Download CDO AP Chemistry Unit 1 Review 2

CDO AP Chemistry
Unit 1 Review 2
1. Why is it that the vast majority of alpha particles that traveled through the gold foil in Rutherford’s experiment
experienced no deflection?
2. Describe the results of the experiment that proved electrons carry a negative charge.
3. What is an isotope?
Questions 4-7 refer to the U-238 isotope.
4. How many protons are contained within the nucleus?
5. How many neutrons are contained within the nucleus?
6. How many electrons are contained within a single neutral isotope of this element?
7. What is the mass of this isotope in amu?
CDO AP Chemistry Christman
Fall 2013
CDO AP Chemistry
Unit 1 Review 2
8. The three naturally occurring isotopes of magnesium are: magnesium-24 (23.985 amu), magnesium-25 (24.986
amu), and magnesium-26 (25.983 amu). Their percent abundances in nature are 78.99%, 10.00%, and 11.01%
respectively. What is the average mass of magnesium?
9. There are two naturally occurring isotopes of bromine: Br-79 (78.918 amu) and Br-81 (80.916 amu). What is the
percentage of each isotope?
10. What is the empirical formula of C4H10?
11. Is CO2 an empirical formula, a molecular formula, or both? Explain.
12. Calculate the mass percent of each element in CaCO3
CDO AP Chemistry Christman
Fall 2013
CDO AP Chemistry
Unit 1 Review 2
13. A vitamin C tablet from a certain company contains 70.0 mg of ascorbic acid (Vitamin C). The entire tablet,
however, has a mass of 0.825 g. Calculate the mass percent of Vitamin C in the tablet.
14. How many moles of acetic acid (CH3COOH) are contained within 24.71 g of acetic acid?
15. How many grams of NaOH are contained within 0.785 moles NaOH.
16. How many carbon atoms are contained in 84.3 g of ethyne (C2H2)?
17. Name the following ionic compounds:
a. Fe2O3
b. FeO
c. ZnCl2
d. AgNO3
e. PbO2
f.
PbSO4
CDO AP Chemistry Christman
Fall 2013
CDO AP Chemistry
Unit 1 Review 2
g. Mg3(PO4)2
h. NaHCO3
i.
KCN
j.
KMnO4
18. Write ionic formulas for the following compounds:
a. Sodium acetate
b. Tin(II) chloride
c. Calcium hydroxide
d. Ammonium sulfate
e. Manganese (II) hypochlorite
f.
Copper (II) nitrite
g. Nickel(II) chlorite
h. Lead (II) nitrate
i.
Potassium sulfide
j.
Aluminum oxide
CDO AP Chemistry Christman
Fall 2013
CDO AP Chemistry
Unit 1 Review 2
19. Name the following molecular compounds:
a.
CO
b. CO2
c. H2O
d. CCl4
e. N2O3
f.
SiO2
g. N2O4
h. CBr4
i.
SO2
j.
S2Cl2
20. Write molecular formulas for the following compounds:
a. Xenon hexafluoride
b. Tetranitrogen tetraoxide
c. Boron trifluoride
d. Carbon tetrabromide
e. Dicarbon tetrafluoride
CDO AP Chemistry Christman
Fall 2013
CDO AP Chemistry
f.
Unit 1 Review 2
Nitrogen tribromide
g. Dinitrogen tetrasulfide
h. Oxygen difluoride
i.
Dinitrogen pentaoxide
j.
Tetraphosphorus decaoxide
21. Write chemical formulas for the following compounds:
a. Carbon monoxide
b. Potassium sulfide
c. Potassium permanganate
d. Nitrogen trichloride
e. Nickel (II) sulfate
f.
Sodium acetate
g. Magnesium iodate
h. Sulfur trioxide
i.
Calcium carbonate
j.
Silver sulfide
CDO AP Chemistry Christman
Fall 2013
CDO AP Chemistry
Unit 1 Review 2
22. Name the following acids:
a. CH3COOH
b. HBrO3
c. H2CO3
d. H2SO4
e. HF
f.
HCl
g. HI
h. H2SO3
i.
HIO3
j.
HCN
23. Write chemical formulas for the following acids:
a. Perchloric acid
b. Nitric acid
c. Hydroiodic acid
CDO AP Chemistry Christman
Fall 2013
CDO AP Chemistry
Unit 1 Review 2
d. Acetic acid
e. Iodic acid
f.
Nitrous acid
g. Hydrochloric acid
h. Hydrobromic acid
i.
Chlorous acid
j.
