Name:_________________
Naming Simple (Type I) Binary Ionic Compounds
Type I ionic compounds are made of a simple metal ion (one that can
only have one charge) and a nonmetal ion. To name the compound
simply write the name of the metal followed by the name of the
nonmetal with an –ide ending.
Example: CaCl2 = calcium chloride
Al2S3 = aluminum sulfide
Write names for the following Type I binary compounds:
1) MgS
11) K2S
2) KBr
12) LiBr
3) Ba3N2
13) Sr3P2
4) Al2O3
14) BaCl2
5) NaI
15) AlN
6) SrF2
16) SrS
7) Li2S
17) Na2O
8) RaCl2
18) MgF2
9) CaO
19) NaBr
10) AlP
20) Sr3P2
Page 1
Writing formulas for Type I Binary Compounds
Since the compounds are ionic (metal with a nonmetal) you
MUST BALANCE THE CHARGES when you write the formula. So please follow the
following steps
a) Write out the formulas and charges for both the positive and negative ions.
b) Combine the ions into a formula so the charges cancel each other out.
Example:
Lithium Oxide = Li+1 and O-2 = Li2O
Aluminum chloride = Al+3 and Cl-1 = AlCl3
For each of the following ionic compounds please do the following:
a) write the symbol and charge for each of the ions
b) write the formula for the compound (so that the charges cancel out)
1) beryllium bromide
9) aluminum sulfide
a)
a)
b)
b)
2) magnesium oxide
10) strontium chloride
a)
a)
b)
b)
3) magnesium sulfide
11) lithium selenide
a)
a)
b)
b)
4) cesium fluoride
12) beryllium phosphide
a)
a)
b)
b)
5) barium sulfide
13) rubidium bromide
a)
a)
b)
b)
6) potassium nitride
14) radium arsenide
a)
a)
b)
b)
7) lithium oxide
15) sodium iodide
a)
a)
b)
b)
8) calcium chloride
16) zinc chloride
a)
a)
b)
b)
Page 2
Name:_______________
Naming Type I Compounds that Contain Polyatomic Ions
When naming compounds that contain polyatomic ions (the ones you have
memorized from page 100 in your book). If they contain simple metals, that
can only have one charge, simply name the metal and name the polyatomic ion.
Example: Li2SO4 = Lithium sulfate
Mg(ClO3)2 = magnesium chlorate
Name the following type I compounds:
1) Li2SO3
8) Ba(C2H3O2)2
2) CsCN
9) Sr(OH)2
3) Ba(NO2)2
10) K2SO3
4) Na2SO4
11) NH4Cl
5) Ca3(PO4)2
12) Be(ClO2)2
6) Al(NO3)3
13) LiMnO4
7) MgCO3
14) NaHCO3
Page 3
Writing Formulas for Compounds with Polyatomic Ions
When writing the formula for an ionic compound that contains polyatomic ions you
MUST BALANCE THE CHARGES of the ions. The only new thing is that if you need
more than one of a polyatomic ion you must put in ( ) with the number you need outside.
If only one of the polyatomic ions is needed leave out the ( ).
Example: Strontium Hydroxide = Sr+2 and OH-1 = Sr(OH)2
Calcium Carbonate = Ca+2 and CO3-2 = CaCO3
For each of the following ionic compounds please do the following:
a) write the symbol and charge for each of the ions
b) write the formula for the compound (so that the charges cancel out)
17) Magnesium sulfate
25) Barium nitrate
a)
a)
b)
b)
18) Calcium nitrate
26) Cesium chlorite
a)
a)
b)
b)
19) Ammonium hydroxide
27) Sodium cyanide
a)
a)
b)
b)
20) Sodium carbonate
28) Magnesium hydroxide
a)
a)
b)
b)
21) Strontium phosphate
29) Potassium permanganate
a)
a)
b)
b)
22) Aluminum sulfite
30) Calcium bicarbonate
a)
a)
b)
b)
23) Barium nitrite
31) Calcium nitrite
a)
a)
b)
b)
24) Sodium bicarbonate
32) Aluminum acetate
a)
a)
b)
b)
Page 4
Name:_______________
Writing Formulas of Compounds with Transition Metals that form More than
One Charge (Section 4.1, pages 89-93)
-
the Roman numeral tells you the charge of the cation (metal)
charges of ionic compounds must add up zero!!!!
Write the formulas of the following compounds:
1) iron (II) sulfide
5) manganese (IV) phosphide
2) copper (I) nitride
6) lead (II) nitride
3) cobalt (III) chloride
7) copper (II) sulfide
4) nickel (II) bromide
8) cobalt (II) phosphide
Naming Compounds Containing Metals that form More than One Charge
(Section 4.1, pages 89-93)
-
these compounds are ionic, so NO PREFIXES!!!!
add a Roman numeral after the cation to indicate the charge of the cation
determine the total negative charge and work backwards to determine the cation charge
Name the following compounds:
1) CuCl
________________________
5) CrS
__________________________
2) Fe2O3
________________________
6) MnN
__________________________
3) PbCl4
________________________
7) FeCl3
__________________________
4) HgO
________________________
8) Cr2O3
__________________________