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Chemistry Chapters 6 & 7: Reactions and Balancing Equations Explained

This guide explores the meaning of chemical symbols, formulas, and equations, including types of reactions like synthesis, decomposition, and combustion. Learn how to balance equations and understand the Law of Conservation of Mass. Discover the steps in balancing redox reactions and the significance of oxidation and reduction.

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Chemistry Chapters 6 & 7: Reactions and Balancing Equations Explained

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  1. By: Dillon Menard Chemistry Chapters 6 & 7

  2. Intro to Ch. 6 & 7 • What does it mean? • Chemical symbols represent elements • Chemical formulas represent compounds • Chemical equations represent reactions • General form of a chemical reaction • Reactants  Products (Substances enter in reaction) ( Substances formed in reaction) • Use subscripts after formulas to indicate the sate of products & reactants • (s) or (cr) = Solids • (l) = Liquids • (g) = Gas • (aq) = Aqueous • (ppt) = Precipitate

  3. Balancing Equations • Law of Conservation of Mass Matter– Matter is not created or destroyed in a chemical reaction. • Atoms are the smallest particles to take place in a reaction, so we must make the total numbers of atoms of each element the same on the reactant side and on the product side • STEPS IN BALANCING EQUATIONS • Correctly write formulas for all reactants and products, using + signs to separate substances. • Make chart that lists all the elements present ( H and O last) • Count the number of atoms of each element and use coefficients as multipliers in front of formulas as needed

  4. Types of Chemical Reactions • Synthesis – When a single compound is formed from simpler compounds or from elements • A + B + C = Compound ( 2H + O2  2H2O ) • Decomposition – When a compound breaks apart into simpler substances • Compound = B + C + D ( 2H2O2  2H2O + O2 ) • Single Replacement – An element combines with a compound to form a new compound and a new element • A + BC  B + AC ( 2Na + CaCl2  2NaCl + Ca )

  5. Double Replacement – The positive ions of two compounds exchange partners. • AB + CD  CB + AD (AgNo3 + NaCl  AgCl + NaNo3) • Combustion – Burning in the presence of oxygen (Two special cases) • Hydrocarbon + Oxygen  Co2 + H2O • CxHy + O2  CO2 + H2O • Carbohydrate + Oxygen  CO2 + H2O • CxHyOz + O2  CO2 + H2O • Two special Double Replacements • Acid + Base  A “salt” + water • HX +BOH  BX + H2O • Two solutions  Precipitate + Another compound

  6. “Redox” Reactions • Oxidation formerly meant “combining with oxygen” • Becomes more positive • Reduction means a “gain of electrons” • Becomes more negative

  7. Steps In Balancing “Redox” Reactions • Step 1 – Find total charges of each element • Step 2 – Connect elements in which the charge has changed • Step 3 – Find gain and loss of electrons • Step 4 – Find change in original subscripts • Step 5 – Find min gain and min loss

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