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Name: ________________________ Oregon City High School AP Chemistry Summer Assignment Welcome to AP chemistry! This summer homework is meant to be a review of the material covered in Chemistry A and B as well as an introduction to the a few concepts in the first three chapters of the AP Chemistry Textbook that we haven’t covered yet. Having the following skills will be essential to your success in AP Chemistry and I will expect that you already have a firm grasp on these topics as we start the year. The following assignment is to be completed over the summer and brought in COMPLETED on the first day of class. NO LATE PAPERS WILL BE ACCEPTED!!! Because this information is part of the first unit of study you will be responsible for all of these concepts on your first test. While you may need to reference materials to help remind you how to do some of these problems (your notes from chemistry A and B, your AP Chemistry textbook, the internet, etc.) please make sure that your work is YOUR OWN as you will be the one responsible for understanding this information. Included is a copy of the periodic table used in AP Chemistry. Notice that this is not the table used in first year chemistry. The AP table is the same that the College Board allows you to use on the AP Chemistry test. Notice that it has the symbols of the elements but not the written names. You may want to spend some time familiarizing yourself with the names and symbols of each element. About the AP Chemistry Course: Since this is a college level course taught in high school, it is very demanding, both in time and effort required. Much of the work involves solving math-type story problems. Homework is assigned each day through all three trimesters. The three weeks before the AP Exam in May will be used for review. The amount of work outside of class depends upon the student and his/her background; however, students should be prepared to spend anywhere from 45 minutes to an hour each night after school on just their Chemistry homework. Those students who are heavily involved in after school activities and / or jobs will have to learn to budget their time very carefully. Why Take AP Chemistry? There are several reasons why a student might want to take AP Chemistry, including (but not limited to!) the following: 1. AP Chemistry will challenge you to the limits of your academic ability. In the past you may have found classes "too easy", and therefore may not have stimulated you to do your very best. This will not be the case in AP Chemistry. 2. AP Chemistry should allow you to achieve college credit while still enrolled in high school. This will save time and money. Some students who have passed the AP Exam elect to take first year college chemistry anyway, where they find the material an easy review, and achieve top grades while others around them are frustrated and struggling in a class which is too large and/or the instructor is unavailable for help. 3. AP Chemistry looks great on your transcript or on a letter of recommendation. More and more colleges and universities are looking for ways a student has distinguished themselves in high school. Being a "straight A" student no longer carries the weight it once did. Taking AP Chemistry is a way of distinguishing yourself in high school. 4. While AP chemistry will be challenging and time consuming (sorry… it is a college class… :/) we will get to perform some fun labs, get to know each other really well, have an unbelievably deep understanding of chemistry, and we will get to do some fun projects (including a field-trip near the end). I look forward to seeing you all at the beginning of the next school year! If you need to contact me during the summer, you can email me and I will get back to you as soon as possible. Jenaya Hoffman OCHS AP Chemistry Teacher [email protected] AP CHEMISTRY CHAPTER 1 REVIEW: MATTER AND MEASUREMENT 1. SI Units and the Metric System Every measurement has two parts: a number and a unit. SI System – 1960 an international agreement was reached to set up a system of units so scientists everywhere could better communicate measurements. Le Système International (SI) was all