Interactive Notebook 4 for 2013-2014



Unit 4 STOICHIOMETRY Interactive Notebook Table of ContentsPageDateStdLearning GoalHomeworkMastery/Effort11/4/1311/5/1311/6/1311/7/1311/8/1311/11/1311/12/1311/13/1311/14/1311/15/1311/18/13PageDateStdLearning GoalHomeworkMastery/Effort11/19/1311/20/1312/2/1312/3/1312/4/1312/5/1312/6/1312/9/1312/10/1312/11/1312/12/13PageDateStdLearning GoalHomeworkMastery/Effort12/13/1312/16/1312/17/13Unit 4 Exam12/18/1312/19/13TRUSD Fall Semester Final EXAM12/20/13TRUSD Fall Semester Final EXAMCalifornia Standard Stoichiometry 3. The conservation of atoms in chemical reactions leads to the principle of conservation of matter and the ability to calculate the mass of products and reactants. a. Students know how to describe chemical reactions by writing balanced equations. b. Students know the quantity one mole is set by defining one mole of carbon-12 atoms to have a mass of exactly 12 grams. c. Students know one mole equals 6.02 × 1023 particles (atoms or molecules). This number, called Avogadro’s number, is known to a high degree of accuracy.d. Students know how to determine the molar mass of a molecule from its chemical formula and a table of atomic masses and how to convert the mass of a molecular substance to moles, number of particles, or volume of gas at standard temperature and pressure. The molar mass of a compound, which is also called either the molecular mass or molecular weight for covalent compounds or formula mass for ionic compounds, is the sum of the atomic masses of the constituent atoms of each element in the molecule. Molar mass is expressed in units of grams per mole. The number of particles in the sample is determined by multiplying the number of moles by Avogadro’s number. The volume of an ideal or a nearly ideal gas at a fixed temperature and pressure is proportional to the number of moles. Students should be able to calculate the number of moles of a gas from its volume by using the relationship that at standard temperature and pressure (0°C and 1 atmosphere), one mole of gas occupies a volume of 22.4 L. e. Students know how to calculate the masses of reactants and products in a chemical reaction from the mass of one of the reactants or products, when the chemical reaction is written as a balanced expression. Atoms are neither created nor destroyed in a chemical reaction.f.* Students know how to calculate percent yield in a chemical reaction. Interactive Notebook Score SheetQuizzes/FormativesDateScore/Max ScoreRetake Needed (yes or no)Peer InitialParent InitialFormative 15 Molar Conversions Formative 16 Percent Composition Formative 17 BalancingReaction EquationsFormative 18 StoichiometryFormative 19 Limiting ReactantsFormative 20 HydratesUnit 4 TestDistrict Final ExamName of Scored AssignmentDate DueScore/MaxPeer InitialsLevel of EffortHistogram – graphic representation of discrete data. Date (x axis) and progress on standards mastery with 5 advanced, 4 proficient, 3 basic, 2 below basis, and 1 incomplete (y axis) 580517012382500Unit 4 Stoichiometry Study GuideCalifornia Chemistry Standard Set 3Key Vocabulary TermsMole (Avogadro’s Number)Percent CompositionMolecular FormulaEmpirical FormulaCoefficientSubscriptReactantsProductsMolar MassAtomic MassLimiting ReactantExcess ReactantMole RatioParticlesLaw of Conservation of MatterSynthesis ReactionDecomposition ReactionSingle Replacement (Displacement) ReactionDouble Replacement (Displacement) ReactionCombustion ReactionConceptsThe Law of conservation of matter: In any physical or chemical change, matter is neither created nor destroyed but merely changed from one form to another. Explain the Law of Conservation of Matter when balancing chemical reactionsDescribe 5 types of Chemical ReactionsSynthesis ReactionDecomposition ReactionCombustion ReactionSingle Displacement ReactionDouble Displacement ReactionItems for Memorization - Avogadro’s Number: 6.02 x 1023Determine the molar mass of a formula e.g., H2O, O2, Ca(OH)2, Fe3(PO4)2Determine percent composition of all of the elements in a formula e.g., H2O, O2, Ca(OH)2, Fe3(PO4)2Determine Empirical and Molecular Formula from percent composition dataPerform the following conversions:Mole to MoleGrams to MoleMoles to ParticlesGrams to ParticlesGrams A to Grams BMole to VolumeVolume to MoleGiven mass of compounds in words be able to do the following adding energy where appropriate:Balance the chemical reaction___R1 + ___R2 ___P1 + ___P2Subscripts and CoefficientsPerform 3 step conversions to evaluate reactant to maximize yield given one of the reactants, then compare to actual reactants to determine limiting and excess reactants.Mass to Mole then Mole ratio then Mole to MassFind the limiting (least: LR) and excess (larger: ER) reactants Grams R1 Grams R2 Grams R2 R1Find the amount of productGrams LR P1Grams LR P2Mass Balance: Grams reactant = Grams product___R1 + ___R2 ___P1 + ___P2 + Energy MOLE & Chemical Formulas: Review Practice 1left24955500A mole (also known as Avogadro's Number) is the number that is used in making calculations involving atoms and molecules. Given the relatively microscopic size of the particles, it would be rather difficult (read: utterly pointless) to calculate amounts in terms of numbers of atoms. So, we use the mole.A mole, (mol for short) is equal to (all together now) 6.022 x 1023 atoms or molecules.The atomic mass given for an element on the periodic table measured out in grams is equal to one mole of atoms of that element.Thus, the Molar Mass (MM) of elements and compounds is the mass, in grams, equal to the atomic and formula masses of those elements and compounds. The unit of Molar Mass is grams/mole. Quick Write In your own words describe what a mole of something means_________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________1 step: particles, grams, or L of gas at STP to moles and moles to particles, grams or L of gas at STP 1) How many moles are in 15 grams of lithium?2) How many atoms are in 2.4 moles of sulfur?3) How many moles are in 5.6 L of argon gas at STP?4) How many moles are in 12.16 g of magnesium?What are the molecular weights of the following compound (inventory and sum)?5) NaOH 6) H3PO47) CuSO48) (NH4)2SO49. Written Explanation of Molar Conversion Problem: Convert 3.5 moles CuSO4 into grams.Part 1: Identification What is your known? _____________________________What are you looking for? __________________________What conversion factor will you use?_______________________________________________________Part 2: Math… Solve the problemPart 3: Explanation Use the following content words to explain how you solved the problem:Known, unknown, convert, units, cancel, calculate, conversion factor, multiply, divide, setup ____________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________10) How many moles are in 21g of sodium fluoride, NaF?Unit 4 – Benchmark Gram/Mole/Volume Conversions – Practice!You may use a periodic table, but NOT a calculator. SHOW YOUR WORK! Problems 1 Assume that you have an 11 gram sample of carbon dioxide gas, CO2 at standard conditions (STP)How many moles of CO2 do you have? How many molecules of CO2 do you have? What volume (in liters) should the sample occupy? Problems 2 Assume that you have a sample of propane gas, C3H8 that occupies 11.2 liters at standard conditions. How many moles of propane are contained in the sample? What is the mass in grams of the sample? How many molecules of propane are in the sample? Problems 3 You have a sample of calcium that contains 0.25 moles of calcium atoms. What is the mass, in grams, of the sample of calcium? How many atoms of calcium does the sample contain? Problems 4 You have a sample of aluminum that contains 2 x 1023 atoms of aluminum. How many moles of aluminum atoms do you have? What is the mass, in grams, of your sample of aluminum? Problems 5 You have a 5.6 liter sample of nitrogen gas, NH3, at standard conditions. How many moles of nitrogen are contained in the sample? What is the mass, in grams, of the sample? Problem 6 How many moles are in 54 grams of water, H2O?How many L do 54 grams of water, H2O occupy at STP2-step Molar Conversion and 1 step Molar Conversion PracticeParticles, grams, or L of gas at STP to moles and then to particles, grams or L of gas at STP How many particles are in 39 grams of aluminum hydroxide, Al(OH)3?1) How many grams and formula units are in 0.02 moles of beryllium iodide, BeI2?2) How many formula units are in 32.5 grams of copper (II) hydroxide, Cu(OH)2?3) How many grams are in 3.3 moles of potassium sulfide, K2S?4) How many molecules are in 1.704 x 103 grams of ammonia, NH3?5) How many grams are in 2.3 x 10-3 moles of calcium phosphate, Ca3(PO4)2?6) What is the mass of 1 mole of lithium hydroxide?7) A saltshaker filled with 29.22 grams of sodium chloride contains how many moles of sodium chloride?8) Which of the following has the greatest mass? Hint convert all to grams first! 4.2 mol of carbon or 1.2 x1024 atoms of CaCO3 or 12.6 g of Al2(NO3)39) In 60 g of N2O there are how many molecules (grams to moles and then to molecules)?10) Find the number of atoms in each of the following:a. 0.25 mole Nib. 2.0 mole S11) Find the volume of each of the following amounts of gas at STP:a. 0.75 mole of O2b. 2.5 moles N212) How many moles are in each of the following volumes of gas at STP?a. 67.2 L CO2b. 56 L HePercent Composition and Chemical FormulasPercent Composition By MassPart divided by the whole!Inventory STEP 1a. CH4 b. Mg(MnO4)2 c. Al2(SO3)3 Molar Mass STEP 2a.CH4 b. MgF2 c. C3H8 Determine the percent composition of each element STEP 3Example: Find the % comp of calcium phosphate: Ca3(PO4)23Ca = 3(40) = 120 g Ca 2P = 2(31) = 62 g P 8O = 8(16) = 128 g Omolar mass 310 g Ca3(PO4)2 Percent composition = Mass of the component X 100Mass of the whole% Ca = 120/310 x 100 = 38.7 %Ca % = 38.7%% P = 62/310 x 100 = 20.0 %P % = 20.0 %% O = 128/310 x 100 = 41.3 %O % = 41.3 % 100 % add up to check your workQuickwrite: Explain how to solve percent composition problems____________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________a.CH4 b. MgF2 c. C3H8 Practice Percent Composition Find the percent compositions of all of the elements in the following compounds:1)CuBr22)NaOH3)(NH4)2S4)N2S25) copper II sulfide6) iron III oxide7) sucrose (C12H22O11)Practice with calculator1. Identify all the steps to find the correct formula for your hydrate. Using the correct formula, calculate the percent of H2O in your hydrateNa2CO3 ? ____H20a. Mass of Crucible and Cover………………………………………49.5gb. Mass of Crucible, Cover & Hydrate………………………53.81c. Mass of Crucible, Cover, and Anhydrous Salt……… 52.722. Write the correct formula for your hydrate. Using the correct formula, calculate the percent of H2O. MgNO3? ____H20a. Mass of Crucible and Cover……………………………………………… 152 gb. Mass of Crucible, Cover & Hydrate………………………………… 157.82gc. Mass of Crucible, Cover, and Anhydrous Salt…………………154.58gWater of Hydration4217035164465000Many ionic compounds incorporate a fixed number of water molecules into their crystal structures. A compound that contains water of hydration is called a hydrate. When expressing the formula for a hydrate, it is necessary to notate the fixed number of H2O molecules following the anhydrous formula for the ionic compound. A large dot is placed between the formula and the H2O molecules. For example: CuSO4 ? 