Welcome to AP CHEMISTRY

Transcription

1 Welcome to AP CHEMISTRY Things To Know for AP Chem with Mrs. Johnson: 1) Get REALLY comfortable with the Periodic Table that I have provided in this packet. Use it for practice problems in the summer work; it is the table we will use all year, and the one you will receive on the AP Chem Exam. And yes, you are seeing correctly, it does not contain element names. 2) By August 30th, 2016, you should be able to complete the skills on the attached checklist in your sleep. These are the skills addressed in the summer assignment and the attached ion memorization charts. If you are not comfortable with skills after completing the assigned problems, find more similar problems in the text to practice (blue questions have answers in the back of the book), and use the resources mentioned at the top of the checklist. I know the summer assignment is lengthy, but it is designed to make sure we are all on the same page at the beginning of the year. Be prepared for a quiz encompassing these skills (mainly naming compounds, polyatomic ions, and acids) in the first week of school. 3) Hearing the material once in class is NOT going to be enough to comprehend everything you need to know to pass the AP exam. Also, I m not going to have time to say it all during class. You will be expected to read textbook sections prior to each class; this is to prime you for the whirlwind of information you will receive in class. Beginning with the summer assignment, learn how to effectively read and glean information from your textbook. The strategy that works best for me is reading short chunks of the text and taking notes as I go. 4) Find a few study buddies in the class with whom you can work effectively. Having a focused friend to work with can be extremely helpful for the sanity of all parties involved. 5) AP Chem is the equivalent of a FULL first year college chemistry course. Most college chem courses include three hours of lecture per week + three hours of lab + one hour of a discussion session. Yes, that s correct, seven hours of class time each week. College instructors will tell you that you should plan to spend at minimumone hour outside of class for every hour spent in class. Are you picking up what I m putting down? This class is going to start fast and get faster. There is no slowing down. Ever. I expect you to work hard, and when it gets tough and crazy and you want to throw your textbook in a bunsen burner, I expect you to work harder. 6) My top priority is for you to pass the AP Chemistry Exam. Sign up for Remind texts. Text the to the number to join. I will update you with announcements, lab dates, etc. In June, I will be updating my website, to include resources and references for our class. Throughout the summer, I will be checking my and will host optional study sessions on Wednesday, July 20th and Wednesday, August 17th (more details to come). During the school year, I am at school ALL THE TIME, and will always make time to meet with you. 1

2 AP Chemistry Summer Assignment, 2016 Required Practice Problems Complete the following endofchapter problems in your Zumdahl textbook. These are due on the first day of class. Please make sure work is neatly shown for all problems. Chapter 1: Problems 5, 8, 16, 25, 26, 49, 62 Chapter 2: Problems 5, 15, 39, 42, 56, 58, 60, 62, 64, 66, 68, 70, 79 Chapter 3:Problems 8, 12, 19, 21, 30, 32, 34, 36, 38, 40, 48, 55, 64, 65, 68, 72, 74, 86, 90, 91, 99, 100, 105 Skills Checklist Use your textbook, the lists provided, and other resources (sciencegeek.net, Bozeman Science videos, Tyler DeWitt videos, etc.) to master the following skills by the first day of class: Memorize the names, formulas and charges of... Straight off the Table ions (pg. 3 of this packet, Ch. 2 of text) Polyatomic ions (pg. 4 of this packet, Ch. 2 of text) Acids (pg. 5 of this packet, Ch. 2 of text) Memorize the seven strong acids, eight strong bases, and seven diatomic elements (pg. 6 of packet) Name chemical compounds (ionic and covalent) (Ch. 2) Use sig figs in measurements and calculations (Ch. 1) Complete calculations in scientific notation (Ch. 1) Quickly complete metric conversions (memorize pico, nano and micro prefixes as well) Calculate molar masses (Ch. 3) Use dimensional analysis to convert between moles, mass, particles and gas volume (Ch. 3) Write and balance chemical equations given a verbal description of the reaction (Ch. 3) Determine the limiting reagent in an experiment (Ch. 3) Solve stoichiometry problems, including limiting reactant problems (Ch. 3) Calculate theoretical yield and percent yield (Ch. 3) 2