based on the metric system. Prefix + base unit Exp: 1 kg = 1000g 1,000,000 micrograms in 1 gram Prefix tells you the power of 10 to multiply by - decimal system -easy conversions *Density of water = 1 g/mL lL Length How many millimeters, mm, are in a meter? _________ Find an object that is 1 mm thick: _________ How many centimeters, cm, are in a meter? __________ Find an object that is 2.5 cm in diameter:_________ Figure out YOUR height: ___________ m ____________ cm ____________ mm Mass How many grams are in a kilogram? _________ A 150 lb person has a mass of __________ kg. Hint: 1 kg = 2.2 lbs Volume – derived from length see picture above. Consider a cube 1m on each edge ∴1.0m3 - a decimeter is 1/10 of a meter so (1m)3 = (10dm)3 = 1,000 dm3 - 1dm3 = 1 liter (L) How many cm3 are in 1 m3? ______________ If 1 cm3 is equal to 1 mL how many cm3 are in a liter? _____________ Using a measuring cup at home find the volume of water (in mL) that will fit in a pop can: _________ If 1 mL of water has a mass of 1 g, how many grams of water are in your pop can? _________ 2. Temperature Conversions Temperature is a measure of the average kinetic energy. Different temperature scales are all talking about the same height of mercury. Notice 1 °C is equal to 1 K K = °C + 273 °C = K – 273 Derivation for the equation for converting ºF to ºC below Normal body temperature is 98.6°F. Convert this temperature to the Celsius and Kelvin scales. ____________ °C ____________ K Liquid nitrogen, which is often used as a coolant for low-temperature experiments, has a boiling point of 77 K. What is this temperature in degrees Celsius? ____________ °C One interesting feature of the Celsius and Fahrenheit scales is that -40°F and -40°C represent the same temperature. Verify that this is true. Show your work. 3. Density Determining Density A chemist, trying to identify the main component of a compact disc cleaning fluid, finds that 25.00 cm3 of the substance has a mass of 19.625 g at 20°C. The following are the names and densities of the compounds that might be the main component. Compound Chloroform Diethyl ether Ethanol Isopropyl alcohol Toluene 1.492 0.714 0.789 0.785 0.867 Which of these compounds is the most likely to be the main component of the compact disc cleaner? __________________ An empty container weighs 121.3 g. Filled with carbon tetrachloride (density 1.53 g/cm3 ) the container weighs 283.2 g. What is the volume of the container? __________________ A student has a cube of aluminum that measures 4 cm wide on each side. What is the volume of this cube? (Volume = length x width x height) __________________ When the student massed the cube on a scale they found that the cube of aluminum had a mass of 165 g. What is the density of this aluminum cube? __________________ Percent error is a measure of how inaccurate a measurement is. Percent Error = |Your Value – Accepted Value| x 100% Accepted value Using a computer, look up the accepted value for the density of aluminum and calculate your percent error for your calculated density. Percent error for Al ___________% 4. Accuracy, Precision, and Types of Error Accuracy – correctness; agreement of a measurement with the true value. Precision – reproducibility; degree of agreement among several measurements. Random error – equal probability of a measurement being high or low. Systematic error – occurs in the same direction each time. Usually due to equipment or experimental flaw. The results of several dart throws show the difference between precise and accurate. (a) Neither accurate nor precise (large random errors). (b) Precise but not accurate (small random errors, large systematic error). (c) Bull’s-eye! Both precise and accurate (small random errors, no systematic error). To check the accuracy of a graduated cylinder, a student filled the cylinder to the 25-mL mark using water delivered from a buret and then read the volume delivered. Following are the results of five trials: Is the graduated cylinder accurate? Is the graduated cylinder precise? What type of error occurred, random or systematic? 