Name AP Chemistry Summer Assignment Welcome to AP chemistry! This summer assignment is intended to help you review the basic topics you learned in pre-ap chemistry that are crucial for your success in AP chemistry. Topic 1: Nomenclature Topic 2: Chemical Reactions Topic 3: Percent Mass Topic 4: Molarity & Dilutions Topic 5: Stoichiometry Topic 6: Electron Configurations & Orbital Diagrams Topic 7: Gas Laws Topic 8: Periodic Trends Topic 9: Lewis Dot Structures & Intermolecular Forces Topic 10: ph Calculations I will be having a review session for the students that took regular chemistry instead of pre-ap chemistry on August 16 th & 17 th from 9:00AM 12:00PM. Students from pre- AP chemistry that want the extra review are also welcomed! This review packet will be due on August 31 st, 2018 by 2:15PM. You will have a nomenclature quiz on 9/3/18 or 9/4/18 depending on when our class meets. So, memorize the polyatomic ions on page 2. If you have questions about this summer assignment, feel free to e-mail me: gomezsz@pwcs.edu or stop by my classroom 2201 before the end of this school year. I hope you have a wonderful summer. Sincerely, Ms. Gomez 1
Topic 1: Nomenclature This is a very important part of AP chemistry. You must review and memorize all the polyatomic ions. You are expected to know how to name and write chemical formulas from day 1. 2
Directions: Write the formula for the following compounds 1. Lithium nitrate 2. Barium carbonate 3. Calcium sulfate 4. Iron (III) hydroxide 5. Aluminum hydroxide 6. Silver nitrate 7. Silver chloride 8. Lead (II) chloride 9. Lead (IV) oxide 10. Copper (II) phosphate 11. Copper (I) oxide 12. Ammonium nitrate 3
13. Sodium acetate 14. Potassium chloride 15. Barium hydroxide 16. Sulfur hexachloride 17. Dinitrogen tetroxide 18. Carbon tetrachloride 19. Phosphorous trichloride 20. Arsenic pentachloride 21. Sodium oxalate 22. Lithium carbonate 23. Potassium perchlorate There will be a quiz on nomenclature and writing formulas on 9/3/18 or 9/4/18. 4
Topic 2: Chemical Reactions Predict the product and write a balanced chemical equation. 1. Sodium metal reacts with water. 2. Lithium metal reacts with a solution of hydrochloric acid (HCl). 3. Magnesium metal is reacted with nitrogen gas. 4. Calcium hydroxide reacts with sodium sulfate. 5. Calcium carbonate is strongly heated in a crucible. 6. Zinc metal is reacted with a solution of copper (II) sulfate. 5
Topic 3: Percent Mass 1. What is the percent mass of carbon in C2H6? 2. How many grams of hydrogen are in a 15.0g sample of C2H6? 3. What is the percent mass of chlorine in PCl3? 4. How many grams of chlorine are in a 5.0g sample of PCl3? 5. What is the percent mass of water in CuSO 4 5H 2 O? 6. How many grams of water are in a 2.50g sample of CuSO 4 5H 2 O? 7. How many grams of fluorine are in a 6.00g sample of SF6? 6
Topic 4: Molarity and Dilutions 1. How many grams of KCl are needed to make a 2.0L solution with a 3.0M concentration? 2. Determine the molarity of a solution that has 58.0g of Na 2 SO 4 dissolved in 3.5L of solution. 3. What volume of water is needed to make a 3.5L solution of 2.0M HCl from a stock solution that has a concentration of 12.0M? 4. What s the volume of a solution that has a concentration of 3.0M and contains 85.0g of KNO3 dissolved? 5. What s the concentration of a 200.0mL solution that has 25.0g of AlCl3 dissolved? 7
Topic 5: Stoichiometry 1. (a) If 15.0g of aluminum chloride are decomposed, how many liters of chlorine gas are produced at STP? AlCl 3 Al + Cl 2 (b) If 5.0g of aluminum chloride are decomposed, how many liters of chlorine gas would be produced at 15.0 and 98kPa? Hint: use PV=nRT to solve for the moles of chlorine gas needed; then do stoichiometry. 2. If 6.0g of zinc metal react with 25.0mL of 2.00M HCl solution, how many liters of H2 would be produced at 25 and 99kPa? Zn + HCl ZnCl 2 + H 2 8