3 Straight off the Table Ions (aka common ions) You will always have a Periodic Table, so you don t necessarily have to commit all of these to memory. Just learn how to use the Periodic Table in order to figure out the charge on ions. These ions can be organized into two groups. 1. Their place on the table suggests the charge on the ion, since the neutral atom gains or loses a predictable number of electrons in order to obtain a noble gas configuration. This was a focus in first year chemistry, so if you are unsure what this means, get help BEFORE the start of the year. a. All Group 1 Elements (alkali metals) lose one electron to form an ion with a 1+ charge b. All Group 2 Elements (alkaline earth metals) lose two electrons to form an ion with a 2+ charge c. Group 13 metals like aluminum lose three electrons to form an ion with a 3+ charge d. All Group 17 Elements (halogens) gain one electron to form an ion with a 1 charge e. All Group 16 nonmetals gain two electrons to form an ion with a 2 charge f. All Group 15 nonmetals gain three electrons to form an ion with a 3 charge Notice that cations keep their name (sodium ion, calcium ion) while anions get an ide ending (chloride ion, oxide ion). 2. Metals that can form more than one ion will have their positive charge denoted by a roman numeral in parenthesis immediately next to the name of the metal Straight off the Table Ions Cations Name H + Hydrogen Li + Lithium Na + Sodium K + Potassium Rb + Rubidium Cs + Cesium Ba 2+ Beryllium Mg 2+ Magnesium Ca 2+ Calcium Ba 2+ Barium Sr 2+ Strontium Al 3+ Aluminum Anions Name H Hydride F Fluoride Cl Chloride Br Bromide I Iodide O 2 S 2 Se 2 N 3 P 3 As 3 Type II Cations Fe 3+ Fe 2+ Cu 2+ Cu + Co 3+ Co 2+ Sn 4+ Sn 2+ Pb 4+ Pb 2+ Hg 2+ Oxide Sulfide Selenide Nitride Phosphide Arsenide Name Iron(III) Iron(II) Copper(II) Copper(I) Cobalt(III) Cobalt(II) Tin(IV) Tin(II) Lead(IV) Lead(II) Mercury(II) 3

4 Polyatomic Ions Most of the work on memorization occurs with these ions, but there are a number of patterns that can greatly reduce the amount of memorizing that one must do. 1. ate anions have one more oxygen than the ite ion, but the same charge. If you memorize the ate ions, then you should be able to derive the formula for the ite ion and viceversa. a. sulfate is SO 4 2, so sulfite has the same charge but one less oxygen (SO 3 2 ) b. nitrate is NO 3 so nitrite has the same charge but one less oxygen (NO 2 ) 2. If you know that a sulfate ion is SO 2 4 then to get the formula for hydrogen sulfate ion, you add a hydrogen ion to the front of the formula. Since a hydrogen ion has a 1+ charge, the net charge on the new ion is less negative by one. a. Example: 3 PO 4 2 HPO 4 H 2 PO 4 Phosphate hydrogen phosphate dihydrogen phosphate 3. Learn the hypochlorite chlorite chlorate perchlorate series, and you also know the series containing iodite/iodate as well as bromite/bromate. a. The relationship between the ite and ate ion is predictable, as always. Learn one and you know the other. b. The prefix hypo means under or too little (think hypodermic, hypothermic or hypoglycemia ) i. Hypochlorite is under chlorite, meaning it has one less oxygen c. The prefix hyper means above or too much (think hyperkinetic ) i. the prefix per is derived from hyper so perchlorate (hyperchlorate) has one more oxygen than chlorate. d. Notice how this sequence increases in oxygen while retaining the same charge: ClO ClO 2 ClO 3 ClO 4 hypochlorite chlorite chlorate perchlorate Ions to Memorize Cations Name Ag + Silver Zn 2+ Zinc 2+ Hg 2 Mercury(I) NH 4 + Ammonium Anions Name NO 2 Nitrite NO 3 Nitrate 2 SO 3 Sulfite 2 SO 4 Sulfate HSO 4 Hydrogen sulfate (bisulfate) OH Hydroxide CN Cyanide 3 PO 4 Phosphate 2 HPO 4 Hydrogen phosphate H 2 PO 4 Dihydrogen phosphate NCS Thiocyanate Carbonite 2 CO 3 Carbonate HCO 3 Hydrogen carbonate (bicarbonate) ClO Hypochlorite ClO 2 Chlorite ClO 3 Chlorate ClO 4 Perchlorate BrO Hypobromite BrO 2 Bromite BrO 3 Bromate BrO 4 Perbromate IO Hypoiodite IO 2 iodite IO 3 iodate IO 4 Periodate CH 3 CO 2 Acetate MnO 4 Permanganate 2 Cr 2 O 7 Dichromate 2 CrO 4 Chromate 2 O 2 Peroxide 3 BO 3 Borate NH 3 Ammonia (no charge) CO 2 2 4