5. States of Matter Step 1.) In the circles below, draw what water molecules (H2O) would look like in the three different states of matter. Step 2.) Describe the speed at which the molecules move in each state of matter. Solid ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ Liquid ____________________________ ____________________________ ____________________________ ____________________________ ____________________________ ____________________________ ____________________________ ____________________________ ____________________________ ____________________________ ____________________________ ____________________________ Gas ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ ___________________________ What is a vapor and how does it differ from a gas? _________________________________________________________________________________________ Give three examples of vapors below. ___________________ ___________________ ___________________ Give three examples of gases below. ___________________ ___________________ ___________________ 6. Dimensional Analysis Use conversion factors to change the units. Each conversion factor = 1 1 foot = 12 inches (equivalence statement) 12 in = 1 ft = 1 ft 1 ft 12 in 72 ft | 12 in = 864 in | 1 ft To convert a unit, multiply your quantity by a conversion factor that “cancels” the undesirable unit and puts the desired unit in the numerator. (Multiply all the numbers on top) ÷ (multiply all numbers on the bottom) Common Conversions 1 inch (in) = 2.54 centimeter (cm) 1 foot (ft) = 12 inches (in) 1 yard (yd) = 3 feet (ft) 1 mile (mi) = 1760 yards (yd) 1 meter (m) = 3.28 feet (ft) 1 mile = 1.61 kilometer (km) 1 pound (lb) = 453.6 grams (g) 2.205 pounds (lb) = 1 kilogram (kg) 1 ounce = 28 grams 60 seconds (s) = 1 minute (min) 60 minute (min) = 1 hour (hr) 24 hours (hr) = 1 day 365 days = 1 year 1 fortnight = 14 days 100 years = 1 century 1 cup (c) = 16 tablespoons (tbsp) 1 gallon = 4 quarts 1000 milliliters (mL) = 1 liter (L) 1.057 quarts = 1 liter (L) 1 kilometer (km) = 0.62 miles (mi) 1000 years = 1 millennium 1 tablespoon (tbsp) = 3 teaspoons (tsp) 3 1 cubic centimeter (cm ) = 1 milliliter (mL) 3.785 liters (L) = 1 gallon (gal) A pencil is 7.00 in. long. What is its length in centimeters? You want to order a bicycle with a 25.5-in. frame, but the sizes in the catalog are given only in centimeters. What size of frame (in cm) should you order? A student has entered a 10.0-km run. How long is the run in miles? The speed limit on many highways in the United States is 55 mi/h. What number would be posted in kilometers per hour? A Japanese car is advertised as having a gas mileage of 15 km/L. Convert this rating to miles per gallon. 7. Classification of Matter Place the following words in the flow chart below: Element Homogeneous Mixture (solution) Homogeneous Heterogeneous mixture (solution) Atom Matter Neutron Proton Pure Substance Compound Nucleus Electron Mixtures can be separated by methods involving only physical changes - Compounds can be decomposed to elements only through chemical changes. List the six physical properties found in Chapter 1 of your book: • • • • • • What is a common chemical property? ____________________ Distillation What physical property would allow you to separate a mixture containing water, alcohol, cyclohexane (a liquid), and salt using the above apparatus? _______________ What would be left over in the distilling flask? __________ Paper chromatograph of ink. (a) A line of the mixture to be separate is placed at one end of a sheet of porous paper. (b) The paper acts as a wick to draw up the liquid. (c) The component with the strongest attraction for the liquid travels faster than those that cling to the paper. 8. Significant Figures There are two kinds of numbers in the world: • exact: o example: There are exactly 12 eggs in a dozen. o example: Most people have exactly 10 fingers and 10 toes. • inexact numbers: o example: any measurement. If I quickly measure the width of a piece of notebook paper, I might get 220 mm (2 significant figures). If I am more precise, I might get 216 mm (3 significant figures). An even more precise measurement would be 215.6 mm (4 significant figures). Significant figures are critical when reporting scientific data because they give the reader an idea of how well you could actually measure/report your data. In any measurement, the number of significant figures is critical. The number of significant figures is the number of digits believed to be correct by the person doing the measuring and always includes one estimated digit. Beaker The first digit is definitely a 4 because the liquid line is between 40 and 50. The second digit is an estimate… 46? 