Chemistry 100
Review for Final
Attention:
Please study problem set 1, 2, and 11 as well. This review
does not contain these chapters.
1. Use the following ions to write the chemical formula for each ionic compound:
a) Ca2+
NO3-
b) Mg2+
SO42-
c) Fe2+
PO33-
d) Ga3+
N3-
2. Find the charge of each element/polyatomic ion in these ionic compounds:
a) Fe(ClO3)2
d) PbI2
b) HgHPO4
e) (NH4)2CO3
c) AlPO3
f) CuNO3
3. Find the name of the following compounds:
a) Ca(HSO4)2
e) SnO2
b) HF
f) LiClO
c) FeCO3
g) H3PO3
d) Al(OH)3
h) HClO2
4. Write the formula for the following compounds:
a) Boron trifluoride
d) Sodium dihydrogen phosphate
b) Hydrochloric acid
e) Barium permanganate
c) Ammonium carbonate
f) Carbon tetrachloride
Dr. Behrang Madani
Chemistry 100
IVC
5. Predict whether a precipitate will form when aqueous solutions of the following
compounds are mixed. If a precipitate will form, write its formula, and write a net ionic
equation. Identify the spectator ions.
a) K2SO4(aq) + Ba(NO3)2(aq) 
b) NaOH(aq) + H2SO4(aq) 
c) AgNO3(aq) + CuCl2(aq) 
d) AlCl3(aq) + Li2CO3(aq) 
6. Balance the following equations:
a) Na+(aq) + CO32-(aq) + Sr2+(aq) + Cl-(aq)  SrCO3(s) + Na+(aq) + Cl-(aq)
b) Cu + Zn2+  Cu+ + Zn
c) Al3+ + Fe  Al + Fe3+
d) Fe2+ + Cu2+  Fe3+ + Cu
7. In the following equations, which species are oxidized and which species are reduced?
Which ones are the oxidizing agents and which ones are the reducing agents?
a) 2Fe3+ + 3Ni  2Fe + 3Ni2+
b) C2H4O(l)+ H2O2(l)  C2H4O2(l) + H2O(l)
8. Identify each of the following unbalanced reaction equations as belonging to one or more
the following categories: precipitation, acid-base, oxidation-reduction, synthesis,
decomposition, single replacement, double replacement, or combustion.
a) I4O9(s)  I2O6(s) + I2(s) + O2(g)
Dr. Behrang Madani
Chemistry 100
IVC
b) HCl(aq) + AgC2H3O2(aq)  AgCl(s) + HC2H3O2(aq)
c) SiCl4(l) + Mg(s)  MgCl2(s) + Si(s)
d) Ca(OH)2(aq) + H2SO4(aq)  CaSO4(s) + H2O(l)
9. Considering the following reaction:
NaClO2(aq) + Cl2(g) → ClO2(g) + NaCl(aq)
If 78.3g of NaClO2 is used, how many grams of NaCl will be formed?
10. Lead(II) nitrate and aluminum chloride react according to the following equation:
3Pb(NO3)2 + 2AlCl3 → 3PbCl2 + 2Al(NO3)3
In an experiment, 8.00 g of lead nitrate reacted with 2.67g of alumium chloride to give 5.15 g
of lead chloride.
a) Which reactant was the limiting reagent?
b) What was the percent yield?
11. Using the equation:
Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)
If 105g of Fe2O3 reacts with 21g CO, what volume of CO2 gas will be formed at STP
condition?
12. Write the complete orbital box diagram, electron configuration, and noble gas notation
for each of the following elements/ions:
a) Iodine, Z = 53
Dr. Behrang Madani
Chemistry 100
IVC
b) Krypton, Z = 36
c) Se2-, Z = 34
d) Ba2+, Z = 56
13. Find the valence level and valence electrons for each of the elements/ions in problem 12.
14. Arrange the elements in each set in order of decreasing the size of the atom (by using only
the periodic table).
a) Ge, C, Si, Sn
b) Be, B, Li
c) K, Rb, Na, Li
d) Sr, I, Sb, Te
15. Arrange the elements in each set in order of increasing ionization energy (by using only
the periodic table).
a) As, Br, Se, Ga
b) P, As, N, Sb
c) Ba, Cs, Pb
d) Sr, Be, Ca, Mg
16. Find the location and the name of the following elements by using their electron
configurations.
a) 1s22s22p63s23p64s2
Dr. Behrang Madani
Chemistry 100
IVC
b) 1s22s22p63s23p64s23d104p65s1
c) 1s22s22p63s23p64s23d104p65s24d105p2
d) [Ar]4s23d104p4
17. What is the same and what is the difference in the electron configuration of:
a) Ca and Sr
b) P and As
18. Arrange the elements in each set in order of increasing electronegativity (by using the
periodic table).