5H2O is the correct formula for the hydrated form of copper (II) sulfate pentahydrate. The water of hydration can be removed by heating the sample. Once heat is applied the H2O molecules are removed as steam to produce an anhydrous salt which often will appear different than its hydrate. Most often a hydrated crystal is of different color than its anhydrous crystal. For this example the anyhydrous salt is CuSO4.The first step to finding the formula for a hydrate is to record the mass of the hydrate. After heating the hydrate, the mass is determined for the anhydrate that remains. The mass of the water that was present is calculated by finding the difference between the mass of the hydrate and the mass of the anhydrate. The mass of the water and the mass of the anhydrate are each converted to moles using their respective molar masses. From this a whole number ratio can be determinedMass of the empty crucible 4.00gMass of the crucible plus hydrate sample 4.50 g hydrate sample mass = 0.50 gMass of the system after heating 4.32ganhydrous sample mass = 0.32 gMass of the system after a second heating 4.32g hydration water mass = 0.18 gThe second heating is to verify that in fact all of the water of hydration was removed.a. Determine the percent water of hydration in the original sample% water of hydration: mass of water mass of hydrate ×100 = 0.18 g0.50 g x 100=36%b. the compounds has the formula CuSO4 ? ?H2O. Determine how many moles of water per mole of anhydrate.CuSO4 molar mass = 159.6g ; moles of CuSO4 = 0.32g/159.6g = 0.0020 molesH2O molar mass = 18.0; moles of H2O = 0.18 g / 18.0g = 0.010 molesc. divide both mole values by the smallest-CuSO4: 0.0020 / 0.0020 = 1H2O: 0.010 / 0.0020 = 55 moles of hydration water for every mole of CuSO4 CuSO4.5H2OWhat is the molar mass of CuSO4.5H2O and is the copper percent by massHydrate Practice 21. A hydrate of magnesium sulfate has a mass of 13.52 g. This sample is heated until no waterremains. The MgSO4 anhydrate has a mass of 6.60 g. Find the formula and name of the hydrate.2. A sample of copper (II) sulfate hydrate has a mass of 3.97 g. After heating, the CuSO4 that remains has a mass of 2.54 g. Determine the correct formula and name of the hydrate.3. When 5.00 g of FeCl3 · xH2O are heated, 2.00 g of H2O are driven off. Find the chemical formulaand the name of the hydrate.4. A sample of the hydrate of sodium carbonate has a mass of 8.85 g. It loses 1.28 g when heated.Find the formula and the name of the hydrate.5. A 16.4 g sample of hydrated calcium sulfate is heated until all the water is driven off. The calcium sulfate that remains has a mass of 13.0 g. Find the formula and the chemical name of the hydrate.6. When 8.00 g of Pb(C2H3O2)2 · xH2O are heated, 1.14 g of H2O are driven off. Find the chemicalformula and the name of the hydrate.7. A hydrate is determined to be 45.43% water and 54.57% CoCl2. Find the chemical formula andname for this hydrate. (*Hint – assume that there is 100 g total of hydrate compound.)Empirical and Molecular FormulasBelieve it or not, there is more than one kind of chemical formula (insert a sharp gasp of surprise here). Judging from the heading of this section, they would be empirical and molecular formulas. Empirical formulas give the lowest whole number ratio of the atoms in a compound, whereas the molecular formula gives the exact composition of one molecule.271843553975Determine the empirical formula from the molecular formula: a) C6H6h) C2H2b) C2H6i) Na2SO4c) C3H8j) C6H4N2d) Fe3(CO)9k) P4O10e) C2H4O2l) Re2Cl6f) N2H4m) Se3O9g) CaBr2n) LiCl00Determine the empirical formula from the molecular formula: a) C6H6h) C2H2b) C2H6i) Na2SO4c) C3H8j) C6H4N2d) Fe3(CO)9k) P4O10e) C2H4O2l) Re2Cl6f) N2H4m) Se3O9g) CaBr2n) LiClEmpirical Molecular HO H2O2CH C2H2 CH C6H6NONO NO2 N2O4Empirical formulas can be calculated using experimental data:Definition: The symbols for the elements combined in a compound, with subscripts showing the smallest whole-number ratio of the different atoms in the compound Given that a certain compound is 69.58% Ba, 6.090% C and 24.32% O, calculate the empirical formula of this compound.Assume that you have 100.00 g of the compound:69.58% Ba = 69.58 g Ba6.090% C = 6.090 g C24.32% O = 24.32 g OConvert the mass of each element to moles of that element:Ba = (69.58 g Ba)(1 mol Ba/137.3 g Ba) = 0.5068 mol BaC = (6.090 g C)(1 mol C/12.01 g C) = 0.5071 mol CO = (24.32 g O)(1 mol O/16.00 g O) = 1.520 mol ODivide through each value by the smallest number of moles (0.5068)to get a 1 : 1.001 : 2.999 ratio, which rounds of nicely to give the formula BaCO3Molecular formulas can be calculated using empirical formulas:A. Definition: A formula for a molecular compound that represents ALL of the atoms found in a single molecule of that compound.The molecular formula is either the same as the empirical formula, or it is a whole number multiple of the empirical formulaExample 2 : Given that the empirical formula of a compound is CH and the molar mass is 104 g/mol, calculate the molecular formula.mass of C = 12.01 g/molmass of H = 1.01 g/mol empirical formula mass = 13.0 g/mol to find the number of CH units in the compound:# CH units = 104 gmole×1 mole13.0 g =8.00The nearest whole number is 8 so the Molecular formula = 8(CH) or C8H8Example 2 : empirical formula = HO and molecular wt. = 34.02Worksheet: Empirical Formulas and Molecular FormulaPart 1: Empirical FormulasWork each of the following problems. SHOW ALL WORK.1. A compound is found to contain 63.52 % iron and 36.48 % sulfur. Find its empirical formula.2. Determine the empirical formula of a compound containing 63.50 % silver, 8.25 % nitrogen, and the remainder oxygen.Part 2: Molecular FormulasWork each of the following problems. SHOW ALL WORK.1. The empirical formula of a compound is NO2. Its molecular mass is 92 g/mol. What is its molecular formula?2. The empirical formula of a compound is CH2. Its molecular mass is 70 g/mol. What is its molecular formula?.3. A compound is found to be 40% Carbon, 6.7% hydrogen and 53.5 % oxygen. Its molecular mass is 60 g/mol. What is its molecular formula?Chemistry: Balancing EquationsThe information in a chemical equation can be looked at in several ways.On this worksheet you will represent particles of the substances involved in a chemical reaction before and after it takes place.The unbalanced equation for the reaction of chlorine gas with hydrogen gas is34664657683400Cl2(g) + H2(g) HCl(g)Each picture shows the same bottle after something happened. The circles show a unitvolume of the gas in the jar. Draw the particles for the third picture.4597401162050044850051149350023837901168400032258007747000128587597790008915407874000297053024130002862580132715003294380209550036957093980003360420127635001082040749300030410152349500 A certain number of The same number ofThe mixture is ignited.Cl2 molecules are H2 molecules areAssume that all theput into the jar. added to the jar.Cl2 and H2 are used up.2. Show the same reaction using the fewest possible molecules. Draw the molecules in these circles.459740116205002474595116840004561205114935003803659080500239458590805004495800901700038392102920900 + Cl2 H2 HCl3. Balance the equation using the smallest possible whole number coefficients.37439608826400________ Cl2(g) + ________ H2(g) ________ HCl(g)4. Suppose you start with different amounts of the reactants. In the empty circle, show the particles after the reaction. (Be sure you account for all the particles.) On the line below the circle, describe what is in the circle.45974011620500247459511684000456120511493500101092085725003013075952500013144507175500905510126365003225165206375003803659080500239458590805004495800901700037820605651400 + 1152525-63500 37439608826400Cl2(g) + H2(g) ________ 19335741460500Chemical ReactionsRead Section 10.1 in textbook (pg 277-283) Describe how you might know a chemical reaction has occurred______________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________Chemical Equations and Reactions Introduction (277-383 textbook)When a piece of magnesium is added to dilute hydrochloric acid, fizzing occurs and hydrogen gas is released from the mixture. The fizzing is evidence that a(n) (1)__________________ has occurred between magnesium and hydrochloric acid. The name given to either magnesium or hydrochloric acid in this case is (2)______________________ , and the hydrogen gas that is released is called a(n) (3)___________________ of the reaction. Some other indications that reactions have occurred might be change of color or (4)_________________ , or formation of a solid (5)____________________ . If a thermometer is placed into a mixture undergoing chemical reaction, you might observed that the temperature has gone up or down, indicating that (6)_________________ was being released or absorbed. The short hand form by which a reaction is represented is called a(n) (7) ____________ . In using this method of representation, you must satisfy the (8)____________________ , a principle that states that matter is neither created nor destroyed. In order to satisfy this principle, you normally select the proper numerical (9)________________ to indicate the number of units of each substance taking part in the chemical change.Explain in words each of the symbols Mg (s) + 2HCl (aq) MgCl2 (aq) + H210.Mg _______________15.(aq)_______________11.(s)_______________16._______________12.+_______________17.MgCl2_______________132_______________18.H2_______________14HCl______________19(g)_______________Balancing Equations Practice Part A: Identify the following parts of each chemical formula by circling the subscripts and drawing a square around the coefficients.H2 2 HCl 4 O2 CH4 3 CO2 2 NaOHPart B: List the symbols for the atoms in each formula and give the number of each element.C2H6 ________________________________________________________________________2Mg(OH)2____________________________________________________________________4Li2O____________________________________________________________________4P4O10________________________________________________________________________________________________________________3Al(OH)3 ____________________________________________________________________Part C: Balance each of the following equations following the procedure described in class. Be sure to show your work.__P + __O2 → P4O10 ___Mg + ___O2 → __MgO___ Al2O3 → ___Al + ___O2 =P = =Mg = =Al = =O = =O = = O=Part D: Practice Problems – Balance each equation using the process from Part C. Name Products___Na + ___Br2 ___NaBr ___C + ___H2 ___CH4__Cl2 + ___NaBr ___NaCl + ___Br2 __H2 + __N2 ___NH3__CuCl2 + __H2S ___CuS + __HCl__C2H6 + ___O2 ___CO2 + ___H2OTo react or not to react? THAT is the question!Chemical changes are a result of chemical reactions. All chemical reactions involve a change in substances and a change in energy. Neither matter nor energy is created or destroyed in a chemical reaction---only changed. There are so many chemical reactions that it is helpful to classify them into 5 general types including Combustion Reactions: 437197599250500SYNTHESIS REACTIONIn a synthesis reaction two or more simple substances combine to form a more complex substance. Two or more reactants yielding one product is another way to identify a synthesis reaction. For example, simple hydrogen gas combined with simple oxygen gas can produce a more complex substance-----water!The chemical equation for this synthesis reaction looks like: reactant + reactant →productTo visualize a synthesis reaction look at the following cartoon: In the cartoon, the skinny bird (reactant) and the worm (reactant) combine to make one product, a fat bird.402907570485000DECOMPOSITION REACTIONIn a decomposition reaction a more complex substance breaks down into its more simple parts. One reactant yields 2 or more products. Basically, synthesis and decomposition reactions are opposites.For example, water can be broken down into hydrogen gas and oxygen gas. The chemical equation for this decomposition reaction looks like: reactant → product + productTo visualize a decomposition reaction look at the following cartoon: In this cartoon the egg (the reactant), which contained the turtle at one time, now has opened and the turtle (product) and egg shell (product) are now two separate substances. 