AP CHEMISTRY THINGS TO KNOW Diatomic Molecules H2-hydrogen gas (do not write H) N2-nitrogen gas (do no write N) O2-oxygen gas (do not write O) F2-fluorine gas (do not write F) Cl2-chlorine gas (do not write Cl) Br2-liquid bromine (do not write Br) I2-solid iodine (do not write I) Strong Acids (H 1+ ) Strong Bases (OH 1- ) HCl-hydrochloric acid HBr-hydrobromic acid HI-hydroiodic acid HNO3-nitric acid H2SO4-sulfuric acid HClO3-chloric acid HClO4-perchloric acid Group 1: LiOH, NaOH, KOH, RbOH, CsOH, FrOH Group 2: Sr(OH)2, Ba(OH)2, Ca(OH)2 Solubility Rules 1. Compounds containing Na 1+ or K 1+ metal cations or the NH4 1+ are soluble. 2. Compounds containing NO3 1- anions are soluble. Periodic Table 1. Know where on the periodic table are the alkali metals, alkaline earth metals, transition metals, halogens, noble gases, lanthanides, and actinides. 2. Know where on the periodic table are the metals, nonmetals, and metalloids. STRUCTURE OF THE ATOM REVIEW PART I: Define the terms and explain the major contributions of each of the following people to our understanding of the atom: 1. John Dalton 2. J.J Thomson 3. Ernest Ruthergord 4. James Chadwick 5. Robert Millikan 6. Democritus 7. Proton 8. Neutron
9. Electron 10. Nucleus 11. Ion 12. Isotope 13. Mass number 14. Atomic number 15. Alpha particle 16. Nucleon 17. Cathode ray tube PART II: Fill in the following table. Symbol C F 1- U Na 1+ Atomic Number 99 Mass Number 14 Protons Neutrons Electrons 12 36 REVIEW: NOMENCLATURE (YOU NEED TO KNOW YOUR CHARGES) PART I: Define the following terms: 1. atom 2. ion 3. cation 4. anion 5. isotope 6. monoatomic 7. organic 8. molecular 9. molecule 10. element 11. compound 12. polyatomic 13. inorganic PART II: Write the names of the following ionic compounds (Metal + Nonmetal/Polyatominc Ion) 1. BaCl2
2. KCl 3. Na2SO4 4. K3PO4 5. Cr2O3 Molecular Compounds (Nonmetal + Nonmetal and insert Greek prefixes when needed) 1. SF4 2. CO2 3. N2O4 4. H2O 5. ClO2 PART III: Write the name. 1. nitrogen trifluoride 2. chlorine dioxide 3. sulfur hexafluoride 4. nitrogen dioxide 5. copper (I) fluoride 6. copper (II) fluoride 7. ammonium acetate PART IV: Fill in formulas for the following combination of ions. Cs 1+ Ca 2+ Al 3+ K 1+ NH4 1+ F 1- S 2- SO4 2- PO4 3- PART V: Are the following chemical or physical changes. 1. Breaking glass 2. Burning wood 3. Making brownies 4. Heating water REVIEW: TYPES OF REACTIONS AND BALANCING PART I: Balance and write the type 1. Al + Cl2 à AlCl3 2. FeCl3 à Cl2 + Fe
3. C + O2 à CO2 4. AlCl3 à Al + Cl2 5. Ag + S8 à Ag2S 6. Fe2O3 + H2O à Fe(OH)3 7. H2 + O2 à H2O 8. HNO2 à N2O3 + H2O 9. HCl + Mg(OH)2 à MgCl2 + H2O 10. CH4 + O2 à CO2 + H2O 11. CCl4 + HF à CCl2F2 + HCl 12. Na + H2O à NaOH + H2 13. BaCO3 + HCl à H2O + CO2 + BaCl2 14. BrF3 + TiO2 à TiF4 + Br2 + O2 15. Mg + CuSO4 à MgSO4 + Cu PART II: Predict the product of the following reactions and balance. 1. Mg + HCl à 2. SrCO3 à 3. K2O + H2O à 4. CH4 + O2 à 5. HCl + NaOH à PART III: Define the following terms or write the symbol. 1. solid 2. liquid 3. aqueous 4. precipitate 5. yields 6. produces 7. heat 8. exothermic 9. endothermic 10. coefficient 11. Given the following reaction: HCl + NaOH à NaCl + H2O a. Name the reactants b. Name the products PART IV: Write and balance the equations represented by words below. 1. Sodium metal reacts with water to form sodium hydroxide and hydrogen gas. 2. The combustion of methane (CH4) to make carbon dioxide and water.
