________ Student Number
Name ____________________________Period _____Date Thursday, December 5, 2013
“Molecule Maker” Ionic Compounds Activity
Don’t Lose This Packet!
MATERIALS:
 Puzzle pieces
NOTE:Please be
sure all of your
puzzle pieces get put
back in thebox when
you are finished!
 Periodic
Table/Polyatomic
ions
 Data sheet
Background:
THE RULES OF THE PUZZLE
 Use the molecule makers to build molecules. Complete the charts with the information
you obtain from your models.

Remember these rules:
1. A molecule is correct only when the cards form a rectangle with no open spaces.
Ex:
2. The number of atoms of each element (or polyatomic ions) is written in the space below
the line and to the right of the symbol as a subscript. Ex. The “2” in H2O
3. When the number of atoms (or polyatomic ions) is one, the one is “understood” and you
do not write anything.Ex. H2O,NOTH2O1
4. The positive atom (or polyatomic ion) is written first in the formula.
Ex. Br-1 + Na+1 = NaBr
5. Use (parentheses) only when necessary that is, if there are more than one polyatomic
ion Ex. CaSO3 no parentheses needed
Ba3(PO4)2 needs parenthesis to show that there are 2 phosphate ions
Naming Ionic Compounds
1.
Naming Cations
a. Naming cations with one ionic charge (fixed charge)
i. The name of the cation is exactly the same as the name of the element. So a lithium atom (Li)
forms a lithium cation (Li+) and a magnesium atom (Mg) forms a magnesium cation (Mg2+).
b. Naming cations with more than one ionic charge –some transition or “other” metals
i. A Roman numeral in parentheses is used as part of the name of the element to indicate the
numerical value of the charge.
ii. Thus, the cation Cu+ is the copper(I) ion and is read as “copper one” while Cu2+ is the copper
(II) ion and is read as “copper two”.
2.
Naming Anions
a. The name of an anion uses the root of that atom name and ends in –ide. So a sulfur atom (S)
forms a sulfide (S2-) anion and a chlorine atom (Cl) forms a chloride anion (Cl-).
3.
Naming compounds with polyatomic ions
a. The name of the polyatomic ion is written unchanged with no Roman numerals. Thus, the
polyatomic ion phosphate is NEVER changed to phosphide.
1
Formula Writing I
Compound made of
Simple Binary Ionic Compounds
Atoms of each element
Formula
2 atom(s) of H
1. hydrogen and sulfur
1atom(s) of S
H2S
____ atom(s) of Ca
2. calcium and chlorine
3.
sodium
andphosphorus
____ atom(s) of Cl
____ atom(s) of Na
____ atom(s) of P
____ atom(s) of Al
4. aluminum and sulfur
____ atom(s) of S
____ atom(s) of ________
5. magnesium andoxygen
____ atom(s) of ________
____ atom(s) of ________
6. aluminum andchlorine
____ atom(s) of ________
____ atom(s) of ________
7. magnesium andfluorine
____ atom(s) of ________
____ atom(s) of ________
8. sodium and sulfur
____ atom(s) of ________
____ atom(s) of ________
9. hydrogen and oxygen
____ atom(s) of ________
____ atom(s) of ________
10. aluminum andoxygen
____ atom(s) of ________
____ atom(s) of ________
11. calcium andphosphorus
____ atom(s) of ________
____ atom(s) of ________
12. calcium and oxygen
____ atom(s) of ________
2
Formula Writing II
Monoatomic and/or
polyatomic ions
Ternary Ionic Compounds (compounds with radicals)
Number of Atoms
(cards)
Positive
ion
Negative
ion
Formula
1. magnesium and
hydroxide
_1__ atom(s) of Mg
_2_ atom(s) of OH
Mg2+
OH-
Mg(OH)2
2. potassium and
sulfate
___ atom(s) of _______
___ atom(s) of _______
___ atom(s) of _______
3. calcium and nitrate
___ atom(s) of _______
4. aluminum and
phosphate
___ atom(s) of _______
5. ammonium and
chlorine
___ atom(s) of _______
6. ammonium and
sulfur
___ atom(s) of _______
7. aluminum and
carbonate
___ atom(s) of _______
8. calcium and
carbonate
___ atom(s) of _______
9. hydrogen and
carbonate
___ atom(s) of _______
10. ammonium and
hydroxide
___ atom(s) of _______
11. sodium and
carbonate
___ atom(s) of _______
12. ammonium and
fluorine
___ atom(s) of _______
___ atom(s) of _______
___ atom(s) of _______
___ atom(s) of _______
___ atom(s) of _______
___ atom(s) of _______
___ atom(s) of _______
___ atom(s) of _______
___ atom(s) of _______
___ atom(s) of _______
3
Formula Writing III
Monoatomic
and/or
polyatomic
ions
1. calcium and
hydroxide
More Ionic Compounds containing Radicals
Positive
ion
Negative
ion
Formula
Compound Name
Number
of atoms
in
compound
Ca+2
OH-1
Ca(OH)2
calcium hydroxide
5
2. hydrogen and
sulfate
3. calcium and
carbonate
4. magnesium
and chlorine
5. ammonium
and sulfate
6. ammonium &
phosphate
7. aluminum
and nitrate
8. calcium and
carbonate
9. hydrogen &
carbonate
10. sodium and
hydroxide
11. lithium and
sulfate
12. strontium
&carbonate
13. fluorine and
ammonium
14. phosphate &
hydrogen
4
Formula Practice Sheet #1
Using what you learned in the "Molecule Maker" formula writing activities, complete the chart by writing the
correct formulas for the following compounds. The first one was been completed for you.
Name of Compound
1. sodium iodide
Positive ion
Negative ion
Formula
Na+
I-
NaI
2. silver sulfide
3. barium sulfate
4. lithium sulfide
5. sodium hydroxide
ClO3-
6. ammonium chlorate
7. zinc sulfate
Zn2+
8. iron(III) phosphate
Fe3+
9. nickel(II) hydroxide
Ni2+
10. chromium(III) oxide
Cr3+
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
5
Formula Writing/Counting Atoms #2
Monoatomic
and/or
polyatomic ions
Positive
ion
Negative
ion
Formula
Compound Name
Number
of atoms
in
compound
1. calcium and
nitrate
2. tin(IV) and
chloride
3. copper(II) and
carbonate
4. barium and
bromide
5. tin(II) and
sulfite
6. nitrate and
ammonium
7. lithium and
phosphorus
8. sodium and
bicarbonate
9. phosphate and
lead(II)
10. magnesium
&hydroxide
11. silver and
sulfide
12. barium and
acetate
13. fluorine and
manganese(II)
14. chromium(III)
and nitrate
15. sulfate and
iron(III)
6
Formula Writing/Counting Atoms #3
Monoatomic
and/or
polyatomic ions
Positive
ion
Negative
ion
Formula
Compound Name
Number of
atoms in
compound
1. chlorate and
calcium
2. nickel(II) and
sulfate
3. carbonate and
copper(I)
4. chlorine and
magnesium
5. tin(II) and
sulfate
6. ammonium
& phosphate
7. aluminum and
nitrate
8. calcium and
sulfite
9. iron(III) and
carbonate
10. hydroxide and
calcium
11. lithium and
sulfate
12. strontium and
carbonate
13. fluorine and
ammonium
14. chromium(III)
and oxide
15. phosphate &
iron(II)
7