517398047434500SINGLE REPLACEMENT REACTION In a single replacement reaction a single uncombined element replaces another in a compound. Two reactants yield two products. For example when zinc combines with hydrochloric acid, the zinc replaces hydrogen. The chemical equation for this single replacement reaction looks like: reactant + reactant → product + productTo visualize a single replacement reaction look at the following cartoon:Notice, the guy in the orange shirt steals the date of the other guy. So, a part of one of the reactants trades places and is in a different place among the products. 5715040195500DOUBLE REPLACEMENT REACTION In a double replacement reaction parts of two compounds switch places to form two new compounds. Two reactants yield two products. For example when silver nitrate combines with sodium chloride, two new compounds--silver chloride and sodium nitrate are formed because the sodium and silver switched places. The chemical equation for this double replacement reaction looks like: reactant + reactant -→ product + productTo visualize a double replacement reaction look at the cartoon showing the hat and people changes.ENERGY OF CHEMICAL REACTIONS Chemical reactions always involve a change in energy. Energy is neither created or destroyed. Energy is absorbed or released in chemical reactions. Chemical reactions can be described as endothermic or exothermic reactions. Endothermic ReactionsChemical reactions in which energy is absorbed are endothermic. Energy is required for the reaction to occur. The energy absorbed is often heat energy or electrical energy. Adding electrical energy to metal oxides can separate them into the pure metal and oxygen. Adding electrical energy to sodium chloride can cause the table salt to break into its original sodium and chlorine parts. Exothermic ReactionsChemical reactions in which energy is released are exothermic. The energy that is released was originally stored in the chemical bonds of the reactants. Often the heat given off causes the product(s) to feel hot. Any reaction that involves combustion (burning) is an exothermic chemical reaction. Handy Checklist for figuring out what type of reaction is taking place:Follow this series of questions. When you can answer "yes" to a question, then stop! 1) Does your reaction have oxygen as one of it's reactants and carbon dioxide and water as products? If yes, then it's a combustion reaction 2) Does your reaction have two (or more) chemicals combining to form one chemical? If yes, then it's a synthesis reaction 3) Does your reaction have one large molecule falling apart to make several small ones? If yes, then it's a decomposition reaction 4) Does your reaction have any molecules that contain only one element? If yes, then it's a single displacement reaction 5) If you haven't answered "yes" to any of the questions above, then you've got a double displacement reactionTypes of ReactionsChoose the correct symbol for the type of reaction. Place that answer in the blank at the beginning of each equation and then balance each equation correctly and write the coefficient set.S = synthesisSD = single displacementD = decompositionDD = double displacementC = combustion1. _____ Na (s) + H2O (l) NaOH (aq) + H2 (g)2. _____ CO (g) + O2 (g) CO2 (g)3. _____ FeS (s) + HCl (aq) FeCl2 (aq) + H2S (g)4. _____ NaNO3 (s) NaNO2 (s) + O2 (g)5. _____ CH4 (g) + O2 (g) CO2 (g) + H2O (g)6. _____ Fe (s) + CuNO3 (aq) Cu (s) + Fe(NO3)2 (aq)7. _____ KI (aq) + Cl2 (g) KCl (aq) + I2 (aq)8. _____ Al (s) + S (s) Al2S3 (s)9. _____ KClO3 (s) KCl (s) + O2 (g)10. _____ C4H10 (g) + O2 (g) CO2 (g) + H2OTypes of Reactions WorksheetBalance the following equations and indicate the type of reaction taking place:1)____ NaBr + ____ H3PO4 ____ Na3PO4 + ____ HBr Type of reaction: ____________________2)____ Ca(OH)2 + ____ Al2(SO4)3 ____ CaSO4 + ____ Al(OH)3 Type of reaction: ____________________3)____ Mg + ____ Fe2O3 ____ Fe + ____ MgO Type of reaction: ____________________4)____ C2H4 + ____ O2 ____ CO2 + ____ H2O Type of reaction: ____________________5)____ PbSO4 ____ PbSO3 + ____ O2 Type of reaction: ____________________6)____ NH3 + ____ I2 ____ N2I6 + ____ H2 Type of reaction: ____________________7)____ H2O + ____ SO3 ____ H2SO4 Type of reaction: ____________________Word Equations Worksheet Write the formula for each and balance the reactions:1)When dissolved beryllium chloride reacts with dissolved silver (I) nitrate in water, aqueous beryllium nitrate and silver (I) chloride powder are made.2)When isopropanol (C3H8O) burns in oxygen, carbon dioxide, water, and heat are produced.3) When dissolved sodium hydroxide reacts with sulfuric acid (H2SO4), aqueous sodium sulfate, water, and heat are formed.4)When fluorine gas is put into contact with calcium metal at high temperatures, calcium fluoride powder is created in an exothermic reaction.5)When sodium metal reacts with iron (II) chloride, iron metal and sodium chloride are formed. Combination (Synthesis) ReactionsTwo or more elements or compounds may combine to form a more complex compound. Basic form: A + X → AX Examples of synthesis reactions: Metal + oxygen → metal oxide EX. 2Mg(s) + O2(g) → 2MgO(s) Nonmetal + oxygen → nonmetallic oxide EX. C(s) + O2(g) → CO2(g) Metal oxide + water → metallic hydroxide EX. MgO(s) + H2O(l) → Mg(OH)2(s) Nonmetallic oxide + water → acid EX. CO2(g) + H2O(l) → ; H2CO3(aq) Metal + nonmetal → salt EX. 2 Na(s) + Cl2(g) → 2NaCl(s) A few nonmetals combine with each other. EX. 2P(s) + 3Cl2(g) → 2PCl3(g) Write the reactant formula, predict the product in words then write the product formula, then balance.calcium + oxygen copper + sulfur copper(II) sulfidecalcium oxide + water aluminum + bromine Decomposition ReactionA single compound breaks down into its component parts or simpler compounds. Basic form: AX → A + X Examples of decomposition reactions: Metallic carbonates, when heated, form metallic oxides and CO2(g). EX. CaCO3(s) → CaO(s) + CO2(g) Most metallic hydroxides, when heated, decompose into metallic oxides and water. EX. Ca(OH)2(s) → CaO(s) + H2O(g) Metallic chlorates, when heated, decompose into metallic chlorides and oxygen. EX. 2KClO3(s) → 2KCl(s) + 3O2(g) Some acids, when heated, decompose into nonmetallic oxides and water. EX. H2SO4 → H2O(l) + SO3(g) Some oxides, when heated, decompose. EX. 2HgO(s) → 2Hg(l) + O2(g) Some decomposition reactions are produced by electricity. EX. 2H2O(l) → 2H2(g) + O2(g) EX. 2NaCl(l) → 2Na(s) + Cl2(g) Write the reactant formula, predict the product in words and write the product formula, then balance.______NaCl ____Na + _____Cl2___ CaBr ___ Ca + ___ Br2____NCl3 ___N2 + ___ Cl2___CCl4 ___C + ___ Cl2___P4O10 ___P4 + ___O2___KI ___K + ___I2Single displacement This is when one element trades places with another element in a compound. These reactions come in the general form of: A + BC ---> AC + BOne example of a single displacement reaction is when magnesium replaces hydrogen in water to make magnesium hydroxide and hydrogen gas: Mg + 2 H2O ---> Mg(OH)2 + H2 Write the reactant formula, predict the product in words and write the product formula, then balance.1. K + AgNO3 →2. Al + H2SO4 →3. Cl2 + KI →4. Li + H2O →Quickwrite: Using one the four examples, explain how you predicted the product and how you balanced the reaction.___________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________Double displacementThis is when the anions and cations of two different molecules switch places, forming two entirely different compounds. These reactions are in the general form: AB + CD ---> AD + CBOne example of a double displacement reaction is the reaction of lead (II) nitrate with potassium iodide to form lead (II) iodide and potassium nitrate: Pb(NO3)2 + 2 KI ---> PbI2 + 2 KNO3 Write the reactant formula, predict the product formula, then balance.1) Ca(OH)2 + H3PO4 6) Al2(SO4)3 + Ca3(PO4)2 2) K2CO3 + BaCl2 7) FeBr2 + K2CO3 3) Cd3(PO4)2 + (NH4)2S 8) Ag2S + CuCl2 4) Co(OH)3 + HNO3 9) Pb(NO3)2 + HI 5) AgNO3 + KCl 10) CuS + KCl Combustion ReactionsOctane (C8H18) is a major component of gasoline. The burning of octane produce carbon dioxide (CO2) as shown in the equation below:2 C8H18 + 25 O2 → 16 CO2 + 18 H20A) Calculate the molar masses of octane and carbon dioxide. Show your calculations and include units in your answer.b) Calculate the amount of carbon dioxide, in grams, produced by the combustion of 100 grams of octane. Show your calucations and include units in your answer.Many people think it is important to reduce the amount of CO2 being released by fuel combustion because CO2 is a greenhouse gas. Propane (C3H8) is another hydrocarbon fuel used to power some motor vehicles. THE combustion of propane is shown in the equation below.C3H8 + 5 O2 → 3 CO2 + 4 H20The combustion of 100 g of propane produces 299.4 g of carbon dioxide. Assume the combustion of propane produces the same amount of energy per gram as the combustion of octane.c. Based on this information and your calculations, identify which fuel, octane or propane, is less harmful to the environment. Justify your answer.___________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________Worksheet: Writing and Identifying Equations CHEMISTRY: A Study of MatterDirections: a) Write balanced equations for the following word equations.b) In the blank to the left of the equation, tell if the equation is synthesis (S), decomposition (D), combustion (C), single replacement (SR), or double replacement (DR)._____ potassium chloride + silver (I)nitrate yields potassium nitrate + silver (I) chloride_____ iron metal + copper (II) sulfate yields iron (II) sulfate + copper metal_____ beryllium fluoride + magnesium yields magnesium fluoride + beryllium_____ aluminum sulfate + barium chloride yields aluminum chloride + barium sulfate_____ zinc metal + oxygen gas yields zinc (II) oxide_____ Ethane (C2H6) + oxygen gas yields carbon dioxide and water_____Aluminum metal reacts with aqueous zinc (II) chloride to produce Zn metal and aqueous AlCl3._____ Iron and sulfur combine and form iron (II) sulfide._____ Solid diphosphorus pentoxide can be produced from the elements oxygen and phosphorus. (Note: Solid elemental phosphorus contains 4 atoms per molecule; it is written P4.)