47? 48? This measurement has 2 significant figures. Graduated cylinder Buret Graduated cylinder has more gradations (lines) so we can get more significant figures. Now we know it is 36 and we can estimate the last digit 36.4? 36.5? 36.6? This measurement has 3 significant figures. A. Determining number of significant figures 1. All non zero numbers are significant (meaning they count as sig figs) 613 has __3__ sig figs 2. 123456 has ____ sig figs Buret has even more gradations so it will give you the most accurate measurement. We know 20.3 and can estimate the last digit. 20.37? 20.38? 20.39? This measurement has 4 sig figs. 17865332 has ____ sig figs Zeros located between non-zero digits are significant (they count) 5004 has __4__ sig figs 602 has ____ sig figs 6000000000000002 has ___ sig figs 3. Trailing zeros (those at the end) are significant only if the number contains a decimal point; otherwise they are insignificant (they don’t count) 5.640 has __4__ sig figs 120000. has ____ sig figs 120000 has ____ sig figs 4. Zeros to left of the first nonzero digit are insignificant (they don’t count); they are only placeholders! 0.000456 has __3__ sig figs 0.052 has ____ sig figs 0.000000000000000052 has ____ sig figs B. Rules for addition/subtraction problems Your calculated value will have the same number of digits to the right of the decimal point as that of the least precise quantity. 6.22 53.6 limiting term has 1 decimal place 14.311 + 45.09091 119.22191 round to 119.2 (1 decimal place) 5365.999 limiting term has 3 decimal places - 234.66706 5131.33194 round to 5131.332 Underline the limiting term and write the answer using the correct amount of significant figures: 17.12 + 30.123 = _________ 1000.00 – 62.5 = ________ 15.05 + 0.0044 + 12.34 = ________ C. Rules for multiplication/division problems When multiplying/dividing, the answer should have the same number of significant figures as the limiting term. The limiting term is the number with the least number of significant figures. 503.29 x 6.177 = 3108.82233 → round to 3109 ↑ limiting term has 4 sig figs 1000.1 = 4.11563786 → round to 4.12 243 ↑ limiting term has 3 sig figs Underline the limiting term and write the answer using the correct amount of significant figures: 35.010 / 1.23 = __________ 0.1700 x 1700. x 1700 = __________ D. Rules for conversions When converting a number, the answer should have the same number of significant figures as the number started with. Some numbers are exact because they are known with complete certainty. Most exact numbers are integers: exactly 12 inches are in a foot, there might be exactly 23 students in a class. Exact numbers are often found as conversion factors or as counts of objects. *Exact numbers can be considered to have an infinite number of significant figures. Thus, the number of apparent significant figures in any exact number can be ignored as a limiting factor in determining the number of significant figures in the result of a calculation. 52.4 in | 1 ft | 12 in ↑ 3 sig figs = 4.366666667 ft → round to 4.37 ft E. Rules for rounding off numbers 1.) If the digit to be dropped is greater than 5, the last retained digit is increased by one. For example: 12.6 is rounded to 13. 2.) If the digit to be dropped is less than 5, the last remaining digit is left as it is. For example: 12.4 is rounded to 12. 3.) If the digit to be dropped is 5, and if any digit following it is not zero, the last remaining digit is increased by one. For example: 12.51 is rounded to 13. Significant Figure Practice Problems How many significant figures does each of the following contain? 1.) 54 _____ 4.) 4.00 _____ 7.) 0.041 _____ 2.) 45678 _____ 5.) 400 _____ 8.) 0.00010 _____ 3.) 4.03 6.) 400. _____ 9.) 