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What is the difference between a chemical reaction and physical change? When you watch a reaction occur, what are some hints that it is a chemical reaction? Ch. 11 Chemical Equations Reactions Describing Chemical Reactions Objectives List three observations that suggest that a chemical reaction has taken place. List three requirements for a correctly written chemical equation. Write a word equation and a formula equation for a given reaction. Balance a formula equation by inspection. Chemical Reactions when a substance changes identity reactants- original products- resulting law of conservation of mass total mass of reactants = total mass of products Chemical Reactions chemical equation represents identities and relative amounts of reactants and products in the chemical reaction uses symbols and formulas Hints of Chemical Rxn heat can also happen with physical changes gas or light bubbles means a gas is being created as product precipitate solid is being created color change Writing Chemical Equations most pure elements written as elemental symbol diatomic molecules molecule containing only 2 atoms some elements normally exist this way H2, O2, N2, F2, Cl2, Br2, I2 other exceptions • sulfur: S8 • phosphorus: P4 Word Equations uses names instead of formulas helps you to write formula equation Example Description: Solid sodium oxide is added to water at room temperature and forms sodium hydroxide. Word Equation: sodium oxide + water sodium hydroxide Formula Equation: Na2O + H2O NaOH Symbols Used in Equations yields reversible above arrow: or heat MnO2 or Pt 25°C 2 atm heated catalyst specific T requirement specific P requirement after a formula: (s) solid (l) liquid (aq) aqueous: dissolved in water (g) gas Text Pg. 323 Chart of symbols used in chemical equations List three observations that suggest that a chemical reaction has taken place. Acids you have to know! HCl hydrochloric acid H2SO4 sulfuric acid HNO3 nitric acid H3PO4 phosphoric acid HC2H3O2 acetic acid Write the chemical equation from the following description: Zinc metal is added to hydrochloric acid to create zinc chloride and hydrogen gas. Aluminum reacts with oxygen to produce aluminum oxide A. B. C. Al + O Al2O3 Al + O2 Al2O3 Al3 + O Al2O3 Aluminum reacts with oxygen to produce aluminum oxide A. B. C. Al + O Al2O3 Al + O2 Al2O3 Al3 + O Al2O3 Phosphoric acid is produced through the reaction between tetraphosphorus decoxide and water A. H3PO4 P4 + H2O B. H3PO4 + H2O P4 C. P4O10 + H2O H3PO4 Phosphoric acid is produced through the reaction between tetraphosphorus decoxide and water A. H3PO4 P4 + H2O B. H3PO4 + H2O P4 C. P4O10 + H2O H3PO4 Iron(III)oxide reacts with carbon monoxide to produce iron and carbon dioxide A. B. C. FeO + CO Fe + CO2 Fe2O3 + CO Fe + CO2 Fe + CO Fe2O3 + CO2 Iron(III)oxide reacts with carbon monoxide to produce iron and carbon dioxide A. B. C. FeO + CO Fe + CO2 Fe2O3 + CO Fe + CO2 Fe + CO Fe2O3 + CO2 Coefficients whole numbers in front of formula distributes to numbers of atoms in formula specifies the relative number of moles and molecules involved in the reaction used to balance the equation Balancing Equations 1. 2. 3. 4. 5. 6. ONLY add/change coefficientsNEVER subscripts!!! balance one type of atom at a time balance polyatomic ions first balance atoms that appear only once second balance H and O last simplify if you can Check at end! Rules for writing and balancing equations – Pg. 327 in text. Writing Equations Write Word equations to help you organize reactants and products Be sure to include symbols showing states of each reactant and product Be sure to write the correct formula for each (crossing over for ionic compounds!) Check your balancing of the equation when you are finished Example 1 Description: Aqueous iron III oxide reacts with hydrogen gas to produce iron metal and liquid water Word Equation: Iron III oxide + hydrogen gas iron + water Example 1 Formula Equation: Fe2O3 (aq) + H2 (g) Fe Balanced Fe2O3 (aq) (s) + H2O (l) Formula Equation + 3H2 (g) 2Fe (s) + 3H2O (l) Example 2 Solid calcium metal reacts with water to form aqueous calcium hydroxide and hydrogen gas. calcium + water calcium hydroxide + hydrogen Ca(s) + H2O(l) Ca(OH)2(aq) + H2(g) Ca(s) + 2H2O(l) Ca(OH)2(aq) + H2(g) Example 3 solid zinc metal reacts with aqueous copper (II) sulfate to produce solid copper metal and aqueous zinc sulfate zinc Zn(s) Zn(s) + copper (II) sulfate copper + zinc sulfate + CuSO4 (aq) Cu (s) + ZnSO4 (aq) + CuSO4 (aq) Cu(s) + ZnSO4 (aq) Example 4 Hydrogen peroxide in an aqueous solution decomposes to produce oxygen and water hydrogen peroxide oxygen + water H2O2 (aq) O2 (g) + H2O (l) 2H2O2 (aq) O2 (g) + 2H2O (l) Example 5 Solid