_____ When hydrogen sulfide (H2S)gas is passed over solid hot iron (III) hydroxide, it reacts to form solid iron (III) sulfide and water vapor. Balancing Formative Practice1.In every balanced chemical equation, each side of the equation has the same number of ____.a.atoms of each elementc.molesb.moleculesd.coefficients2.What are the coefficients that will balance the skeleton equation below?AlCl3 + NaOH → Al(OH)3 + NaCla.1, 3, 1, 3c.1, 1, 1, 3b.3, 1, 3, 1d.1, 3, 3, 13.When the equation Fe + Cl2 → FeCl3 is balanced, what is the coefficient for Cl2 ?a.1c.3b.2d.44.When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed. The balanced equation for this reaction is ____.a.KH + BaCl → KCl + BaHc.2KOH + BaCl2 → 2KCl + Ba(OH)2 b.KOH + BaCl → KCl + BaOHd.KOH + BaCl2 → KCl2 + BaOH5.When the following equation is balanced, what is the coefficient for HCl? Mg(s) + HCl(aq) → MgCl (aq) + H2 (g)a. 6b. 3.c. 1d. 26.What are the coefficients that will balance the skeleton equation below? N2 + H2 → NH3 a.1, 1, 2c.3, 1, 2b.1, 3, 3d.1, 3, 27. Which of the following is a balanced equation representing the decomposition of lead(IV) oxide?a.PbO2 → Pb + 2Oc.Pb2O → 2Pb + Ob.PbO2 → Pb + O2 d.PbO → Pb + O2 8.What are the missing coefficients for the skeleton equation below?Cr(s) + Fe(NO3)2 (aq) → Fe(s) + Cr(NO3)3 (aq)a.4, 6, 6, 2c.2, 3, 3, 2b.2, 3, 2, 3d.1, 3, 3, 19.What are the missing coefficients for the skeleton equation below? Al2(SO4)3 (aq) + KOH(aq) → Al(OH)3 (aq) + K2SO4 (aq)a.1, 3, 2, 3c.4, 6, 2, 3b.2, 12, 4, 6d.1, 6, 2, 310.What is the balanced chemical equation for the reaction that takes place between bromine and sodium iodide?a.Br2 + NaI → NaBr2 + Ic.Br + NaI2 → NaBrI2 b.Br2 + 2NaI → 2NaBr + I2 d.Br + NaI2 → NaBr + I2 Law of Conservation of Mass In any physical change or chemical reaction, mass is neither created nor destroyed. Therefore, the sum of the masses of the reactants is equal to the sum of the masses of the products.Reactants are written in the left hand side of the arrow while the products are in the right hand side.massreactants = massproductsmercury(II) oxide decomposes to yield mercury metal and oxygen gas 2HgO 2Hg + O2216 g = 200 g + 16 g massreactants = massproductsSample Problem:a. In an experiment, 10.00 g of red mercury (II) oxide powder is placed in an open flask and heated until it is converted to liquid mercury and oxygen gas. The liquid mercury has a mass of 9.26 g. What is the mass of oxygen formed in the reaction?2HgO 2Hg + O2b. A student carefully placed 15.6 g of sodium in a reactor supplied with an excess quantity of chlorine gas. When the reaction was complete, the student obtained 39.7 g of sodium chloride. How many grams of chlorine gas reacted? How many grams of sodium reacted?Practice Problems: Solve the following problems. Write the reactants and products. CIRCLE YOUR ANSWERS.In the complete reaction of 22.99 g of sodium with 35.45 g of chlorine, what mass of sodium chloride is formed? 3. In a flask, 10.3 grams of aluminum reacted with 100.0 g of liquid bromine to form aluminum bromide. After the reaction, no aluminum remained, and 8.5 grams of bromine remained unreacted. How many grams of bromine reacted? How many grams of compound were formed?4. A 10.0-g sample of magnesium reacts with oxygen to form 16.6 g of magnesium oxide. How many grams of oxygen reacted?5. From a laboratory process designed to separate water into hydrogen and oxygen gases, a student collected 10.0 g of hydrogen and 79.4 g of oxygen. How much water was originally involved in the process?6. A 12.2-g sample of X reacts with a sample of Y to form 78.9 g of XY. What is the mass of Y that reacted?7. A 28.0-g sample of nitrogen combines completely with 6.0 g of hydrogen gas to form ammonia. What is the mass of ammonia formed?8. A substance breaks down into its component elements when it is heated. If 68.0 g of the substance is present before it is heated, what is the combined mass of the component elements after heating?9. A 13.0-g sample of X combines with a 34.0-g sample of Y to form the compound XY2. What is the mass of the reactants?10. Sodium chloride can be formed by the reaction of sodium metal and chlorine gas. If 45.96 grams of sodium combines with an excess of chlorine gas to form 116.89 g of sodium chloride, what mass of chlorine gas is used in the reaction?5669974-14630400297243538735000S’more Stoichiometry Definitions: ‘Stoichio’ means element and ‘metry’ means the process of measuring. The mass and quantity relationships among reactants and products in a reaction are found using the process of stoichiometry.Problem:If you are given one bag of large marshmallows, what is the maximum number of S’mores that can be made?How many boxes of graham crackers and how many chocolate bars are needed to make this many S’mores?Solutions:1st Step: Write a chemical equation using the following symbols:SubstanceSymbolUnit Mass Graham CrackerS7.00 gMarshmallowMm7.10 gChocolate PiecesOr3.30 gS’moreS2MmOr3________ g2nd Step: Balance the equation: What does the equation tell us? What do the coefficients represent?They represent the ratio of the ___________ or the ______________.3rd Step: Calculate the unit mass of the S’more (S2MmOr3)below:4rth Step: Calculating the number of units (or moles) given:Determine the number of unit marshmallows that are available in the bag. If there are 454 g marshmallows in one bag, how many marshmallows do you have?5th Step: Finding the units of other substances in the reaction:Now, determine how many units of graham crackers and chocolate segments are needed to make the maximum number of s’mores available.5th Step: Convert your number of graham crackers and chocolate segments into mass (gram):When you go to the store, you cannot quickly determine the exact number of graham crackers or chocolate segments there are in a box or bar. The mass is easy to read, however. Using mass values, you can quickly determine how much you need to buy.6th Step: Finally-convert the masses into your needed units.In this case, if a box of graham crackers has a mass of 254 g, how many boxes do you need? Also, if one chocolate bar has a mass of 49.5 g, how many bars do I need?Now we will transfer this process into the language of chemical reactions. When you complete this problem, get it checked by your teacher and you will be rewarded with the necessary items to make your S’more!If we were to add a piece of solid Cu to an aqueous solution of silver nitrate, the Silver would be replaced in a single replacement reaction forming aqueous copper (II) nitrate and solid silver. How much silver is produced is 15.00 grams of Cu is added to the solution of excess silver nitrate? Show all work and don’t forget to use significant figures.Steps 1 and 2: Write and balance the chemical equation:Step 3: Convert g Cu to moles Cu:Step 4: Convert moles of Cu to moles of Ag produced:Step 5: Convert moles Ag to grams of Ag produced:Step 6: If silver metal sells for %4.50/ounce, could you get rich from this lab? (How much would it be worth?) Conversion factor: (1 gram = 0.0353 oz)Extra: Try writing this entire stoichiometric process on one line. Remember to cancel out all necessary units!Stoichiometry Flowchart0130810Liters gas A (at STP)Particles A (atoms/molecules)sLiters gas A (at STP)Mole AMoles BParticles B (atoms/molecules)Mass B(in grams)Mass A(in grams)(in grams)00Liters gas A (at STP)Particles A (atoms/molecules)sLiters gas A (at STP)Mole AMoles BParticles B (atoms/molecules)Mass B(in grams)Mass A(in grams)(in grams)Interpretation of EquationsSilicon nitride is used in the manufacturing of high-temperature thermal insulation for heat engines and turbines. It is produced by the following reaction.3Si(s) + 2N2(g) → Si3N4(s)Interpret the equation in terms of particles, moles, and masses.How many moles Si______________________________________________________________________N2_____________________________________________________________________Si3N4__________________________________________________________________________________________________________How many particles Si______________________________________________________________________N2_____________________________________________________________________Si3N4__________________________________________________________________________________________________________How many grams Si______________________________________________________________________N2_____________________________________________________________________Si3N4__________________________________________________________________________________________________________Show using the grams calculated above that mass is conserved in the reaction.Finding and Using Molar Ratios The coefficients in a balanced chemical equation can be used to determine the relative number of molecules, formula units, or moles of a compound involved in a chemical reaction. Example: N2 (g) + 3 H2 (g) --> 2 NH3 (g)1 molecule of N2 reacts with 3 molecules of H2 to form 2 molecules of NH3OR1 mole of nitrogen (N2) reacts with 3 moles of hydrogen (H2) to form 2 moles of ammonia (NH3)The coefficients in a balanced equation can be used to write a molar ratio. Molar ratios are conversion factors that can be used to relate: moles of product formed from a certain number of moles of reactant moles of reactant needed to form a certain number of moles of a product. The number of moles of a particular reactant needed to completely react with a certain number of moles of a second reactant. For the following reaction:4 NH3 (g) + 5 O2 (g) --> 4 NO (g) + 6 H2O (g) the following molar ratios can be written: 4 moles NH3; 4 moles NH3; 4 moles NH3; 5 moles O2 ; 5 moles O2 ;4 moles NO 5 moles O2 4 moles NO 6 moles H2O 4 moles NO 6 moles H2O 6 moles H2O The inverses of each of these molar ratios can also be written.Practice Using Mole Ratios What is the molar ratio between Li and N2 in the following reaction:6 Li (s) + N2 (g) --> 2 Li3N (s) 2. The heat from a welder’s torch is produced by the burning (combustion) of acetylene gas. The reaction is represented by the following balanced chemical equation.2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g)Write the mole ratios from the balanced equation. There are 6.3. Limestone (CaCO3) is treated with hydrochloric acid and water to manufacture calcium chloride hexahydrate. This compound is used to melt ice and snow on pavements and roads. The following balanced chemical equation represents the reaction.CaCO3(s) + 2HCl(aq) + 5H2O(l) →CaCl2?6H2O(s) + CO2(g)How many moles of calcium chloride hexahydrate will be produced from 4.00 mol calcium carbonate?How many moles of hydrogen chloride will be needed to produce 1.25 mol of the hydrate?c. If 15 mol water is available for the reaction, how many moles of carbon dioxide will be released? Mole/Mole Practice CHEMISTRY: A Study of Matter1. ___NO + ___O2 → ___NO2a. 2 moles of NO will react with ______ mole(s) of O2 to produce ______ mole(s) of NO2.b. if 3.6 moles of O2 react with unlimited NO how many mole NO2 will be produced?c. How many moles of NO must react to form 4.67 moles of NO2?2. ___NH3 + ___O2 → ___N2 + ___H2Oa. 20 moles of NH3 are needed to produce ______ moles of H2O.b. How many moles of N2 will be produced if 3.5 moles of O2 react?3. ___AlF3 + ___O2 → ___Al2O3 + ___F2a. 20 moles of AlF3 will produce ______ moles of F2.b. ______ moles of AlF3 will react with 0.6 moles of O2.4. ___C3H8 + ___O2 → ___CO2 + ___H2Oa. How many moles of oxygen react with 11 moles of C3H8?b. How many moles of CO2 are produced if 3.5 moles of water are produced?5. ___O2 + ___Fe → ___Fe2O3a. Fill in the following word equation--______ moles of oxygen gas react with ______ moles of iron to produce _____ moles of iron (III) oxide.b. ______ moles of O2 are required to produce 3.0 moles of iron (III) oxide.Quickwrite: Explain how to balance a chemical equation and then to use the chemical equation to determine a mole ratio to solve a mole A → mole B problem. Using problem 5 for example. _________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________Stoichiometry Practice I1 To prevent corrosion and make paints adhere better, some aluminum products are treated with chromium (III) phosphate before finishing. Chromium (III) phosphate (CrPO4) is commercially produced by treating chromium metal with orthophosphoric acid (H3PO4).Balance the following equation for the reaction.