AP Chemistry Summer Review
Name______
AP Chemistry Summer Review
This assignment has been created to ensure that you are fully prepared for the first day of school. This review covers many of the main topics studied in your first year chemistry or Pre-AP Chemistry class. This material will be assessed within the topics studied in this course. The review allows for you to refresh your memory over the summer as well to ensure that you are ready to use these skills within the units that we will be studying. What many students find difficult about AP Chemistry is not the new content, but remembering to do all of the “little things” and utilizing your skills from Pre-AP Chem. Refer to the power points (see website or handout version or email Ms. Tirone for the powerpoints), the Zumdahl textbook (if you signed one out) or your first year chemistry class notes if you need help. Good luck and please feel free to email us with any questions you may have!
Email: Ms. Tirone- or
Mr. Demko-
We will be available in August at school for extra help- dates to be released August 1st- for updated information please sign up for Remind.com updates by texting: @apchemtiro to 81010
- Chemical Formulas
- Write formulas for the following substances:
- Barium sulfate
- Ammonium chloride
- Carbon monoxide
- Silicon tetrachloride
- Magnesium fluoride
- Sodium oxide
- Sodium sulfide
- Copper (I) iodide
- Zinc sulfide
- Potassium carbonate
- Hydrobromic acid
- Perbromic acid
- Lead (II) acetate
- Sodium permanganate
- Lithium acetate
- Potassium cyanide
- Iron (III) hydroxide
- Silicon dioxide
- Nitrogen trifluoride
- Chromium (III) oxide
- Calcium chlorate
- Sodium thiocyanate
- Cobalt (III) nitrate
- Nitrous acid
- Ammonium phosphate
- Potassium chromate
- Name each of the following compounds (Give acid names where appropriate)
- CuSO4
- PCl3
- Li3N
- BaSO3
- N2F4
- KClO4
- NaH
- (NH4)2Cr2O7
- HNO2
- Sr3P2
- Mg(OH)2
- Al2S3
- AgBr
- P4O10
- HC2H3O2
- CaI2
- MnO2
- Li2O
- FeI3
- Cu3PO4
- PCl3
- NaCN
- Cs3N
- Zn (NO3)2
- N2O
- HF
- Chemical Equations
Tell the type of reaction, predict the products and write a balanced chemical equation for each of the following, as shown in the example:(Hint: You may need the use of a solubility chart. Check in your textbook).
Ex: Solutions of silver nitrate and magnesium iodide are combined.
This is a double replacement reaction.
2AgNO3 + MgI2 2AgI + Mg(NO3)2
- Ammonium sulfate reacts with barium nitrate,
- Zinc metal is added to a solution of copper (II) chloride.
- Propane gas (C3H8) is burned in excess oxygen.
- Sodium hydroxide solution is added to a solution of iron (III) bromide.
- Chlorine gas is bubbled through a solution of sodium bromide.
- Solutions of lead nitrate and calcium iodide are combined.
- Sulfuric acid is combined with solid magnesium hydroxide.
- Isopropyl alcohol (C3H7OH) is burned in air.
- Iron metal shavings are added to hydrochloric acid.
- Sodium metal is added to distilled water.
- Mathematics and Chemistry
(Includes Stoichiometry, Gas Laws, Molarity, Percent Composition and Acid-Base Chemistry)
Please show ALL WORK. Include any and all relevant equations. Make sure to watch for SIGNIFICANT FIGURES. Please box your answers.
- Benzene contains only carbon and hydrogen and has a molar mass of 78.1 g/mol. Analysis shows the compound to be 7.74% H by mass. Find the empirical and molecular formulas of benzene.
- Find the mass percent of nitrogen in each of the following compounds:
- NO2
- N2O
- Calcium carbonate decomposes upon heating, producing calcium oxide and carbon dioxide gas.
- Write a balanced chemical equation for this reaction.
- How many grams of calcium oxide will remain after 12.25 g of calcium carbonate is completely decomposed?
- What volume of carbon dioxide gas is produced from this amount of calcium carbonate? The gas is measured at 0.95 atm and 10C.
- Hydrogen gas and bromine gas react to form hydrogen bromide gas.
- Write a balanced chemical equation for this reaction.
- How many grams of hydrogen bromide gas can be produced from 3.2 g of hydrogen gas and 9.5 g of bromine gas?
- How many grams of which reactant is left unreacted?
- What volume of HBr, measured at STP, is produced in b)?
- When ammonia gas, oxygen gas and methane gas (CH4) are combined, the products are hydrogen cyanide gas and water.
- Write a balance chemical equation for this reaction.
- Calculate the mass of each product produced when 225 g of oxygen gas is reacted with an excess of the other two reactants.
- If the actual yield of the experiment in part b is 105 g of HCN, calculate the percent yield.
- A 2.29 g sample of an unknown acid is dissolved in 1.0 liter of water. A titration required 25.0 ml of 0.500 M NaOH to completely react with all the acid present (neutralizing it). What is the molar mass of the acid?
- Cinnamic acid contains only carbon, hydrogen and oxygen, and is found by analysis to be 73.0% C and 5.4% hydrogen. In a titration, 18.02 ml of 0.135M NaOH is found to neutralize 0.3602 g of cinnamic acid.
- Find the empirical formula of this compound.
- Find the molar mass of this compound.
- Write the molecular formula for this compound.
- Potassium nitrate decomposes when heated, forming potassium nitrite and oxygen gas.
- Write a balanced chemical equation for this reaction.
- What mass of KNO3 would be needed to produce 18.4 liters of oxygen gas, measured at 775 mmHg and 15C?
- What mass of KNO2 would also be produced?
- If you combine 25 mL of 1.2 M lead (II) nitrate with 37 mL of 0.95 M hydrochloric acid, a precipitate forms. What is the precipitate and how many grams of it are formed? What is pH of the solution after the reaction?
- Ethyl alcohol melts at -114oC and boils at 78oC. The heat of fusion at -114oC is 105 J/g, and the heat of vaporization at 78oC is 870 J/g. If the specific heat of solid ethyl alcohol is taken as 0.97 J/g-oC and that for the liquid as 2.3 J/g-oC, how much heat is required to convert 16.0 g of ethyl alcohol at -130oC to the vapor phase at 78oC?