Student Name: __________________________ Book# ________________

AP Chemistry Summer Work Packet

All students taking Honors or AP science courses are required to complete a review packet prior to the start of the course. Each course’s packet is designed to help the student review material that was learned in prerequisite science classes. The material is necessary for the student to successfully begin the honors/AP course that he/she has chosen. A pretest will be administered the first day of class to assess the students’ knowledge of the science concepts covered in the packet. This pretest will not be reflected on the marking period grade, however the work done in the summer packet will be graded. The teacher will personally consult with the parent/student to discuss their future in the class if: 1. the student does not show adequate knowledge of the subject material covered on the pretest. 2. the student does not complete the summer work packet by the first day of class. 3. the student does not hand in the summer work packet on the first day of class. I have read and understand the information written above. Student signature: ______________________________________________ Parent/guardian signature: ________________________________________ I attest that all of the work contained in this packet is my own. Student signature: ______________________________________________ To: Parents/Guardians of students in Mr. Huie’s Chemistry classes We will be using a program called Mastering Chemistry this year in our classes. It is an internet accessed program designed to tutor and help student practice fundamental concepts in our class. With it, we can monitor how much time is spent practicing, doing homework, and reviewing concepts. It comes highly recommended, and will aid in the learning required in this course. It costs $23 + $2 shipping for a 1 year subscription and will be accessible from any network or computer. You can review the program at Masteringchemistry.com. Please send in the money as soon as possible with your child, so that the subscriptions can be ordered in a timely fashion. Please sign this note and have it returned to me to verify that you have received this information. If you have any questions, please feel free to contact me. Regards, Mr. Huie rphuie@gmail.com ______________________________ ____________________________ Student Name Parent Signature

AP Chemistry Summer Packet Mr Huie

rphuie@gmail.com - feel free to email me with questions over the summer WELCOME to AP chemistry! The AP curriculum includes all of the topics and the labs that we need to complete before the 2015 AP test on Monday, May 4th. All of you will find AP chemistry to be challenging, some of you will find it to be down-right hard. There is a lot to cover and while we can do it we will all need to work very hard. You should expect this class to be SIGNIFICANTLY more difficult than your first chemistry class. This means that we cannot slow down if you don’t understand a topic. You need to make sure that you are staying up with all assignments, and coming in for help if you need extra help. We need to use our class time effectively so the goal of this summer packet is that you will have reviewed much of the material from your first chemistry class. We will not just review material from before. This assignment should be completed and ready to turn in by the FIRST day of class in September , no excuses. We will have take-home work over all academic year breaks (Thanksgiving, Winter, and Spring) this will be to cover and review material without wasting class time. WHY DO WE HAVE TO DO SUMMER WORK? - It is a review of basic content covered in chemistry I, which you may not have seen for over a year. - It provides the necessary fundamentals you will need to be successful in AP chemistry. To not do the summer assignment or to do it poorly is to seriously endanger your prospects of being successful in AP chemistry. - There will not be enough time before the AP exam in May to cover the necessary content without this head start. Students are encouraged to work together to complete the summer assignment. THAT DOES NOT MEAN COPY! You should spread the out the following assignments over several weeks. Do not try to cram them in towards the end of the summer or you will get stressed out before school starts. AP Chemistry will be taught with the assumption that all students are taking the AP exam in the spring. AP Chemistry First Day Test – will consist of the following areas, be prepared! 1) polyatomic ions (including name, symbol, and charge) 2) Variable charges for transition metals 3) Naming Acids 4) Naming Ionic Compounds 5) Naming Covalent Compounds 6) Using sig. figs appropriately SO WHAT IS THE SUMMER WORK? All work should be done neatly and clearly on paper and organized in the order it was assigned. All work for every problem including units throughout is necessary for AP. This is an expectation on the AP exam in the spring and we want to get into the good habit early _____ Part 1 - Memorize Charges of Common Ions - If you know me or had me before you know I believe this is a vital part of AP chemistry. They will not give you an ion chart so it is essential that you have this done prior to school beginning. I suggest notecards and lots of practice. _____ Part 2 – Read and Review Pages in Book

