Though this is a highly rigorous course, each of you is very capable of being successful; you wouldn t be enrolled in the course if you weren t.

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Alaina Preston
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1 Welcome to AP Chemistry! Congratulations, you have chosen to take one of the most challenging AP courses offered. AP Chemistry involves problem solving to integrate your laboratory, math and logical reasoning skills. This class will require you to spend more time than you are probably used to preparing for lab and class. You will be expected to work independently and in your lab groups a minimum of 5-6 hours per week, outside of class in order to prepare and understand the material. Given our short Dublin school year, you will be expected to meet outside of the normal class meeting times, staying into study blocks and evenings to finish the required lab component and to prepare for upcoming class projects. You will have assignments to do over breaks and weekends. Though this is a highly rigorous course, each of you is very capable of being successful; you wouldn t be enrolled in the course if you weren t. To ensure that we begin the year all in the same place, I am sending you this review packet. Inside you will find review questions which cover the range of material I expect you to know from your general chemistry course. Your summer assignment: Print the review packet Solve all problems, showing all of your work. No work, no credit Bring this packet to the first day of class to discuss and review. If you have trouble, you may use any high school chemistry textbook to help, such as McGraw Hill Chemistry Concepts and Applications, but you can borrow any chemistry text from your local library. Each of you need to purchase the Princeton Review Cracking the AP Chemistry Exam review book, 2016 edition (see classbooks.com) You will need to purchase a student lab notebook with spiral binding by Hayden McNeil with 100 carbonless duplicate sets. You must bring this lab notebook to the first day of class. (see classbooks.com) Also, you must purchase a college level chemistry textbook: Chemistry the Central Science by Brown/LeMay/Bursten or Chemistry by Zumdahl/Zumdahl. You can buy any edition. The most recent edition will be expensive. I like the Brown/LeMay/Bursten textbook. (see classbooks.com) Purchase a 3-ring binder and dividers. You will need a binder that is for chemistry only to track your materials throughout the year.!1

2 Bring back to school any materials you still have from previous chemistry courses, these can be helpful for review, and any textbooks you may have at home. I am really excited to have the opportunity to teach this course, I hope that you are ready to learn some chemistry and have some fun in the lab! Please me if you have any questions, See you in September!!2

3 !3

4 Draw the Lewis Dot Structures for the following elements: H Mg Na B O S F Ne He Ar For each of the following 1. determine oxidation numbers of each element 2. write symbols for each ion, positive ion first 3. write the formula for the compound (make sure that you have balanced the charges) 4. check that you have balanced the charges- overall charge of the formula is zero 1. Lithium and Sulfur a. b. c. d. 2. Boron and Fluorine a. b. c.!4

5 d.!5

6 Write the chemical formula for each of the following: Strontium fluoride Sodium hydroxide Manganese (III) chloride Manganese (VII) oxide Copper (II) phosphate Chlorine dioxide Dichlorine heptoxide Iron (III) oxalate pentahydrate Name the following compounds: remember the rules for naming compounds (ionic, covalent and transition metals) KI ZnCr2O7 PbCl2 Cr (OH)2 NO2 MgCO3 3H2O NiCl2 6H20 Cl2O Label the 4 parts of the following piece of the periodic table:!6

7 Arsenic 33 As Fill in the blanks in the table below for neutral atoms. Use only the information given in the table. Atomic number Mass number Number of protons Strontium Number of neutrons Mercury Uranium Number of electrons Tungsten Calculate the average atomic mass of magnesium using the following data for three magnesium isotopes. Show your work, be careful of significant figures, and show units. Isotope Mass (u) Fractional Abundance Mg Mg Mg !7

8 !8

9 a. Complete the table below: Element Period Mass Volume Density Al 3 1.1mL 2.70g/mL In g 7.31g/mL Tl g 1.4mL b. Using the data table above, with the period on the X-axis and the density on the Y-axis, draw a graph below. Label the x and y axes, and show units. c. Based on the graph from above, predict the density of Ga which is in the same group as Al, In and Tl, and in period 4. Show your prediction on the graph.!9

10 For each of the elements listed below a. Is this an ionic or a covalent compound? b. Name the compound c. Draw the Lewis Dot Structure for each of the elements before the reaction d. Draw the Lewis Dot structure for after the elements react 1. Li2O a. b. c. d. 3. CO2 a. b. c. d.!10

11 Write a balanced equation and indicate the reaction type (single displacement, double displacement, decomposition, synthesis, or combustion for each of the following reactions. 1. aluminum nitrate(aq) + sodium hydroxide(aq) aluminum hydroxide(s) + sodium nitrate (aq) 2. sulfur trioxide(g) sulfur dioxide(g) + oxygen(g) Determine the number of atoms of B in a 14.5g sample: Determine the number of moles in a sample of 1.45 x atoms of Cu Determine the mass in grams of 5.87 mol NaCl! 11

12 Balance the following chemical reaction, and then predict the mass of the following based on the chemical equations: HgO(s) Hg(l) + O2(g) How many grams of HgO are required to make 17.5 g Hg? How many moles of O2 are made if you begin the reaction with 12.2 g HgO? chlorine(g) + sodium iodide(s) sodium chloride(s) + iodine(g) 1. Write a balance chemical equation for the above reaction. 2. Calculate the theoretical yield of sodium chloride in grams, if 13.7 g of chlorine gas is used up in the reaction. (assume there is excess sodium iodide) 3. Calculate the percent yield if 18.4 grams of sodium chloride are produced.!12

13 25.0 L of oxygen gas react with iron metal to form of iron(iii)oxide at STP. How many grams of iron metal are needed to react with the oxygen gas? How many moles of iron(iii)oxide will be produced in this reaction? Fe(s) + O2(g) Fe2O3(s) Magnesium bromide(aq) + chlorine(g) magnesium chloride(aq) + bromine(g) If 41.3 L of bromine gas are produced at 25.0ºC and 2.30atm, a. How much chlorine gas (moles) was used up in the reaction? b. What would the volume of this chlorine gas have been at 1.00 atm and 25ºC?!13

14 What is the molarity of a solution prepared by dissolving mol of ethanol, C2H5OH, in enough water to make ml of solution? What mass of iron (III) chloride, FeCl3, is needed to prepare a 1.00 L of a 0.255M solution? Find the volume in ml of 0.75M Cu(OH)2 required to oxidize 35.0 ml of 0.60M MgHPO3 in acidic solution. Assume the reaction which occurs is the oxidation of HPO3 2- by Cu(OH)2 to give PO4 3- and Cu2O. (hint- REDOX- balance the reaction using the halfreaction method)!14

AP Chemistry - Ms. Ganz Welcome to AP Chemistry

AP Chemistry - Ms. Ganz Welcome to AP Chemistry AP is a college level course. The course is designed to be equivalent to the inorganic chemistry course usually taken during the first year of college. This