Unit Packet 5
Ionic Compounds
Cost: $1
Prosser Chemistry
Name: ___________________
Period: _____
Introduction to Ionic Bonding
1. For the following elements, indicate the orbital notation in the diagram, write the abbreviated electron
configuration, identify the element as a metal or a non-metal, indicate whether it will gain or lose
electrons to form a stable octet, and identify how many electrons will be transferred in the process.
Orbital Notation
a.
Short Electron Configuration
Beryllium (Be)
Bonding Habits
Metal or Non-metal?
Gain or Lose Electrons?
# of Electrons: _____
b.
Fluorine (F)
Metal or Non-metal?
Gain or Lose Electrons?
# of Electrons: _____
c.
Sulfur (S)
Metal or Non-metal?
Gain or Lose Electrons?
# of Electrons: _____
2.
In general, do metals have a tendency to gain or to lose electrons?
In general, do non-metals have a tendency to gain or to lose electrons?
3. Fill in the following charts for each element given.
Lithium
A. Electron configuration
B. Number of electrons in the outer energy level
C. Will the atom have a tendency to gain or lose electrons?
D. How many electrons will be gained or lost?
E. If the atom gains or loses the electrons as stated in D above,
what will be the net charge on the newly formed ion?
Potassium
A. Electron configuration
B. Number of electrons in the outer energy level
Why do lithium and potassium
form ions with the same charge?
How do their positions on the
periodic table relate to this issue?
C. Will the atom have a tendency to gain or lose electrons?
D. How many electrons will be gained or lost?
E. If the atom gains or loses the electrons as stated in D above,
what will be the net charge on the newly formed ion?
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Calcium
A. Electron configuration
B. Number of electrons in the outer energy level
C. Will the atom have a tendency to gain or lose electrons?
D. How many electrons will be gained or lost?
E. If the atom gains or loses the electrons as stated in D above,
what will be the net charge on the newly formed ion?
Magnesium
A. Electron configuration
B. Number of electrons in the outer energy level
Why do calcium and magnesium form
ions with the same charge? How do
their positions on the periodic table
relate to this issue?
C. Will the atom have a tendency to gain or lose electrons?
D. How many electrons will be gained or lost?
E. If the atom gains or loses the electrons as stated in D above,
what will be the net charge on the newly formed ion?
4. A neutral iron atom loses three electrons to form an ion.
a. How many protons does the ion have? ____________
b. How many electrons does the ion have? ____________
c. What is the charge on the ion? ____________
5. A neutral sulfur atom gains two electrons to form an ion.
a. How many protons does the ion have? ____________
b. How many electrons does the ion have? ____________
c. What is the charge on the ion? ____________
d. Where do you think the two electrons came from?
6. Explain how ionic compounds are formed.
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Forming Ionic Compounds
1. Normally a calcium atom has 20 protons and 20 electrons. How many protons and electrons does a +2 calcium
ion have?
2. Normally a sulfur atom has 16 protons and 16 electrons. How many protons and electrons does a -2 sulfur ion
have?
3. Predict the formula of the ionic compound which will be formed from each of the following pairs of ions.
+
2S
_________________
3+
Cl
_________________
Na
Fe
Ca
2+
O
2-
_________________
2+
Mg
F
_________________
+
Cl
_________________
3+
NO3-
_________________
K
Fe
Na
Ca
+
2+
3+
Al
SO4
Br
O
-
2-
2-
_________________
_________________
_________________
4. Predict the formula of the ionic compound which will be formed from each of the following pairs of atoms. (Use
your periodic table.)
a. K and S
b. Ca and F
c. Mg and O
d. Li and N
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5. Given the formula CaCO3, if the calcium ion has a +2 charge, what is the charge on the CO 3 ion?
6. Use the following ions to form 10 different compounds. You may use each ion more than once.
Na+ S2-
I-
PO43-
NH4+
Zn2+
Fe3+
SO42-
a. __________________
b. ___________________
c. __________________
d. ___________________
e. __________________
f. ___________________
g. __________________
h. ___________________
i. __________________
j. ___________________
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Name ___________________________
Naming Ionic Compounds
This activity will challenge your ability to recognize patterns and apply those patterns to new situations. It will also
introduce you to the general rules for naming simple chemical compounds. You will need to use your periodic table
and what you now know about how compounds are formed to help you.
Part 1 Below are some chemical formulas and their names.
NaCl
CaCl2
K2 O
Al2O3
sodium chloride
calcium chloride
potassium oxide
aluminum oxide
MgO
Na2S
Li3N
magnesium oxide
sodium sulfide
lithium nitride
1. List any patterns you see among the formulas and their names.
2. The first element in each compound is what kind of element? __________________
3. The second element in each compound is what kind of element? ________________
4. What kind of bonding is holding these compounds together? __________________
5. Fill in the blanks in the following rule for naming ionic compounds.
Ionic compounds are formed between ions which have ________________ charges.
When naming ionic compounds, the name of the ________________ ion goes first.