3. Hydrochloric acid reacts with sodium hydroxide to make water and sodium chloride. 4. Calcium carbonate decomposes to make carbon dioxide and calcium oxide. 5. Calcium carbonate and hydrochloric acid to produce carbon dioxide, water, and calcium chloride. REVIEW: THE MOLE PART I: Determine the molar masses of these compounds: (a) NaOH (b) Ag2CO3 (c) (NH4)2CO3 PART II: Solve the following mole problems and correct number of significant figures. 1. How many moles of aluminum are there is 15.32 g of aluminum? 2. How many moes of NaCl are there in 152.3 g of NaCl? 3. How many grams of Pb are there in 0.535 moles of lead? 4. How many molecules of propane (C3H8) are in 30.0 g of propane? 5. Calculate the molarity of 10.0 g NaCl in 200.0 ml of solution? 6. How many grams of NaOH are need to prepare 1.50 L of a solution that is 0.200 M? PART III: Find the % composition of percent by mass composition: 1. H2O 2. Na2SO4 PART IV: Find the empirical and molecular formulas. 1. Hydroquinone is an organic compound commonly used as a photographic developer. It has a molar mass of 110.1 g/mol and a composition of 65.45% C, 5.45% H, and 29.09% O. Calculate the molecular formula of hydroquinone. 2. Fructose is a very sweet natural sugar that is present in honey, fruits, and fruit juices. It has a molar mass of 180.1 g/mol and a composition of 40.0% C, 6.70% H, and 53.3% O. Calculate the molecular formula of fructose.
PART V: Solve the following dilutions: Useful information: M1 x V1 = M2 x V2; sketch and label bottles showing the following dilutions! 1. What will be the molarity of the resulting solutions made by mixing the following? a. 200. ml 12 M HCl + 200. ml water b. 60.0 ml 0.60 M ZnSO4 + 500. ml water 2. Calculate the volume of concentrated reagent required to prepare the diluted solutions indicated: a. 12 M HCl to prepare 400. ml of 6.0 M HCl b. 15 M NH3 to prepare 50. ml of 6.0 M NH3 REVIEW: STOICHIOMETRY 1. Given the equation C + SO2 à CS2 + CO2 (a) How many grams of CO2 can be formed from 0.512 mol of C? (b) If the reaction produces 40.6 g of CO2, how many moles of SO2? (c) How many moles of CS2 can be made from 1.00 mol of C? (d) How many grams of CO2 of C are needed to produce 221 g of CS2? 2. The reaction for the combustion of propane is C3H8 + O2 à CO2 + H2O (a) If 5.0 mol of C3H8 and 5.0 mol of O2 are reacted, how many moles of CO2 can be produced? (b) If 3.0 mol of C3H8 and 20.0 mol of O2 are reacted, how many moles of CO2 can be produced? 3. Iron was reacted with a solution containing 400. g of copper (II) sulfate. The reaction was stopped after 1 hour, and 151 g of copper was obtained. Calculate the percent yield of copper obtained. Fe + CuSO4 à Cu + FeSO4 4. Silver bromide was prepared by reacting 200.0 g of magnesium bromide and an adequate amount of silver nitrate. Calculate the percent yield if 375.0 g of silver bromide was obtained from the reaction: MgBr2 + AgNO3 à Mg(NO3)2 + AgBr