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Leader: Tina Akinyi Course: Chem 177 Supplemental Instruction Instructor: 4/23/15 Iowa State University Date: ADAPTED FROM SARA PARUPSKI’S SI WORKSHEETS REVIEW FOR FINAL (1-4) Chapter 1 Difference between atom, element, compound, molecule, mixture, pure substance Identify Solids, Liquids, and Gases, also in context with periodic table Physical versus chemical properties and changes. Intensive versus extensive Unit Conversion Density Significant Figures Precision versus accuracy 1. Label the following as heterogeneous, homogeneous solution or pure substance. If it is a pure substance is it an atom or a compound? a. Koolaid b. Snickers Blizzard c. O3 d. Li e. CH3 f. Ni g. A nickel coin 2. Are the following physical or chemical properties? intensive or extensive? a. Color b. Reactivness c. Boiling point d. Density e. Flammability f. Molarity 3. If you have 37 x 10-5 Mg (Mega grams) and 104 mL of a solution, what is the density? 4. How long is the pencil? 1 in 2in 3in 4in 1060 Hixson-Lied Student Success Center 515-294-6624 [email protected] http://www.si.iastate.edu 5. Calculate the following calculations? a. 5.52 + 4.1 + 3.238 b. 3.3 x 78.66 Chapter 2 Dalton’s Atomic Theory and Laws of Chemical Combinations (mass, composition, proportions) Proton versus Neutrons versus Electrons Percent abundance, and mass spectrometry Periodic trends (diatomic, metals, nonmetals, metalloids, cations versus anions) Ionic (transferring of electrons) versus covalent (shared electrons) Naming: ionic, covalent, ions (oxy-ions), acids (binary and oxy-acids) 1. Fill in the following table Symbol Protons Neutrons Electrons Net Charge 27Al3+ O2- Kr 48 8 17 18 18 0 2. Name the following compounds or give the formula a. Silver Bromide b. Cobalt (III) Oxide c. Lithium Iodinde d. Lead (II) Nitride e. Al(CN)3 f. SnSe2 g. Cu3P h. NH4Cl i. Diphosphorus Pentoxide j. Carbon tetrabromide k. Dinitrogen trioxide l. N2O m. NI3 n. CCl4 3. Fill in the tables: Formula Name Formula Name Carbonate ion CNSulfate ion Hydroxide ion Phosphate ion Acetate Ion Ammonium ion ClONO3 ClO2 NO2ClO3 ClO4- Formula Name Hypochlorous Acid Chlorous acid Chloric acid Percholoric acid Hydrocholoric acid H2S(aq) H2S(g) 4. How many lines on a mass spectroscopy would N2O give? Also find the molar mass of Oxyen. Isotope Atomic Mass 14N 14.0031 15N 15.0001 Abundance (%) 99.632 0.368 Isotope 16O 17O 18O Atomic Mass 15.9949 16.9991 17.9992 Abundance (%) 99.757 0.038 0.205 Chap 3 Balancing Equations: Conservation of mass and atoms What drives a chemical reaction (precipitating a solid, evolution of a gas, formation of a nonelectrolyte (H2O) Combination, Decomposition, Combustion Moles versus mass versus moleculesmoving between units Stociometry, limiting reagents, and percent yield 1. Write the empirical and molecular formula for the following molecule: 9 Carbons, 6 Bromines, 3 Oxygens, and 9 Hydrogens 2. Complete and balance the following reactions: a. Combination ___ H2 + ___ F2 b. Decomposition ___ B2O3 c. Combustion ___ C4H10 3. Balance the following equations: a. __H2SO4 + ___ HI ___H2S + ___ I2 + ___H2O b. ___FeS2 + ___ O2 ___Fe2O3 +___ SO2 c. ___Al + ___FeO ___Al2O3 +___Fe d. ___K + ___Br2 KBr e. ___P4 + ___O2 P2O5 f. ___C7H16 + ___O2 ___CO2 + ___H2O g. ___C3H5OH + ___O2 ___CO2 + ___H2O 4. Write and balance the following reactions: a. Zinc Carbonate can be heated to form Zinc Oxide and Carbon Dioxide b. When Iron and water are left to sit, hydrogen gas is released and Iron (III) Oxide forms. 5. If you have 4 g NaOH, and 10 g HBr, what is the limiting reagent and how much salt is produced? In lab if you produce1 g salt, what is the percent yield? 6. How many moles of Al atoms are needed to combine with 1.58 mol of O atoms to make aluminum oxide, Al2O3? Chapter 4 electrolytes versus nonelectrolytes, strond versus weak, strong acids and bases Molarity, dilution Precipitate Acid/Base (neutralizations) titrations, limiting reagents for aqueous solutions. REDOX oxidation numbers, LEO goes GER (OIL RIG) 1. Complete the molecular and write the complete ionic, and net ionic equations for the following reactions, if a reaction will not occur say NO REACTION a. ___Li2CO3 (aq) + ___Co(C2H3O2)2 (aq) b. ___Fe(NO3)3 (aq) + ___K2S (aq) c. ___Pb(NO3)2 (aq) + ___Li2SO4 (aq) 2. What are the strong acids? 3. Assign Oxidation states to the following equations and tell what is being oxidized and what is reduced? a. Zn + 2HCl -> Zn2+ + H2 +2Cl- b. 4 Fe + 3 O2 → 2 Fe2O3 c. C6H12O6 + 6 O2 → 6 CO2 + 6 H2O 4. You are performing a titration with HCl and Ba(OH)2 a. You start with 10 g HCl and mix it with 10 mL of water, what is the concentration? b. If you want to dilute it to .01 M, how much water must be added? c. If you tritate that with 25 mL of unknown Ba(OH)2 what is the concentration of that unknown? d. How much H2O is produced?