IONIC COMPOUNDS
Write the correct formula and name for the following combinations of elements when they
form ionic compounds.
Steps …
1.
Find the correct charge for each ion
2.
Make total positives = total negatives
3.
Name metal first and non-metal 2nd with the ending “ide”
a.
hydrogen and chlorine
b.
hydrogen and oxygen
c.
lithium and sulphur
d.
potassium and nitrogen
e.
beryllium and chlorine
f.
magnesium and sulphur
g.
calcium and sulphur
h.
i.
lithium and potassium
potassium and oxygen
Name the following ionic compounds
NaCl
BaO
H 2S
CaF2
K2O
BBr3
CaBr2
KI
Predict the formulae for the following
(Don’t forget to make the compound’s total ionic charge neutral)
sodium oxide
aluminum oxide
magnesium nitride
magnesium iodide
rubidium oxide
strontium fluoride
lithium nitride
calcium nitride
IONIC COMPOUNDS
Write the correct formula and name for the following combinations of elements when they
form ionic compounds.
Steps …
1.
Find the correct charge for each ion
2.
Make total positives = total negatives
3.
Name metal first and non-metal 2nd with the ending “ide”
j.
hydrogen and chlorine
H1+ Cl1-
HCl
hydrogen chloride
k.
hydrogen and oxygen
H1+ O2-
H 2O
hydrogen oxide
l.
lithium and sulphur
Li1+ S2-
Li2S
lithium sulphide
m.
potassium and nitrogen K1+ N3-
n.
beryllium and chlorine
Be2+ Cl1-
BeCl2 beryllium chloride
o.
magnesium and sulphur
Mg2+ S2-
(Mg2S2)
p.
calcium and sulphur
Ca2+ S2-
CaS
q.
lithium and potassium
Li1+ K1+
?????
r.
potassium and oxygen
K1+ O2-
K2O
Li3N lithium nitride
Name the following ionic compounds
NaCl
sodium chloride
BaO
barium oxide
H 2S
hydrogen sulphide
CaF2
calcium fluoride
K2O
potassium oxide
BBr3
boron bromide
CaBr2
calcium bromide
KI
potassium iodide
MgS
magnesium sulphide
calcium sulphide
potassium oxide
Predict the formulae for the following
(Don’t forget to make the compound’s total ionic charge neutral)
sodium oxide
Na1+ O2-
Na2O
sodium oxide
aluminum oxide
Al3+ O2-
Al2O3
aluminum oxide
magnesium nitride
Mg2+ N3-
Mg3N2
magnesium nitride
magnesium iodide
Mg2+ I1-
MgI2
magnesium iodide
rubidium oxide
Rb1+ O2-
Rb2O
rubidium oxide
strontium fluoride
Sr2+ F1-
SrF2
strontium fluoride
lithium nitride
Li1+ N3-
Li3N
lithium nitride
calcium nitride
Ca2+ N3-
Ca3N2
calcium nitride
What if an atom has more than one ionic charge???
 Some metals on the periodic table have ___ or ___ ionic
_________ (affects how they form ionic compounds)
 e.g. Copper can have ionic charge ___ or ____
What happens when these two different forms of copper
make a compound with chloride?
Ionic Charges:
__
__
__
__
Cu
Cl
Cu
Cl
Balance charges: (__) + (__) = __
Chemical formula:
Name:
____
copper (I) chloride
(__) + __(__) = __
____
copper (II) chloride
*use Roman numerals to describe the ionic charge for the
metal (only necessary if there is more than one possible ionic
charge!)
Roman Numerals
I, II, III, IV, V, VI, VII, VIII, IX ,X
Write formulae for the following:
tin (II) fluoride
copper (II) bromide
iron (II) oxide
manganese (IV) sulphide
tin (IV) nitride
What if an atom has more than one ionic charge???
 Some metals on the periodic table have two or more ionic
charges (affects how they form ionic compounds)
 e.g. Copper can have ionic charge 1+ or 2+
 What happens when these two different forms of
copper make a compound with chloride?
Ionic Charges:
1+
1-
2+
1-
Cu
Cl
Cu
Cl
Balance charges: (1+) + (1-) = 0
Chemical formula:
Name:
(2+) + 2(1-) = 0
CuCl
CuCl2
copper (I) chloride
copper (II) chloride
*use Roman numerals to describe the ionic charge for the
metal (only necessary if there is more than one possible ionic
charge!)
Roman Numerals
I, II, III, IV, V, VI, VII, VIII, IX ,X
Write formulae for the following:
tin (II) fluoride
Sn2+ F1-
SnF2
copper (II) bromide
Cu2+ Br1-
CuBr2
iron (II) oxide
Fe2+ O2-
FeO
manganese (IV) sulphide
Mn4+ S2-
(Mn2S4)
tin (IV) nitride
Sn4+ N3-
Sn3N4
MnS2
To figure out the charge on the metal from the formula start with the
NON-metal (i.e. the 2nd element that ends in “ide”)
1. You can always predict the charge of the anion because it will not change
(just count families)
2. Count how many of the non metal are present and multiply this times the
charge … this will give the total negatiive charge
3. The total positive charge must be the same size as the total negative
charge so that the compound can remain electrically neutral.
4. Divide this total positive charge by the number of metal elements present
and this will give the charge on each metal.
5. Write the name using the correct roman numeral
e.g.
1.
2.
3.
4.
5.
Fe2O3
O (oxide) is always -2
3 O’s present so total negative charge is 3 x (-2) = -6
Total positive charge must be +6 (to balance the -6 of the oxides)
+6 / 2 Fe atoms = +3 so each Fe atom must be charge +3
Name this compound iron (III) oxide
Name the following compounds using the Roman Numeral System:
PbCl2
FeO
NiCl2
PbCl4
Fe2O3
NiCl3
To figure out the charge on the metal from the formula start with the
NON-metal (i.e. the 2nd element that ends in “ide”)
6. You can always predict the charge of the anion because it will not change
(just count families)
7. Count how many of the non metal are present and multiply this times the
charge … this will give the total negatiive charge
8. The total positive charge must be the same size as the total negative
charge so that the compound can remain electrically neutral.
9. Divide this total positive charge by the number of metal elements present
and this will give the charge on each metal.
10. Write the name using the correct roman numeral
e.g.
Fe2O3
6. O (oxide) is always -2
7. 3 O’s present so total negative charge is 3 x (-2) = -6
8. Total positive charge must be +6 (to balance the -6 of the oxides)
9. +6 / 2 Fe atoms = +3 so each Fe atom must be charge +3
10. Name this compound iron (III) oxide
Name the following compounds using the Roman Numeral System:
PbCl2
FeO
NiCl2
Lead (II) chloride
Iron (II) oxide
Nickel (II) chloride
PbCl4
Fe2O3
NiCl3
Lead (IV) chloride
Iron (III) oxide
Nickel (III) chloride