5 You should know the acid names and formulas. Use the associated ion formulas to look for patterns in the naming schemes. Learning patterns will lessen the amount of rote memorization you need to do. Acid Formula Acid Name HF Hydrofluoric Acid HCl Hydrochloric Acid HI Hydroiodic Acid HBr Hydrobromic Acid HNO 3 Nitric Acid HNO 2 Nitrous Acid HCN Hydrocyanic Acid HSCN Thiocyanic Acid HClO 4 Perchloric Acid HClO 3 Chloric Acid HClO 2 Chlorous Acid HClO Hypochlorous Acid HC 2 H 3 O 2 Acetic Acid HMnO 4 Permanganic Acid H 2 SO 4 Sulfuric Acid H 2 SO 3 Sulfurous Acid H 2 CO 3 Carbonic Acid H 2 CrO 4 Chromic Acid H 3 PO 4 Phosphoric Acid Associated Ion Formula Name F Fluoride Cl Chloride I Iodide Br Bromide NO 3 Nitrate NO 2 Nitrite CN Cyanide SCN Thiocyanate ClO 4 Perchlorate* ClO 3 Chlorate* ClO 2 Chlorite* ClO Hypochlorite* C 2 H 3 O 2 Acetate MnO 4 Permanganate 2 SO 4 Sulfate* 2 SO 3 Sulfite 2 CO 3 Carbonate 2 CrO 4 Chromate 3 PO 4 Phosphate* Acid Naming Hints acids of monoatomic anions (Where anion ends in ide) HydroXic Acid Example: HCl = hydrochloric acid (anion Cl is chloride) Example: HBr = hydrobromic acid PerXate ion corresponds to PerXic Acid Xate ion corresponds to Xic Acid Xite ion corresponds to Xous Acid HypoXite ion corresponds to hypoxous Acid 5

6 Strong Acids and Bases 7 STRONG ACIDS 8 STRONG BASES HCl hydrochloric acid HBr hydrobromic acid HI hydroiodic acid HNO 3 nitric acid HClO 3 chloric acid HClO 4 perchloric acid H 2 SO 4 sulfuric acid LiOH lithium hydroxide NaOH sodium hydroxide KOH potassium hydroxide RbOH rubidium hydroxide CsOH cesium hydroxide Ca(OH) 2 calcium hydroxide Sr(OH) 2 strontium hydroxide Ba(OH) 2 barium hydroxide The Seven Diatomic Elements (*Mnemonic: Seven on the seven. On the Periodic Table, the diatomics make the shape of a seven, beginning with element number 6

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