1. What are type I compounds are composed of?
Metal cation with only one charge and a non-metal anion
2. Given the compound formula of a type II compound, example FeO, how does
one determine the charge on the cation?
By using the charge on the anion to determine the total negative and positive
charge within the compound
3. When working with type III compounds why is charge not considered?
Type III compounds are covalent, no charges
4. What are type II compounds composed of?
A metal cation with multiple charges and a non-metal anion
5. What does the Roman numeral in a type II compound represent?
The charge on the cation
6. Why can the quantities of a type I compound be ignored when naming the
compound? Example: MgF2 is called Magnesium fluoride, the 2 is ignored.
Yes they can. Since both ions have a single charge there is only one possible
ratio, MgF2, that can form a neutral compound
7. What are type III compounds composed of?
Two nonmetals covalently bonded
Name each of the following:
8. Al2S3
Aluminum sulfide
9. FeO
Iron (II) oxide
10. SO2
Sulfur dioxide
11. MgO
Magnesium oxide
12. MgCl2
Magnesium chloride
13. ZrN
Zirconium (III) nitride
14. CsI
Cesium iodide
15. Na3N
Sodium nitride
16. CBr4
Carbon tetrabromide
17. BeCl2
Beryllium chloride
18. NiCl
Nickel (I) chloride
19. LiBr
Lithium bromide
20. KCl
Potassium chloride
21. MgI2
Magnesium iodide
22. IBr
Iodine monobromide
23. MnO2
Manganese (IV) oxide
24. Why can’t any of the polyatomic ions we’ve studies be part of a type III
compound?
They are ions and type III compounds are covalently bonded (no charges)
25. What type of compound (I, II, or III) does NH 4+ always form and why?
Type I, definitive single oxidation state
Write the compound formula for the following:
26. Iron (III) bromide
FeBr3
27. Calcium iodide
CaI2
28. Iodine pentafluoride
IF5
29. Vanadium (III) oxide
V2O3
30. Lithium sulfide
Li2S
31. Magnesium iodide
MgI2
32. Cobalt (II) Sulfide
CoS
33. Manganese (IV) carbonide Mg2C
34. Oxygen difluoride
OF2
35. Potassium Chloride
KCl
36. Barium phosphide
Ba3N2
37. Chromium (III) nitride
CrN
38. Aluminum sulfide
Al2S3
39. Iron forms both 2+ and 3+ cations. Write the formulas for the oxide, sulfide,
and chloride compound of each iron cation and give the appropriate name
for each compound.
FeO – Fe2O3 - FeS – Fe2S3 – FeCl2 – FeCl3
40. Nitrogen and oxygen form numerous binary compounds, including NO, NO2,
N2O4, N2O5, N2O. Give the name of each of these compounds.
Nitrogen monoxide – Nitrogen dioxide – Dinitrogen tetroxide
dinitrogen pentoxide – dinitrogen monoxide
41. Most metallic elements form oxides, and often the oxide is the most common
compound of the element that is found in the earth’s crust. Write the
formulas for the oxides of the following metallic elements
a. Potassium
K2O
b. Magnesium MgO
c. Zinc(II)
ZnO
d. Lead(II)
PbO
e. Aluminum
Al2O3
42. In which of the following pairs is the name incorrect? Give the correct name
for the formulas indicated.
f.
g.
h.
i.
j.
Ag2O, disilver monoxide
Silver (I) oxide
N2O, dinitrogen monoxide Correct
Fe2O3, Iron (II) oxide
Iron (III) oxide
PbO2, lead oxide
Lead (II) oxide
Cr2O3, chromium (III) oxide Correct