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Chemical Changes (Reactions)

Chemical Changes (Reactions). Reactants Products Synthesis Single Replacement Double Replacement Decomposition. Chemical Reactions. Indicators Fizzing (gas produced) Color change Gets cloudy/precipitant (solid produced) Heat released or absorbed Light emitted Odor changes.

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Chemical Changes (Reactions)

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  1. Chemical Changes (Reactions) • Reactants • Products • Synthesis • Single Replacement • Double Replacement • Decomposition

  2. Chemical Reactions • Indicators • Fizzing (gas produced) • Color change • Gets cloudy/precipitant (solid produced) • Heat released or absorbed • Light emitted • Odor changes

  3. Chemical Reactionshttp://ed.ted.com/lessons/if-molecules-were-people-george-zaidan-and-charles-morton • Reactants  Products • H2O2 H2O + O2 • What are the reactants? What are the products?

  4. Chemical Reactions There are 4 kinds of Chemical Reactions that occur: Synthesis Decomposition Single Double Replacement Replacement

  5. Chemical Reactions • Synthesis • Two or more reactants are combined to form one product. +

  6. Chemical Reactions • Decomposition • One reactant breaks down into two or more products. +

  7. Chemical Reactions • Single Replacement • An element and a compound combine. • One element from the reactants replaces another in the products. + +

  8. Chemical Reactions • Double replacement • Two compounds combine. • Two elements in the reactants switch places in the products. + +

  9. Chemical Reactions-Practice Identifying • Example #1 • H2 + O2 H2O Which is it? • Synthesis • Decomposition • Single Replacement • Double Replacement

  10. Chemical Reactions Which is it? • Synthesis • Decomposition • Single Replacement • Double Replacement • Example #2 • Li3P  Li + P

  11. Chemical Reactions Which is it? • Synthesis • Decomposition • Single Replacement • Double Replacement • Example #3 • Na + MgCl2 Mg + NaCl

  12. Chemical Reactions • Example #4 • SiCl4 + O2 SiO + Cl2 Which is it? • Synthesis • Decomposition • Single Replacement • Double Replacement

  13. Chemical Reactions • Example #5 • C5O3 C + O2 Which is it? • Synthesis • Decomposition • Single Replacement • Double Replacement

  14. Chemical Reactions • Example #6 • Rb2O + AlF3 RbF + Al2O3 Which is it? • Synthesis • Decomposition • Single Replacement • Double Replacement

  15. Chemical Reactions Law of conservation of Matter Atoms are not created or destroyed The number of atoms at the START of a reaction, there must be the same number of atoms AFTER the reaction. Equations must be balanced!

  16. Chemical Reactions Balancing Chemical Equations STEPS: Count the number of atoms for each element in the reactants and in the products. Compare the numbers to see if each element is balanced (equal) with itself. Use WHOLE NUMBER coefficients to “fix” unbalanced elements. Do not change the subscripts!

  17. Chemical Reactions • Example #1 • H2 + O2 H2O

  18. Chemical Reactions • Example #2 • Li3P  Li + P

  19. Chemical Reactions • Example #3 • Na + MgCl2 Mg + NaCl

  20. Chemical Reactions • Example #4 • SiCl4 + O2 SiO + Cl2

  21. Chemical Reactions • Example #5 • C5O3 C + O2

  22. Chemical Reactions • Example #6 • Rb2O + AlF3 RbF + Al2O3

  23. Chemical Reactions • Example #7 SnO2 + H2 → Sn + H2O

  24. Chemical Reactions • Example #8 • Mg(ClO3)2 + Na  NaClO3 + Mg

  25. Chemical Reactions • Example #9 • Al2(SO4)3 + RbF  AlF3 + Rb2SO4

  26. Chemical Reactions • Identify and Balance • Al + F2 AlF3

  27. Chemical Reactions • Identify and Balance • Ca(MnO4)2 + FeCl4 CaCl2 + Fe(MnO4)4

  28. Chemical Reactions • Identify and Balance • Si3O  Si8 + O2

  29. Chemical Reactions • Identify and balance • Cs2O + N2 Cs3N + O2

  30. Warm Up • Classify the following chemical reactions as decomposition, single replacement, double replacement or synthesis: • For the first equation, what are the reactants and what are the products? • Write the chemical formula for Barium Nitride

  31. Acids and Bases

  32. Acids & Bases • Acids • Examples: Citric Acids, Gastric Acid, Battery Acid, Sodas, tomatoes, etc. • Properties: corrosive, produce H+ ions, sour taste, electrolytes, pH range = 0-6.9 • Examples of Formulas: HCl, H2SO4, H3PO4, HNO3, etc

  33. Acids & Bases • Bases • Examples: Soaps, Cleaning supplies, Hair Relaxers, etc. • Properties: corrosive, produce OH- ions, bitter taste, electrolytes, slippery feel, ph range 7.1 to 14 • Examples of Formulas: NaOH, KOH, Mg(OH)2, Al3(OH), NH3, NH4OH

  34. Acids & Bases-pH Scale

  35. Acids and Bases-Compare & Contrast

  36. 9. Electrolyte 10. pH = 13 11. pH = 4 12. H2SO4 13. HBr 14. FrOH 15. Corrosive 16. Bitter taste Acids and Bases--Identify • pH =2 • HF • pH= 7 • RbOH • Ca(OH)2 • pH= 9 • Sour taste • Slippery feel

  37. Acids & Bases • Neutralization Reactions • Only an Acid can neutralize a base, and only a Base can neutralize an acid. • H+ comes off of the Acid and OH- comes off of the Base • Acid + Base  Water + Salt • HCl + KOH  H2O + KCl

  38. Acid/Base Neutralization • HBr + LiOH  _________ + _________ • FrOH + HCl  _________ + _________ • H2S + Mg(OH)2 ________ + _______ • ______ + HF  H20 + KF • ______ + CsOH  H20 + CsI

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