– Reading implies taking notes(mapping) on any topics you are not familiar with or do not understand so that you will have them to study from AND/OR to ask me questions in the fall. GET USED TO READING! This is ABSOLUTELY necessary for AP Chemistry! Your book will be: Brown/LeMay/Bursten: Chemistry A Central Science 11e AP. - Chapter 1: Matter and Measurement o Everything in this chapter is basic but important. You may skim through if you find it easy. Learn all of table 1.4 (S.I. Base units) except Luminous intensity, and table 1.5. o Make sure you know the names of the common devices in figure 1.20 on page 17. o Pay particular attention to rules for significant figures.

- Chapter 2: Atoms, Molecules, and Ions o Simple review. All sections are important. - Chapter 3: Stoichiometry: Calculations with Chemical Formulas o Be sure to know general types of reaction and how to balance. o Be able to perform all types of math. o Get general idea of mass spectrometry.

- It is highly recommended that you do advanced reading and note-taking on chapter 4,6,7 and 8 as well as these will be near the beginning of the course and will be covered very quickly because they are a review of chemistry I.

_____ Part 3 – Complete the practice problems provided. _____ Part 4 – LAST PART – Come to school in the fall with your COMPLETED Summer packet - Scientific calculator. It does not need to be a graphing calculator, though you are welcome to use a graphing calculator if you already have one. - a LARGE notebook (2 or 3 inches) to be designated exclusively to AP CHEMISTRY - I HIGHLY RECOMMEND HAVING an AP exam review workbook. Any will do. Pick one that you feel comfortable with. I will be using the Princeton Review book Remember on the AP exam you must show all work including units or you will lose points. If you get the correct answer but do not show work you will not receive any points. (Accordingly, in this class and this packet credit will NOT be given for answer-only responses!) SO. . . you need to show all work for every problem including - equation you will be using (if applicable) - knowns/unknowns (if applicable) - plugged in equation and any algebraic work

Chapter 1 : 1. States of Matter : Classifying them by both physical state and composition Pure Substances and knowing the differences between Elements vs.

Compounds Mixtures or “solutions” 2. Properties of Matter Physical vs. Chemical properties Intensive vs. extensive properties Changes of State 3. Units of Measurement Matter are quantitative Know how to use Scientific measurements which is the metric system How to use and determine SI units ; Length , Mass and Temperature etc 4. Uncertainty in Measurement Precision is how closely individual measurement to another vs. Accuracy

refers to how closely individual measurement agrees with CORRECT value.

Significant Figures ; all digits of a measure quantity 5. Dimensional Analysis Using significant figures and the metric system for conversions Questions 1.2 Classify each of the following as a pure substance or a mixture, if a mixture indicate whether it’s a homogeneous or heterogeneous mixture : a) air , b) tomato juice ; c) iodine crystals ; d) sand . 1.19 Perform the following conversions: a) 25.5mg to g ; b)4.0 X 1010 m to nm; c)0.575mm to um 1.29 Make following conversions a) 62°F to degrees C ; b) 216.7°C to degrees F; c) 233°C to degrees K; d) 315° K to degrees F; e) 2550°F to degrees K 1.36 Indicate the numbers of significant figures in each of the following measured quantities ? A)1282 kg; b) 0.00296 s; c) 8.070mm; d) 0.0105 L e) 9.7750 X 10¯4cm 1.37 Round each the following numbers to four significant figures, and express the result in standard exponential notation: a) 300.235800; b)456.500; c)0.006543210; d) 0.000957830; e)50.778 X 10³; f) - 0.035000 1.68 A 32.65-g sample of a solid is placed in a flask. Toluene , in which the solid is insoluble, is added to the flask so that the total volume of the solid