___Cr(s) + ___H3PO4(aq) → ____ H2(g) + ____CrPO4(s)How many moles of chromium metal are needed to produce 735 g of chromium (III) phosphate?The reaction of 208 g chromium will release how many moles of hydrogen gas?2. Sand (silicon dioxide) and charcoal (carbon) are combined to form silicon carbide (SiC), a compound used in high-strength ceramic materials.a. Balance the following equation for the reaction._____SiO2(s) + _____C(s) → _____SiC(s) +___CO(g)b. What mass of silicon carbide will be produced from the reaction of 352 g silicon dioxide?c. If 1.00 g of carbon is reacted, what mass of carbon monoxide is released?Stoichiometry Practice II When Miss Elizabeth was younger she made more mistakes then she does now (thank goodness). One mistake was after having to get a new battery for her car she thought she could get some money for recycling it instead of leaving it with auto shop. Well she carried it around in her trunk for a week while trying to find a place and much to her surprise it tipped over and spilled sulfuric acid (H2SO4) which ate away at the carpet. Once she saw what had happened she added some lye (sodium hydroxide) which neutralized the acid producing water and sodium sulfate. Write and balance the chemical equation.How many grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide and you have an excess of sulfuric acid?How many grams of sulfuric acid would be neutralized by 200 grams of sodium hydroxide?If in fact 25 grams of sulfuric acid spilled would she have to add more sodium hydroxide? Check how much sodium hydroxide she would need to neutralize 25 grams of sulfuric acid and then compare that amount with 200 grams.QUICK WRITE: Explain how you solved the question did she add enough sodium hydroxide or not?_________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________Stoichiometry Practice IIIAmmonia gas reacts with oxygen gas to form nitrogen monoxide and water1. Write the chemical reaction formula and balance2.How many moles of oxygen gas are needed to react with 23 moles of ammonia3.How many grams of NO are produced when 25 moles of oxygen gas react with an excess of ammonia. Having an excess means that you don’t have to worry about how much ammonia you are starting with and you have enough to react with all the oxygen gas available in this case 25 moles.4. If 24 grams of water are produced, how many moles of nitrogen monoxide are also formed.5. How many grams of oxygen are needed to react with 6.78 grams of ammonia?Summarize how you would go about calculating the grams of product given the grams of reactant you start with.___________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________Stoichiometry Practice IVThe compound calcium carbide, CaC2 is made by reacting calcium carbonate with carbon. Industrially, calcium carbide is produced industrially in an electric arc furnace at 2000 °C. This method has not changed since its invention in 1888. Calcium carbide in contact with water, a chemical reaction immediately begins, which yields two new compounds, one of which is acetylene, a very useful flammable gas. .Balance the equation:CaCO3 + C → CaC2 + CO21. How many moles of carbon are needed produce 5.0 moles of CO2?2. How many grams of calcium carbide are produced when 4.0 moles of carbon react with an excess of calcium carbonate?3. How many moles of carbon dioxide are produced when 50 gram of calcium carbonate react with an excess of carbon?4. How many grams of carbon are needed to react with 200 grams of calcium carbonate?5.. How many grams of calcium carbonate are needed to form 641 grams of calcium carbide?Discuss which step is hardest for you to remember.____________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________Stoichiometry Practice VOctane (C8H18) an important fuel hydrocarbon in gasoline. Higher octane fuel is typically called premium gas and costs more. Octane is combusted as shown below:2 C8H18 + 25 O2 → 16 CO2 + 18 H2OWrite all possible molar ratios from this equation (there are 6 ratios)How many moles of CO2 would be produced by reacting 0.67 moles of octant with excess oxygen? (5.4 mol)How many moles of H2O would be produced by reacting 0.67 moles of octane with excess oxygen? (6.0 mol H2O)If we react 228 g of octane C8H18 with oxygen, how many mole of O2 are required? If we react 228 g of octane C8H18 with excess oxygen, how many mole of CO2 are produced?If we react 228 g of octane C8H18 with excess oxygen, how many mole of H2O are produced?Discuss why balanced reactions are needed to solve stoichiometry problems.____________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________g. If we wish to make 7.5 mol CO2, how many grams of C8H18 will be used? (107 C8H18)h. If we wish to make 7.5 mol CO2, how many grams of O2 do we need? (375 g O2)i. If we wish to make 7.5 mol CO2, how many grams of H2O will be produced? (152 g H2O)j. If we have 3.56 g C8H18, how many grams of O2 do we need to react with it?k. If we have 3.56 g C8H18, how many grams of CO2 do we produce?l. If we have 3.56 g C8H18, how many grams of H2O do we produce?m. Using the answers from j, k, and l for burning 3.56 g of octane, check if the law of conservation of mass is obeyed or not. Write the equation and grams to verify sum of reactants equals sum of products2033904-127000Limiting Reagent WorksheetDefinition of Limiting Reactant: The reactant that limits the amounts of the other reactants that can combine and the amount of product that can form in a chemical reaction." I want to make chocolate chip cookies. I look around the HUGE kitchen I work in and find 40 lbs. of butter, two lbs. of salt, 1 gallon of vanilla extract, 80 lbs. of chocolate chips, 200 lbs. of flour, 150 lbs. of sugar, 150 lbs. of brown sugar, ten lbs. of baking soda and TWO eggs. It should be clear that it is the number of eggs that will determine the number of cookies that I can make."Limiting Reactant - The reactant in a chemical reaction that limits the amount of product that can be formed. The reaction will stop when all of the limiting reactant is consumed. Excess Reactant - The reactant in a chemical reaction that remains when a reaction stops when the limiting reactant is completely consumed. The excess reactant remains because there is nothing with which it can react.No matter how many tires there are, if there are only 8 car bodies, then only 8 cars can be made. Likewise with chemistry, if there is only a certain amount of one reactant available for a reaction, the reaction must stop when that reactant is consumed whether or not the other reactant has been used up. Example Limiting Reactant Calculation: A 2.00 g sample of ammonia is mixed with 4.00 g of oxygen. Which is the limiting reactant and how much excess reactant remains after the reaction has stopped? First, we need to create a balanced equation for the reaction:4 NH3(g) + 5 O2(g)4 NO(g) + 6 H2O(g)Next we can use stoichiometry to calculate how much product is produced by each reactant. NOTE: It does not matter which product is chosen, but the same product must be used for both reactants so that the amounts can be compared.The reactant that produces the lesser amount of product in this case is the oxygen, which is thus the "limiting reactant." Next, to find the amount of excess reactant, we must calculate how much of the non-limiting reactant (ammonia) actually did react with the limiting reactant (oxygen).We're not finished yet though. 1.70 g is the amount of ammonia that reacted, not what is left over. To find the amount of excess reactant remaining, subtract the amount that reacted from the amount in the original sample. We will use this kind of thinking, with mole ratios and molar masses AND Balanced equations to figure out which reactant is limiting the reaction’s production of products.For the following reactions, find the following:Which of the reagents is the limiting reagent?What is the maximum amount of each product that can be formed?How much of the other reagent is left over after the reaction is complete?Answer the questions above given 18 grams of carbon reacts with 16 grams of oxygen to form carbon dioxideC + O2 CO2Answer the questions above given 18 grams of carbon reacts with 8 grams of hydrogen to form methane.C + 2H2 CH4Answer the questions above given 7.5 grams of nitrogen monoxide reacts with 8 grams of oxygen to form nitrogen dioxide.___NO + ___O2 → ___NO2At high temperatures, sulfur combines with iron to form the brown-black iron (II) sulfide:Fe (s) + S (l) →?FeS (s)In one experiment, 7.62 g of Fe are allowed to react with 8.67 g of S.a. What is the limiting reagent, and what is the reactant in excess?b. Calculate the mass of FeS formed.Percent Yield Calculations1)Balance this equation and state which of the types of reaction is taking place:____ Mg + ____ HNO3 ____ Mg(NO3)2 + ____ H2Type of reaction: _______________________2)If I start this reaction with 40 grams of magnesium and an excess of nitric acid, how many grams of hydrogen gas will I produce?3)If 1.7 grams of hydrogen is actually produced, what was my percent yield of hydrogen? -65405114934004)Balance this equation and state what type of reaction is taking place: Type of reaction: ______________________ NaHCO3 ____ NaOH + ____ CO25)If 25 grams of carbon dioxide gas is produced in this reaction, how many grams of sodium hydroxide should be produced?6)If 50 grams of sodium hydroxide are actually produced, what was my percent yield?Percent Yield Worksheet1)Write the equation for the reaction of iron (III) phosphate with sodium sulfate to make iron (III) sulfate and sodium phosphate.2)If I perform this reaction with 25 grams of iron (III) phosphate and an excess of sodium sulfate, how many grams of iron (III) sulfate can I make?3)If 18.5 grams of iron (III) sulfate are actually made when I do this reaction, what is my percent yield?4)Is the answer from problem #3 reasonable? Explain.5)If I do this reaction with 15 grams of sodium sulfate and get a 65.0% yield, how many grams of sodium phosphate will I make?Note Taking Guide: Episode 604 CHEMISTRY: A Study of MatterChemical Equations? a ___________________ way of reporting the _____________ of a _____________ _____________4108704102235Reactants? the _____________ substances in a _____________? placed on the _____________ side of the _____________Products? the substances _____________ during a __________________________? placed on the _____________ side of the ____________→ arrow is read as ______________Coefficients? used to ____________ ______________? represent the ______________ of _________________, ______________, or __________ of the _____________.212178923495Law of Conservation of Mass Mass of Reactants = Mass of ProductsMass _____________ be _____________ or _____________.42545009601222555208445554918618940832664408382087757095885Zn + HCl ZnCl2 + H2 H2 + O2 H2O C3H8 + O2 CO2 + H2OGuidelines for Balancing Equations? Start by _____________ an _____________ _____________.? Draw _____________ around each _____________ in the _____________.? Begin with __________ molecules or formula unit of the ___________ containing the ___________atoms.? Balance _____________ ions that appear on __________ sides of the _____________ as a single unit.? Balance _____________ and _____________ atoms _____________.KNO3→ KNO2 + O2Hydrogen and oxygen combine to produce water.7 Diatomic Elemental Molecules? Diatomic: _____________ _____________? ___________, __________, ____________, ___________, ___________, ____________, ___________Carbon disulfide reacts with oxygen to produce carbon dioxide and sulfur dioxide.Note Taking Guide: Episode 605 Descriptive Abbreviations( _____ ) ____________( _____ ) ____________( _____ ) ____________( _____ ) ____________Determining State at Room TemperatureAll ____________ are solids except for ____________, which is a ____________.Most ____________ are ____________ with these exceptions:liquid – ____________solids – ____________, ____________, ____________,____________, ____________, and ____________All ____________ are solids.____________ compounds are ____________, unless stated otherwise.____________ compounds are ____________, unless stated otherwise.When heated, solid mercury(II)oxide yields mercury and oxygen gas.Classifying Reactions1. Synthesis:____________ or ____________ substances combine to form a more____________ substance.____________ ??____________Fe (s) + ____________ ??____________H2O (l) + ____________ ??