Final Exam Review
I. Write the formula, the name, and type of intramolecular bond that would be formed for a compound made up
of
1. Calcium and Chlorine
3. Hydrogen and Oxygen
5. Lithium and Fluorine
2. Magnesium and Nitrogen
4. Sulfer and Carbon
6. Bromine and Silicon
II. Write formula for the following compounds
7. Iron (III) Iodide
8. Silver (I) Nitride
9. Tin (II) Phosphate
10. Aluminum Carbonate
11. Ammonium Oxide
12. Diphosphorous pentoxide
13. Xenon pentafluoride
14. Lead (IV) Arsenate
III.
15.
17.
19.
21.
Write names for3
N2O
KF5
Fe2(CO3)3
BF3
16. SO3
18. (NH4)2(SO4)
20. CuO
21. BeCl2
IV. Name the three types of intramolecular bonds, and describe the position/location of the valence electrons in
each.
V. Balance the following equations
22. H2 + N2  NH3
24. Pb3(AsO4)2 + Sn(SO3)4  PbSO3 + Sn3(AsO4)4
23. CaCl2 + HCl + O2  CaO + H2O + ClO3
25. Fe + O2  Fe3O4
VI. For each of the following, identify the type of reaction that would occur, write the name of the products that
would form, write and balance a complete molecular equation
26.
28.
30.
31.
Hydrogen + Sulfer
Potassium Carbide + Silver
F2 + Zn(NO3)2 
Lithium sulfate + Copper (II) Acetate
27.
29.
30.
32.
Magnesium sulfide + Oxygen 
Sodium Chlorate 
Al(OH)3 
Oxygen + Calcium 
VII. For each of the following, identify the type of reaction that would occur, write the name of the products
that would form, write and balance a complete molecular equation, ionic equation and a net ionic equation.
33. Hydrogen chloride (hydrochloric acid) reacts with sodium carbonate
34. Lead (IV) nitrate reacts with calcium bromide to form the precipitate Lead (IV) bromide
35. Ca(CN) + H2SO4 (sulfuric acid)
VIII. Show all work for the following calculations
36. What is the molar mass and percent composition of Nickle (VI) phosphate
37. What is the molar mass and percent water and anhydrate in Copper (I) carbonate tetrahydrate
38. How many atoms in 48.6 grams of Neon?
39. How many grams in 3.46 moles of Tin (IV) peroxide
40. How many molecules in .43 moles of carbon tetrachloride
41. A well-known reagent in analytical chemistry, dimethylglyoxime, has the empirical formula C2H4NO. If its
molar mass is 116.1 g/mol, what is the molecular formula of the compound?
42. Nitrogen and oxygen form an extensive series of oxides with the general formula NxOy. One of them is a
blue solid that comes apart, reversibly, in the gas phase. It contains 36.84% N. What is the empirical formula of
this oxide?
43. An unknown compound was found to have a percent composition as follows:
47.0 % potassium, 14.5 % carbon, and 38.5 % oxygen. What is its empirical formula? If the true molar
mass of the compound is 166.22 g/mol, what is its molecular formula?
44. If 3.65 x 1024 molecules of Aluminum carbonate reacts with 41 grams of sodium…
a. what type of reaction occurs?
b. Would it take place spontaneously?
c. What would the products be?
d. Write and balance the equation
e. Which reactant is the limiting reactant?
f. How many grams remain of each reactant after the reaction is complete?
g. How many grams of each product has been formed when the reaction has been completed.
h. What is the percent yield if 6.92 x 10 24 atoms of solid product are produced?
IX. For each of the following molecules: Draw a correct Lewis structure showing the correct molecular
geometry and labeling the angles, name the electron geometry, the molecular geometry, and the hybridization.
45. water
49. Nitrogen trihydride
46. Carbon dioxide
50. Silicon tetrafluoride
47. SF6
51. Nitrate ion
X. Determine which has the greater melting point. Explain why.
a. water
b. Carbon dioxide
c. SF6
48. ClO3152. NH2COOH
d. Nitrogen trihydride
XI. Determine the types of intermolecular and intramolecular bonds in each of the following, and describe the
interactions between molecules.
53. Carbon tetraflouride
54. water
55. Carbon monoxide
56. Sodium chloride