and liquid together is 50.000mL . The solid and toluene together weigh 58.58 g . The density of toluene at the temperature of the experiment is 0.864 g/mL. What is the density of the solid ? Chapter 2 1. Atomic Theory Atom are building blocks of matter ; John Dalton Theory Atomic Structure ; subatomic particles Radioactivity given off 2. Atomic Structure Proton , Neutron , electrons Quantity Electronic charge Atomic Mass vs. Isotopes vs. Mass Numbers Knowing how to calculate the Atomic Weight 3.Periodic table Knowing how to read the P.T Know how to name and count by Groups 4. Molecules vs. Chemical Formulas Molecular Compounds Molecular Formulas Empirical Formulas 5 Ions and Ionic Compounds Cation vs. Anion [ knowing the difference and identifying each in a

compound ] Polyatomic ions Charges of Cations and Anions 6.Naming for Formulas Prefixes used for naming binary compounds formed between nonmetals Rules for naming anions in a acidic formula Questions 2.11The radius of an atom of Krypton is about 1.9 A. a)Express this distance in nm and in pm. b)How many Krypton atoms would have to be a lined up to span 1.omm? C)If the atoms is assumed to be a sphere, where is the volume in a cm³ of a single Kr atom ? 2.29 For the following elements, write its chemical symbol, locate it in the periodic table, and indicate whether it is a metal, metalloid, or a nonmetal: a)silver; b)helium; c)phosphorus; d)cadmium; e)calcium; f)bromine; g)arsenic 2.35 Determine the molecular and empirical formulas of the following :

a)The organic solvent benzene , which has six carbon atoms and six hydrogen atoms. b) The compound silicon tetrachloride, which is silicon atom and four chlorine atoms and is used in the manufacture of computer chips. 2.22 What is the mass in amu of a carbon -12 atom? b)Why is the atomic weight of carbon reported as 12.011 in the periodic table? 2.16 Each of the following nuclide is used in medicine. Indicate the number of protons and neutrons in each nuclide: a)phosphorus-32 b)chromium -51 c) cobalt-60 d)technetium-99 e)iodine-131 f)thallium-201 Chapter 3 1. Chemical Equations Balancing equations Knowing what is and how to use Stoichiometry Law of Conservation Reactants vs. Products [ knowing the difference and identifying them] 2. Types of Reactions Combustions Reactions Decompositions“ ” Combinations “ ” Knowing the difference between molecular and formula weight 3. The MOLE A mole of ANY substance = Avogadro’s Law [ 6.02 X 10²³] Mass of a mole expressed in grams. Molar Mass [ g/m] Knowing how to calculate as well as convert grams to mole [ vice versa ] 4. Limiting Reactant Knowing how to calculate using stoichiometry in a balanced equation Theoretical yield [ quantity of products calculated to form when all of the

limiting reagents reacts] Percent Yield compares to theoretical yield Questions: 3.63 a) Define the terms limiting reactant and excess reactant. b)Why are the amounts of products formed in a reaction determined only by the amount of limiting reaction 3.67A manufacturer of bicycles has 4250 wheels , 2755 frames, and 2255 handlebars. A)How many bicycles can be manufactured using these parts? B) How many parts of each kind are left over? C) which part limit’s the production of the bicycles ? 3.69 Sodium hydroxide reacts with carbon dioxide as follows:

2NaOH(s) + CO2(g) → Na2CO3 (s) + H20 (l) Which reagent is the limiting reactant when 1.70 mol NaOH and 1.00 mol CO² are allowed to react? How many moles of Na2CO3 can be produced ? How many moles of the excess reactant remain after the completion of the reaction? 3.71 The Fizz produced when an Alka - Seltzer tablet is dissolved in water is due to the reaction between sodium bicarbonate and citric acid : 3NaHCO3 (aq) + H3C6H5O7 (aq) → 3CO2(g) + 3H2O (l) +Na3C6H5O7(aq) In a certain experiment 1.00g of citric acid are allowed to react. A) which is the limiting reactant? B) How many grams of carbon dioxide form ? C) How many grams of the excess reactant remain after the limiting reactant is completely consumed ? 3. 73 Solutions of sodium carbonate and sliver nitrate react to form solid sliver carbonate and a solution of a sodium nitrate. A solution containing 6.50g of sodium carbonate is mixed with one containing 7.00g of sliver nitrate. How many grams of sodium carbonate, sliver nitrate, sliver carbonate, and sodium nitrate are present after the reaction is complete ? Chapter 4. 1. Properties of Aqueous Solutions Knowing what a aqueous solution is Solvents & Solutes Aqueous Solutions containing ions are Electrolytes vs. nonelectrolytes Strong electrolytes vs. weak electrolytes Knowing what and how to reach Chemical equilibrium 2. Precipitation Precipitate or a Salt MEMORIZE Solubility Rules for precipitation to occur [p. 118] Exchange reactions or metathesis reactions In a precipitation reaction knowing how to identify spectator ions Complete ionic equations and Molecular equations 3. Acids and Base ! What makes a formula acid or base Strong electrolytes = strong acids or bases. Vice versa Neutralization Reaction 4. Redox Reactions Knowing the difference between Reduction and oxidation [ oxidized=

meaning loses electrons ; reduced= meaning gains electrons Knowing what Oxidation Numbers are used for

O2 acids, and salts oxidizes many metals Redox between metals and acids/ salts = displacement reaction Knowing what activity series are 5.Concentrations Molarity (M)= moles of solute/volume of solution in L Dilution M1V1=M2V2 Molality = moles of solute per kilogram of solvent defines concentration Questions: 4.11 Using the solubility guidelines , predict whether each of the following compounds is a soluble or insoluble in water: a)NiCl2 ; b) Ag2 S c) Cs3PO4 d)SrCO3 e) (NH4)2 SO4 4.13 Will Precipitation occur when the following solutions are mixed? If so write the balanced chemical equation for the reaction. A) Na2 CO3 and AgNO3 ; b) NaNO3 and NiSO4 ; c) FeSO4 and Pb(NO3)2 . 4.15Write the balanced complete ionic equation and net ionic equations for the reactions that occurs when each of the following solutions is mixed. a)Na2 CO3(aq) and MgSO4(aq). 4.29 Write a balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reactions. a)Cr2 (SO4)3(aq) + (NH4)2 CO3(aq)→ b)AgNO3(aq) +K2 SO4(aq) → c)Pb(NO3)2 (aq) + KOH(aq)→ 4.23 Separate samples of a solution of an unknown salt are treated with dilute solutions of HBr, H2 SO4, and NaOH. A precipitate forms only with H2 SO4. Which of the following cations could be the solution contain: K+ Pb²+ and Ba²+ ? 4.27 Classify each of the following substances as a no electrolyte , weak electrolyte, or a strong electrolyte in water : a) H2SO3 b) C2 H5OH (ethanol) Chapter 6 1. Line Spectrum Wavelengths produces spectrums Continuous spectrums = rainbow of colors contains all light of all

wavelengths Bohr Model [p.207] Energy levels ; ground state and excited states and zero state 2. Wave behaviors Heisenberg ‘s uncertainty principle

