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Chemical Reactions Activity • On a blank sheet of paper, list all reactions that you can think of. – Ex: List animals • Cat, dog, fish, alligator, horse, lion… • Group the reactions you listed into columns across your paper. – Ex: Group animals • Cat Lion Dog Horse Fish Alligator Activity • Give a name to each group you formed. – Do they blow up? Form a gas? Etc. – Ex: Name animal groups • Feline Cat Lion Domestic Dog Horse Aquatic Fish Alligator • What group names did you come up with? Activity • How do we know that a chemical reaction has occurred? • Discuss: What criteria would you use to assess if a chemical reaction has occurred? Indicators of Chemical Reactions • • • • Light and Heat Gas Precipitate Color Change Characteristics of Chemical Equations • The equation must represent known facts. • The equation must contain the correct formulas for the reactants and products. • The law of conservation of mass must be satisfied. Word Equations • Represent the reactants and products in a chemical reaction with words • Only uses qualitative descriptions • Does not give quantities of products or reactants Methane + oxygen carbon dioxide + water Word Equations • Reactants on the left, products on the right • = yield, produce, or form Formula Equations • Represents the reactants and products of a chemical reaction by their symbols or formulas Methane + oxygen CH4(g) + O2(g) carbon dioxide + water OR CO2(g) + H2O(g) Formula Equations • Only uses qualitative descriptions; no amounts of reactants or products • To show the amounts of products and reactants, the equation must be balanced Balancing Equations • Coefficients must be added to a formula equation to be properly balanced. CH4(g) + 2O2(g) CO2(g) + 2H2O(g) Practice • Write word and formula equations for the following reactions: 1. Aluminum reacts with oxygen to produce aluminum oxide. 2. Iron (III) oxide reacts with carbon monoxide to produce iron and carbon dioxide. Practice 3. Solid sodium oxide is added to water at room temperature and forms sodium hydroxide (dissolved in the water). 4. Phosphoric acid is produced through the reaction between tetraphosphorus decoxide and water. Practice • Translate the following chemical equations into a sentence: 1. CS2(l) + 3O2(g) CO2(g) +2SO2(g) 2. BaCl2(aq) + Na2CrO4(aq) BaCrO4(s) + 2NaCl(aq) 3. NaCl(aq) + AgNO3(aq) NaNO3(aq) + AgCl(s) Significance of Chemical Equations • Debate: Pros vs. Cons of Chemical Equations – Take two minutes to come up with your arguments either for or against using chemical equations. Significance of Chemical Equations 1. The coefficients of a chemical reaction indicate relative, not absolute, amounts of reactants and products. 2. The relative masses of the reactants and products of a chemical reaction can be determined from the reaction’s coefficients. 3. The reverse reaction for a chemical equation has the same relative amounts of substances as the forward reaction. Balancing Chemical Equations 1. Write the word equation for the reaction. water hydrogen + oxygen 2. Write the formula equation. H2O(l) H2(g) + O2(g) 3. Balance the formula equation according to the law of conservation of mass. 4. Double check the number of atoms on each side. Steps: a. Balance the different types of atoms one at a time. b. First balance the atoms of elements that only appear once on each side of the equation. c. Next balance all other atoms. d. Balance H and O atoms LAST. Practice 1. The reaction of zinc with aqueous hydrochloric acid produces a solution of zinc chloride and hydrogen gas. 2. Magnesium and hydrochloric acid react to produce magnesium chloride and hydrogen. 3. Aqueous citric acid reacts with solid magnesium hydroxide to produce aqueous magnesium nitrate and water. 3-2-1 • 3 things you learned • 2 connections you made • 1 question you still have Activity • Groups of 3-4 people • Design your own equation for your classmates to balance. • Each group will present their equation, so the class can balance it. • Be prepared to explain the correct balancing and answer any questions from your classmates. Synthesis Reaction • A + B → AB 1. 2Mg + O2 → 2MgO 2. Na(s) + Cl2(g) → 3. MgO + H2O → 4. Sodium reacts with fluorine to produce sodium fluoride. Combustion • CxHy + O2→ CO2 + H2O 1. C10H8 + 12 O2 → 10 CO2 + 4 H2O 2. CH4(g) + O2(g) → 3. The burning of propane, C3H8, results in the production of carbon dioxide and water vapor. Single- Displacement • E+C→E+C 1. Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s) 2. Br2 + KCl → 3. Mg + HCl → 4. When solid aluminum is placed in aqueous lead(II) nitrate, the aluminum replaces the lead and solid lead and aqueous aluminum nitrate are formed. Double-Displacement • AB + CD → CB + AD 1. NaCl + AgNO3 → NaNO3 + AgCl 2. HCl(aq) + NaOH(aq) → 3. KI + Pb(NO3)2 → 4. Iron (II) sulfide reactions with hydrochloric acid to form hydrogen sulfide gas and iron (II) chloride. Decomposition • C→ 1. H2SO4 → H2O + SO3 2. HgO(s) → 3. KClO3 → 4. Calcium hydroxide decomposes to produce calcium oxide and water. Discuss • What if there was no combustion reaction? What would be different in your life? • What would be an alternative to using the activity series? What type of reaction was this demonstration? A. B. C. D. E. Synthesis Reaction Decomposition Reaction Single-Displacement Reaction Double-Displacement Reaction Combustion Reaction Carousel Brainstorming