Bromic acid
24. Write chemical formulas for the following hydrates:
a. Magnesium perchlorate hexahydrate
b. Calcium chromate dehydrate
c. Aluminum chloride hexahydrate
d. Copper (II) sulfate pentahydrate
e. Barium chloride dehydrate
CDO AP Chemistry Christman
Fall 2013
CDO AP Chemistry
Unit 1 Review 2
25. An experiment was performed in which a 5.00 g sample of aluminum metal was burned in oxygen to produce
9.45 g of aluminum oxide. Use this data to determine the empirical formula of the aluminum oxide.
26. When crystalline copper (II) sulfate, CuSO4 xH2O is heated in air above 100˚ C, it loses the water molecules and
also its blue color. If 9.60 g of CuSO4 is left after heating 15.01 g of the hydrate, calculate the number of moles of
water originally present in the compound and then determine the value of “x” in the formula.
CDO AP Chemistry Christman
Fall 2013
CDO AP Chemistry
Unit 1 Review 2
27. It was found that a compound contained 68.1% carbon 13.7% hydrogen and 18.2% oxygen by mass. Determine
the empirical and molecular formula of the compound if the molar mass is 176.34 g/mol.
Balancing Equations Balance the Following Equations
28. Ca + HOH  Ca(OH)2 + H2
29. Cl2O7 + H2O  HClO4
30. Fe + O2  Fe3O4
31. C6H14 + O2  CO2 + H2O
32. Ca3(PO4)2 + H2SO4  Ca(H2PO4)2 + CaSO4
CDO AP Chemistry Christman
Fall 2013
CDO AP Chemistry
Unit 1 Review 2
Stoichiometry
33. Answer the following questions for this equation: 2H2 + O2  2H2O
a. What is the H2/H2O ratio?
b. Suppose you had 20 moles of H2 on hand and plenty of O2, how many moles of H2O could you make?
c. What is the O2/H2O mole ratio?
d. Suppose you had 20 moles of O2 and enough H2, how many moles of H2O could you make?
34. Given the following equation: 2K + Cl2  KCl How many grams of KCl are produced from 2.50 g of K and
excess Cl2.
CDO AP Chemistry Christman
Fall 2013
CDO AP Chemistry
Unit 1 Review 2
35. Given the following equation: 2NaClO3  2NaCl + 3O2 How many grams of NaCl are produced when 80.0
grams of O2 are produced?
36. The reusable booster rockets of the U.S. space shuttle employ a mixture of aluminum and ammonium perchlorate
for fuel. A possible equation for this reaction is: 3Al(s) + 3NH4ClO4(s)  Al2O3(s) + AlCl3(s) + 3NO(g) +
6H2O(l) What mass of NH4ClO4 should be used in the fuel mixture for every kilogram of aluminum?
37. In the reaction PCl5 --> PCl3 + Cl2, 104.3 g of PCl5 are used, and 30.0 g of Cl2 are produced. What is the % yield
of Cl2 in this reaction?
CDO AP Chemistry Christman
Fall 2013
CDO AP Chemistry
Unit 1 Review 2
38. Methane (CH4) reacts with O2 to form CO2 and water. If 30.0 grams of CH4 and 64.0 grams of O2 are mixed and
the reaction goes to completion, how many grams of H2O will form?
39. How many grams of CO2 can be produced from 7.61 grams CS2 and 8.00 grams O2 in the following reaction:
CS2 + 3O2 --> CO2 + 2SO2
CDO AP Chemistry Christman
Fall 2013
CDO AP Chemistry
40. A
a.
b.
c.
Unit 1 Review 2
84.1 g sample of phosphorous reacts with 85.0 g oxygen gas to form diphosphorus pentoxide.
What is the limiting reactant?
What is the theoretical yield in grams of P2O5?
If only 123 g of P2O5 are produced, what is the percentage yield?
41. In the combustion of CH4 (methane) to give CO2 and water, when 10.0 grams of CH4 are mixed with 10.0 grams
of O2, how many grams remain (if any) of the reagent "in excess"?
CDO AP Chemistry Christman
Fall 2013
CDO AP Chemistry
Unit 1 Review 2
42. A 1.0857 g sample of a compound containing only carbon, hydrogen and oxygen was burned in excess oxygen.
3.190 g of carbon dioxide and 0.9360 g of water were produced. Find the empirical formula of the compound.
43. A confiscated white substance, suspected of being cocaine, was purified by a forensic chemist and subjected to
elemental analysis. Combustion of a 50.86-mg sample yielded 150.0 mg CO2 and 46.05 mg H2O. Analysis for
nitrogen showed that the compound contained 9.39% N by mass. The formula of cocaine is C17H21NO4. Can the
forensic chemist conclude that the suspected compound is cocaine?
CDO AP Chemistry Christman
Fall 2013