3. How many liters of oxygen gas are produced at STP from the complete combustion of 34.0g of methane gas, CH4, with excess oxygen gas? 4. How many grams of CaSO 4 are produced when 25.0mL of 2.3M solution of CaCl2 react with excess Na2SO4? CaCl 2(aq) + Na 2 SO 4(aq) CaSO 4(s) + 2NaCl (aq) 5. How many grams of Cu(OH)2 are produced from the reaction of 25.0mL of 3.0M CuCl2 with excess NaOH? 9
Topic 6: Electron Configurations and Orbital Diagrams 1. Write the full electron configuration for the following atoms. a. Silicon b. Calcium c. Cobalt 2. Write the noble gas electron configuration for the following atoms. a. Arsenic b. Phosphorous c. Gold d. Copper 3. Draw the orbital diagram (arrows and boxes) for the following atoms. a. Beryllium b. Boron c. Magnesium d. Aluminum 10
Topic 7: Gas Laws 1. A 250mL sample of nitrogen gas (N2) has a pressure of 99kPa at 25. If the pressure is increased to 113 kpa and the temperature drops to 10, what would be the new volume, in liters? Assume the number of moles remains constant. 2. The volume of 21.0g of oxygen gas (O2) is 15.6L and the pressure is 2.5 atm. Calculate the temperature. 3. The volume of 5.0 moles of nitrogen gas is 7.0L. What would be the volume, in ml, of 13.0 moles, assuming the temperature and the pressure remain constant? 4. How many grams of CO2 gas occupy a volume of 750mL at 1.3atm and 20.0? 11
Topic 8: Periodic Trends 1. Arrange the following atoms by increasing (small big) atomic radius. Mg, Ca, Si, O, Se Ni, B, Ge, Sr, Ba Ge, As, B, Al, Cl 2. For each set, identify the ion with the largest ionic radius. Al +3, O 2, S 2, Mg +2 Mg +2, Ca +2, Se 2, Br 3. Arrange the following atoms by increasing (low high) electronegativity. Mg, Al, Ca, Ar N, P, Cl, I Ti, Co, Al, Ne 4. Arrange the following atoms by increasing ionization energy. Si, S, Ar, Br Ca, Be, P, Br 12
Topic 9: Lewis Dot Structures In Lewis dot structures, the least electronegative element goes in the center, except for hydrogen. When a compound is organic, the carbon is placed in the center. If more than one carbon is present, they re first connected with a single bond and the rest of the atoms are distributed evenly. More bonds are used between the carbons as needed. Draw the Lewis dot structure for each molecular and determine the molecular geometry, polarity, and main type of intermolecular force for the compound. CH2O CF2H2 C2H2 Molecular Geometry Molecular Geometry Molecular Geometry Polarity Polarity Polarity Main Intermolecular Force Main Intermolecular Force Main Intermolecular Force 13
PCl3 CBr3F BF3 Molecular Geometry Molecular Geometry Molecular Geometry Polarity Polarity Polarity Main Intermolecular Force Main Intermolecular Force Main Intermolecular Force H2O NH3 HF Molecular Geometry Molecular Geometry Molecular Geometry Polarity Polarity Polarity Main Intermolecular Force Main Intermolecular Force Main Intermolecular Force 14
Topic 10: ph Calculations 1. Determine the ph of the following solutions. a) A solution with a hydroxide ion concentration of [OH ]=1.6x10 3 M b) A solution with a hydrogen ion concentration of [H + ]=1.6x10 2 M c) A solution with a hydroxide ion concentration of [OH ]=2.6x10 8 M d) A solution with a hydrogen ion concentration of [H + ]=4.6x10 13 M 2. Find the concentration for hydroxide [OH ] and hydrogen ions [H + ] from the ph or poh given. a) poh= 3.02 [OH ]= [H + ]= b) ph= 11.99 [OH ]= [H + ]= c) ph = 9.95 [OH ]= [H + ]= d) poh= 9.01 [OH ]= [H + ]= 15