION 6.1: INTRODUCTION TO CHEMICAL BONDING
1. Give the name and symbol of the ion formed when
a. a chlorine atom gains one electron.
c. an oxygen atom gains two electrons.
b. a potassium atom loses one electron.
d. a barium atom loses two electrons.
2. How many electrons are lost or gained in forming each ion?
a. Mg2+
b. Brc. Ag+
d. Fe3+
3. Classify each of the following as a cation, anion, or atom.
a. Be
c. Cu2+
e. O2+
b. Na
d. I
f. Ca2+
g. Cs+
h. Ne
4. Classify each of the following as a molecular compound or an ionic compound.
a. CO2
c. NaCl
e. MgCl2
b. N2
d. H2O
5. What types of elements tend to combine to form molecular compounds?
SECTION 6.3 IONIC CHARGES
1. What is the charge on the ion typically formed by each element?
a. oxygen
c. sodium
e. nickel, 2 electrons lost
b. iodine
d. aluminum
f. magnesium
2. How many electrons does the neutral atom gain or lose when each ion forms?
a. Cr3+
c. Li+
e. Cl32+
b. P
d. Ca
f. O23. Name each ion. Identify each as a cation or anion.
a. Sn2+
c. Bre. H3+
+
b. Co
d. K
f. Mn2+
SECTION 6.4 IONIC COMPOUNDS
1. Write the formulas for these binary ionic compounds.
a. magnesium oxide
c. potassium iodide
b. tin(II) fluoride
d. aluminum chloride
e. sodium sulfide
f. iron (II) bromide
2. Write the formulas for the compounds formed from these pairs of ions.
a. Ba2+, Clc. Ca2+, S2e. Al3+, O2+ +
b. Ag , I
d. K , Br
f. Fe2+, O23. Name the following binary ionic compounds.
a. MnO2
c. CaCl2
e. NiCl2
g. CuCl2
b. Li3N
d. SrBr2
f. K2S
4. Write formulas for the following tertiary ionic compounds.
a. sodium phosphate
c. sodium hydroxide
b. magnesium sulfate
d. potassium nitrite
5. Name the following compounds.
a. NaNO3
c. Na2SO4
b. FeCl3
d. K2CO3
h. SnCl4
e. ammonium chloride
f. potassium hydrogen carbonate
e. Cu(OH)3
f. Li3PO4
Reveiw Module / Chapters 5–8
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Worksheet #3: Formula Writing Sheet #1
Complete the chart by writing the correct formulas for the following compounds.
Name of Compound
Positive ion
Negative
ion
Formula
1. sodium Iodide
Na+
I-
NaI
2. silver sulfide
Ag+
S2-
Ag2S
3. barium sulfate
4. lithium sulfide
5. sodium hydroxide
6. ammonium chlorate
ClO3-
7. zinc sulfate
8. iron(III) phosphate
9. nickel (II) hydroxide
10. chromium (III) oxide
11. iron (III) sulfate
12. copper (II) nitrate
13. copper (II) carbonate
14. magnesium phosphide
15. aluminum nitrate
16. sodium phosphate
17. aluminum sulfate
18. aluminum sulfide
19. iron (III) sulfite
20. ammonium carbonate
Reveiw Module / Chapters 5–8
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Worksheet #4: Formula Writing Sheet 2
Complete the chart by writing the correct formulas for the following compounds.
Compound made
of
Positive
ion
Negative
ion
Formula
Compound Name
1. calcium and
nitrate
2. tin (IV) and
chloride
3. copper (II) and
carbonate
4. barium and
bromide
5. tin (II) and
sulfite
6. Ammonium and
Nitrate
7. Lithium and
phosphorus
8. Sodium and
Bicarbonate
9. Lead (II) and
Phosphate
10. magnesium and
hydroxide
11. silver and
sulfide
12. barium and
acetate
13. fluorine and
manganese (II)
14. Chromium (III)
and nitrate
15. sulfate and
Iron (III)
Reveiw Module / Chapters 5–8
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Worksheet #5: Lots of Ionic Naming
Name the following ionic compounds: (CN-1 = cyanide)
1. NaBr
2. Sc(OH)3
3. V2(SO4)3
4. NH4F
5. CaCO3
6. NiPO4
7. Li2SO3
8. Zn3P2
9. Sr(C2H3O2)2
10. Cu2O
11. Ag3PO4
12. SnS2
13. Ti(CN)4
14. KMnO4
15. Pb3N2
16. CoCO3
17. Cu(NO2)2
18. Fe(HCO3)2
Reveiw Module / Chapters 5–8
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Chapter 15 Practice Problems WS
Read each question or statement and respond in your notebook.
SECTION 15.1 : ELECTRON CONFIGURATION IN IONIC BONDING
1. For each element below, state (i) the number of valence electrons in the atom, (ii) the electron dot
formula, and (iii) the chemical symbol(s) for the most stable ion.
a. Ba
b. I
c. K
2. How many valence electrons does each atom have?
a. gallium
b. fluorine
c. selenium
3. Write the electron configuration for each of the following atoms and ions.
a. Ca
c. Na+
e. O2-
b. chlorine atom
d. phosphide ion
4. What is the relationship between the group number of the representative elements and
the number of valence electrons?
5. How many electrons will each element gain or lose in forming an ion? State whether the
resulting ion is a cation or anion.
a. strontium
c. tellurium
e. bromine
b. aluminum
d. rubidium
f. phosphorous
SECTION 15.2: IONIC BONDS
1. Use electron dot structures to predict the formula of the ionic compounds formed when the
following elements combine.
a. sodium and bromine
d. aluminum and oxygen
b. sodium and sulfur
e. barium and chlorine
c. calcium and iodine
2. Name the compounds formed when the following elements combine.
a. magnesium and oxygen
c. lithium and hydrogen
b. sodium and fluorine
3. Which of these combinations of elements are most likely to react to form ionic compounds?
a. sodium and magnesium
c. potassium and iodine
b. barium and sulfur
d. oxygen and argon
Reveiw Module / Chapters 5–8
45