____________2. DecompositionA ____________ substance is ____________ ____________ into____________ or more ____________ substances.555561518415Activity Series of MetalsDecreasing ActivityLithiumPotassiumBariumCalciumSodiumMagnesiumAluminumManganeseZincChromiumIronCadmiumNickelTinLead(Hydrogen)CopperMercurySilverGold00Activity Series of MetalsDecreasing ActivityLithiumPotassiumBariumCalciumSodiumMagnesiumAluminumManganeseZincChromiumIronCadmiumNickelTinLead(Hydrogen)CopperMercurySilverGoldAB ??____________2H2O (l) ??____________ + ________________________ ??____________ + ____________3. Single Replacement66503549842500A free ___________ replaces a ___________ ___________ element in a __________.A + BY ??____________ + ____________Zn (s) + __________ ??___________ + ___________2Al (s) + __________ ??___________ + ___________Cu (s) + MgCl2 (aq) ??____________Activity Series: an _________ of elements in the order of their _________ to ________4. Double ReplacementThe ____________ of reacting ____________ ____________ each other.Normally takes place in an ____________ ____________.Also called ____________ reactionsAX + BY ??____________ + ____________2KI (aq) + __________ ??__________ + __________Precipitate: an ____________ ____________may be ____________ in an equation by ____________ or ____________?NaCl (aq) + ___________ ??__________ + _________5. CombustionInvolves the ____________ of a substance with ____________.Often called ____________.The ____________ ____________ of a ____________ produces ____________ and ____________.CxHy + O2 ??____________ + ____________C3H8 (g) + 5O2 (g) ??____________ + ____________CH4 (g) + __________ ??___________ + ___________Note Taking Guide: Episode 801 CHEMISTRY: A Study of MatterStoichiometrystudy of the ____________ relationships in a ____________ ____________based on ________________ equations2 Mg + O2 → 2 MgOThe ___________ in a ___________ ___________ give the ___________ ___________ for the ___________ involved in the ___________.Ex. Problem: When elemental aluminum reacts with elemental iodine, aluminum iodide is produced.mole ratios: _____ Al: _____ I2_____ Al: _____ AlI3_____ I2: _____ AlI3If you start with 4 moles of Al, how many moles of Al3 will be produced?Problem SetN2H4 + N2O4→ N2 + H2OBE SURE TO BALANCE THE EQUATION FIRST!!Mole to MoleKnown 2.72 moles N2H4 how many moles N2O4 = Known 2.72 moles N2H4 how many moles N2 = Moles and GramsHow many moles of water will be produced when _______ grams of hydrogen gas react with the oxygen in the air?(Hint: To “make the switch” between different substances in a reaction, use the ______ ratio from the ___________ equation.)Problem Set Two BE SURE TO BALANCE THE EQUATION FIRST!!In photosynthesis, carbon dioxide and water react to form glucose, C6H12O6 and oxygen gas.___CO2 + ___H2O → ___C6H12O6 + ___O2If 15.6 grams of carbon dioxide react, how many moles of glucose will be produced?How many grams of carbon dioxide must react to produce 0.25 moles of glucose?When nitrogen and hydrogen react, they form ammonia gas, which has the formula NH3. If 56.0 g of nitrogen are used up in the reaction, how many grams of ammonia will be produced?Summary Explain in your own words________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________438150-6604000Culinary Chemistry: Stoichiometry Made SimpleBackgroundStoichiometry is based on the law of conservation of mass which states that the mass of the reactants in a chemical reaction equals the mass of the products. Stoichiometry provides a means for researchers to use calculations in order to predict the amount of product (mass, moles, volume) that can be produced by a given quantity of reactants as well as the percent yield for that chemical reaction. This would be important in the manufacturing of drugs in determining a quantity of substance needed and, keeping in mind that medication may react or change in accordance with other metabolic processes of the body, may require an additional amount to compensate for these effects. Both pharmaceutics and pharmacokinetics address quantifying the amount of drug necessary for each patient, with a unique weight, and how to best deliver that drug. You will play the role of pharmacologist by reacting baking soda and vinegar and using stoichiometry to calculate quantity of product yield.CH3COOH + NaHCO3 ? NaCH3COO + H2O + CO2 Vinegar baking sodasodium acetatewatercarbon dioxideObjective: To predict the amount of carbon dioxide gas expected as a product and to calculate percent yield.Materials:4 g baking soda50 mL vinegar1 mL disposable pipette2-250 mL beakers50-mL graduated cylinderdigital balanceProcedureTaskResponse1. Weigh a clean, dry 250-mL beaker on the digital balance. Record the mass (g) of this empty beaker.2. Mass out 4 g of baking soda (NaHCO3) in the 250-mL beaker that you weighed in #1. Calculate the number of moles in 4 g of baking soda (NaHCO3). Show your work.3. Measure 50 mL of vinegar (CH3COOH) using the 50-mL graduated cylinder. Using the second 250-mL beaker, record the mass (g) of the vinegar.4. Using a 1-mL disposable pipette, add 1 mL of vinegar to the baking soda. What observations provide evidence that a chemical reaction is occurring?7054856753225009544057942580005. Continue adding vinegar to the baking soda 1 mL at a time until the chemical reaction no longer occurs. How will you know that a chemical reaction is no longer occurring?6. When your group is confident that there is no longer a chemical reaction, weigh the beaker with the new products. Record the total mass (g).7. Calculate the mass (g) of the products only by subtracting the weight of the beaker that you recorded in #1.8. Record the final weight (g) of the unused vinegar.9. Based on your measurements, calculate the amount of carbon dioxide (CO2) that was released as a product.10. Calculate the expected amount of carbon dioxide that would be produced by the chemical reaction.11. How does your expected CO2 produced compare to the actual CO2 produced? Can you explain any possible sources of error?12. Calculate percent yield of CO2.actual yield -theoretical yield X 100 = % yield13. Calculate percent error.actual yield – theoretical yield X 100 = % error theoretical yield14. The law of conservation of matter and energy states that matter is not created nor destroyed during a reaction. If this is true, then explain why the mass of the products is less than the total mass of the reactants.P a r t B . R o o t C a n a l St o i c h i o m et r yCalcium hydroxide is sometimes used in dentistry to temporarily fill the space left by a root canal. The equation for the formation of calcium hydroxide can be found below. Balance the chemical equation by placing the appropriate coefficients on the lines._____ CaCl2 + NaOH ? ??Ca(OH)2 + NaClTaskResponse1. Calculate the molar mass of the reactants and the products in the chemical reaction above.Molar Mass (g/mol)ReactantsCaCl2NaOHProductCa(OH)2NaClImagine that a dentist performs this reaction four times using different amounts of the reactants. Fill in themissing information below.ReactionQuantityReactantsProductsCaCl2NaOHCa(OH)2NaCl1Moles1.00 mol2.00 mol1.00 mol2.00 molGrams2Moles0.500 molGrams55.5 g37.0 g58.5 g3Moles0.200 mol0.100 molGrams4MolesGrams10.0 gTaskResponse2. How many moles of Ca(OH)2 are formed for every mole of NaOH used?3. For every 0.50 mol of Ca(OH)2 formed, how many moles of NaCl are formed?4. How many grams of calcium chloride, CaCl2, do you need to make 20.0 g of calcium hydroxide, Ca(OH)2?P a r t C . H uma n B o n e s S t o i ch i o m e t ryThe chemical equation for the reaction that forms calcium phosphate, the main ingredient in human bones, can be found below. Balance the chemical equation by placing the appropriate coefficients on the lines. CaCl2 + Na3PO4 ? ??Ca(PO4)2 + NaClTaskResponse1. Calculate the molar mass of the reactants and the products in the chemical reaction above.Molar Mass (g/mol)ReactantsCaCl2Na3PO4ProductCa(PO4)2NaClImagine that a physician performs this reaction four times using different amounts of the reactants in order to develop human tissue for bone grafting. Fill in the missing information below.ReactionQuantityReactantsProductsCaCl2Na3PO4Ca(PO4)2NaCl1Moles3.00 mol2.00 mol1.00 mol6.00 molGrams2Moles2.00 molGrams666 g620 g702 g3Moles0.200 mol0.100 molGrams4MolesGrams9.92 gTaskResponse2. For every mole of Na3PO4 used, how many moles ofCa3(PO4)2 are formed?3. For every 0.500 mol of Ca(PO4)2 formed, how many moles of CaCl are used?4. How many grams of calcium chloride (CaCl2) do you need to make 20.0 g of human bone? DOW goes Agro…Agrosciences, that is!Imagine you are working as a chemist at Dow Chemicals. You are responsible for ordering chemicals for a new fertilizer that Dow will be producing next year. The following information is necessary for your order:63817537465001 mole contains 6.02 x 1023 molecules1 mole of gas takes up 22.4 L (or 22.4 dm3) of space1 mole of fertilizer requires 2 moles of NH3 and 3 moles of CH4Directions: Use the above information to solve the following problems. Show your work.1. You are making 150, 000 moles of fertilizer. a. How many moles of NH3 do you need?b. How many moles of CH4 do you need?2. a. How much will the NH3 weigh in grams?b. How much will the CH4 weigh in grams?3. Your storage tank holds 1, 000, 000 L. How many moles of gas would it hold?4. You place your order, but the company that provides CH4 can only obtain 15,000 moles of CH4. How many moles of NH3 will you be able to use with this quantity of CH4?5. Using your information from question #4…a. How many molecules of NH3 will you order?b. How much volume in liters (L) will it take up?c. How much will it weigh in grams?6. If it costs $1.75 per mole of fertilizer produced, how much will it cost to make 150, 000 moles?Identify the Controls and Variables -514357874000Experiment 1 Smithers is greedy and wants more money so he needs workers that work harder. Smithers thinks that a special juice will increase the productivity of workers. He creates two groups of 50 workers each and assigns each group the same task (in this case, they're supposed to staple a set of papers). Group A is given the special juice to drink while they work. Group B is not given the special juice. After an hour, Smithers counts how many stacks of papers each group has made. Group A made 1,587 stacks, Group B made 2,113 stacks.You have been hired to evaluate the Smithers experiement.1. What was the initial observation?_________________________________________________2. Identify Smithers’ hypothesis______________________________________________________________________________________________________________________________3. Which is the control group? ____________________________________________________4. Which is the experimental group? ________________________________________________5. Identify the independent variable. _______________________________________________6. Identify the dependent variable. _________________________________________________7. What factors were controlled?__________________________________________________8. What is the outcome?