a) As, N, P, Sb
b) O, C, N, F
c) Be, Sr, Ca, Mg
d) As, Se, Ga, Br
19. Draw the Lewis structure for each covalent compound.
a) CH3OCH3
b) CH3CH2OH
c) HCN
d) COCl2
20. Predict the shape of each molecule and bond angles by using VSEPR.
a) SCl2
b) CH3COOH
Dr. Behrang Madani
Chemistry 100
IVC
c) C2H2
d) P2H4
21. In problem 20, which of the molecules are polar? Why?
22. In K2O, use the electron configuration of potassium and oxygen and then K+ and O2- to
show how an ionic bond is produced between them. The electron configuration of potassium
ion and oxide ion are similar to which noble gases?
23. Describe how we would prepare the following solutions:
a) 280 mL of 27% v/v solution of ethanol, C2H6O, in water.
b) 623 mg gram of 13.7% w/w solution of coffee in water.
24. Find w/v % of a solution if 0.23 moles NaI is dissolved in water to make 2.3L solution?
25. Suppose 82.6g sucrose, C12H22O11, dissolved in enough water to give 725 mL solution.
What is the molarity of this solution?
Dr. Behrang Madani
Chemistry 100
IVC
26. Assuming that the volumes are additive. 263 mg of ammonium sulphate, (NH4)2SO4, is
dissolved in water to make 3.6L solution. If we add 1.2 L water to this solution, what would
be the molarity?
27. What mass of potassium chloride would be needed to precipitate the silver ion from 98
mL of 0.26 M AgNO3 solution?
KCl(aq) + AgNO3(aq) → AgCl(s) + KNO3(aq)
28. In question 27, how many molecules (formula) of silver chloride form when a 1.66 g of
KCl is added to 73 mL of 0.64 M AgNO3 solution?
29. Find the oxidation state (oxidation number) for each element in the following
molecules/ions.
a) S in H2SO4?
b) C in Na2CO3?
c) Cr and C in Cr(C2H3O2)2?
d) P in HPO42- ?
Dr. Behrang Madani
Chemistry 100
IVC
e) Cr in HCr2O7- ?
30. Given the unbalanced equation below:
Fe2+(aq) + Cr2O72-(aq) + H+(aq) → Fe3+(aq) + Cr3+(aq) + H2O(l)
a. identify the oxidation state of each element
b. identify the oxidizing agent
c. identify the reducing agent
31. Given the unbalanced equation below:
B2O3(s) + Cl2(g) → BCl3(l) + O2(g)
a. identify the oxidation state of each element
b. identify the oxidizing agent
c. identify the reducing agent
32. Blance each chemical equation using half-reactions method.
a) BrO3-(aq) + Cu+(aq) → Br-(aq) + Cu2+(aq)
b) S2O82-(aq) + Cr3+(aq) → SO42-(aq) + Cr2O72-(aq)
c) MnO4-(aq) + C2O42-(aq) → Mn2+(aq) + CO2(g)
Dr. Behrang Madani
Chemistry 100
IVC
33. A balloon contains 4 moles of an ideal gas with a volume of 5.0 L. If an additional 8
moles of the gas is added at constant pressure and temperature, what will be the final volume
of the balloon?
34. If 2.6 moles of nitrogen gas are confined to a 6.0 L vessel at 177 °C and 12.0 atm. If the
vessel is allowed to expand isothermically (constant temperature) to 36.0 L, what would be
the final pressure?
35. How many grams of nitrogen will occupy a 7.5 liter container at STP?
36. Suppose you have 56g of ammonia gas (NH3) at 264°F, occupying a container which is
500. mL in size. What is the pressure of this gas in atmospheres?
37. When sodium bicarbonate, NaHCO3(s), is heated. Sodium carbonate (Na2CO3) is
produced, with the evaluation of water vapor and carbon dioxide gas.
2NaHCO3(s)  Na2CO3(s) + H2O(l) + CO2(g)
What total volume of gas, measured at 29C and 769 torr, is produced when 1.50g of
NaHCO3(s) is completely converted to Na2CO3(s)?
38. Suppose that 4.18g of oxygen gas and 3.68g of nitrogen gas are confined in a 11.3-L
container at 36°C. What would be the pressure of container? Calculate the partial pressure of
each gas in this mixture.
Dr. Behrang Madani
Chemistry 100
IVC