The name of the _____________ ion goes second and it always ends in __________.
6. Try naming the following compounds.
NaBr
CaF2
BaO
Al2S3
7. Now try to write the formulas for the following compounds.
potassium chloride
calcium bromide
sodium sulfide
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Naming Ionic Compounds (Part 2)
Below are some more compounds and their names.
FeCl2
FeCl3
Cu2O
CuO
iron (II) chloride
iron (III) chloride
copper (I) oxide
copper (II) oxide
PbO
PbO2
lead (II) oxide
lead (IV) oxide
The patterns for naming these compounds is a little more difficult to see at first.
1. The first element in each compound is a ________________________________.
2. What do you know about the charge of the first elements in these compounds?
3. How are the first elements in these compounds different from the first elements in the compounds in part 1?
4. What type of bonding is holding these compounds together? _______________
5. How are the names of these compounds different from the names of the ionic compounds in part 1?
6. Remembering that the total charge must equal zero in an ionic compound, what do you think the roman numerals
in the names of these compounds stand for?
7. How will you know when to use roman numerals in the name of an ionic compound?
8. Try to name these compounds.
FeBr3
NiS
CoCl2
9. Now try to write the formulas for the following compounds.
copper (I) chloride
iron (III) oxide
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Introduction to Polyatomic Ions
Fill in the symbols for the following polyatomic ions:
sulfate __________
nitrate ___________
phosphate ___________
hydroxide ________
carbonate ________
bicarbonate __________
ammonium _______
acetate __________
Fill in the blanks in the following table:
CATION
Ca2+
ANION
FORMULA
NAME
ClMgCO3
ammonium sulfate
Fe3+
NO3NaHCO3
tin (IV) oxide
SnCl4
manganese (III) oxide
Pb2+
S2BaSO4
lead (II) hydroxide
AlPO4
K+
ClAgNO3
sodium carbonate
Al3+
O2HgO
calcium sulfate
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Naming Ionic Compounds Worksheet
1. Name each of the following ionic compounds.
a. MgI2
________________________________
b. Na2S
________________________________
c. CaBr2
________________________________
3. Name the following ionic compounds whose metals do not have a fixed charge.
a. CuCl2
________________________________
b. CoS
________________________________
c. Cu2S
________________________________
4. Name the following compounds that contain polyatomic ions.
a. Na2CO3
________________________________
b. Mg(NO3)2
________________________________
c. Cu3PO4
________________________________
5. Write the formulas for the following compounds that contain polyatomic ions.
a. sodium carbonate
____________________
b. calcium carbonate
____________________
c. iron (II) phosphate
____________________
6. Write the formulas for the following compounds.
a. calcium chloride
____________________
b. magnesium oxide
____________________
c. iron (II) bromide
____________________
d. iron (III) nitrate
____________________
e. iron (III) nitride
____________________
f. lead (IV) oxide
____________________
g. aluminum sulfide
____________________
h. cobalt (III) chloride
____________________
i. cobalt (III) carbonate
____________________
j. aluminum fluoride
____________________
k. lithium sulfate
____________________
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l. manganese (II) phosphide
____________________
m. magnesium hydroxide
____________________
7. Name each of the following compounds.
a. MgI2
________________________________
b. CoS
________________________________
c. Cu2S
________________________________
d. CaO
________________________________
e. AlCl3
________________________________
f. MnO2
________________________________
g. BaF2
________________________________
h. Na2SO4
________________________________
i. FeCO3
________________________________
j. Ca3P2
________________________________
k. MnO2
________________________________
l. Al2(SO4)3
________________________________
m. HgO
________________________________
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Moles and Formulas
1. Give the name of each of the following compounds. Then calculate the molecular mass for each compound.
Name
Molecular Mass
NH4Cl
CaSO4
Fe(OH)3
Fe2(SO4)3
Sr(NO3)2
AlCl3
-4
2. What is the mass of 3.57 x 10
mol of N2O5?
3. How many moles are in 194 g of NH3?
32
4. What is the mass of 8.75 x 10
molecules of C6H8O6?
5. Aspartame is the chemical name for Nutrasweet. Its molecular formula is C 14H18N2O5.
a. Find the molecular mass of Nutrasweet.
b. If you used 1.50 g of Nutrasweet in a glass of tea, how many moles did you use?
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Moles and Formulas (Part 2)
1. What is a mole?
2. What is the mass of 1 mole of carbon dioxide - CO2? ___________________
3. What is the mass of 1 mole of barium nitrate - Ba(NO3)2? ___________________
4. Give the name of each compound and calculate how many moles are present in each of the following samples.
a. 2.0 x 10-3 g of SnO2
name:
b. 62.8 g of BaCl2
name:
5. Give the name of each compound and calculate the mass of each of the following samples.
a. 5.0 mol of Li2CO3
name:
b. 0.054 mol Co(NO3)2
name:
6. Give the formula and find the number of molecules present in the following sample.
0.0908 g of nickel (II) chloride
formula:
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