_________________________________________________________9. Given the experimental design, what should Smithers' conclusion be? ______________________________________________________________________________________________________________________________________________________________________________10. How do you think the experiment could be improved? _______________________________________________________________________________________________________________________________________________________________________________________Bellringers11/4/13 What is the molar mass of Ca(NO2) 211/5/13 Which best describes the current atomic theory?A Atoms consist of electrons circling in definite orbits around a positive nucleus.B Atoms are composed of electrons in a cloud around a positive nucleus.C Atoms can easily be split, at which time they become radioactive.D An atom’s mass is determined by the mass of its neutrons.After 1911, most scientists accepted the theory that the nucleus of an atom was very dense and very small and had a positive charge. What led scientists to accept this theory?A Dalton’s theory of the atom was over 100 years old.B Scientists before 1911 used the scientific method of inquiry improperly.C A new model proved that the quantum theory of the atom was inaccurate.D Rutherford did an experiment firing alpha particles at a thin piece of gold foil.What is the nuclear composition of uranium-235?A 92 electrons + 143 protonsB 92 protons + 143 electronsC 143 protons + 92 neutronsD 92 protons + 143 neutronsWhich best describes the relationship between subatomic particles in any neutral atom?A The number of protons equals the number of electrons.B The number of protons equals the number of neutrons.C The number of neutrons equals the number of electrons.D The number of neutrons is greater than the number of protons.What is the identity of the ion that consists of 7 protons, 6 neutrons and 10 electrons? What is the identity of the ion that consists of 9 protons, 10 neutrons, and 10 electrons?11/6/13 What is the mass of 3.01 x 1023 particles of CaSO4?11/7/13 What is the name of the compound PbO2 ?A lead oxideB lead(II) oxideC lead oxide(II)D lead(IV) oxideWhat is the chemical formula for calcium nitrate?A CaNO3B Ca(NO2) 2C Ca(NO3) 2D Ca 3 N2Explain how you determined the formula.4800600-1143000011/8/13 Which substance listed in the table is a liquid at 27°C? A IB IIC IIID IV40005004508500The table shows the lattice energy for some ionic compounds. Based on these data, which of these compounds would require the most energy to separate the bonded ions?11/11/13What type of bonding is associated with compounds that have the following characteristics:?high melting points?conduct electricity in the molten state?solutions conduct electricity?normally crystalline solids at room temperature.A covalentB ionicC hydrogenD metallicWhat situation results in a polar covalent bond?A. two nonmetals bonding, with a small difference in electronegativityB. two nonmetals bonding, with a large difference in electronegativityC. two metals bonding, with a small difference in electronegativityD. a metal and a nonmetal bonding, with a large difference in electronegativity11/12/13 Which is a unique characteristic of the bonding between metal atoms?A Atoms require additional electrons to reach a stable octet.B Atoms must give away electrons to reach a stable octet.C Atoms share valence electrons only with neighboring atoms to reach a stable octet.D Delocalized electrons move among many atoms creating a sea of electrons.High pressure helps to disrupt hydrogen bonds. How would high pressure affect the temperature at which ice will melt?A. High pressure will lower the temperature at which ice will melt.B. High pressure will raise the temperature at which ice will melt.C. Hydrogen bonds do not affect the freezing point, so it will not change the temperature at which ice will melt.D. The freezing point will remain the same because the high pressure will negate the effect of the hydrogen bondsExplain why you selected the answer you did________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________11/13/13Which pair of elements would most likely bond to form a covalently bonded compound?A sodium and fluorineB barium and chlorineC phosphorus and oxygenD magnesium and sulfurA solid element looks silvery and shiny when its surface has been freshly sanded and polished. It will stretchwithout breaking if enough pulling force is applied. This element is most likely classed as aa. periodic element. b. nonmetal.c. halogen.d. noble gas. e. metal.The set of elements containing only nonmetals isa. I, H, Ag. b. C, Cl, Li.c. Al, Sr, K.d. Br, Fe, He. e. Cl, S, P.The set of elements containing only metals isa. Cu, Br, Fe.b. Zn, Li, Ca.c. Sr, Al, Cl. d. K, O, Ag. e. P, Ag, N.In the Periodic Table, elements with similar properties are grouped ina. diagonal rows. b. horizontal rows.c. periods. d. vertical columns.e. rectangular blocks.11/14/13 2745105698500Which of the three types of radiation will penetrate the paper and wood? A alpha, beta, gammaB alpha and beta onlyC gamma onlyD beta onlyComplete and identify the type of nuclear equation92238U →90234Th+ ______41160702603500In the figure, what type of nuclear activity is represented? A fissionB fusionC alpha emissionD beta emissionThe half-life of phosphorus-32 is 14.30 days. How many milligrams of a 20.00 mg sample of phosphorus-32 will remain after 85.80 days?A 3.333 mgB 0.6250 mgC 0.3125 mgD 0.1563 mg11/15/13 A chemical reaction is represented by the following word equation:magnesium + sulfuric acid → hydrogen + magnesium sulfatea. What are the products of this reaction?b. What are the reactants in this reaction?When fluorine gas is put into contact with calcium metal at high temperatures, calcium fluoride powder is created in an exothermic reaction. Write out the formula for the reactants and product, then balance.11/18/13Which of the following is a chemical property of a substance? The substancea. floats on the surface of mercury.b. is clear and colorless.c. is attracted by a magnet.d. is soluble in water.e. coats itself with an oxide when exposed to air.When zinc metal is dropped into hydrochloric acid, which gas or gases would be produced?a. oxygen, hydrogen, and carbon dioxide gasesb. hydrogen and oxygen gasesc. oxygen gas onlyd. carbon dioxide gas onlye. hydrogen gas only11/28/13 Which best explains why cations are smaller than the atoms from which they are formed?A The metallic atom gains electrons, causing a larger effective nuclear pull.B The metallic atom loses electrons, resulting in loss of an entire energy level.C The nonmetallic atom gains electrons, causing a larger effective nuclear pull.D The nonmetallic atom loses electrons, resulting in loss of an entire energy level.Diagram a bohr atom that has become a cation11/19/13 Which correctly lists four atoms from smallest to largest radii?A. I, Br, Cl, FB. F, I, Br, ClC. Si, P, S, ClD. Cl, S, P, Si11/30/13 Which have the lowest electronegativities?A alkali metalsB halogensC rare earth elementsD transition metals11/20/13 How many molecules are contained in 55.0 g of H2SO4 ?A 0.561 moleculeB 3.93 moleculesC 3.38 x1023 moleculesD 2.37 x 1024 molecules12/2/13 A compound has an empirical formula of CH2O and a molecular mass of 180 g. What is the compound’s molecular formula?A C3H6O 3 B C6H12O6C C6H11O7D C12H22O1112/3/13 Which of the following shows the correct number of atoms of each element in the formula Mg(NO3)2A 1 magnesium atom, 2 nitrogen atoms, and 6 oxygen atomsB 1 magnesium atom, 2 nitrogen atoms, and 5 oxygen atomsC 1 magnesium atom, 1 nitrogen atom, and 6 oxygen atomsD 1 magnesium atom, 1 nitrogen atom, and 5 oxygen atoms12/4/13Which example indicates that a chemical change has occurred?A When two aqueous solutions are mixed, a precipitate is formed.B As ammonium nitrate dissolves in water, it causes the temperature of the water to decrease.C Alcohol evaporates when left in an open container.D Water is added to blue copper(II) chloride solution. The resulting mixture is lighter blue in color.List out some other indicators of a chemical change (refer to Unit 2 IN)12/5/13 Atoms of the noble gases are generally inert because —A they are too large to reactB they are not chargedC they are neutral atomsD their outer electron levels are filled12/6/13What coefficients are required to balance this equation? _Fe2O3 ??_CO →?_Fe ??_CO2A 2, 6, 3, 6B 1, 3, 2, 3C 1, 1, 2, 2D 1, 1, 2, 112/9/13Consider this reaction: NH3 (g) ??HCl (g) →?NH4Cl (s)Which type of reaction does this equation represent?A combustionB decompositionC single replacementD synthesis12/10/13There is no doubt that a chemical reaction has occurred ifa. there has been an overall volume change.b. the form or state has been changed.c. a new substance has been formed.d. there has been a change of state.e. heat has been given off.Which of the following is a physical property of sugar?a. It decomposes readily.b. It is a white crystalline solidc. It's composition is carbon, hydrogen, and oxygen.d. It turns black with concentrated sulfuric acid.e. It can be decomposed with heat.12/11/13If the quantity of 1 mol of carbon is 12, what can be said about the quantity of 1 mol of lithium?A. 1 mol of lithium should also be 12 g.B. 1 mol of lithium should be 3 g (atomic number).C. 1 mol of lithium should be 4 g (number of neutrons).D. 1 mol of lithium should be 7 g (atomic weight).If one mole of carbon-12 has a mass of 12 g, what should be the mass of 1 mol of the isotope carbon-13 (atomic number = 6; atomic mass = 13)?A. 6 gB. 7 gC. 12 gD. 13 g12/12/13 What products are formed when the metal potassium is added to water?A K and H2OB KOH and H2OC K2O and H2D KOH and H2Consider this reaction:3Ca (s) ??2H3PO4 (aq) →?Ca3(PO4)2 (s) ??3H2 (g)How many moles of calcium are required to produce 60.0 g of calcium phosphate?A 0.145 moleB 0.194 moleC 0.387 moleD 0.581 mole12/13/13 Methane (CH 4) is combusted/burned in oxygen according to this balanced chemical equation:CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (g)What volume of carbon dioxide is formed when 9.36 liters of methane are burned in excess oxygen at STP?A 9.36 LB 15.0 LC 18.7 LD 22.4 L12/16/13 Which set of equipment would be most useful to determine the density of a liquid?A Balance and periodic table48825156477000B Periodic table and graduated cylinderC Balance and graduated cylinderD Graduated cylinder and thermometerWhat is the volume of the liquid in the graduated cylinder? A 13.00 mLB 13.50 mLC 14.00 mLD 14.50 mLA student is given a container of potassium nitrate crystals. In order to determine the exact mass of the potassium nitrate using a triple beam balance, he must know the —A mass of the filled container and the chemical formula for potassium nitrateB mass of the filled container and the density of potassium nitrateC volume of the filled container and the volume of the potassium nitrateD mass of the empty container and the mass of the filled container12/18/13Iodine-131 is a radioactive isotope with a half-life of 8 days. How many grams of a 64 g sample of iodine-131 will remain at the end of 24 days?Copper sulfide is formed when copper and sulfur are heated together. In this reaction, 127 grams of copper reacts with 41 g of sulfur. After the reaction is complete, 9 g of sulfur remains unreacted. What is the mass of copper sulfide formed?Quarter II Review Questions Practice TestElements from which two groups in the periodic table would most likely combine with each other to form an ionic compound? From: Virginia End-of-Course Assessments, 2001 Chemistry A1 and 2 B1 and 17 C16 and 17 D17 and 18What is the approximate mass of one mole of CO2? From: 2008 Virginia End-of-Course Assessments, Chemistry A 24 g B 44 g C 28 g4343400-444500 D 56 gA student calculated the molar mass of Ca(OH)2 as follows:The answer he calculated is wrong. Which labeled step contains his mistake?A. Step 1B. Step 2C. Step 3D. Step 4In chemical compounds, covalent bonds form when — From: 2003 Virginia End-of-Course Assessments, ChemistryA. the electronegativity difference between two atoms is very largeB. electrons are completely transferred between two metalsC. pairs of electrons are shared between two nonmetal atoms D. two nonmetal ions are attracted to each other by opposite charges477964518669000If the diagram below was the correct representation for the Lewis structure of a molecule, then the X would be representative of the element — From: 2003 Virginia End of Course Assessments, ChemistryA OxygenB. NitrogenC. FluorineD. PotassiumThe sample below contains approximately 9.03 x 1023 atoms of Carbon. The sample most likely contains…A. 1 mole of CarbonB. 