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Identify, give evidence for, predict products of, and classify the following types of chemical reactions: 1. Synthesis (combination) 2. Decomposition 3. Single Replacement 4. Double Replacement 5. Neutralization (acid/base) 6. Combustion Synthesis Decomposition Neutralization Single displacement Double displacement Combustion A chemical change: any change in which a new substance is formed. Evidence of a Chemical Change: Release of energy as heat Release of energy as light Change in color Formation of a gas Change in odor… 1. Neutralization: Acid(H) + Base(OH) salt + H(OH) 2. Combustion: AB + oxygen CO2 + H2O 3. Synthesis: A + B AB 4. Decomposition: AB A + B 5. Single displacement: A + BC AC + B 6. Double displacement: AB + CD AD + CB Synthesis reactions are also known as FORMATION reactions. Two or more reactants (usually elements) join to form a compound. – A + B AB where A and B represent elements – The elements may form ionic compounds, like… – Sodium metal and chlorine gas combine to form sodium chloride. – 2Na + Cl2 2NaCl Sodium added to chlorine gas See pages 258 - 259 (c) McGraw Hill Ryerson 2007 Types: Synthesis Example C + O2 C + O O O C O C C O O C CC O O C C C C C C CC C General: A + B AB OTHER EXAMPLES… 1. Elements that form ionic compounds: Magnesium metal reacts with oxygen gas to form magnesium oxide. • 2Mg + O2 2MgO 2. Elements that form covalent compounds: Nitrogen gas and oxygen gas join to form dinitrogen monoxide. • 2N2 + O2 2N2O SYNTHESIS REACTION (iron + sulphur): http://www.youtube.com/watch?v=A5H6DVe5FAI (c) McGraw Hill Ryerson 2007 See pages 258 - 259 • Decomposition reactions are the opposite of synthesis reactions. – A compounds breaks down into two or more products (often elements). –AB A + B where A and B represent elements 1. Ionic compounds may decompose to produce elements, like the following: • Table salt, sodium chloride, can be broken down into sodium metal and chlorine gas by melting salt at 800ºC and running electricity through it. • 2NaCl 2Na + Cl2 See page 260 (c) McGraw Hill Ryerson 2007 See page 260 (c) McGraw Hill Ryerson 2007 Types: Decomposition Example: NaCl Cl Na General: Cl + Na AB A + B Types: Decomposition Example 2HgO O Hg O Hg General: Hg + O O Hg AB A + B 2. Covalent compounds may decompose into elements, like the following: • By running electricity through water, the water molecules decompose into hydrogen and oxygen gases. • 2H2O 2H2 + O2 DECOMPOSITION REACTION: http://www.youtube.com/wa tch?v=NddwtXEA_Ak See page 260 (c) McGraw Hill Ryerson 2007 • Single replacement reactions replace one element from a compound with another element. – A compound and an element react, and the element switches places with part of the original compound. • A + BC B + AC where A is a metal, or • A + BC C + BA where A is a non-metal See page 261 (c) McGraw Hill Ryerson 2007 Types: Single displacement Example: Zn + CuCl2 Cu Cl + Cl General: Zn Zn Cl + Cu Cl AB + C AC + B 1. When A is a metal: • Aluminum foil in a solution of copper(II) chloride produces solid copper and aluminum chloride. • 2Al + 3CuCl2 3Cu + 2AlCl3 2. When A is a non-metal: • When fluorine is bubbled through a sodium iodide solution, iodine and sodium fluoride are produced. • Fl2 + 2NaI I2 + 2NaF SINGLE REPLACEMENT: http://www.youtube.com/watch?v=hKtynbVtMKc • Double replacement reactions swap elements between 2 compounds that react together to form two new compounds. – Two compounds react, with elements switching places between the original compounds. AB + CD AD + CB See page 262 (c) McGraw Hill Ryerson 2007 See page 262 (c) McGraw Hill Ryerson 2007 Types: Double displacement Example: MgO + CaS Mg + O General: Ca S Mg S + Ca O AB + CD AD + CB Two solutions react to form a precipitate (solid) and another solution. Ionic solution + ionic solution ionic solution + ionic solid. AB + CD AD + CB – When potassium chromate and silver nitrate react, they form a red precipitate, silver chromate, in a solution of potassium nitrate. – K2CrO4 + 2AgNO3 Ag2CrO4 + 2KNO3 silver chromate DOUBLE REPLACEMENT: http://www.youtube.com/watch?v=opY3FLrPTa4 (c) McGraw Hill Ryerson 2007 • Neutralization reactions occur when an acid (most compounds starting with H) and a base (most compounds ending in OH) react to form a salt and water. • Neutralization reactions are a type of double replacement. • Acid + base salt + water HX + MOH MX + H2O where X and M are elements See page 263 (c) McGraw Hill Ryerson 2007 1. Sulfuric acid is used to neutralize calcium hydroxide: • H2SO4 + Ca(OH) 2 CaSO4 + 2H2O 2. Phosphoric acid helps to neutralize the compounds that cause rust, such as iron(II) hydroxide. • H3PO4 + 3Fe(OH)2 Fe3(PO4)2 + 6H2O NEUTRALIZATION: http://www.youtube.com/watch?v=_P5hGzA6Vb0 See page 263 (c) McGraw Hill Ryerson 2007 • Combustion reactions occur when a compound or element react with oxygen to release energy and produce an oxide. – Also sometimes referred to as hydrocarbon combustion. CXHY + O2 CO2 + H2O where X and Y represent integers METHANOL + oxygen: http://www.youtube.com/watch?v=98JuJ-G1qXY&feature=related See page 264 (c) McGraw Hill Ryerson 2007 TYPES OF COMBUSTION REACTION • COMPLETE COMBUSTION: • A combustion reaction of hydrocarbons that uses all the available fuel and produces only carbon dioxide, water and energy. This reaction can occur when there is plentiful oxygen. Example: CH4 + 2O2 CO2 + H2O Types of Combustion • INCOMPLETE COMBUSTION: • A Combustion reaction of hydrocarbons that may produce carbon, carbon monoxide, carbon dioxide, soot, water and energy. • This reaction occurs when there is insufficient supply of oxygen. COMBUSTION • Combustion of Hydrogen: • 2H2 + O2 2H2O • Combustion of phosphorus: • P4 + 5O2 P4O10 1. Natural gas (methane) is burned in furnaces to heat homes. »CH4 + O2 CO2 + 2H2O + energy 2. An acetylene torch is used to weld metals together. »2C2H2 + 5O2 4CO2 + 2H2O + energy 3. Carbohydrates like glucose combine with oxygen in our body to release energy. Acetylene torch »C6H12O6 + 6O2 6CO2 + 6H2O + energy See page 264 (c) McGraw Hill Ryerson 2007 MOVIE TO REVIEW: http://www.bcscience.com/bc10/pgs/videos_013_chemical_reactions.html (c) McGraw Hill Ryerson 2007 Take the Section 6.1 Quiz See page 265