Name: ____________________________
Ionic Bonding Review
We’ve already done the bonding unit, but you’ll need to know how atoms bond ionically in the next unit on
Chemical reactions. You have all the information and prior resources to refresh yourself on how to form ionic
compounds and to finish this packet. It will be due Monday!!!
Ionic bonding occurs between a metal and a nonmetal. As you know, opposite charges attract.
Ionic bonding is when two ions of opposite charge attract and bond to each other forming an ionic compound.
Consider the following examples of formulas for ionic compounds:




One Na+ (sodium ion) and one Cl- (chloride ion) bond to make NaCl, “sodium chloride.”
One Mg2+ (magnesium ion) and two F- (fluoride ion) bond to make MgF2, “magnesium fluoride.”
Three Ca2+ (calcium ion) and two N3- (nitride ion) bond to make Ca3N2, “calcium nitride.”
One Al3+ (aluminum ion) and one N3- (nitride ion) bond to make AlN, “aluminum nitride.”
1. Consider the formula NaCl in the above example. It tells us that one Na+ ion is bonded to one Cl- ion. What is
the overall charge for NaCl? Is it positive, negative, or neutral?
2. Consider MgF2.
a) What is the charge on a magnesium ion?
b) What is the charge on a fluoride ion?
c) What is the overall charge on MgF2? Note: The formula “MgF2” tells us that one Mg2+ ion bonds with two Fions.
3. What is the overall charge on any ionic compound?
4. Calcium nitride is written like this: Ca3N2
a) What is the charge on one calcium ion?
b) What is the charge on one nitride ion?
c) In the formula, Ca3N2, there are 3 calcium ions. What is the total charge on 3 calcium ions? (Hint: multiply 3
times your answer to part a.)
d) In the formula, Ca3N2, there are 2 nitride ions. What is the total charge on 2 nitride ions? (Hint: multiply 2
times your answer to part b.)
e) Why MUST it written like Ca3N2and not something like CaN2 or Ca2N3? (Hint: think about what your answers
to part c and d equal when added together.)
5. How do you ALWAYS write an ionic compound’s formula? (Hint: is the cation or anion first?)
6. What is wrong with the formula P2Na3? Write the correct formula.
7. Write the formula when the following atoms bond ionically:
a. lithium and chlorine
h. Bromine and calcium
b. barium and sulfur
i.
Nitrogen and beryllium
c. magnesium and iodine
j.
Phosphorus and strontium
d. oxygen and aluminum
k. Calcium and selenium
e. calcium and phosphorus
l.
f.
m. Gallium and sulfur
sodium and sulfur
g. Aluminum and nitrogen
Oxygen and radium
n. Lithium and phosphorus
Transition Metals: Remember, the elements in the d-block don’t have a set charge to them. Their charges can
change depending on the anion they are bonded to. The two exceptions are Silver (Ag) is +1 and Zinc (Zn) is +2. You
need to find the overall anion’s charge in order to find the transition metals charge.
8. Find the charge of the transition metal in each formula. Remember, you’re finding the charge of just one atom
of that metal.
Ex) Fe2O3 = one Fe atom = +3
a. CoO
f.
SnI2
b. CrCl3
g. HgBr2
c. MnBr2
h. AuCl3
d. CrP
i.
HgS
e. NiF2
j.
Au2O3
Polyatomic ions: Polyatomic ions are treated just like regular ions. They have an overall charge to them that allows
them to bond ionically with other ions. Here’s a list of the polyatomic ions you’ve worked with:
Phosphate: (PO4)3Cyanide: (CN)Sulfate: (SO4)2Ammonium: (NH4)+
Nitrate: (NO3)
Acetate: (C2H3O2)2Carbonate: (CO3)
Hydroxide: (OH)9. Write the formula for the following compounds.
a. Potassium phosphate
e. Copper (II) Cyanide
b. Gold (III) carbonate
f.
c. Zinc sulfate
g. Sodium Acetate
d. Silver nitrate
h. Potassium Carbonate
Aluminum Hydroxide
i.
Ammonium Sulfate
k. Chromium (IV) Nitrate
j.
Calcium Hydroxide
l.
Barium Phosphate
Balancing Equations: To complete a chemical reaction, you must understand how the reactants bond ionically to
form the compounds. You must also balance a reaction for it to be complete. Remember, when balancing you want
equal numbers of each atom on both sides of the reaction. Start with an atom that is unbalanced on both sides and
balance it by ONLY ADDING COEFFICIENTS to the front of the compound/molecule.
Balance the following equations:
Mg 
1.
HCl +
2.
Na2S +
Be(OH)2 
3.
BaF2 +
NaNO3 
4.
Ca3(PO4)2 +
5.
Zn(NO3)2 +
Mg 
6.
Ca(NO3)2 +
Al2(CO3)3 
7.
C4H8
+
O2
8.
Al2(CO3)3
+
9.
Li
10.
Na2CO3
11.
Mg
+
CuCl 
MgCl2
12.
CaCl2 +
Al(NO3)3

Ca(NO3)2
+
AlCl3
13.
Ca3(PO4)2
+
Al

Al(PO4)
+
Ca
14.
C3H8
+
O2

CO2
H2O
15.
Ca
+
O2

CaO
16.
N2O5 
N2
+
O2
+
MgCl2
+
Na(OH)
+
BeS
Ba(NO3)2
+
NaF
K2SO4 


K3PO4
Mg(NO3)2
CO2

Na
+
+
+
CaCO3
+
Na(NO3) 
Br2
H2
CaSO4
Zn
+
Al(NO3)3
H2O
Al(NO3)3 +
Na2CO3
LiBr
C
+
O2
+
+
Cu