copper metal reacts with aqueous silver nitrate to produce solid silver metal and aqueous copper (II) nitrate copper + silver nitrate silver + copper (II) nitrate Cu (s) + AgNO3 (aq) Ag Cu (s) + 2AgNO3 (aq) 2Ag (s) (s) + Cu(NO3)2 (aq) + Cu(NO3)2 (aq) Example 6 Carbon dioxide gas is bubbled through water containing solid barium carbonate, creating aqueous barium bicarbonate carbon dioxide + water + barium carbonate barium bicarbonate CO2 (g) + H2O (l) + BaCO3 (s) Ba(HCO3)2 (aq) CO2 (g) + H2O (l) + BaCO3 (s) Ba(HCO3)2 (aq) Example 7 Acetic acid solution is added to a solution of magnesium bicarbonate to create water, carbon dioxide gas, and aqueous magnesium acetate. acetic acid + magnesium bicarbonate water + carbon dioxide + magnesium acetate HCH3COO (aq) + Mg(HCO3)2 (aq) H2O(l) + CO2 (g) + Mg(CH3COO)2 (aq) 2HCH3COO (aq) + Mg(HCO3)2 (aq) 2H2O(l) + 2CO2 (g) + Mg(CH3COO)2 (aq) Write the balanced formula equation for: Lithium metal is added to a solution of aluminum sulfate to make aqueous lithium sulfate and aluminum metal. Types of Chemical Reactions Types of Chemical Reactions 5 basic types discussed here not all reactions fall in these categories you should be able to: categorize a reaction predict the product(s) 1. Synthesis also called combination reaction reactants: more than one can be elements or compounds products: only one compound A + X AX where A is the cation and X is anion 1. Synthesis Rubidium and sulfur Rb (s) + S8 (s) Rb2S (s) Magnesium and oxygen Mg (s) + O2 (g) MgO (s) Sodium and chlorine Na (s) + Cl2 (g) NaCl (s) Magnesium and fluorine Mg (s) + F2 (g) MgF2 (s) 1. Synthesis calcium oxide and water CaO(s) + H2O(l) Ca(OH)2 (aq) sulfur dioxide and water SO2 (g) + H2O (l) H2SO3 (aq) calcium oxide and sulfur dioxide CaO (s) + SO2 (g) CaSO3 (s) 2. Decomposition opposite of synthesis usually require energy reactants: only one compound products: more than one usually elements but can be compounds AX A + X 2. Decomposition water H2O (l) H2 (g) + O2 (g) calcium carbonate CaCO3 (s) CaO (s) + CO2 (g) calcium hydroxide Ca(OH)2 (s) CaO (s) + H2O (l) carbonic acid H2CO3 (aq) CO2 (g) + H2O (l) 3. Single Replacement an element replaces a similar element in a compound reactants: 1 element & 1 compound products: 1 element & 1 compound A + BX B + AX Y + AX X + AY 3. Single Replacement zinc and hydrochloric acid Zn (s) + HCl (aq) ZnCl2 (aq) + H2 (g) iron and water Fe (s) + H2O (l) FeO (aq) + H2 (g) magnesium and lead (II) nitrate Mg (s) + Pb(NO3)2 (aq) Mg(NO3)3 (aq) + Pb chlorine and potassium bromide Cl2 (g) + KBr (s) KCl (s) + Br2 (g) (s) 4. Double Replacement two similar elements switch places reactants: 2 compounds products: 2 compounds AX + BY BX + AY 4. Double Replacement barium chloride and sodium sulfate BaCl2 (aq) + Na2SO4 (aq) NaCl (aq) + BaSO4 (s) iron sulfide and hydrochloric acid FeS (aq) + HCl (aq) FeCl2 (aq) + H2S (g) hydrochloric acid and sodium hydroxide HCl (aq) + NaOH (aq) NaCl (aq) + H2O (l) potassium iodide and lead (II) nitrate KI (aq) + Pb(NO3)2 (aq) KNO3 (aq) + PbI2 (s) 5. Combustion Only responsible for one type releases energy in form of heat/light reactants: hydrocarbon + O2 H2O and CO2 as the only products Ex: CH4 + O2 CO2 + H2O Combustion propane and oxygen C3H8(g) + O2(g) CO2(g) + H2O(g) Practice Classify each of the following reactions one of the five basic types: Na2O + H2O NaOH synthesis Zn (s) (aq) ZnCl2 (aq) + H2 (g) single replacement Ca (s) + 2HCl + 2H2O (l) Ca(OH)2 (aq) + H2 (g) single replacement Practice 2H2O2 (aq) decomposition Cu (s) single replacement (s) +Cu(NO3)2 (aq) + O2 (g) CO2 (g) + H2O combustion ZnO (s) (l) + 2AgNO3 (aq) 2Ag C2H4 (g) O2 (g) + 2H2O +C (s) 2Zn single replacement (s) (g) + CO2 (g) Practice Na2O (s) + H2O(l) Ca(OH)2 KCl (aq) + H2 (g) (s) + O2 (g) decomposition H2SO4 (aq) + NaHCO3 (s) single replacement KClO3 (s) (l) synthesis Ca(s) + 2CO2 (g) + H2O BaCl2 (aq) HCl double replacement (aq) + BaSO4 (s) Activity Series Activity Series Pg. 333 Activity ability of an element to react easier it reacts, higher the activity activity series list of elements organized according to activities from highest to lowest Activity Series metals greater activity, easier to lose electrons easier to become a cation nonmetals greater activity, easier to gain electrons easier to become an anion Activity Series used to predict whether single replacement reactions will occur most active is on top an element can replace anything below it but not any above it Practice zinc Zn and hydrofluoric acid (s) + HCl calcium and lead (II) nitrate and lithium sulfate Cu (s) + Li2SO4 (aq) no reaction bromine ZnCl2 (aq) + H2 (g) Ca (s) + Pb(NO3)2 (aq) Ca(NO3)2 (aq) + Pb (s) copper (aq) and iron (II) chloride Br2 (l) + FeCl2 (aq) no reaction