Welcome to AP Chemistry
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- Wesley Carpenter
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1 Dear AP Chemistry Student: Welcome to AP Chemistry We hope you are ready for a fun, yet challenging year. AP Chemistry involves really understanding chemistry concepts and being able to apply them to all sorts of different problems. Students who finish AP Chemistry come out with a much better understanding of the world around them as well as a great sense of accomplishment. AP Chemistry is a difficult class, but with motivation and effort, you will definitely succeed. This document contains the Required AP Chemistry Summer Assignment. The work for this assignment is due the first day of class and will count as a homework assignment. Separate documents contain Summaries of Review Topics and Optional Practice Problems and Answers that you may find useful to try. We will spend the first week of school reviewing Significant Figures, Dimensional Analysis, Writing Formulas, Naming Compounds, Balancing Equations, and Stoichiometry. Each day there will be a quiz on the material reviewed the previous day. We encourage you to form a study group and begin by working on the summer assignment together. The course is much easier if you have a support system. If you are having problems on the assignment, please feel free to contact Ms. Caruso at scaruso@cpsd.us or Ms. Zhaurova at izhaurova@cpsd.us. Remember, this assignment is review of Chemistry so if you are feeling overwhelmed you may want to talk to us about the pacing and structure of the course to see if it is a good fit for you. Have a great summer! Can t wait to work with you next year! The CRLS AP Chemistry Teachers, Ms. Caruso Ms. Zhaurova Summer Assignment: Where there are blank spots, you should take notes on that particular topic. Use the Summaries of Review Topics, your notes from CP or HN Chemistry, or look around online. Documents may be found on Aspen on the AP Chemistry Page. After logging onto Aspen, click on Page Directory and add the AP Chemistry Page (it s the one with the flask icon.) You may need to log out and back in to see the icon. Check out the College Board website to see the Big Ideas, Learning Objectives and Science Practices that are included in the AP Chemistry Curriculum. 1
2 Review of Chemistry Topics AP Chemistry Ms. Caruso and Ms. Zhaurova Write notes in the empty spaces using information from the summary packet: General Information for Finding Significant Figures of a Number Rules for Calculations Using Significant Figures When multiplying and dividing: When adding and subtracting Perform the following calculations using the rules for significant figures. On the first line, write the unrounded calculation and on the second line, write the rounded calculation m x m = = m 2 42 m = = ml ml + 6 ml = = g 28.9 g = = cm x 3.2 cm x cm = = cm cm cm = = m 3 4 m = = kg kg = = mm x mm x mm = = x 10 3 m x 10 2 m = = **If you aren t sure, use 3 significant figures on the AP exam!** 2
3 Metric prefixes and conversions Complete conversions. Show work below and answers on the line. 1. Convert 125 ml to L 5. Convert 36.5 g to kg 2. Convert 734 nm to m 6. Convert 9.8 mg to kg 3. Convert mg to µg 7. Convert 87 ml to cm 3 4. Convert 1.6 mg to g 8. Convert 0.75 L to cm 3 Temperature Conversion Use summary packet to fill in this information: To Kelvin from Celsius: To Celsius from Kelvin: 1. Convert 86 C to K: 1. Convert 300 K to C: 2. Convert 21 C to K: 2. Convert 352 K to C: Classification of Matter Basics Use the summary packet/other resources to help you fill in these notes/questions. Matter 3
4 1. Describe how each type of matter can be separated/broken down. Element: Compound: Heterogeneous Mixtures: Homogeneous Mixtures: 2. Classify the following as an element, compound, heterogeneous mixture, or homogeneous mixture. a. Mud b. Carbon c. NaCl (aq) d. H 2 e. CO f. Sugar water g. Air h. Carbon dioxide 3. Which technique would you use to separate a suspended solid from a liquid? a. Distillation b. Chromatography c. Filtration 4. Determine if the following if a chemical change or a physical change? a. Melting Ice b. Burning Wood c. Cutting Paper d. Boiling water e. Dissolving f. Combustion g. Freezing water h. Evaporating perfume Review Atomic Structure Use the summary packet to fill in the information below: Subatomic Particle Location Mass Charge Proton Neutron Electron 4
5 Mass # is equal to How to determine # protons _ How to determine # neutrons How to determine # electrons in a neutral atom Element Name Atomic Symbol Atomic Number Mass Number Number of Protons Number of Electrons Number of Neutron Sodium Hydrogen Oxygen Chlorine Argon Periodic Table Basics Use the summary packet/other resources to help you with this section. 1. What are the rows called in the periodic table: 2. What are the columns called in the periodic table: 3. How is the periodic table organized? _ Group 1A Group 2A Group 3A Group 4A Group 5A Group 6A Group 7A Group 8A Name N/A N/A N/A N/A # Valence electrons Charge of Ion 5