3. Quantum Mechanics and Atomic Orbital’s Schrodinger proposed wave equations Subatomic particles Probability and electron density Orbitals; wave functions knowing (n) in electron shell N & 1 values = sub shells 4. Electron Configuration ! Hund’s Rules Know how to indicate electron configuration of an atom Main Groups Valence electrons vs. core electrons Transitions lanthanide actinide and F blocks elements Questions : 6.39.According to the Bohr model , an electron in the ground state of a hydrogen atom orbital’s the nucleus at a specific radius of 0.53 A. In a quantum mechanical description of the hydrogen atom, the most probable distance of the electron from the nucleus is 0.53 A. Why are these statements different. 6.41.a) For n=4 what are the possible values of l ? b ) For l=2 what are the possible values of m1? 6.43Give numerical values of n and l corresponding to teach of the following designations: a)3p b)2s c)4f d)5d ? 6.51 For a given value of the principle quantum number, n, how do energies of the s, p , d, and f sub shells vary for a) hydrogen b) a many electron atom? 653.a)What are the possible values of the electron spin quantum number ? b) what piece of experimental equipment can be used to distinguish electron that have different values of the electron spin quantum number ? c) Two electrons in an atom both occupy the 1s orbital. What quantity must be different of the two electrons? What principle governs the answers to this question? 6.55What is the maximum number of electrons that can occupy each of the following sub shells: a)3d b)4s c)2p d)5f ? 6.59Write a condensed electron configurations for the following atoms, using the appropriate noble -gas core abbreviations a)Cs b)Ni c)Se d)Cd e)Ac f)Pb Chapter 7

1. Development of Periodic Table Mendeleev and Meyer arranged elements by sequences 2. Effective Nuclear Charge Zeff = Z - S Coulombs Law 3. Sizes of atoms and ions Important property is the size Bonding atomic radius Increase and decrease of size determine by position on periodic table 4.Ionization Energy Determined by position on periodic table What is the ionization energy of an atom 1 & 2 ionization energy 5. Electron Affinities Know equation It measures attractions of the atom for the added electron 6. Metals Nonmetals and Metalloids Know each of their characteristic : common texture appearance melting

points , Good or Bad Conductors Group Trends Questions : 7.15 How do sizes of atoms change as we move a)from left to right b)from top to bottom , on the periodic table c)Arrange the following atoms in order of increasing atomic radius: F,P,S, A 7.16 a)Among the nonmetallic elements, the change in atomic radius in moving one place left or right in a row up or down. Explain these observations b) Arrange the following atoms in order of increasing atomic radius: Si S Ge Se. 7.18 Using only the periodic table , arrange the following atoms in order of increasing radius: a) Cs K Rb b) In Te Sn c) P Cl Sr 7.31 a) Why are ionization energies always positive quantities ? b) Why does F have a larger first ionization energy than O ? c) Why is the second ionization energy of an atom always greater than its first ionization ene 7.46 Arrange the following pure solid elements in order of increasing electrical conductivity : P Ag and Sb . Explain the reasoning of you used. Chapter 8 1. Chemical Bonds

3 types of Bond : ionic covalent non covalent ; know their characteristics Bond energies Charges and attractions determine bonds Lewis Dot Structures ; know how to draw for any bond and steps ! Octet Rule Multiples bonds : Single Double and Triple Bond enthalpy and length 2. Ionic Bonds Lattice energy Polyatomic ions Transition-metal ions 3.Bond Polarity and electro negativity Know the difference between each Non Polar Covalent The attraction causing the bonding Lims Pauling Dipole and dipole moments 4. Resonance Structure Happens due Lewis dot structure inadequate to represent a particular

molecule (or ion ) Know its characteristics : [ # of electrons shared ] Questions 8.5 Write the Lewis symbol for atoms of each of the following elements: a)Ca b) P c) Ne d) B 8.6 What is the Lewis dot symbols for the following atoms or ions : a)Mg b)As c) Sc³+ d) Se²¯ ? 8.7 Using Lewis symbols, diagram the reaction between Magnesium and oxygen atoms to give the ionic substance MgO. 8.11 Predict the chemical formula of the ionic compound formed between the following pairs of elements: a) Al and F b) K and S c) Y and O d) Mg and N 8.13 Write the electron configuration for each of the following ions and determine which ones possess noble-gases configurations a)Sr²+ b) Ti²+ c) Se²- d)Ni²- e) Br- f)Mn³-

8.27 Using the Lewis symbols and structures, diagram the formation of SiCl4 from Si and Cl atoms