190909090 _____ _____ Round the following numbers as indicated: 10.) To four figures: 3.682417 21.860051 375.6523 112.511 45.4673 ________ _______ _______ _______ _______ 2.473 5.687524 7.555 8.235 _______ _______ _______ _______ 79.2588 0.03062 3.4125 41.86632 _______ _______ _______ _______ 11.) To one decimal place: 1.3511 ________ 12.) To two decimal places: 22.494 _________ Which number in each of the additions/subtractions is the limiting term, and how many decimal places should the answer of each addition/subtraction have? Write the answer with the correct amount of significant figures. 13.) 55.43 + 44.333 + 5.31 + 9.2 = _______________ # of sig figs _______ 14.) 890.019 + 890.1234 + 890.88788 = _______________ # of sig figs _______ 15.) 69.99999 – 45.44444444 = _______________ # of sig figs _______ 16.) 3.461728 + 14.91 + 0.980001 + 5.2631 = _______________ # of sig figs _______ Which number in each of the multiplication/division problems is the limiting term, and how many sig figs should the answer of each multiplication/division have? Write the answer with the correct amount of sig figs. 17.) 343.4 / 34.337 = _______________ # of sig figs _______ 18.) 0.000000003 x 30.03030 = _______________ # of sig figs _______ 19.) (1.3) x (5.724) = _______________ # of sig figs _______ 20.) (6305) / (0.010) = _______________ # of sig figs _______ 21.) (6.78 x 10-4) x (1.4 x 102) = _______________ # of sig figs _______ 22.) 12.5 x 75 = _______________ # of sig figs _______ AP CHEMISTRY CHAPTER 2 REVIEW: ATOMS, MOLECULES, & IONS 1. Using either your purple notes from Chemistry A and B or the internet define the following terms. LAW OF CONSERVATION OF MASS: THE LAW OF DEFINITE PROPORTIONS: Define and give an example. THE LAW OF MULTIPLE PROPORTIONS: Define and give an example. DALTON’S ATOMIC THEORY OF MATTER: Give the four parts of his theory. I. II. III. IV. Using the knowledge gained in Chemistry A what are TWO MODIFICATIONS that have been made to Dalton’s Atomic Theory? In your own words describe how J.J. Thomson’s experiment with the cathode ray tube led to the discovery of electrons. Draw a picture of the cathode ray tube and what happened when a magnet was brought close to the ray. What was the name of the “model” that was born from this experiment? Draw it. In your own words describe how Rutherford’s Gold Foil experiment led to the discovery of the nucleus. Draw a picture of the gold foil experiment. What was the name of the “model” that was born from this experiment? Draw it. 2. NAMING COVALENT MOLECULES, IONIC COMPOUNDS, AND ACIDS Rules for Naming Covalent Compounds (nonmetal + nonmetal) A. Use prefixes to indicate the number of each element in the molecule. mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-. B. Drop the mono prefix if there is only one of first element in the molecule. Exp: CO2, carbon dioxide. (no mono) C. Ending of the last element changes to –ide. Rules for Naming Ionic Compounds (metal + nonmetal) A. Balance Charges (charges should add up to zero). B. Cation (+ ion) is always written first (in name and in formula). Cation has same name as on periodic table. You may need to indicate the charge of the cation in the name using roman numerals if it is multivalent. Exp: FeCl3 is Iron(III) chloride whereas FeO is iron(II) oxide. C. Change the ending of the anion (-ion) to –ide (unless polyatomic ion, then named as given). I. Name these binary compounds of two nonmetals. IF7__________________________ N2O5____________________________ N2O4________________________ As4O10___________________________ PCl3_________________________ S2Cl2____________________________ XeF2 _____________________________ SF6_______________________________ II. Name these binary compounds with a fixed charge metal. AlCl3 _______________________ MgO____________________________ KI__________________________ SrBr2 ___________________________ CaF2 ________________________ Al2O3___________________________ BaI2______________________________ Na2S _____________________________ III. Name these binary compounds of multivalent cations (use roman numerals). CuCl2 ______________________ Fe2O3____________________________ PbCl4_______________________ Cu2S_____________________________ AuI3________________________ CoP_____________________________ SnO______________________________ HgS______________________________ IV. Name these compounds with polyatomic ions. Fe(NO3)3_________________________ NaOH__________________________ Ca(ClO3)2________________________ KNO2__________________________ NH4NO2_________________________ Cu2Cr2O7 _______________________ Cu2SO4___________________________ NaHCO3__________________________ Acids- If the formula has hydrogen written first, then this usually indicates that the hydrogen is an H+ cation and that the compound is an acid. Rules for Naming an Acid A. When the name of the anion ends in –ide, the acid name begins with the prefix hydro-, the stem of the anion has the suffix –ic and it is followed by the word acid. -ide becomes hydro _____ic Acid Example: Cl- is the Chloride ion so HCl = hydrochloric acid HCl ________________________ HI _________________________ H2S _______________________ HF _______________________ B. When the anion name ends in –ite, the acid name is the stem of the anion with the suffix –ous, followed by the word acid. -ite becomes ______ous Acid Example: ClO2- is the Chlorite ion so HClO2. = Chlorous acid. C. When the anion name ends in –ate, the acid name is the stem of the anion with the suffix –ic, followed by the word acid. -ate becomes ______ic Acid Example: ClO3- is the Chlorate ion so HClO3 = Chloric acid. **I like to remember this rule as “I ate something and it was icky.” I. HNO3, which contains the polyatomic ion nitrate, is called nitric acid. HNO2, which contains the polyatomic ion nitrite, is called nitrous acid. Name the following acids using the correct naming rule. HClO4__________________________ H2SO4__________________________ HC2H3O2_________________________ H3PO4__________________________ HNO2__________________________ H2CrO4__________________________ H2C2O4_________________________ H2CO3__________________________ II. Name these compounds appropriately. CO____________________________ NH4CN _________________________ HIO3__________________________ NI3____________________________ AlP ____________________________ OF2___________________________ LiMnO4________________________ HClO __________________________ SO2___________________________ CuCr2O7_______________________ K2O____________________________ HF____________________________ FeF3__________________________ KC2H3O2________________________ MnS__________________________ III. Write the chemical formulas. Tin (IV) phosphide _____________ copper (II) cyanide ____________ Magnesium hydroxide _____________ sodium peroxide ____________ Sulfurous acid _____________ lithium silicate ____________ Potassium nitride _____________ chromium (III) carbonate ____________ Gallium arsenide _____________ cobalt (II) chromate ____________ Zinc fluoride _____________ dichromic acid ____________ 3. PERCENT COMPOSITION Complete the following problems showing all work. 1. A 0.941 gram piece of magnesium metal is heated and reacts with oxygen. The resulting magnesium oxide product weighed 1.560 grams. Determine the percent composition of each element in the compound. 2. Determine the empirical formula given the following data for each compound: a) Fe = 63.53%, S = 36.47% b) Fe = 46.55%, S = 53.45% 3. A compound contains 21.6% sodium, 33.0% chlorine, 45.1% oxygen. Determine the empirical formula of the compound. AP CHEMISTRY CHAPTER 3 REVIEW: CHEMICAL REACTIONS AND STOICHIOMETRY 1. SOLUBILITY RULES I. Review solubility rules and identify each of the following compounds as soluble or insoluble in water. You must memorize these solubility rules: Salts of NH4+, Na+, K+ and NO3- are always soluble. SOLUBILITY GUIDELINES Compounds Solubility Exceptions Salts of alkali metals (group 1A) and Soluble Some lithium compounds ammonium (NH4+) All nitrate, chlorate and acetate salts Soluble Sulfate salts Soluble Cation is Pb, Ag, Hg, Ba, Sr, or Ca Halide (group 7A halogen ions) salts Soluble Cation is Ag, Hg or Pb Acids (H in front) Soluble carbonates, phosphates, chromates, Cation is alkali metal (group 1A) or Insoluble sulfides, hydroxides and oxides ammonium *salts = ionic compounds Na2CO3 ___________ CoCO3 _____________ Pb(NO3)2 _____________ K 2S ___________ BaSO4 _____________ (NH4)2S _____________ AgI ___________ Ni(NO3)2 _____________ KI _____________ FeS ___________ PbCl2 _____________ CuSO4 _____________ Li2O ___________ Mn(C2H3O2)2 _____________ Cr(OH)3_ _____________ AgClO3 ___________ Sn(SO3)4 _____________ FeF2 _____________ II. Write out the balanced chemical equation for each of the following double replacement reactions. Predict whether each of these double replacement reactions will give a precipitate or not based on the solubility of the products. If yes, identify the precipitate and write it on the line to the right. silver nitrate and potassium chloride ____________ magnesium nitrate and sodium carbonate ____________ strontium bromide and potassium sulfate ____________ cobalt (III) bromide and potassium sulfide ____________ ammonium hydroxide and copper (II) acetate ____________ lithium chlorate and chromium (III) fluoride ____________ 2. BALANCING EQUATIONS AND TYPES OF REACTIONS I. Balance the following equations with the lowest whole number coefficients. ____S8 ____ SO3 + ____ O2 ____C10H16 + ____ Cl2 ____ C ____Fe ____ Fe2O3 + ____ O2 + ____ HCl ____CO2 ____C7H6O2 + ____ O2 ____KClO3 ____ KCl + ____ H2O + ____ O2 ____H3AsO4 ____As2O5 + ____ H2O ____V2O5 + ____ HCl ____VOCl3 + ____ H2O ____Hg(OH)2 + ____ H3PO4 ____ Hg3(PO4)2 + ____ H2O II. Balance the following equations, indicate the states of matter for each compound, and indicate the type of reaction taking place: 1) ____ NaBr ( ) + ) ____ Al2(SO4)3 ( ) ____ H3PO4 ( ____ Na3PO4 ( ) + ____ HBr ( ) Type of reaction: ____________________ 2) ____ Ca(OH)2 ( )+ ____ CaSO4 ( ) + ____ Al(OH)3 ( ) Type of reaction: ____________________ 3) ____ Mg ( ) + ____ Fe2O3 ( ) ____ Fe ( ____ CO2 ( ) + ____ MgO ( + ____ H2O ( + ____H2 ( ) Type of reaction: ____________________ 4) ____ C2H4 ( ) + ____ O2 ( ) ) ) Type of reaction: ____________________ 5) ____ PbSO4 ( ) ____ PbSO3 ( ) + ____ O2 ( ____N2I6 ( ) Type of reaction: ____________________ 6) ____NH3 ( ) + ____I2 ( ) Type of reaction: ____________________ ) ) 3. WRITING CHEMICAL EQUATIONS Mole Ratio from coefficients 4. STOICHIOMETRY AND LIMITING REACTANTS 1. Given the equation below, what mass of water would be needed to react with 10.0g of sodium oxide? Na2O + H2O 2NaOH 2. 2NaClO3 2NaCl + 3O2 What mass of sodium chloride is formed along with 45.0g of oxygen gas? 3. 4NH3 + 5O2 4NO + 6 H2O What mass of water will be produced when 100.0g of ammonia is reacted with excess oxygen? 4. If the reaction in #3 is done with 25.0g of each reactant, what is the maximum amount of product that could be made? Which reactant would be the limiting reactant? 5. Na2S + 2AgNO3 Ag2S + 2NaNO3 If the above reaction is carried out with 50.0g of sodium sulfide and 35.0g of silver nitrate what is the maximum amount of silver sulfide that could be made? What is your limiting reactant? What mass of the excess reactant remains? 6. 6NaOH + 2Al 2Na3AlO3 + 3H2 What volume of hydrogen gas (measured at STP) would result from reacting 75.0g of sodium hydroxide with 50.0g of aluminum? SOLUBILITY GUIDELINES Activity Series of Metals Name Symbol Lithium Li Potassium K Calcium Ca Sodium Na Magnesium Mg Aluminum Al Zinc Zn Iron Fe Lead Pb Hydrogen H Copper Cu Mercury Hg Silver Ag Platinum Pt Gold Au Compounds Solubility Exceptions Soluble Some lithium compounds Soluble - Soluble Cation is Pb, Ag, Hg, Ba, Sr, or Ca Soluble Cation is Ag, Hg or Pb acids (have an ___ in front) carbonates, phosphates, chromates, Soluble - sulfides, hydroxides, and oxides Insoluble Cation is alkali metal or ammonium (NH4+) Salts of alkali metals and ammonium All nitrate, chlorate and acetate salts Water line sulfate salts halide salts (halogens) Acid line *salt is an ionic compound 1 J = 0.2390 cal 4.184J = 1 cal ΔH = m x C x ΔT M = mol / L %v / v = M1V1 = M2V2 volume of solute × 100% volume of solvent Pressures: 1 atm = 101.3 kPa = 760 mmHg = 760 torr Boyle’s Law € P1V1 = P2V2 Combined Gas Law Charles’ Law V1 V2 = T1 T2 Ideal Gas Law %m / v = € K = °C + 273 P1 V1 P2 V2 = T1 T2 PV=nRT R = 8.31 P1 P2 = T1 T2 mass of solute (g) × 100% volume of solvent (mL) STP = 1 atm and 273K € Gay-Lussac’s Law € 1000 cal = 1 Cal Partial Pressures L × kPa mol × K Ptotal = P1 + P2 + P3 € € € or R = 0.0821 L × atm mol × K moles gasX x Ptotal = PX € total moles