1.5 moles of CarbonC. 1 molecule of Carbon53701955461000D. 6.022 x 1023 molecules of CThe structural formula of methane is shown. From the elements making up the compound, this molecule is most likely… A. crystalline B. ionic C. covalent D. highly polarA compound has the empirical formula CH2O and a gram-formula mass of 60 grams per mole. What is the molecular formula of this compound? From: 2009 Aug NY Regents (Chemistry)A) CH2OB) C2H4O2 C) C3H8OD) C4H8O4The mass of one atom of Potassium is...1.54 x 1022 gB 6.49 x 10-23 gC. 3.15 x 10-23 gD. 1.14 x 1022 gWhich atom in the ground state has the most stable valence electron configuration? From: 2009 June NY Regents (Chemistry)KB. SiC. ScD.KrStandard temperature and pressure refers to: a) 0 atm and 273 Kb) 1 atm and 273 Kc) 101.325 kPa and 0 Kd) more than one of the aboveThe Law of Conservation of Mass states that mass is neither created nor destroyed in an ordinary chemical reaction. When an iron nail rusts, it seems to get heavier in mass. Does the iron nail follow the Law of Conservation of Mass?No, rusting is an exception to the Law of Conservation of Mass.No, since rusting is a chemical change it does not follow the Law of Conservation of Mass.Yes, the iron rearranges its protons so that the masses are the same before and after the reaction and rusting follows the Law of Conservation of Mass.Yes, iron chemically combines with the oxygen in the air so if you add the oxygen into the mass of the chemicals before the reaction, the mass after the reaction is the same.When wood burns, a small amount of ashes is made. Why is the mass of the wood before the fire not equal to the mass of the ashes after the reaction?The mass of the wood has been destroyed.The mass of the wood and the oxygen that allowed it to burn will equal the mass of the ashes and the gas given off during the burning.The mass of the wood and the ashes equals the mass of the oxygen and the smoke given off during the time that the wood burned.The wood has holes in it so it is actually lighter in mass than it appears. The mass of just the wood will equal the mass of just the ashes after the burning.How does the Law of Conservation of Mass apply to a burning candle?The amount of wax before the reaction equals the amount of energy afterwards.The mass of the wick before the reaction equals the mass of the smoke afterwards.The mass of the wick, wax that burned and the oxygen that helped the flame before the reaction equals the mass of the smoke and the gases released after the reaction.The mass of the molecules of the candle before the reaction equals the mass of the candle and burned wick after the reaction.Which of the following reactions best illustrates the Law of Conservation of Mass?H2O2 → H2O + O2Na + CuS → Na2S + 2 CuK + AgCl → KCl + AgNaOH + 2 HCl → NaCl + H2OWhen sodium chloride reacts with calcium oxide to form sodium oxide plus calcium oxide, which of the following equations best illustrates the Law of Conservation of Mass?A. NaCl + CaO → Na2O + Ca Cl2B 4 NaCl + CaO → 2 Na2O + CaCl2C 2 NaCl + CaO → Na2O + CaCl2D 3 NaCl + 2 CaO → Na2O + 3 CaCl217. In the following reaction: 2NaN3 decomposes to form 2Na + 3N2. If 500 grams of NaN3 decomposes to form 323.20 grams of N2. How much Na is produced?18. How many moles of magnesium oxide are produced when 96 grams of oxygen gas react with 133 grams of magnesium metala) 3.00 mol MgOb) 6.00 mole MgOc) 5.47 mol MgOd) 2.74 mol MgO19. In a chemical reaction, the mass of the products _______.a) is less than the mass of the reactants b) is greater than the mass of the reactantsc) is equal to the mass of the reactantsd) has no relationship to the mass of the reactantsATOMIC STRUCTURE REVIEW WORKSHEET What are cathode rays? Why are they called cathode rays? Do the cathode rays have a charge, if so what is the charge on each particle? What are the differences in charge and mass among protons, neutrons, and electrons? A particular atom of potassium contains 19 protons, 19 electrons, and 20 neutrons. What is the atomic number of this atom? What is the mass number? Write the isotopic symbol for this potassium nucleus (as we did in class.)How many electrons, neutrons, and protons are in atoms of chlorine with a mass number of 35 (neutral state)? How many electrons, neutrons, and protons are in the atoms of thorium with a mass number of 232 (neutral state)? Yttrium was discovered in 1794. It is one of the elements used in superconductors. How many electrons, protons, and neutrons are in an atom of yttrium-88 (neutral state)? Compare the amount of energy involved in chemical changes to the amount of energy resulting from nuclear changes. What are the differences among the three types of natural radiation?Complete the following ChartIsotopeMass NumberProtonsNeutronElectrons in the Neutral AtomType of Elementcarbon-14phosphorus-32nickel-63iridium-192iron-54Find the average atomic mass of silver if 51.83% of the silver atoms occurring in nature have a mass of 106.905 amu and 48.17% of the atoms have a mass of 108.905 amu. Bonding Basics Review Section A: Complete the chart using a periodic table to help you. 577900868580Type of Element00Type of ElementAnswer these questions: An atom that gains one or more electrons will have a ____________________ charge. An atom that loses one or more electrons will have a ____________________ charge. An atom that gains or loses one or more electrons is called an ____________. A positive ion is called a ______________ and a negative ion is called an _______________. Section B: What is an ionic bond? Atoms will transfer one or more ______________________ to another to form the bond. Each ion is left with a ______________________ outer shell. An ionic bond forms between a ____________ with a positive charge (cation) and a ____________ with a negative charge (anion). Section C: What is a covalent bond? Atoms ______________________ one or more electrons with each other to form the bond. Each atom is left with a ______________________ outer shell. A covalent bond forms between two ______________________ elements. Draw Lewis Dot Structures showing CO2 and H2O and NH3 and N2What is the octet rule? __________________________________________________________What are some exceptions to the octet rule and how many electrons do these exceptions "desire"_______________________________________________________________________________________________Section D: What is a metallic bond? ______________________________________________________________________________________________________________________________________________________________________________________________ Section E: What kind of reaction? NaOH + KNO3 --> NaNO3 + KOH _____________________________CH4 + 2 O2 --> CO2 + 2 H2O _____________________________2 Fe + 6 NaBr --> 2 FeBr3 + 6 Na _____________________________ CaSO4 + Mg(OH)2 --> Ca(OH)2 + MgSO4 _____________________________Pb + O2 --> PbO2 _____________________________f. Na2CO3 --> Na2O + CO2_____________________________Mole Relationships in Chemical ReactionsThe mole provides a convenient way of finding the amounts of the substances in a chemical reaction. The diagram below shows how this concept can be applied to the reaction between carbon monoxide (CO) and oxygen (O2), shown in the following balanced equation. O2(g) + 2 CO (g) 2CO2(g)Use the equation and the diagram to answer the following questions.2377440128905001. What information is needed to make the types of conversions shown by double-arrow 1 in the diagram?2. What conversion factors would be needed to make the conversions represented by double-arrow 2 in the diagram for CO? By double-arrow 6 for CO2?3. What information is needed to make the types of conversions represented by double-arrows 3 and 7 in the diagram?4. What conversion factors would be needed to make the conversions represented by double-arrow 3 in the diagram for CO?5. Why is it not possible to convert between the mass of a substance and the number of representative particles, as represented by double-arrow 4 of the diagram?6. Why is it not possible to use the mass of one substance in a chemical reaction to find the mass of a second substance in the reaction, as represented by double-arrow 5 in the diagram?Study Guide – Finals – 1st sem 13-14A. Use the letters corresponding to the element(s) described below. More than one letter may fit the description.1. an alkali metal 8. an alkaline earth metal 2. a noble gas 9. an active nonmetal3. a metalloid 10. an inner transition element 4. a transition element 11. a halogen 5. a nonmetal 12. a metal 6. a lanthanide13. an actinide 7. has 7 valence electrons 14. has same Lewis structure as silicon8. has this lewis structure B. Periodic trends:PropertyGroupPeriodAtomic radiusIonization energyElectronegativity Which group hasa. largest atomic radius b. highest ionization energy c. lowest electronegativity d. smallest size Compare cations and ions with their respective atomsC. Complete the table: SymbolNameAtomic NumberMassNumberNumber of protonsNumberof neutronsNumberof electronsCobalt-5828583340Describe the following:AtomsNucleusDistinguish:Ionic bondsCovalent bondsMetallic bondWhat type of elements give off valence electrons to achieve a configuration of a noble gas?How is a covalent bond formed?Write the Lewis structure for NH3What type of elements receive valence electrons to achieve a configuration of a noble gas?How is an ionic bond formed?Write the Lewis structure for CO2Which group of metals is the most chemically active?Write the Lewis structure for F2Write the Lewis structure for C2H4Which group of nonmetals is the most chemically active?Write the Lewis structure for O2The composition of a com-pound contains only C, O, and H atoms. What type of bond does the compound have? According to the periodic table, which two elements in each set of elements will likely form an ionic bond?A 1 14 17 18B 2 3 17 18 Write the Lewis structure for H2OGiven the chemical formula of a compound, how will you tell whether the compound is an ionic compound or molecular compound?Elements in the same group have similar physical and chemical properties because they have the same number of _____________? Of the seven diatomic molecules, which ones contains A double bond?A triple bond?Write the Lewis structure for N2What type of elements have atoms arranged in crystal structure?Solid, liquid or gas?Which groups on the periodic table would form ions with the following charges: 1+ c. 2+1- d. 2-Show how you determine the mass of one mole of CO2In the periodic table, what group of elements has the most stable valence electron configuration in the ground state? Using the electronegativity values on p 263, how would you know if the bond between two atoms is ionic?Show how you determine the mass of one mole of Mg (C2H3O2)2In a binary ionic compound, one of the elements is Cl. Which of the following would the other element most likely to be?Cl I Mg BrGiven different pairs of atoms, how would you decide which has the most polar bond?Show how you determine the mass of one mole of Fe(NO3)3What are the seven diatomic molecules?The Lewis structure of an atom has eight dots. Name the elements with the same Lewis structure.Given several bars of different metals each containing one mole. Identify the metals with the following approximate masses. 27 g 65 g 59 g40 gWhich part of the periodic table are these located?metals __________nonmetals _________metalloids _________ Which one has a larger ion than its neutral atom?a. Ca b. Fc. Zn d. CsWhat type(s) of elements would make a. ionic bondb. covalent bond ................
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