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Chemistry 1 Honors
June 2010
FINAL REVIEW
Chemical Bonding (Ch 6/7)
2. Give the correct names and formulas for ionic and covalent compounds.
Ex: Give the formulas for : a. lead (II) nitrate Pb(NO3)2
b. magnesium chloride MgCl2
c. dinitrogen pentoxide N2O5
d. nitric acid HNO3
Give the correct name for
a) CO2 carbon dioxide
b. CuSO4•5H2O copper (II) sulfate pentahydrate
c. FePO4 iron (III) phosphate
d. MgO magnesium oxide
3. Know how to draw Lewis structures for atoms and molecules including polyatomic ions and resonance
structures.. Ex: Draw the Lewis structures for
a) HF
b) PO43-
4. Know how to predict molecular shapes using VSEPR theory.
Ex: What is the shape a) NF3 trigonal pyramid b) H2S
v-shaped/angular
Chemical Equations and Reactions (Ch 8)
8. Know how to properly balance chemical equations: For example
a) Write a balanced chemical equation for the reaction where nitrogen gas and hydrogen gas combine to give
ammonia gas.
N2 + 3 H2 → 2 NH3 Synthesis/ combination
b) Write a balanced chemical equation for the reaction between sodium chloride and silver nitrate to produce
sodium nitrate and silver chloride.
NaCl + AgNO3 → NaNO3 + AgCl Double displacement
c) Write a balanced equation for the reaction where aluminum and lead (II) nitrate react to produce lead and
aluminum nitrate.
2 Al + 3 Pb(NO3)2 → 3 Pb + 2 Al(NO3)3
Single displacement
d) Write a balanced equation for the decomposition of calcium carbonate into calcium oxide and carbon
dioxide.
CaCO3 → CaO + CO2 decomposition/ analysis
e) Write a balanced equation for the complete combustion of propane (C3H8)
combustion
C3H8 + 5 O2 → 3 CO2 + 4 H2O
11. In the reaction of aluminum and lead nitrate (above) what was the mole ratio of lead (II) nitrate to aluminum
nitrate? 3:2
12. How many moles of nitrogen gas would be required to completely convert 6 moles of hydrogen gas to
ammonia? 2 moles
Stoichiometry (Ch 9 and selected calculations from Ch 3 and Ch 7 )
13. Determine the percent composition for Na2CO3 43.38% Na 11.33% C 45.285% O
14. What is the percent composition for a compound that contains 1.30 g of aluminum and 1.15 g of oxygen?
53.1% Al 46.9% O
15. An unknown compound is analyzed and found to contain 40.0% carbon, 6.67 % hydrogen, and 53.3%
oxygen. a) What is the empirical formula for the compound? CH2O
b) If the molar mass is 150 g/mol, what is the molecular formula? C5H10O5
16. What is the formula mass of Mg3(PO4)2? 262.855 amu What is the molar mass? 262.855 g
17. What is the mass of 4.5 moles of NaHCO3? 378 g
18. How many moles of HCH3COOH are in 53.4 g? .875 mol
Chemistry 1 Honors
June 2010
19. How many atoms of oxygen in the 53.4 g of HCH3COOH? 1.05 x 1024 atoms
20. N2O5 + H2O → 2 HNO3 (unbalanced equation)
a) When the equation is balanced, what is the mole ratio of N2O5 to HNO3?
b) How many moles of HNO3 will be produced when 0.51 mol of N2O5 react? 1.02 moles
21. Magnesium burns in oxygen to produce magnesium oxide. How many moles of oxygen are needed to burn
0.52 mol of magnesium? 0.26 mol
22. Determine the mass of zinc chloride produced when 5.30 g of zinc react with excess hydrochloric acid.
11.0 g
23. What mass of sodium chloride is produced when chlorine reacts with 0.29 g of sodium iodide? .113 g
24. CaCO3 + 2 HCl → CaCl2 + CO2 + H2O (unbalanced equation)
a) How many liters of carbon dioxide are produced at STP when 400.g of CaCO3 react with excess HCl?
89.5 L
25. When 0.75L of hydrogen react with bromine gas, what volume of hydrogen bromide gas will be produced?
1.5 L
26. 3Fe + 4H2O → Fe3O4 + 4H2
a) When 36.0 g H2O is mixed with 67.0 g Fe, what is the limiting reactant? Fe
b) What mass of iron oxide can be produced? 92.6 g
c) If 90.2 g of iron oxide are actually produced, what is the percent yield? 97.4%
Solutions (Ch 12 (part) + Ch 13 sec 1)
28. Write a net ionic equation for the reaction between BaCl2 and Na2SO4.
Ba2+ + SO42- → BaSO4
29. What is the molarity of a solution containing 0.303 mol KCl in 5.23 L of solution? .0579 M
30. What is the molarity of a solution containing 250 g NaCl in 3.00 L of solution? 1.43 M
31. How many moles of HCl are present in 0.65 L of a 0.33 M solution? .215 mol
32. What’s the volume of a 0.444 M solution of NaOH containing 2.45 moles of NaOH? 5.52 L
Acids and Bases (ch 14 and 15).
36. What is the pH of a solution containing 1.00 x 10-5 M H3O+ ions? 5 Is it acidic or basic? acid
37. If a solution has a pOH of 5.78 what is its pH? 8.22 Is it acidic or basic? basic
38. If a solution contains 2.30 x 10-8 M OH- ions what is [H3O+]?. 4.35 x 10-7M basic
39. What is the [H3O+] of a solution with pH = 10.3? 5.01 x 10-11 M What is its pOH? 3.7
Gases
48. A gas has a pressure of 608 mm Hg in a container with a volume of 545 cm3. If the container’s volume is
increased to 1065 cm3, what will the pressure of the gas be? 311 mm Hg
49. What will the volume of a gas sample be at 100. °C if its volume at 23.1 °C is 51.3 L? 64.6 L
50. If the pressure of a gas at 23 °C is 1.01 atm, what is its pressure at 35.0 °C? 1.05 atm
51. What is the partial pressure of oxygen in a flask at 1.20 atm if the flask contains nitrogen with a pressure of
0.50 atm, carbon dioxide at 0.60 atm and oxygen? .10 atm
55. How many moles of gas at 95.0 °C does it take to fill a 3.00 L flask to a pressure of 2.00 atm? .199 mol
56. What is the molar mass of a 2.18 g sample of gas that occupies 2.00 L at 1.02 atm and 25.0 °C? 26.1 g/mol
60. You have two balloons. Balloon 1 is filled with helium. Balloon 2 is filled with oxygen. How many times
faster is helium’s effusion rate compared to that of oxygen? 2.8 times faster
Reaction Energy (ch 16 sec 1)
63. What is the specific heat of a metal if a 35.0 g sample absorbed 48 J as it was heated from 293 K to 313 K?
.0686 J/g °c
64. If a piece of metal is heated from 10.0 °C to 60.0 °C, what is ∆T? 50.0 °c
Chemical Equilibrium (Ch 18 part)
69. 2CO(g) + O2(g) → 2CO2(g)
Chemistry 1 Honors
June 2010
Describe what happens if the above system comes to equilibrium and then more CO gas is added.
Equilibrium shifts right, decreases O2, increases CO2
Describe what happens if the above system comes to equilibrium and then the pressure is increased.
Equilibrium shifts right, decreases O2 and CO, increases CO2