6 Memorizing Polyatomic Ions Memorizing the polyatomic ions is VERY important for you to quickly write and name formulas. You are expected to know them all year. For each of the 25 polyatomic ions listed below, you will make an index card. To save cards, cut each card in half. On one side of the card, write the name of the ion, on the other side write the formula and charge. Whenever you get a free moment, look at one side of the card and guess the other side. Have your mom, brother, friend quiz you with them. Keep doing this for one week and you should have them memorized. Selected Polyatomic Ions H 3 O + hydronium OH hydroxide NH 4 + CO 3 2 HCO 3 PO 4 3 NO 2 NO 3 O 2 2 Hg 2 2+ C 2 H 3 O 2 CH 3 COO ammonium ClO 3 carbonate CrO 4 2 hydrogen carbonate Cr 2 O 7 2 phosphate MnO 4 nitrite SO 3 2 nitrate SO 4 2 peroxide HSO 4 dimercury (I) S 2 O 3 2 acetate (both forms) ClO ClO 2 CN cyanide ClO 4 SCN thiocyanate C 2 O 4 2 chlorate chromate dichromate permanganate sulfite sulfate hydrogen sulfate thiosulfate hypochlorite chlorite perchlorate oxalate Hydrogen Carbonate is also called Bicarbonate. You should know both forms of acetate You need to be able to go from the name to the ion (with the correct charges) and from the ion to the name. Sometimes grouping them by charge helps. Create your own practice quiz where you actually have to write your answers. This is much different than just flipping over flash cards. There will be a quiz on this during the first two weeks of school. 6
7 Review Writing Formulas from Names of Ionic Compounds Write Notes from Summary Packet of writing formulas for ionic compounds: 1. ammonium phosphate 9. iron (II) oxide 2. iron (III) oxide 10. lead (II) nitrate 3. calcium chloride 11. potassium nitrite 4. magnesium hydroxide 12. aluminum sulfate 5. copper (II) sulfate 13. lead (IV) chromate 6. copper (I) sulfate 14. potassium permanganate 7. sodium bicarbonate 15. zinc nitrate 8. aluminum sulfite 16. sodium thiocyanate Review Naming Ionic Compounds Write Notes from the summary packet here on naming: ***Zinc 2+ and Silver + do not need Roman Numerals*** 1. FeSO 4 _ 9. FeCl 3 _ 2. CuC 2 H 3 O 2 _ 10. PbSO 4 _ 3. Fe 2 O 3 _ 11. NaHSO 4 _ 4. Ag 2 SO4 _ 12. NiBr 3 _ 5. ZnCO 3 _ 13. Al(OH) 3 _ 7
8 Review Writing Formulas of Covalent Compounds and Acids From Names Write Notes from summary packet here on writing formulas for covalent compounds: 1. carbon monoxide 4. dinitrogen pentoxide 2. carbon tetrachloride 5. hydrochloric acid 3. sulfur trioxide 6. nitric acid Review Naming Covalent Compounds Write Notes from summary packet here on naming covalent compounds and acids: 1. CO 2 _ 4. HBr _ 2. N 2 O 4 _ 5. H 2 SO 4 _ 3. CBr 4 _ 6. H 2 SO 3 _ Review Balancing and Classifying Equations Classify and Balance the following Equations as Synthesis, Decomposition, Single Replacement, Double Replacement, and Combustion. 1. N 2 + H 2! NH 3 2. KClO 3! KCl + O 2 3. AlBr 3 + K 2 SO 4! KBr + Al 2 (SO 4 ) C 8 H 18 + O 2! CO 2 + H 2 O C 3 H 8 + O 2! CO 2 + H 2 O 6. Na + H 2 O! NaOH + H 2 8
9 Write the conversion factors on each line: Review Mole Conversions Mass (g) Particles (atoms, molecules) Mole Volume (L) Do the following conversions: 1. What is the molar mass of K 2 SO 4? 2. What is the molar mass of Ca 3 (PO 4 ) 2? moles of C 6 H 12 O 6 to grams g of KMnO 4 to moles 5. How many grams are there in 1.5 x molecules of CO 2? 9
10 6. How many grams are in a sample of NH 3 gas occupies 75.0 liters at STP? 7. How many atoms are there in 1.3 x molecules of NO 2? 8. A 5.0 gram sample of O 2 is in a container at STP. What volume is the container? 9. a. How many molecules of O 2 are in the container in Problem 6? b. How many oxygen atoms are there? Review Stoichiometry Use the equation below for questions C 4 H O 2! 8 CO H 2 O 1. What is the number of moles of butane (C 4 H 10 ) needed for producing 3 moles of CO 2? _ 10
11 2 C 4 H O 2! 8 CO H 2 O 2. How many grams of water will be produced if 10 g of butane were reacted with excess oxygen? _ 3.What volume of butane at STP is needed to produce 20 g of CO 2? _ 4. How many molecule of carbon dioxide are produced from 3 moles of butane? _ Concentration Molarity Basics Use online resources to help you with this section: Formula for Molarity: 1. How many moles of NaCl are dissolved in a 0.2 M solution of 500 ml? 2. How many liters of solution yields a 0.5 M solution made of 3.5 moles of NaOH? 3. A 1500 ml solution with 100 g of KOH completely dissolved, calculate the molarity. 11
12 4. Calculate the molarity of a 750 ml solution with 54 g of HCl completely dissolved. 5. Calculate the molarity of a 1.0 L solution with 94.5 g of HNO 3 completely dissolved. Formula for a Dilution: 1. How much concentrated 18 M sulfuric acid is needed to prepare 250 ml of a 6.0 M solution? 2. How much concentrated 12 M HCl is needed to prepare 100 ml of a 2.0 M solution? 3. How much concentrated 6 M acid is needed to prepare 500 ml of a 3 M solution? **End of Summer Assignment** 12
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