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Chemistry Chapters 6 & 7

By: Dillon Menard. Chemistry Chapters 6 & 7. 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

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Chemistry Chapters 6 & 7

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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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